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Glossary/Index

A taste of 177 Alanine (Ala, A) triprotic. See Triprotic acid silk and 690 Abbreviated electron configuration, of types 162 structure of 678 multi-electron atoms 433–436 weak 163–165 Alar 361 Absolute zero Zero kelvins (0 K), the Acid-base reaction 180–188 Alcohol Compounds that contain a lowest possible temperature, equiva- strong acid with base hydrocarbon group with one or more - ° lent to 273.15 C. It is the point 181–185 -OH groups attached. 84, 663. See beyond which motion can no longer uses 180 also Methanol, Ethanol, and 2-pro- be decreased. 18 writing equations 183 panol Accuracy How closely a measured Acidic paper, preserving books with 187 bonds and 555 value approaches the true value of the Acidic solution A solution with a sig- Aldehyde A compound that has a hy- property. 20 nificant concentration of drogen atom or a hydrocarbon group Acetaldehyde, determining Lewis struc- + , H3O . 160 connected to a -CHO group. 665 ture 464–465 Acid rain 167 Aldol, molecular structure of 669 Acetamide 668 pH and 178 Alka-Seltzer 526 , solubility of compounds Acrylamide 621 Alkaline earth metals Group 2 (or 2A) with 141 Activated complex 611 on the periodic table; See also Beryl- Acetic acid 162–165, 664 Activation energy The minimum lium, Magnesium, and Calcium 43 dissolved in water 164 energy necessary for reactants to reach ion charges of 97 formulas 162 the activated complex and proceed to Alkali metals Group 1 (or 1A) on the freezing point of 162 products. 612 periodic table; See also Lithium, So- glacial 162 Active site A specific section of the pro- dium, Potassium, and Cesium 43 molecular structure of 162 tein structure of an enzyme in which as organic acid 162 ion charges of 96–97 the substrate fits and reacts. 69 0 Alkane A hydrocarbon (a compound production 528, 654 Actual yield The amount of product solubility in water 593 composed of carbon and hydrogen) in that is actually obtained in a chemical which all of the carbon-carbon bonds taste of 160 reaction. 382 uses 162, 654 are single bonds. 661 Adams, Mike 674 Alkene A hydrocarbon that has one or as weak acid 163 Addition, rounding off for 29 9–300 Acetone 666 more carbon-carbon double bonds. Addition polymer A polymer that con- 662 boiling point of 546 tains all of the atoms of the original evaporation of 536 Alkyne A hydrocarbon that has one or reactant in its structure. This category more carbon-carbon triple bonds. use 567 includes polyethylene, polypropylene, vapor pressure of 540 662 and poly(vinyl ). 693–694 Alpha emission The process of releas- Acetylene 451, 662 Adipic acid 351 molecular structure of 451 ing an alpha particle by atoms that Adults have too many protons to be stable. water solubility of 580 effects of ionizing radiation on 73 0 See also 720 Acid. Arrhenius acid fingerprints of 54 1 See nuclear equations for 723–725 binary. Binary acid Aerosol can 541 Alpha helix 680–681 bleach and 188 Agent Orange 364 Alpha particle The emission from ra- Brønsted-Lowry 188–192 Aging, oxidizing agents and 212 dioactive nuclides that is composed of conjugate acids and bases 189 Agitation, rate of solution and 590–591 See two protons and two neutrons in the carboxylic acid. Carboxylic acid Agricultural Research Service of North form of a helium nucleus. 720 characteristics 160 Carolina State University 266 effects on body 73 0–731 classification of strong or weak 16 6, AIDS 673 penetration of the body 731 176–177 Air 509–510 Alternate Synthetic Pathways Award 621 defined 18 8 density of 302 See Alternative Solvents/Reaction Conditions diprotic. Diprotic acid gases in 510 Award 272 identifying 176–177 internal combustion engine and See Alum. See Aluminum monoprotic. Monoprotic acid 492 Aluminum 44 names and formulas of 168–170 in lungs 493 See ion formation 49, 97 . Oxyacid Air bags 526 Aluminum , production and use pH 178–179 Air pollution See 235 polyprotic. Polyprotic acid catalytic converters and 221 Aluminum chloride 108 in saliva 177 ozone and 266–267 strong 165 volatile organic solvents and 514 Aluminum fluoride, production and use Study Sheet, indentifying 176 401 G-1 G-2 Glossary/Index

Aluminum hydroxide, dissolving in acid Amphoteric substance A substance Arrhenius acid According to the 184 that can act as either a Bronsted- Arrhenius theory, any substance that + Aluminum 132 Lowry acid or a Bronsted-Lowry base, generates hydronium ions, H3O , Aluminum sulfate depending on the circumstances. 191 when added to water. 160–167. See old books and 187 Amylase 688 also Acid production and use 410 Amylopectin 676–677 binary acid 162 water purification 37 4 Amylose 676–677 compared to Brønsted/Lowry acids Americium-241 and smoke detectors Analogies, to electron behavior 414 188–192 735 Anastas, Paul T. 5 defined 16 0 Amide A compound with the general Anderson, Carl 437 names and formulas for 168–170 formula RCONR, in which each R Androstenedione 686, 687 organic (or carbon-based) acid 162 represents hydrogen atoms or hydro- Aniline, production and use 399, 402 162 carbon groups. 668 Animal fat 585 reactions with bases 180–187 in digestion 689 Anion An ion formed from an atom strong and weak 163–166 as peptide bond 680 that has gained one or more elec- Arrhenius base A substance that Amine A compound with the general trons and thus has become negatively produces hydroxide ions, OH-, formula R3N, in which R represents charged. 49 when added to water. 174–178. See a hydrogen atom or a hydrocarbon formation 95–96 also Base group (and at least one R group being in batteries 225–226 compared to Brønsted/Lowry bases a hydrocarbon group). 667–668 in classifying types of compounds 188–192 1-Aminobutane 667 78 defined 17 3 Aminopeptidase 688 in ionic bond formation 75–76 reactions with acids 180–187 Amino acid The monomer that forms monatomic 96 strong and weak 173–176 the protein polymers. They contain an naming 98–99, 104–106 Arsenic (As) amine and a carbox- polyatomic 101–103 bonding patterns of 452 ylic acid group separated by a carbon. structure of ionic compounds 100 most common bonding pattern 455 678–679 writing formulas 107–108 Asparagine (Asn, N), structure of 679 in origin of life 640-642 Anode The electrode at which oxida- Aspartame 705, 711 protein fomation and 680 tion occurs in a voltaic cell. It is the Aspartic acid (Asp, D) in silk 690 source of electrons and is the negative in bridges 682 173–174 electrode. 225 structure of 679 covalent bond formation 451 Antacid 126, 506 Asphalt, London forces in 556–557 hydrogen bonds and 555 Antarctica, ozone hole over 271 Asymmetry, in polar 552, 553 Lewis structure of 81 Anthropogenic sources, of methyl bro- Atmosphere, layers 268 molecular geometry 469 mide 272 Atmosphere (atm), as unit of pressure molecular shape of 87 Anti-electron (positron) 437 485 origin of life and 641 Antimatter 437 Atmospheric pressure 485 pH of 179 Antioxidant, aging and 212 boiling-point temperature and production 504, 621 Antiparticle 437 545–546 uses 173, 570 Antiseptic, iodine as 556 Atom The smallest part of the element weak base 173–174 Application, in scientific method 8 –9 that retains the chemical characteris- , use 653 Aquamarine 362 tics of the element itself. 46–48 Ammonium chloride, crystal structure Aqueous solution A solution in which atomic numbers of 51 of 101 water is the solvent. 134 chemical bonds between 73–77 Ammonium ion Arene (or aromatic compound) A com- in chemical reactions 126–128 covalent bond formation 452 pound that contain the benzene ring. counting by weighing 331–334 Lewis structure 101 662–663 electron 48 solubility of compounds with 141 Arginine (Arg, R), structure of 679 electron configurations and orbital Ammonium , in cold packs 264 Argon diagrams 424, 431, 456 Ammonium , space shuttle in air 510 excited and ground state 421 and 245 in incandescent light bulbs 496 as formula unit 339 Ammonium , fertilizers and in neon lights 509 mass numbers of 51–52 213 Aromatic. See Arene A compound that molar mass of 335–336 Ammonium , use 10 8 contain the benzene ring. nuclear reactions of 720–724 Amount of substance, base unit of 10 Aromatic compounds. Compounds that nuclear stability of 718 Amphere, as unit of measure 11 contain the benzene ring. See Arene oxidation numbers of 213–220 Amphetamine 582 Arrhenius, Svante August 160 protons, neutrons, and electrons 47 Glossary/Index G-3

radioactive decay of 720–724 Bacteria 236 into electrical energy using redox reac- size of 47 tooth decay and 186 tions. 224–229. See also Voltaic cell size of nucleus 47 Baking powder 73 defined 22 4, 225 structure of 46–50 Balance, electronic 23, 300 dry cell 226–227 Atomic mass The weighted average of Balanced chemical equation nickel-cadmium batteries 228 the masses of the naturally occurring coefficient12 7 rechargeable 228 isotopes of an element. coefficients to conversion factors zinc-air 229 calculations 336 369–370 Beef fat 584–585 defined 33 3 in equation stoichiometry 368–375 Bends, the 596 relative 333 Balancing chemical equations 128–133 Benitoite 362 Atomic mass unit (u or amu) One- steps in 129 Bent geometry The molecular geom- twelfth the mass of an atom of Study Sheet 129 etry formed around an atom with two carbon-12. Carbon-12 is the isotope Ball-and-stick model A representation bond groups and two lone pairs or of carbon that contains 6 protons, of a that uses balls for atoms two bond groups and one lone pair. 6 neutrons, and 6 electrons. 47, and sticks for covalent bonds. 54 469 332–333 of acetic acid molecule 162 Benzedrine 582 Atomic number The number of pro- for acetylene 471 Benzene 351 tons in an atom’s nucleus. It estab- for boron trifluoride 47 0 Berkelium (Bk) 725 lishes the element’s identity. 51 for ethane 471 Beryllium (Be) in nuclear equations 722–726 for methane 468 electron configuration and orbital in nuclides 716–717 for organic molecules 660 diagram 426 Atomic orbitals of ammonia 87 formation of 742 1s 416–418 of methane 87 Beta emission The conversion of a 2p 421 of water 88 neutron to a proton, which stays in 2s 419–420 Band of stability On a graph of the the nucleus, and an electron, called a 3d 422 numbers of neutrons versus protons beta particle in this context, which is electron cloud 418 in the nuclei of atoms, the portion ejected from the atom. 720 electron spin and 426 that represents stable nuclides. 719 nuclear equations for 723–725 for first 10 elements 42 7 Barium ion, solubility of compounds Beta particle A high-velocity electron order of filling 42 5, 428–430 with 141 released from radioactive nuclides that probability and 418 Barium sulfate 143 have too many neutrons. 720 relative energies 420 Barnes, Randy 687 effects on body 73 0–731 See also shapes 419 Base 173–177. Arrhenius base penetration of the body 731 Atomic weight See also Atomic mass Arrhenius 174 Beta sheet 680 333 Brønsted-Lowry 188–192 Big Bang 742 Binary acid Attraction. See also Gravitational attrac- carbonate 175 Substances that have the aq tion; Electrostatic attraction; Strong classification of strong or weak general formula of HX( ), where 176–177 X is one of the first four halogens: force; Particle-particle attractions conjugate 190 HF(aq), HCl(aq), HBr(aq), and between gas particles 484 defined 17 3 HI(aq). 162 between liquid particles 534 identifying 175–176 formulas 168 intermolecular 547–557 in acid-base reactions 180–188 naming 168 particle-particle attraction 547–562 pH 178–179 Binary covalent compound A com- Aurum 41 strong 173 pound that consists of two - Automobile Exhaust 71 Study Sheet, indentifying 176 lic elements. Average, weighted 331 weak 174–175 memorized names 90 Avogadro’s Law Volume and the Base units The seven units from which names without prefixes 9 3 number of gas particles are directly all other units in the SI system of naming 91–92 proportional if the temperature and measurement are derived. 10–11 prefixes used to name 9 1 pressure are constant. 491 table of 11 recognizing from formulas 91 Avogadro’s number The number of Basic solution A solution with a recognizing from names 93 atoms in 12 g of carbon-12. To four significant concentration of hydroxide systematic names 90–92 significant figures, it is 6.022× 1023. ions, OH-. 173 writing formulas 93–94 333–334 Battery A device that has two or more Binary An ionic B voltaic cells connected together. The compound whose formula contains term is also used to describe any one symbol for a metal and one sym- Bacon, Roger 287 device that converts chemical energy bol for a nonmetal. 104 G-4 Glossary/Index

Binding energy The amount of energy and 740 Cadmium (Cd) released when a nucleus is formed. Boron trifluoride 45 3 in nickel-cadmium batteries 228 737 Bovine pancreatic trypsin inhibitor nuclear plant control rods and 740 Biocatalyst 621 (BPTI) 680–682 Caffeine 59 7 Biochemistry The of biologi- Boyle’s Law The pressure of a gas is in- removal from coffee 51 5 cal systems. 674–687 versely proportional to the volume it taste of 159 Biomolecule 674–687 occupies if the number of gas particles Calamine 364 amino acids and protein 678–682 and the temperature are constant. Calcium (Ca), ion formation 97 carbohydrate 674–677 486–487 Calcium , production 402 how form 640–642 Brain, intoxicating liquids and 89 Calcium carbonate 126, 264, 616 steroid 685–686 Brain cancer, treatment for 741 acid rain and 167 triglycerides 683 Brandes, Jay A. 641 as antacid 506 Bismuth, in the creation of element 111 Breathing 493 formation in pipes of 144 52 Bristlecone pines and carbon-14 dating in limestone caverns 204 Bitter taste 177 734 natural sources of 144 Blake, William 413 Bromide ion, solubility of compounds oil production and 186 Bleach with 141 precipitation reaction 137–140 dangerous combination with acid Bromine (Br) solubility in water 593 188 in halons 272 Calcium chloride 126 pH of 179 most common bonding pattern 455 Calcium dihydrogen phosphate, Blocks, in periodic table 428–429 structure 55 production and use 407 Blood use 570 Calcium hydrogen , production pH of 179 Bromomethane, and threshold limit and use 243 Blue litmus paper, detecting acids with value, or TLV 522 Calcium nitrate 108, 137–138 180 Brønsted-Lowry acid A substance that Calcium phosphide (or photophor), Boiling The conversion of liquid to va- donates protons, H+, in a Bronsted- empirical formula for 348 por anywhere in the liquid rather than Lowry acid-base reaction. See Acid, Calorie (with an uppercase C), Cal just at the top surface. 542–546 Brønsted-Lowry The dietary calorie. In fact, a Calorie defined 54 4 Brønsted-Lowry acid-base reaction A is a kilocalorie or 4184 joules. 257 how bubbles form 542–544 chemical reaction in which a proton, calorie (with a lowercase c), cal A Boiling-point temperature The H+, is transferred. See Acid-base reac- common energy unit. Equivalent to temperature at which a liquid boils. tion, Brønsted-Lowry 4.184 joules. 257 It is also the temperature at which Brønsted-Lowry base A substance that Cancer, boron fusion and 741 the equilibrium vapor pressure of the accepts protons, H+, in a Bronsted- Capsaicin 583 Carbohydrate liquid becomes equal to the external Lowry acid-base reaction. See Base, Sugar, starch, and pressure acting on the liquid. 544 Brønsted-Lowry cellulose. Also called saccharides. effect of external pressure 54 4–546 Bubbles 674–677 Carbon-13 733 strengths of attractions and 546 in boiling liquid 544 Carbon-14, radioactive decay of 733 Bond. See Chemical bond how form in liquid 542–544 Carbon-14 dating The process of Bond angle The angle formed by in soft drinks 596 determining the age of an artifact that straight lines (representing bonds) Bunsen burner, hottest part of flame 31 4 contains material from formerly living connecting the nuclei of three adja- Bureau International des Poids et plants or animals by analyzing the cent atoms. 86, 468 Mesures (BIPM) 11 ratio of carbon-14 to carbon-12 in the Bond dipole A polar covalent bond, Butadiene 524 object. 733–734 which has an atom with a partial posi- Butane, molecular structure of 82 Carbonate ion 175 tive charge and an atom with a partial 1,4-Butanediol (BD) 354 reaction with acids 185 negative charge. 549 Butanoic acid solubility of compounds with 141 Bond polarity, predicting 548–552 molecular structure of 583, 664 in weak bases 175 Books, preserving 187 solubility of 583 Carbonic acid 597 Boron (B) 2-Butanone 666 Carbon (C) 48 brain cancer treatment and 741 Butylated hydroxytoluene (BHT) 662 bonding pattern 82 covalent bonding pattern 454 Butyl ethyl ether 660 combustion and 219 covalent bond formation 453 Butyric acid 664 covalent bond formation 450–451 electron configuration and orbital diamond as 47 diagram 426 C electron configuration and orbital nuclear power plant control rods Cadaverine 667 diagram 426–427 Glossary/Index G-5

in heavy-ion therapy 52 tion occurs in a voltaic cell. It is the double bond 83 isotopes of 333 positive electrode. 225 energy and 253–254 medical use 52 Cation An ion formed from an atom ionic bond 75–77 most common bonding pattern 455 that has lost one or more electrons most common bonding patterns 83 in pig iron 509 and thus has become positively nonpolar covalent 74 Carbon black 381 charged. 49 polar covalent 74 Carbon dioxide formation of 95, 96–97 predicting bond type 77–79, in automobile exhaust 71 monatomic 548–549 as dry ice 255 naming 99 summary 76 catalytic converter and 221 roles in body 100 triple bond 83 in combustion reactions 219 names 105 Chemical change. See Chemical reaction decaffeinating coffee and51 5 polyatomic 101 . See Compound global warming and 384 produced by ionizing radiation 730 Chemical Elements. See Element greenhouse gas 597 Celgene Corporation 673 Chemical engineering 609 Lewis structure of 83 Cellulose 674, 676–677 Chemical equation 126–133 polarity 552 molecular structure of 677 for acid-base reactions 183–187 in soft drinks 596 Celsius scale 18–19 balancing 128–133 solid to gas 576 Celsius to Fahrenheit conversion polyatomic ions 129, 132 solubility in water 593 312–314 Study Sheet 129 spray painting and 514 Celsius to Kelvin conversion chemical calculations and 367 supercritical 514 312–314 complete 140 Carbon dioxide torpedos 597 Cesium (Cs), electron configuration of complete ionic 139 Carbon monoxide 434 heat and 128 catalytic converters and 221 Cesium-137 730 interpreting 126–128 covalent bond formation 453 Cesium chloride, crystal structure of molecular 140 in hydrogen gas production 622 101–102 net ionic 140 incomplete combustion and 221 Chain-growth (or addition) poly- physical states and 127 Lewis structure of 453 mers A polymer that contains all of special conditions and 127–128 as pollutant 221 the atoms of the original reactant in Chemical equilibrium. See Equilibrium in synthesis gas 622 its structure. This category includes A concise writ- Carbon tetrachloride, use and produc- polyethylene, polypropylene, and ten description of the components tion 526 poly(vinyl chloride). 693 of a chemical compound. It identi- Carboxylic acid A compound that have Chain reaction A process in which one fies the elements in the compound a hydrogen atom or a hydrocarbon of the products of a reaction initiates by their symbols and indicates the group connected to a -COOH (or another identical reaction. 739 relative number of atoms of each -CO2H) group. 162, 185, 664 Chapter Objectives 6 element with subscripts. 70–71. See in acid-base reactions 185 Charge also forming name of 169 in atoms 47 for acids 168–170 Carboxypeptidase, in digestion 688 in chemical bonds 76, 548–551 for binary covalent compounds 93 Carnegie Institution 641 in HCl molecules 74 in chemical equations 127 Carothers, W. H. 691 in hydrogen bonds 553 conversion factors from 342–345 Catalyst A substance that speeds a of ions 95–98 for monatomic ions 98 chemical reaction without being in London forces 556 of polyatomic ions 103 permanently altered itself. 270, in molecules 552–553 of polymers 691–694 618–621, 621 in water molecules 87 Chemical nomenclature automobile catalytic converter 221 Charge cloud, for electrons 48, 418–421 binary acids 168 atoms as 271 Charles’ Law The pressure of a gas is binary covalent compounds 90–94 from chlorofluorocarbons 27 1 inversely proportional to the vol- memorized Names 90 defined 27 0 ume it occupies if the number of names without prefixes 9 3 equilibrium and 638–639 gas particles and the temperature are naming 91–92 green chemistry and 621 constant. 489 prefixes used to name 9 1 homogeneous and heterogeneous Chemical bond An attraction between recognizing from formulas 91 620–621 atoms or ions in chemical com- recognizing from names 93 as 270 pounds. Covalent bonds and ionic systematic names 90–92 in producing hydrogen gas 622 bonds are examples. 73–77. See ionic 104–108 Catalytic converter 221, 620–621 also Ionic bond; Covalent bond oxyacids 169 Cathode The electrode at which reduc- angles between 86–88, 468–474 summary 171–172 G-6 Glossary/Index

Chemical reaction The conversion of diatomic molecules of 55 chemical equation. 127 one or more pure substances into one electrolysis and 227 Coffee or more different pure substances. in ionic bonds 75 pH of 179 126 ion formation 95 removing caffeine 51 5 acid-base 180–189 Lewis structure of 80 Cold-start emissions, catalytic converters chemical equations for 126–128 most common bonding pattern 455 and 221 collision theory for 610 product of the electrolysis of salt 39 Cold packs 264 combination 218 reaction with alkali metals 42 Collision theory A model for the combustion 219–221 structure 55 process of chemical change. 610– completion 164 threshold limit value, or TLV, and 616, 658–664, 674–680, 688–696, converting to names 171–172 522 716–722 decomposition 219 use and production 525, 604 orientation 615 double-displacement 136 valence electrons 456 steps 610–612 endothermic 264–265 Chlorine-36 734 summary 615–616 energy and 263–265 Chlorine gas, molecules of 80 Combination (or synthesis) reaction equilibrium constants for 626–631 Chlorobutane, formation of 382 The joining of two or more elements exothermic 263–264 Chlorofluorcarbon, CFC Compound or compounds into one product. 218 general process, collision theory composed of just carbon, chlorine, Combinatorial chemistry 673 610–616, 658–664, 674–680, and fluorine. 27 0–272 Combined gas law equation 500 688–694, 690–696, 716–722 damage to ozone 270 Combustion analysis, empirical and neutralization 180–187 polystyrene foam and 272 molecular formulas from 353 oxidation-reduction 208–211 substitutes 272 Combustion reaction Rapid oxida- precipitation 137–143. See 1-Chloropropane, melting point of 313 tion accompanied by heat and usually also Precipitation reaction Chocolate, taste of 177 light. 219–220 predicting extent of 626–629 Cholesterol, structure of 685–686 incomplete 221 rate 616–620 Chromite 384 Study Sheet 220 concentration effect 61 7–618 (III) oxide 108 Complete (or molecular) equation A temperature effect 61 6–617 as catalyst 622 chemical equation that includes reversible 163, 621–622 catalytic converter and 221 uncharged formulas for all of the reversible reaction and equilibrium empirical formula of 346 reactants and products. The formulas 621–625 production and use 401, 408 include the spectator ions, if any. 140 single-displacement 222 Chromium (Cr), sources of 365 Complete combustion 219–220 synthesis 218 Chyme 688 Complete electron configuration types of 218–224 Chymotrypsin, in digestion 688 430–432 Chemistry The structure and behavior Citric acid 160 Complete ionic equation A chemi- of matter. 4. See also Organic chem- taste of 177 cal equation that describes the actual istry; Biochemistry Citrine 362 form for each substance in solution. combinatorial 673 Clark, Desmond 733 For example, ionic compounds that Green. See Green Chemistry Classification of Matter 7 0–73, 126– are dissolved in water are described as nuclear 715–725 129, 160–163, 168–171, 178–183, separate ions. 139 organic 657–672 188–191, 208–211, 213–216, 218– Completion reaction 164 suggestions for studying 5 221, 224–227, 250–253, 263–269 Compound A substance that contains Chemists 4 mixture 71 two or more elements, the atoms of Children pure substance 71 these elements always combining in effects of ionizing radiation on 73 0 Study Sheet 72, 500, 507, 512, 550 the same whole-number ratio. 70 fingerprints of 54 1 Classifying compounds 78 binary covalent 90 Chili peppers 583 Cleaning with soap and detergent binary ionic 104 Chloral hydrate 464 586–587 classification 7 8 Chloride ion 49 Clean Air Act of 1967 523 element versus 70 in sodium chloride 70 Clinton, Bill 5 ionic 78 solubility of compounds with 141 Coal, acid rain and 167 molar masses of 337–341 Chlorine (Cl) Cobalt-60 molecular 78 as anion 75–76 cancer radiation treatment and 731 as pure substance 70–73 bleach and 188 food irradiation and 735 Computer-based tools that accompany catalyst for ozone destruction gamma ray emission and 722 this text 7 618–620 Coefficients The numbers in front Concentration The number of particles in chlorofluorocarbons 27 0 of chemical formulas in a balanced per unit volume. For gases, it is usu- Glossary/Index G-7

ally described in terms of moles of gas Copper(II) oxide, in catalytic converter natural function. 689 particles per liter of container. Sub- 221 Density, mass Mass divided by volume. stances in solution are described with Copper sulfate, reaction with zinc 301–305 molarity (moles of solute per liter of 222–223 calculating for gases 498 solution). 617 Corliss, Jack 641 of common substances 302 disruption of equilibrium and 634 Corundum 359 definition 30 1 equilibrium constants and 626–629 Counting by weighing 331–333 determination of 304–305 rate of reaction and 617–618 Covalent bonding patterns 454–455 substance identification and 30 2 Condensation The change from vapor Covalent bond A link between atoms temperature and 301 to liquid. 534 that results from their sharing two units of 302 dynamic equilibrium between electrons. 54 Designing Safer Chemicals Award 5 evaporation and 537–539 common bonding patterns 454 Detergent 587 rate of 537 double bonds 83 cleaning with 586–587 Condensation (or step-growth) poly- formation of 74 pH and 179 mer A polymer formed in a reaction most common bonding patterns that releases small molecules, such as 455 Deuterium 50–51 water. This category includes nylon polar or nonpolar 548 in heavy water 313 and polyester. 691 triple bond 83 DEZ treatment 187 Condensation reaction A chemical Creatine 687 Diamond 47 reaction in which two substances Critical temperature 514 atoms in 48, 334 combine to form a larger molecule Cronenberg, David 7 London forces in 558–559 with the release of a small molecule, Crude oil 556–557 Diatomic Composed of paired atoms. such as water. 680 Crystals Solid particles whose compo- The diatomic elements are 2H , N2, Condensed formula 659 nent atoms, ions, or molecules are O2, F2, Cl2, Br2, and I2. 55 Confirmation, in scientific method9 arranged in an organized, repeating Dichlorine monoxide, production and The molecule or ion pattern. 139 use 247 that forms when one H+ ion is added Cubic centimeter 15 Dichloromethane, in decaffeinating cof- to a molecule or ion. 189 Cubic meter 12 fee 515 Conjugate acid-base pair Two mol- ion, determing Lewis structure Dietary calorie, Cal Equivalent to 4.184 ecules or ions that differ by one +H 461–462 kJ 257 ion. 189–190 Cycle, in electromagnetic radiation 261 Dietary Supplement and Health Act of Conjugate base The molecule or ion Cyclopropane 713 that forms when one H+ ion is re- 1994 687 Cysteine (Cys, C) Diethyl ether, structure of 665 moved from a molecule or ion. 190 disulfide bonds between 68 2 Diethyl zinc (DEZ), in book preserva- Conservation of Energy, Law of 252 structure of 679 Control rods Rods containing sub- tion 187 stances such as cadmium or boron D Difference in electronegativity, in (which are efficient neutron absorb- predicting bond type and polarity ers), used to regulate the rate of d block, on periodic table 428–429 548–549 nuclear fission in a power plant and Dacron, as polyester 693 Digestion The process of converting to stop the fission process if necessary. Dalton’s Law of Partial Pressures The large molecules into small molecules 740 total pressure of a mixture of gases is that can move into the blood stream equal to the sum of the partial pres- Conversion factor A ratio that de- to be carried throughout the body. sures of each gas. 509–513, 547–551, scribes the relationship between two 688–690 621–625 units. 288–290 Digestive enzymes 688–690 atomic mass as 335 Dead Sea Scrolls 734 Digital readouts 23 density as 303 Decaffeination 51 5 Dihydrogen phosphate, as amphoteric English-metric 292 Decimal place 191 in equation stoichiometry 372 calculators and 294 See formula mass as 340 measurements and 293 Dimensional analysis. Unit analysis from percentage 306 rounding for addition and subtrac- Dimethyl ether, Lewis structure for 464 metric-metric 289 tion and 299 Dipole A molecule that contains an molecular mass as 337 Decomposition reaction The conver- asymmetrical distribution of positive percentage 306 sion of one compound into two or and negative charges. Cooling, in evaporation 536–537 more simpler substances. 219 bond 549 Copper(II) ion, voltaic cells and 224– Denature To change the tertiary struc- induced 556–557 226 ture of a protein, causing it to lose its instantaneous 556–557 G-8 Glossary/Index

Dipole-dipole attraction The intermo- E Electron capture In radioactive nu- lecular attraction between the partial clides that have too few neutrons, the negative end of one polar molecule E.I. Du Pont de Nemours and Company combination of an electron with a and the partial positive end of another 691 proton to form a neutron, which stays polar molecule. 547 Earth, elemental composition of 743 in the nucleus. 721 hydrogen bonds and 554 Electric cars, zinc-air batteries in 229 nuclear equations for 723–725 London forces and 556 Electric current, base unit of 11 Electron cloud 48, 418 Diprotic acid An acid that can donate Electric field, in electromagnetic radia- Electron configuration A description two hydrogen ions per molecule in a tion 261 of the complete distribution of an reaction. 162 Electric power plant, using nuclear fis- element’s electrons in atomic orbitals. Dirac, Paul Adrien 437 sion 738–741 424, 426–427 Direct-contact method 515 Electric spark, ozone created by 266 abbreviated 433–436 Disaccharide Sugar molecule composed Electrode A electrical conductor placed Study Sheet 431, 456 of two monosaccharide units. 676 in the half-cells of a voltaic cell. 225 Electron group geometry A descrip- digestion products 688 Electrolysis The process by which a tion of the arrangement of all the Dispersion forces. See London forces redox reaction is pushed in the non- electron groups around a central atom Disproof, in scientific method 9 spontaneous direction or the process in a molecule or polyatomic ion, Disruption of equilibrium 634–640 of applying an external voltage to a including the lone pairs. 469 catalysts and 638–639 voltaic cell, causing electrons to move Electron sharing, in chemical bonds 74 concentrations and 634–637 from what would normally be the Electron spin 424, 426 Le Chatelier’s Principle 638–640 cell’s cathode toward its anode. 227 Electron transfer, in chemical bond Distance, between particles of gases 484 Electrolyte The portion of a voltaic cell formation 75–76 Distillation, of salt water 39 that allows ions to flow. 22 6 Electron volt (eV) An energy unit Disulfide bond A covalent bond Electromagnetic radiation. See Radiant equivalent to 1.6 × 10-19 joules. It is between two atoms on cysteine energy often used to describe the energy as- amino acids in a protein structure. Electron A negatively charged particle sociated with nuclear changes. 737 682 found outside the nucleus of an atom. Electroplating 227 Division, rounding off for 29 4 48, 414–418 Electrostatic force (or electromagnetic DNA (deoxyribonucleic acid) in atoms 48–50 force) The force between electrically aging and 212 in batteries 224 charged particles. 718 hydrogen bonding in 554 as beta decay 720–721 Element A substance that cannot be Dolomite rock, hard water and 144 in chemical bonds 74, 448–454 chemically converted into simpler Dopamine, Parkinson’s disease and 8 constructing Lewis structures and substances; a substance in which all Double-displacement reaction A 456 of the atoms have the same number chemical reaction that has the form: electronegativity and 548 of protons and therefore the same AB + CD to AD + CB 136 in ions 48–50 chemical characteristics. 38–57 acid-base 184 in isotopes 50–51 artificial 5 2 precipitation 136–139 like guitar strings 414–416 atomic mass of 335 Double-exchange reaction. See Double- in metallic elements 56 compound versus 70–71 displacement reaction in multi-electron atoms 424 diatomic 55 Double-replacement reaction. See Dou- octets of 80 electronegativities of 548 ble-displacement reaction in oxidation-reduction reactions electron configurations and orbital Double bond A link between atoms 208–211 diagrams 431, 456 that results from the sharing of four particle interpretation of the wave isotopes of 50–51 electrons. It can be viewed as two 2- character 418 list of common 41 electron covalent bonds. 83, 451 as standing wave 416 magic numbers for 737 Dow Chemical Company 272 valence 79 making new elements 52 Dry cell battery, chemistry of 226–227 waveform of 416 metallic 56–57 Dry ice 576 Electron-dot symbol A representa- metalloids or semimetals 44 Dynamic equilibrium A system that tion of an atom that consists of its metals 43 has two equal and opposing rates of elemental symbol surrounded by dots molar masses of 335–336 change, from state A to state B and representing its valence electrons. names of 40, 41–42 from state B to state A. There are 79–80, 83, 450 naturally occurring isotopes 51 constant changes between state A Electronegativity A measure of the 43 and state B but no net change in the electron attracting ability of an atom nuclear stability of 718–719 amount of components in either state. in a chemical bond. 548–551 in ordinary substances 69 See Equilibrium Study Sheet 550 origin of 742 Glossary/Index G-9

oxidation numbers of 213–218 291 tial pressure of vapor above a liquid in particle interactions 558 Environment, chemistry and 4 a closed system with a dynamic equi- periodic table of 42–46 Environmentally Benign Chemistry. librium between the rate of evapora- as pure substances 71 See Green Chemistry tion and the rate of condensation. solids, liquids, and gases 45 Environmental Protection Agency 5, 539–540 structure of 46–57 728 in bubble formation 543–544 symbols for 41 Enzyme A naturally occurring catalyst. table of percent abundances in 618, 688–690 temperature and 540 Earth’s crust, waters, and atmo- digestive 688–690 Ester A compound with two hydrocar- sphere 743 metallic cations in 100 bon groups surrounding an Element 111, creation of 52 why specific 69 0 atom. 666–667 Element 114, creation of 52 Epictetus 288 in fingerprints 54 1 Emerald 362 Epinephrine 582 olestra as 684–685 Empirical formula A chemical formula Equation. See Chemical equation, Estradiol, structure of 686 that includes positive integers that de- Nuclear equation; Ideal gas equation Ethanamide 668 Equation stoichiometry scribe the simplest ratio of the atoms Calculations Ethane 82 of each element in a compound. 346 that make use of the quantitative solubility in hexane 581 calculating 346–350 relationships between the substances 1,2-Ethanediol 663 converting to molecular formula in a chemical reaction to convert 350–353 the amount of one substance in the Ethanoic acid 664 Shudy Sheet 348 chemical reaction to the amount of Ethanol (or ethyl alcohol) Enamel 186 a different substance in the reaction. in combustion reactions 219 Endergonic changes Changes that 371–375 density of 301 absorb energy 253 ideal gases and 502–509 hydrogen bonds in 554–555 energy diagram 614–615 molarity and 388–392 as intoxicating liquid 89 Endothermic change A change that Study Sheet 391 Lewis structure 84 leads a system to absorb heat energy Equilibrium 621–622 mixing with water 576–577 from the surroundings. 265 disruption of 634–640 production of 628 Energy The capacity to do work. dynamic 538–540 solubility in water 593 250–252 effect of catalyst 63 8–639 See activation 612–614 effect on changing concentrations Ethene. Ethylene chemical bonds and 253–254 634–637 Ether A compound with two hydrocar- chemical changes and 263–265 gas solutions and 594–595 bon groups surrounding an oxygen conservation of. See Law of Conser- heterogeneous 630–631 atom. 665 vation of Energy homogeneous 624 Ethylene (or ethene) 451 endergonic (or endogonic) changes Le Chatelier’s Principle and 638– polyethylene formation and 693 253 640 Ethylene dibromide 272 of events 258 reversible reactions and 621–633 Ethylene glycol 663 exergonic (or exogonic) changes saturated solution and 592–593 in polyester formation 692 254 ski shop analogy for 625 Ethylene oxide, use and production 527 exothermic 264 Equilibrium constant A value that de- See in food 258 scribes the extent to which reversible Ethyl alcohol. Ethanol heat 259–260 reactions proceed toward products be- Ethyl butanoate 667 kinetic. See Kinetic Energy, KE fore reaching equilibrium. 626–629 Ethyne. See Acetylene nuclear 737–742 calculating values for 627–628 Evaporation The conversion of a liquid of photons 260–262 extent of reaction and 629 to a gas. 37, 535–536 potential 252–253 with heterogeneous equilibria cooling and 536 radiant 260–262 630–632 rate of. See Rate of evaporation storage in the body 674 table of 628 Exact numbers, significant figures and units of 257 temperature and 632–633 295 water formation and 257 writing expressions for 626–627 Examples, in this book 6 Energy diagram 614–615 Equilibrium constant expression An Excited state Energy level. See Principal energy level expression showing the ratio of the The condition of an atom Engineering, chemical 609 concentrations of products to the con- that has at least one of its electrons in English-metric unit conversion factors centrations of reactants for a reversible orbitals that do not represent the low- 292, 369 reaction at equilibrium. 626 est possible potential energy. 421 English system, metric system versus 14, Equilibrium vapor pressure The par- Exercises, in this book 6 G-10 Glossary/Index

Exergonic changes Changes that Fluorine-18 Gamma ray A stream of high-energy release energy. 254 positron emission tomography and photons. 261, 722 energy diagram 614 732 antimatter and 437 Exhaust 71 Food harmful effects of 73 0–731 Exhaust systems, catalytic converters and Calories in 258 penetration of the body 731 221 digestion of 688–690 in radioactive decay 722 Exothermic change A change that leads food, important substances in 674–685 Gas The state in which a substance can to heat energy being released from the Food and Drug Administration (FDA) easily change shape and volume. 34, system to the surroundings. 264 515 37–38. Expansion, of solids 35 Food irradiation 735 Avogadro’s Law 491 Experimentation, in scientific method Force, weight as 16 in book preservation 187 8–9 Forensic chemistry 541 breathing and 493 External kinetic energy 259 652, 665 calculations determing Lewis structure 460–461 F equation stoichiometry 502 in herbicide formation 621 Study Sheet 507–508 f block, of elements 429 production and use 237, 653 using the combined gas law Fahrenheit scale 18–19 Formic acid, molecular structure of 664 equation 500–502 Formula. See Chemical formula; Empiri- Fahrenheit to Celsius conversion Study Sheet 500 cal formula; Molecular formula 312–313 using the ideal gas equation Formula mass The weighted average of Family All the elements in a given col- 494–499 the masses of the naturally occurring umn on the periodic table; also called Study Sheet 495 formula units of the substance. It is group. 43 using the molar volume at STP the sum of the atomic masses of the Fat 683 503 atoms in a formula unit. 340–341 digestion products 688 Charles’ Law 489 Fertilizer calculations 341 Formula unit concentration effect on reaction ammonia and 621 A group represented by a substance’s chemical formula, that rates 617 nitric acid and 496 Dalton’s Law of Partial Pressures Feynman, Richard 418 is, a group containing the kinds and numbers of atoms or ions listed in the 509–513, 547–551 15-minute rule 6, 7 study sheet 512 Fingerprints 541 chemical formula. 339 Fortrel 693 densities of 302 Fireworks equilibrium constants and 626–627 calcium nitrate in 108 Fractional charge, in chemical bonds 74 expansion 575 light emitted from 421 France, zinc-air batteries in 229 Gay-Lussac’s Law 488 Fire extinguishers, sodium carbonate in Free radicals Particles with unpaired greenhouse gases 384–385 175 electrons. 730 heterogeneous equilibria and Fission Nuclear reaction that yields en- Fructose 674–675 Functional group 630–632 ergy by splitting larger atoms to form A small section of an ideal 485 more stable, smaller atoms. 738–739 organic molecule that to a large extent ideal gas calculations 494–502 Flame retardant, in 103 determines the chemical and physical Flashtubes 523 characteristics of the molecule. 662 instrument-carrying balloons and Flerov Laboratory of Nuclear Reactions Furnace method 368 493 Fusion 52 Nuclear reaction that yields internal combustion engine and Fluorapatite, tooth decay and 186 energy by combining smaller atoms to 492 Fluoride ion, tooth decay and 186 make larger, more stable ones. 738, liquids changing from and into Fluorine (F) 742 534–536 model 484 covalent bond formation 449–450 G diatomic molecules of 55 molar volume 503 electron configuration and orbital Galactose 674–675 noble 43 diagram 427 Galapagos Islands, global warming ex- partial pressure of 509–513, 595 how made 365 periments at 385 particle collisions 484 hydrogen bonds and 553 Galileo Galilei 9 pressure 485 most common bonding pattern 455 Gallium-67, radioactive decay of 724 pressure and industrial safety oxidation numbers and 214 Galvanizing nails 132 501–502 production of 396–397 Gamma aminobutanoic acid, gamma properties of 485 structure of 55 aminobutyric acid, or GABA 669 race cars and air density 499 valence electrons of 449 intoxicating liquids and 89 real 484 Glossary/Index G-11

relationships between properties Giga (G) prefix 1 3 ion formation 95 484–491 Girard, Georges 11 London forces in 556–557 relationship between number of gas Glacial acetic acid 162 in periodic table 43 particles and pressure 490 Glioma 741 Halons 272 relationship between number of gas Global warming 384–385, 597, 621, Hard water, soaps and detergents in 587 particles and volume 491 673, 687, 741 Hearst, William Randolph 167 relationship between pressure and Glucose 674–675 Heat The energy that is transferred temperature 488 empirical and molecular formulas from a region of higher temperature relationship between volume and of 346 to a region of lower temperature as pressure 486–487 Glutamic acid, structure of 679 a consequence of the collisions of relationship between volume and Glutamine, structure of 679 particles. 260 temperature 489 Glycerol or glycerin 663 in chemical equations 128 solubility of 594–595 Glycine, structure of 678 in endothermic reactions 265–266, typical particle velocities 484 Glycogen 676–677 614–615 universal gas constant 494 Gold (Au) as energy 260 vapor as 534 atom of 47 transfer 259–260 volume occupied by particles 484 as malleable 43 Heat of reaction 264 Gaseous elements 45 origin of name 41 Heavy-ion therapy 52 Gasoline 221, 661 scanning tunneling microscope im- Heavy water, freezing point of 313 in catalytic converters 221 age of 46 Heidelberg Radiology Clinic 52 combustion of 219 Gold-198, radioactive decay of 724 Helium composition of 82 Graduated cylinder 21 to avoid the bends 596 in internal combustion engines 492 Gravitational attraction, weight and 16 formation 742 Gastric juice 506 Greenhouse gases 384, 597 Helium-4, in treating brain cancer 741. pH and 179 Greenspan, Alan 48 See also Alpha particles Gas pressure. See also Gas Green Chemistry 5 Hematite 363 boiling-point temperature and exter- decaffeinating coffee and51 5 Hemoglobin 221 nal 542–544 Designing Safer Chemicals Award 5 carbon monoxide poisoning and breathing and 493 development of new and better 221 in bubble formation 542–544 catalysts 621, 673, 687, 741 iron ions in 100 in combined gas law equation Green Chemistry Challenge Awards Heptane, octane rating and 661 500–502 5 Heterogeneous catalyst A catalyst that Dalton’s Law of partial pressures Green Chemistry Program 5 is in the same phase as the reactants 509–513 Making Chemicals from Safer Reac- (so that all substances are gases or all equilibrium vapor 539–541 tants 351 are in solution). 620 Heterogeneous equilibrium in gas stoichiometry 502–509 Sea-Nine antifoulant and 5 An in ideal gas equation 494 spray paint and 514 equilibrium in which the reactants internal combustion engine and and products are not all in the same Ground state The condition of an atom 492 phase (gas, liquid, solid, or aqueous). whose electrons are in the orbitals that number of gas particles and 490 630–631 give it the lowest possible potential standard 503 Hexane, solubility in 578–581 energy. 421 temperature and 488 1-Hexanol 660 Group All the elements in a given col- volume and 486–487 3-Hexanol, molecular structure of 660 umn on the periodic table; also called Gas stoichiometry 502–509 High-density polyethylene (HDPE) 693 family. 43 Gay-Lussac’s Law The pressure of a Histidine, structure of 679 Guitar strings, like electrons 414–416 gas is inversely proportional to the Homogeneous catalyst A catalyst that volume it occupies if the number of H is in the same phase as the reactants gas particles and the temperature are (so that all substances are gases or all constant. 488 Half-life The time it takes for one-half are in solution). 620 Geometric sketch 86 of a sample to disappear. 726–728 Homogeneous equilibrium An equi- Geometry 467–471. See Molecular Half-reaction Separate oxidation or librium system in which all of the shape reduction reaction equation in which components are in the same phase Study Sheet 472 electrons are shown as a reactant or (gas, liquid, solid, or aqueous). 624 German Cancer Research Center 52 product. 210 Hormone 685 Gesellschaft fur Schwerionenforschung Halogen Huber, Claudia 641 (GSI) 52 bonding pattern 81 Hydrazine, production and use 410 Gide, Andre 33 covalent bond formation 454 Hydride ion 98 G-12 Glossary/Index

Hydriodic acid oxidation number of 214 acids and 160–166 forming name of 168 position on preiodic table 45 pH and 178–180 production and use 407, 654 production and use 244, 621–624 Hydrophilic (“water loving”) A polar Hydrobromic acid, forming name of structure 54 molecule or ion (or a portion of a 168 in synthesis gas 622 molecule or polyatomic ion) that is Hydrocarbon Compounds that contain Hydrogen atom, electron wavesforms in attracted to water. 582 only carbon and hydrogen. 82, 557 416–423 Hydrophobic (“water fearing”) A catalytic converters and 221 The intermolecular nonpolar molecule (or a portion of a in combustion reactions 219 attraction between a nitrogen, oxygen, molecule or polyatomic ion) that is in internal combustion engines 492 or fluorine atom of one molecule not expected to mix with water. 582 London forces among 556–557 and a hydrogen atom bonded to a Hydrothermal vent 641–642 solubility of 579 nitrogen, oxygen, or fluorine atom in Hydroxide ion Hydrochloric acid 160–161, 621 another molecule. 553–555 covalent bond formation 453 as binary acid 162 in ethanol/water solutions 576 Lewis structure of 101 dissolving basic 184 predicting existence of 559 solubility of compounds with 141 dissolving in water 160 in proteins 682 Hydroxides Compounds that contain dissolving limestone 186 Hydrogen bromide, threshold limit hydroxide ions. 173 in formation of magnesium chloride value, or TLV 522 Hydroxyapatite, in tooth enamel 186 247 Hydrogen carbonate ion 3-Hydroxybutanal 669 forming name of 168 as amphoteric 191 17-Hydroxyprogesterone, molecular in gastric juices 506 as weak base 175 structure of 686 in processing corn syrup 160 Hydrogen chloride 74 ion production and use 74, 161, 236, chemical bonds in 74 in bleach 188 325, 525 dipole-dipole attractions 547 sunlight and swimming pools 241 reaction with calcium carbonate dissolved in water 160 Hypothesis, in scientific method 8 –9 126 Lewis structure of 80–81 as strong acid 163, 165, 166 solubility in water 593 I Hydrochlorofluorocarbons (HCFCs) Hydrogen cyanide 621 272 molecular geometry of 471 Ideal Gas A gas for which the ideal gas Hydrofluoric acid Hydrogen fluoride model is a good description. 485 forming name of 166 hydrogen bonds and 553 calculations involving 494–502 light bulbs and 237 Lewis structure of 81 equation stoichiometry and used to make CFCs 236 Hydrogen halides, as polar molecules 502–507 Hydrogenation A process by which 553 Ideal gas constant (R) 494 hydrogen is added to an unsaturated Hydrogen , Lewis structure of 81 Ideal Gas Equation 494–499 triglyceride to convert double bonds Hydrogen peroxide combined gas law equation and 500 to single bonds. This can be done by aging and 212 equation stoichiometry and combining the unsaturated triglycer- composition of 73 504–509 ide with hydrogen gas and a platinum dark bottles and 243 Ideal gas model The model for gases catalyst. 683 empirical and molecular formulas that assumes (1) the particles are Hydrogen (H) of 346 point-masses (they have mass but no in acid-base reactions 180–192 as oxidizing agent 212 volume) and (2) there are no attrac- acids and 160–165 Hydrogen sulfate ion 188 tive or repulsive forces between the atomic orbitals 416–423 as cleaning agent 188 particles. 485 from Big Bang 742 as weak acid 166 Incandescent light bulbs 496 in Brønsted-Lowry acids and bases Hydrogen sulfide Induced dipole 556 188–190 Lewis structure of 81 Industrial chemistry 4, 5 combustion 126, 219, 263 threshold limit value, or TLV 522 Infrared (IR) radiation 262 covalent bond formation 450 Hydrolysis A chemical reaction in Inner transition metals The 28 ele- electronegativity of 548 which larger molecules are broken ments at the bottom of the periodic formation from water 219 down into smaller molecules by a table. 44 formation of hydrogen molecules reaction with water in which a water Insoluble substances 140–141, 578–581 450 molecule is split in two, each part Instantaneous dipole 556 in formation of water 126–127 joining a different product molecule. Intermolecular attraction Attraction ion formation 96 689 between molecules. 553–557 + isotopes of 50–51 Hydronium ion H3O 160–161 dipole-dipole attraction 547 nuclear fusion of 742 in acid-base reactions 180–185 hydrogen bonds 553–555 Glossary/Index G-13

London forces 556–557 names to formulas 107–108 J Internal combustion engine 492 polyatomic ions is 101–103 effects of weather on 49 8 reactions of acids with 181 Jeans, James Hopwood 48 gases and 492 recognizing from formulas 104 Jesus of Nazareth 734 Jewelry, elements in 41 Internal kinetic energy. See Thermal solutility of 141 Joule, J The accepted SI unit for energy. Energy solution of 133–135 257 International System of Measurement as strong and weak bases 175 10–19 structure of 100–102 K abbreviations 13 types of 104 metric prefixes 1 2–13 uses of 94, 102 Kaposi’s sarcoma 673 units derived from base units 12 Ionizing radiation Alpha particles, beta Kelvin, a temperature unit 19 Intestines 689 particles, and gamma photons, which Kelvin scale 11, 18–19 Intoxicating liquids 89 are all able to strip electrons from gas temperature and 485 Iodide ion, solubility of compounds with atoms as they move through matter, temperature conversions for 141 leaving ions in their wake. 730 312–314 Iodine (I) Iridium (Ir), in catalytic converter 221 Kerosene, London forces and 556 beta emission and 720 Iridium-192, checking pipe joints and Ketone A compound that have a hy- diatomic molecules of 55 735 drogen atom or a hydrocarbon group electron capture and 721 connected to a -CHO group. 666 London forces and 556 Iron(II) sulfate, in global warming ex- periments 385 Kettering, Charles F. 414 most common bonding pattern 455 Khirbat Qumrân 734 Iron(III) sulfate, formula mass calcula- name of 41 Kilocalorie (kcal, Cal) 257 tions for 341, 343 production and use 235 Kilogram (kg) 11 Iron-59 736 structure of 55 Kilojoule (kJ) 258 Iron (Fe) tincture of 556 Kilometer (km) 13 electron configuration and orbital Iodine-125 Kilopascal (kPa) 485 diagram for 432 electron capture by 736 Kilo (k) prefix 1 3 formation of 743 radioactive decay of 721 Kinetic energy, KE The capacity to do formation of pig 218, 509 iodine-131 730–731 work resulting from the motion of an Iodine pentafluoride, production and use global warming and 384–385 object. 251 243, 405 as limiting reactant in global warm- chemical reactions and 263–264 Ion Any charged particle, whether posi- ing 384 in formation of water 263 tively or negatively charged. 48–50 Island of stability, of nuclides 719 internal and external 259 See also anion 49. Anion Isobutene, use 662 mass and 251 See also cation 49. Cation Isoleucine (Ile, I), molecular structure of reactant molecules 611–612 charges on monatomic 98 of 678 solution of ammonium nitrate and formation of 75 Compounds that have the 264 monatomic anion charges 96 same molecular formula but different velocity and 251 monatomic anion names 98 molecular structures. 464 Kinetic molecular theory. See Particle monatomic cation. See Cation, Lewis structures of 464–465 nature of matter monatomic of organic compounds 658 Knockout drops 464 polyatomic. See Polyatomic ion Isooctane 661 , light bulbs and 499 predicting charges 95–98 Isopropyl alcohol. See 2-propanol Krypton-81 717, 734 size of 100 Isotopes Atoms that have the same spectator 139–140 number of protons but different num- L symbols for 49 bers of neutrons. They have the same Ionic bond The attraction between a Lactase, in digestion 688 atomic number but different mass cation and an anion. 75–77 Lactic acid, in cosmetic lotion 205 numbers. 50–52 in ionic compounds 78 Lactose, or milk sugar 676 of artificial elements 5 2 predicting existence of 548–551 Laskowski, Edweard R. 687 Ionic compound A compound that atomic numbers of 51 Latent fingerprints 54 1 consists of ions held together by ionic of carbon 333 Lawrence Laboratory 725 bonds. 78, 94–108 mass numbers of 51 Law of Conservation of Energy as bases 175 in nuclear reactions 722 Energy can be neither created nor de- binary 104, 107, 208–210 symbol for 716–717 stroyed, but it can be transferred from formulas to names 104–106 Isovaleraldehyde 665–666 one system to another and changed formula mass of 340–341 from one form to another. 252 G-14 Glossary/Index

L-dopa 8 groups as far apart as possible. It leads Magic numbers and nuclear stability 52, Lead(II) ion, solubility of compounds to angles of 180° between the groups. 737 with 141 471 Magnesium (Mg), meals ready to eat lead-206, in radioactive decay series 729 Linear molecules 471, 472 (MREs) and 573 Lead-acid batteries, chemistry of 229 Line drawing 582, 659 Magnesium chloride, production and Lead (Pb) Ling Po 7 use 247 in creating elements 110 52 Liquid The state in which a substance Magnesium oxide 106 density of 301 has a constant volume at a constant Magnesium sulfate, use 205 gasoline and 244 temperature but can change its shape. Magnetic field, in electromagnetic radia- Lebowitz, Fran 287 34, 36 tion 261 Leclanché cell 226–227 boiling 542–544 Magnetic imaging (MRI) 732 Length 14–15 dissolving gases in 594 Main-group element The elements in range of 15 dissolving solids in 588–593 groups 1, 2, and 13 through 18 (the Leucine (Leu, L), structure of 678 dynamic equilibrium between va- “A” groups) on the periodic table; also Levi, Primo 3 pors and 595 called representative elements. 44 Levocarbidopa, in Parkinson’s disease 8 heterogeneous equilibria and Malleable Capable of being extended Levodopa, in Parkinson’s disease 8 630–631 or shaped by the blows of a hammer. Lewis electron-dot symbols 79 Liquid-liquid solutions 136 43 Lewis structure A representation Liquid elements 45 Maltase, in digestion 688 of a molecule that consists of the Liter 12 Maltose, molecular structure of 676 elemental symbol for each atom in Lithium-7, in treating brain cancer 741 Manganese (Mn) the molecule, lines to show covalent Lithium (Li) in dry cell batteries 226–227 bonds, and pairs of dots to indicate from Big Bang 742 how made 360 lone pairs. 80–84, 450, 455–465 electron configuration and orbital Manganese(II) oxide, naming 105 general steps for drawing 458, 484 diagram 426 Manganese(II) phosphate resonance and 465–467 formation of 742 production and use 242 simple procedure 83–85 Lithium batteries 229 uses 205 Study Sheet 456–457 Lithium hydroxide, uses 173 Manganese dioxide, in dry cell batteries Le Chatelier’s principle If a system at Litmus, detecting acids and bases with 226–227 equilibrium is altered in a way that 180 Marble, acid rain and 167 disrupts the equilibrium, the system London forces The attractions pro- Margarine 683 will shift so as to counter the change. duced between molecules by instanta- Martin, John 384–385 638–640 neous and induced dipoles. 556–557 Mass The amount of matter in an Libraries, of drugs 673 molecular size and 556 object. Mass can also be defined as Life Lone pair Two electrons that are the property of matter that leads to hydrogen bonds and 554 not involved in the covalent bonds gravitational attractions between origin of 640–641 between atoms but are important for objects and therefore gives rise to Light bulbs weight. 16–17 explaining the arrangement of atoms argon gas in 512 base unit of 11 in molecules. They are represented by filament evaporation in 49 6, 499 density and 301–303 pairs of dots in Lewis structures. 80, flash tubes 52 3 of elements and compounds 450 fluorescent 52 1 342–346 Los Angeles, photochemical smog in “Like dissolves like” guideline, for solu- English-metric unit conversions of 266 bility 578–581 309 Low-density polyethylene (LDPE) 693 Lime 245 kinetic energy and 251 Lucretius 177 Limestone 186, 616 measuring 16–17 Luminous intensity, base unit for 11 acid rain and 167 percentage by 306–307 Luminous tubes 501 increasing permeability of 161 range of 17 Lungs, gases in 493 Limestone caverns 204 weighted average 331 Lye. See Sodium hydroxide Limiting reactant The reactant that weight and 16–17 Lye soap 586 runs out first and limits the amount Mass density Mass divided by volume Lysine (Lys, K) of product that can form. 376–381 (usually called density). 301–305 molecular structure of 679 global warming and 384–385 as conversion factor 303–305 how chosen 376–377 in salt bridges 682 Mass number The sum of the number Study Sheet 380 M of protons and neutrons in an atom’s Linear geometry The geometric ar- nucleus. 51 rangement that keeps two electron “Mickey Finn” sedative 464 binding energy versus 738 Glossary/Index G-15

in nuclear equations 723 combustion of 250 of solids 34–35 in nuclides 716 covalent bond formation 451 strengths and weaknesses of 448 Mass percentage 306 in hydrogen gas production valence-bond 449–454 Matches, chemicals in 131 621–624 Moderator A substance in a nuclear Matter Anything that has mass and molecular shape 86–87, 468 reactor that slows neutrons as they takes up space. 16 solubility in water 593 pass through it. 740 chemistry and 4 Methanethiol, in natural gas 219 Molarity (abbreviated M) Moles of classification of 7 0–73 Methanoic acid 664 solute per liter of solution. 387–392 existence of 437 Methanol 447 equation stoichiometry and origin of 742 density of 304 388–392 as solid, liquid, or gas 34–38 hydrogen bonds and 555 Molar mass The mass in grams of one Mayo Clinic 687 as polar molecule 553 mole of substance. 335–338 McGwire, Mark 687 production and use 244, 527, 627 from atomic mass 335 Meals ready to eat (MRE) 573 water solubility of 580 calculations using atomic mass 336 Measurement 9, 9–23 Methionine (Met, M), structure of 679 calculations using ionic formula digital readouts 23 3-Methylbutanal 665–666 mass 341 International System of 10–11 Methylene chloride, in decaffeinating reporting values from 20 coffee 51 5 calculations using molecular mass trailing zeros and 22 2-Methylpropene 662 338 uncertainty in 20–23, 293 Methyl alcohol 83. See also Methanol in equation stoichiometry 370–374 Medicine, uses of radioactive substances Methyl bromide 272 in ideal gas equation 495 in 731–732 determing Lewis structure 458–459 from ionic formula mass 340 Mega (M) prefix 1 3 ozone layer and 3 from molecular mass 337–338 Meitner, Lise 40 threshold limit value, or TLV, and Molar volume at STP 503 Meniscus, in measurement 21 522 Mole (mol) The amount of substance Menstrual cycles, hormones in 686 Methyl cyanoacrylate, molecular struc- that contains the same number of Menthol 584 ture of 473 particles as there are atoms in 12 g of Metal-nonmetal compounds Methyl ethyl ketone or MEK, molecular carbon-12. 11, 333–334 bonds in 549 structure of 666 in equation stoichiometry 502–509 formulas and names of 104 Metric-metric unit conversions 289–291 in ideal gas equation 503 Metallic bond The attraction between Metric prefixes 1 2–13 Molecular compound A compound the positive metal cations that form table of 13 composed of molecules. In such the fundamental structure of a solid Metric system 10. See also International compounds, all of the bonds between metal and the negative charge from System of Measurement atoms are covalent bonds. 78 the mobile sea of electrons that sur- MeV (million electron volts) 737 attractive forces in 559 round the cations. 558 Microwaves 262 in oxidation-reduction reactions Metallic elements 44 micro (m) prefix 1 3 211 attractive forces in 558–559 Mifepristone 705 water solubility of 579 ion charges of 96–98 Milk, pH of 179 Molecular dipole A molecule with an Metalloids or semimetals The ele- Millimeter of (mmHg), as unit asymmetrical distribution of positive ments that have some but not all of of pressure 485 and negative charge. 547 the characteristics of metals. 44 milli (m) prefrix 13 Molecular equation. See Complete bonding patterns of 457 Miscible Can be mixed in any propor- equation in periodic table 44 tion without any limit to solubility. Molecular formula The chemical Metals The elements that (1) have a 576 metallic luster, (2) conduct heat and Mixture A sample of matter that con- formula that describes the actual electric currents well, and (3) are mal- tains two or more pure substances and numbers of atoms of each element in leable. 43, 56–57 has variable composition. 71 a molecule of a compound. 346 electrolysis to purify 227 of gases 509 from empirical formula 350–353 forming cations 95 Model A simplified approximation of empirical formulas versus 346 sea of electrons model 57 reality. Study Sheet 352 Meter 10, 11 calculating 387 Molecular geometry The description Methamphetamine, molecular structure collision theory as 610–616 of the arrangement of all the atoms of 582–583 of gases 37 around a central atom in a molecule Methamphetamine hydrochloride ideal gas 485 or polyatomic ion. This description 582–583 of liquids 36 does not consider lone pairs. 467– Methane 82, 447 of metallic elements 56 474. See also Geometry G-16 Glossary/Index

Molecular mass The weighted aver- Monsanto Company 621 solubility of compounds with 141 age of the masses of the naturally Moss Landing Marine Laboratories 384 Nitric acid occurring molecules of a molecular Mount Everest, atmospheric pressure at acid rain and 167 substance. It is the sum of the atomic the top 545 formation of 640 masses of the atoms in a molecule. MTBE 665 forming name of 169 337–338 Multiplication production and use 241 calculating 338 rounding off for 29 4–299 reaction with sodium hydroxide in calculating molecular formulas significant figures for29 4–299 181–183, 181–185 350–351 Mylar, as polyester 693 solution of 181 Molecular models 54 as strong acid 165 Molecular polarity, predicting 552 N Nitride ion, forming name of 98 Molecular Shape 86–88 Names Nitril hydratase 621 ball-and-stick model 86 for acids 168–170 Nitrogen-13, radioactive decay of 724 geometric sketch 86 for binary covalent compounds 90 Nitrogen-14, in radiocarbon dating 726 space-filling model 8 6 for chemical compounds 171–172 Nitrogen (N) Molecular size, London forces and for elements 40–41 covalent bond formation 451 556–557 for ionic compounds 98–106 diatomic molecules of 55 Molecule An uncharged collection of for organic compounds 661 electron configuration and orbital atoms held together with covalent Nano (n) prefix 1 3 diagram 427 bonds. 54 Natrium 41 ion formation 96 covalent bonds in 448–454 Lewis structure 83 diatomic 55 Natural gas 447 Nature, elements found in 40 liquid 257 as formula unit 339 London forces and 558 of hydrogen 54 Neon (Ne) most common bonding pattern 81, in molar mass 337 electron configuration and orbital 455 shapes of 86–87, 467–474 diagram 427 structure of 55 Momentum, of particles in evaporation luminous tubes and 501 triple bonds in 83 535 in neon lights 501, 513 Nitrogen dioxide Monatomic anions Negatively charged Nerve cells acid rain and 167 particles, such as Cl-, O2-, and intoxicating liquids and 89 nitric acid and 640 N3-, that contain single atoms with a taste and 177 ozone production and 266–267 negative charge. 96. See also Anion, Net ionic equation A chemical equa- threshold limit value, or TLV and monatomic tion for which the spectator ions have 522 charges 96 been eliminated, leaving only the naming 98 substances actively involved in the Nitrogen molecules, velocities of 484 Monatomic cation Positively charged reaction. 140 Nitrogen monoxide 620 particles, such as Na+, Ca2+, and Net rate of solution 589–591 in acid rain 167 Al3+, that contain single atoms with a Neutralization reaction A chemical catalytic breakdown of 620 positive charge. 97. See also Cation, reaction between an acid and a base. how made 496 monatomic See Acid-base reaction oxidation-reduction and 211 formation 96–97 Neutron An uncharged particle found Nitrogen narcosis 596 naming 99 in the nucleus of an atom. 47 Nitrogen oxides roles in body 100 in nuclear fission 73 8–739 in automobile exhaust 257 Monatomic ion, charges 98 as nuclear glue 718 ozone and 266–267 Monoethanolamine 637 nuclear stability and 718–719 Nitroglycerine, in decomposition reac- Monomer The repeating unit in a poly- Newton (N), a unit of force 16 tions 219 mer. 676 NiCd batteries. See Nickel-Cadmium Nitrosyl chloride, production and use in addition polymers 693 batteries 655 in polysaccharides 676–677 Nickel (Ni), in the creation of elements Nitrosyl fluoride, molecular geometry in proteins 678 110 and 111 52 473 Monoprotic acid An acid that donates Nickel-60, gamma ray emission by 722 Nitrous oxide, formation of 130 one hydrogen ion per molecule in a Nickel-cadmium battery, chemistry of Noble gases, structure 53 reaction. 162 228 Node The locations in a waveform Monosaccharide Sugar molecule with Nicotine 361 where the intensity of the wave is one saccharide unit. 674 Nippoldt, Todd B. 687 always zero. 415 Monosodium glutamate (MSG), taste Nitrate ion Nomenclature. See Chemical nomen- and 177 resonance and 465–467 clature Glossary/Index G-17

Nonmetals The elements that do not Nucleus The extremely small, positively amine 667–668 have the characteristics of metals. charged core of the atom. 47 arene 662–663 Some of the nonmetals are gases at of atom 47 carboxylic acid 664 room temperature and pressure, some creation of new elements and 52 condensed formula 659 are solids, and one is a liquid. Various electrons around 416–422 ester 666–667 colors and textures occur among the of helium atoms 53 ether 665 nonmetals. 43 mass number and 51 how to describe 658–660 forming anions 95 stability of 718 ketone 666 most common bonding patterns 83 Nuclide A particular type of nucleus line drawing 582, 659 Nonpolar covalent bond A covalent that is characterized by a specific table of types 670–671 bond in which the difference in elec- atomic number (Z) and nucleon Organophosphorus compounds 361 tron-attracting ability of two atoms in number (A). 716 Oxalic acid 664 a bond is negligible (or zero), so the band of stability of 719 uses 160 atoms in the bond have no significant in nuclear equations 722–726 Oxidation Any chemical change in charges. 74 radioactive 727 predicting existence of 548–551 symbol 716–717 which at least one element loses elec- Nonpolar molecular substance, solubility uses for radioactive (table) 736 trons, either completely or partially. and 578–579 Numbers, exact or not 295 208–209, 211 Normal boiling-point temperature Nutrients, for phytoplankton 384 Oxidation-reduction reaction The The temperature at which the equi- Nylon 691 chemical reactions in which there librium vapor pressure of the liquid molecular structure of 691 is a complete or partial transfer of equals one atmosphere. 545 production of 350, 691–692 electrons, resulting in oxidation and North Carolina State University 266 Nylon-66 350–351 reduction. These reactions are also Notation, for nuclides 716–717 called redox reactions. 208–211 Nuclear chemistry The study of the O within batteries 224–229 properties and behavior of atomic half-reaction 210 nuclei. 715 “Oil rig” mnemonic 209 oxidation 208 Nuclear decay series A series of radio- Objectives 6 oxidation numbers (or states) active decays that lead from a large Observation, in scientific method 8 –9 213–218 unstable nuclide, such as - Octane rating 661 reduction 209 238, to a stable nuclide, such as lead- Octet of electrons 80–81, 456–457 206. 729 Oil 186, 556–557 uses of 207 Nuclear energy 737–742 Oil industry 186 Oxidation number (or state) A tool Nuclear equation The shorthand nota- Olestra 684–685, 742–743 for keeping track of the flow of elec- tion that describes nuclear reactions. Oligopeptide 680 trons in redox reactions. 213–218 It shows changes in the participating Open-chain forms, of monosaccharides assignment of oxidation numbers nuclides’ atomic numbers (the num- 674–675 214 ber of protons) and mass numbers Orange juice, pH of 179 Study Sheet 214 (the sum of the numbers of protons Orbitals See Atomic orbitals . See Oxidation number and neutrons). 722–726 Orbital diagram A drawing that uses Oxidizing agent A substance that gains Nuclear fission 73 8–739 lines or squares to show the distribu- electrons, making it possible for an- Nuclear fusion 742 tion of electrons in orbitals and ar- other substance to lose electrons and rows to show the relative spin of each Nuclear power plant 740–741 be oxidized. 210 electron. 424, 426–427 Nuclear reaction A process that results aging and 212 Study Sheet 431, 456 in a change in an atomic nucleus (as defined 21 0 opposed to a chemical reaction, which Organic acid Carbon-based acids. 162 oxidation numbers and 213–218 involves the loss, gain, or sharing of Organic chemistry The branch of ozone as 266 electrons). 722–726 chemistry that involves the study Oxoacid. See Oxyacid Nuclear reactors 738–741 of carbon-based compounds. 82, Oxyacid (oxoacid) Nuclear stability 718–719, 737–738 658–672 Molecular sub- Nucleon number The sum of the num- Organic compound 658–672 stances that have the general formula bers of protons and neutrons (nucle- alcohol 663 HaXbOc. In other words, they contain ons) in the nucleus of an atom. It is aldehyde 665 hydrogen, oxygen, and one other ele- also called the mass number. 716 alkane 661 ment represented by X; the a, b, and c Nucleons The particles that reside in alkene 662 represent subscripts. 162 the nucleus of atoms (protons and alkyne 662 names for 169 neutrons). 716 amide 668 as polar molecule 553 G-18 Glossary/Index

Oxygen (O) gas character, the partial pressure of group or family 43 absorbing ultraviolet radiation 269 any gas in a mixture is the pressure hydrogen, position on periodic table bonding patterns 81, 455 that the gas would yield if it were 45 in combustion reactions 219–221 alone in the container. 509 metals, nonmetals, and metalloids covalent bond formation 452–453 effect on gas solubility 59 5 44 diatomic molecules of 55 equilibrium vapor pressure as modern model of the atom and electronegativity of 548 539–540 428–436 electron configuration and orbital Particle-particle attractions 547, 621 order of filling of atomic orbitals diagram 427 summary 558–559 and 428–430 in formation of water 126–127 Particles periods 45 in internal combustion engines 492 in atoms 47 representative (or main-group) ion formation 95–96 attractive forces among 547–560 elements, transition metals, and oxidation numbers for 214 in collision theory 610 inner transition metals 44 in ozone layer 269 in condensation 534 Periods The horizontal rows on the structure 55 in evaporation 535–536 periodic table. 45 Ozone 266–273 in gases 37 Peroxides, oxidation numbers of 214 absorbing ultraviolet radiation 269 in liquids 36 Petroleum 556–557 chlorine catalyzed destruction radiant energy as 260–261 pH 178–179 618–620 in solids 34–35 acid rain and 178 damage from chlorofluorocarbons space occupied 37 Pharmaceuticals 673 270 Particle nature of matter 34–38 Phenylalanine (Phe, F), molecular struc- destruction 269–270 gas 34, 37–38 ture of 679 as greenhouse gas 384 liquid 34, 36 Phosgene gas, production and use 655 as pollutant 266 solids 34–35 Phosphate, production 213 process of destruction 610–614 Pascal (Pa), pressure unit 485 Phosphate ion, solubility of compounds ultraviolet radiation and 269 Pearl ash, empirical formula for 349 with 141 uses 266 Pentane Phosphate rock, in furnace method 330 Ozone hole 271 hexane solubility of 578 Phosphide ion 98 Ozone layer in solution 136 Phosphoric acid 188 CFCs and 270 water solubility of 578 forming name of 169 effect of halons on 27 2 Pepper, spiciness of 583 furnace method of preparation 330 formation of 269 Pepsin, in digestion 688 neutralizing 390 Peptide A substance that contains two production of 368 P or more amino acids linked together reaction with sodium hydroxide by peptide bonds. 680 184 p block, of elements 428–430 how form 640–642 in toilet bowl cleaners 188 Paint spraying, preventing air pollution Peptide bond An amide functional uses 160, 163 514 group that forms when the carboxylic Phosphorus (P) Palladium, in catalytic converter 221 acid group on one amino acid reacts bonding pattern 81 Pancreatic amylase, in digestion 688 with the amine group of another covalent bond formation 452 Pancreatic lipase, in digestion 688 amino acid. 680 in furnace method 368 Paper, saving acidic 187 Percentage 306–307 ion formation 96 Parkinson’s disease 7–8 as conversion factor 306 London forces in 558 positron emission tomography and by mass, definition 30 6 most common bonding pattern 455 437 by volume 306 in oxidation-reduction reactions scientific method and 7 –8 Percentage calculations 306–307, 311 215 Partially hydrogenated triglycerides in calculating empirical formulas in photophor 347 683–684 349 production of 213, 408 Partial charge in calculating molecular formulas Phosphorus pentachloride, production in chemical bonds 74, 548–551 353 and use 246 in hydrogen bonds 553 Percent yield The actual yield divided Phosphorus tribromide 383 in London forces 556–557 by the theoretical yield times 100. Phosphorus trichloride, production and Partial electron transfer in oxidation-re- 382–384 use 630 duction reactions 211 why less than 100% 382–383 Photochemical smog, formation of Partial pressure The portion of the to- Periodic table of the elements 42–46 266–267 tal pressure that one gas in a mixture electronegativity and 548 Photons Tiny, massless packets or par- of gases contributes. Assuming ideal group number 43 ticles of radiant energy. 260 Glossary/Index G-19

Photophor, empirical formula for 347 repeating units. 676 Precipitate A solid that comes out of Physical states, in chemical equations addition 693–694 solution. 137 127 formulas for 691 Precipitation The process of forming a Physics polysaccharides as 676–677 solid in a solution. 137 chemistry and 34 proteins as 680 tooth decay and 186 of electrons 414–423 synthetic 690–695 Precipitation reaction A reaction in origin of matter and 640–641 Polypeptide 680. See also Protein which one of the products is insoluble Phytoplankton, global warming and nylon as 691 in water and comes out of solution as 384–385 silk as 690 a solid. 137–143 Pico (p) prefix 1 3 Polypropylene 694–695 of calcium carbonate 137–140 Pig iron, formation of 509 Polyprotic acid An acid that can do- Study Sheet 142 Plastic fingerprints 54 1 nate more than one hydrogen ion per writing equations for 142–143 Platinum (Pt) 56 molecule in a reaction. 162 Precision The closeness in value of a as catalyst 640 Polysaccharide Molecule with many series of measurements of the same in catalytic converters 221, 620 saccharide units. 676 entity. The closer the values of the density of 302 digestion products 688 measurements, the more precise they Plutonium-239 Polystyrene 694–695 half-life 727 chlorofluorocarbons and 27 2 are. 20 in radioactive wastes 728 Positron A high-velocity anti-electron in reporting measured values 293 See radioactive decay 727 released from radioactive nuclides that Prefixes. Metric prefixes Plutonium (Pu), in creation of new ele- have too few neutrons. 437, 721 Preserving books 187 ments 52 discovery of 437 Presidential Green Chemistry Challenge Polarity Positron emission In radioactive nu- Award 272, 621 of amphetamine and epinephrine clides that have too few neutrons, the Pressure Force per unit area. See Gas 582 conversion of a proton to a neutron, pressure of bonds 548–549 which stays in the nucleus, and a Pressure cooker 544 of capsaicin 583 positron, which is ejected from the Primary battery A battery that is not molecular 552 nucleus. 721 rechargeable. 228 predicting in molecules 552–553 nuclear equations for 723–725 Primary protein structure The se- solubility and 578 Positron emission tomography (PET) quence of amino acids in a protein Polar covalent bond A covalent bond 437, 732 molecule. 680 in which electrons are shared unequal- Potassium-40 Principal energy level A collection of ly, leading to a partial negative charge radioactive decay of 721 orbitals that have the same potential on the atom that attracts the electrons uses for 721 energy for a hydrogen atom, except more and to a partial positive charge Potassium carbonate, empirical formula for the first (lowest) principal energy on the other atom. 74 determination 349 level, which contains only one orbital dipole-dipole attractions and Potassium , production and use (1s). 420 547–548 398 Probabilities, electron behavior and 414, predicting in molecules 548–552 Potassium hydroxide, production and use 418 Polar molecular substance, solubility and 173, 245 Products The substances that form in 578–579 Potassium nitrate a chemical reaction. Their formulas Polonium-210, radioactive decay of 724 production and use 237 are on the right side of the arrow in a Polonium-218, in radioactive decay 729 in voltaic cells 226 chemical equation. 127 Poly(ethylene terephthalate) 695 Potassium perchlorate, production and Progesterone, molecular structure of 686 Poly(vinyl chloride), PVC 694–695 use 399 Polyatomic ion A charged collection Potassium , production Proline (Pro, P), molecular structure of of atoms held together by covalent and use 401 679 bonds. 101–103 Potassium phosphate 141 Propane 82 balancing equations and 129, 132 Potato chips 684 1,2,3-Propanetriol 663 formulas and names 103 Potential energy (PE) A retrievable, 2-Propanol with hydrogen 103 stored form of energy an object pos- hydrogen bonds in 554 Lewis structures 101 sesses by virtue of its position or state. Lewis structure 84 nonsystematic names 103 252 molecular structure of 554 Polychlorinated biphenyl (PCB) 353 chemical reactions and 263–265 2-Propanone 666 Polyester 692–693 electron orbitals and 420 Propionic acid Polyethylene 693 in formation of water 263 molecular structure of 580 Polymer A large molecule composed of stability and 252–254 water solubility 580 G-20 Glossary/Index

Proportionality Radiator coolants 578 strengths of attractions and 536 direct 487 Radioactive decay One of several surface area and 536 inverse 487 processes that transform a radioactive temperature and 537 Propylene nuclide into a more stable product or three factors that determine 536 hexane solubility of 581 products. 719 Rate of solution. See Solution, Rate of in polypropylene 694 effects on body 73 0–731 Ratio Propylene glycol, molecular structure of rates and half-life 726–728 empirical formulas and 346 578 Radioactive decay series 728–729 molar 345 Protein Natural polypeptide. 678–679, Radioactive emissions neutron-to-protons 718–719 680 alpha particle 720 stoichiometric 376 alpha helix 680 beta emission 720 Rational drug design 673 beta sheet 680 gamma rays 722 Reactants The substances that change digestion products 688 positron emission 721 in a chemical reaction. Their formulas disulfide bond 68 2 Radioactive nuclide An unstable nu- are on the left side of the arrow in a hydrogen bond 682 clide whose numbers of protons and chemical equation. 127 primary structure 680 neutrons place it outside the band of equilibrium disruption and 634– ribbon convention 681 stability. 719 636 salt bridge 682 Radioactive substances limiting 377–381 secondary structure 680 smoke detectors, pipe joint check, Reaction. See Chemical reaction tertiary structure 681–682 food irradiation, radioactive trac- Reaction Rate. See Rate of chemical Proton A positively charged particle ers 735 reaction found in the nucleus of an atom. 47 uses 731–736 Rechargeable batteries 228 in artificial elements 5 2 Radioactive tracer A radioactive Recycling 694 in atoms 47–48 nuclide that is incorporated into Redox reaction. See Oxidation-reduction in Bronsted-Lowry acids and bases substances that can then be tracked reaction 188 through detection of the nuclide’s Reducing agent A substance that loses in ions 48–49 emissions. 735 electrons, making it possible for an- in isotopes 50–51 Radiocarbon (or carbon-14) dating other substance to gain electrons and mass number and 51 The process of determining the age of be reduced. 210 MRI and 732 an artifact that contains material from Reduction Any chemical change in nuclear stability and 718–719, 737 formerly living plants or animals by which at least one element gains elec- in nuclides 716–717 analyzing the ratio of carbon-14 to trons, either completely or partially. origin of the elements and 742 carbon-12 in the object. 733–734 209, 211 Publication, in scientific method 9 Radio waves 261, 262 Red giant stars 743 Pure substance A sample of matter that Radium-226 Red litmus paper, detecting bases with has constant composition. There are half-life 727 180 two types of pure substances: ele- radioactive decay 729 Reilly, William K. 270 ments and compounds. 71 use 736 Relative atomic mass 333 Putrescine, molecular structure of 667 Radon-222 Relative solubilities 578 half-life 727 Representative elements The elements Q lung cancer and 728 in groups 1, 2, and 13 through 18 in radioactive decay series 729 (the “A” groups) on the periodic table; Quantum mechanics 437 Rags, in paper 187 also called main-group elements. 44 Quick lime, formation of 245 Rapture of the deep 596 Research, in scientific method 8 R Rate of chemical reaction The number Research chemist 609 of product molecules that form (per- Resonance The hypothetical switch- Race cars and air density 499 haps described as moles of product ing from one resonance structure to Radiant energy Energy that can be de- formed) per liter of container per another. 465–467 scribed in terms of oscillating electric second. 616–620 Resonance hybrid A structure that and magnetic fields or in terms of concentration effect 61 7–618 represents the average of the reso- photons. 260–262 temperature and 616–617 nance structures for a molecule or spectrum 262 Rate of condensation The number of polyatomic ion. 466 the wave view 261 particles moving from gas to liquid Resonance structures Two or more wavelength 261 per second. 537 Lewis structures for a single molecule Radiation Rate of evaporation The number of or polyatomic ion that differ in the effects on the body 73 0–731 particles moving from liquid to gas positions of lone pairs and multiple treatment for cancer 731 per second. 535–537, 536–537 bonds but not in the positions of the Glossary/Index G-21

atoms in the structure. 466 Schrodinger, Erwin 416 citrine as 362 Reversible reaction A reaction in Science in furnace method 330 which the reactants are constantly chemistry as 7–9 purifying silicon from 379–380 forming products and, at the same existence of matter and 437 Silk time, the products are reforming the mathematics in 413 molecular structure of 690 reactants. 163, 621–622 Scientific Method 7 –9 nylon as substitute for 690 in chemical equilibrium 621–625 Scientific model A simplified approxi- Silver (Ag) disruption of equilibrium for 634 mation of reality. See also Model 34, density of 302 equilibrium constants for 626 56, 448 ion charges of 99 percent yield and 382 Scientific notation 4 –5 melting point of 314 Review Skills sections 6 Scuba diving, gas solubility and 596 Silver ion, solubility of compounds with Rhodium, in catalytic converter 221 Sea-Nine antifoulant 5 141 Ribbon convention for proteins 681 Seaborg, Glenn 725 Silver nitrate, in precipitation reaction Ring forms, of monosaccharides Seawater, pH and 179 142 674–675 Sea of electrons model for metals 57 Single-displacement reaction Chemi- Roasting 384 Second (s), as unit of measurement 11 cal change in which atoms of one Rohm and Haas Company 5 Secondary (or storage) battery A element displace (or replace) atoms Roman numeral, in naming monatomic rechargeable battery. 228 of another element in a compound. cations 99 Secondary protein structure The ar- 222–223 Roots of nonmetal names 92 rangement of atoms that are close to Sinkhole 204 Roscoelite 365 each other in a polypeptide chain. Sixth principal energy level, electron Rounding off 29 3–301 Examples of secondary structures are orbitals of 423 for addition and subtraction alpha helix and beta sheet. 680–681 SI System of Measurement. See Interna- 299–301 Second period elements, electrons in tional System of Measurement for multiplication and division 425–427 Slaked lime 245 294–299 Selenide ion 98 Smelling salts 653 Roundup 621 Selenium Smog RU-486 705 bonding pattern 81 formation of photochemical Ruby 359 covalent bond formation 453 266–267 ion formation 95–96 nitrogen dioxide in 629 S most common bonding pattern 455 Smoke detectors 735 Semimetals The elements that have Soap 584, 586–587 Saccharide Sugar, starch, and cellulose. some but not all of the characteristics Society for Heavy-Ion Research 52 Also called carbohydrates. 674–677. of metals. 44 Sodium (Na) See also Carbohydrate Serine (Ser, S) electrolysis and 227 Saliva, tooth decay and 186 hydrogen bonds between 682 formation from sodium chloride Salt. See Sodium chloride molecular structure of 679 219 Salt bridge (in proteins) A covalent Shape. See Molecular shape ion 75–76 bond between two sulfur atoms on Shell 420. See also Principal energy ion formation 96 cysteine amino acids in a protein level Sodium aluminum sulfate, in baking structure. 682 Shroud of Turin 734 powder 73 Salt bridge (in voltaic cells) A device Side-chain, in anion acid 678 Sodium bromide, use 600 used to keep the charges in a voltaic Significant figures The number of Sodium carbonate cell balanced. 226 meaningful digits in a value. The reaction with acid 175 Salt taste 177 number of significant figures in a uses 175 Salt water separation 40 value reflects the value’s degree of un- Sodium chlorate, production and use San Simeon, California, protection from certainty. A larger number of signifi- 244 acid rain in 167 cant figures indicates a smaller degree Sodium chloride Saturated solution A solution that has of uncertainty. 293–301 electrolysis and 227 enough solute dissolved to reach the counting the number of 295–296 formation 76 solubility limit. 592, 592–593 zeros and 296 formula mass of 340 dynamic equilibrium and 588–593 Silicon (Si) 126 formula unit of 339 formation of 592–593 electronics grade 379 oxidation-reduction and 208–209 Saturated triglyceride A triglyceride metallurgical grade 379 solubility in water 593 with single bonds between all of the purifying 379–380 solution in water 133–135 carbon atoms. 683 from silicon dioxide 377 structure of 100–101, 101 Scale, calcium carbonate in 144 Silicon dioxide taste of 177 G-22 Glossary/Index

Sodium chromate 384 also be called homogeneous mixtures. Harmless Dietary Supplements or Sodium dichromate, production and use chemical reactions in 573 Dangerous Drugs 687 400, 408 dynamic equilibrium and 588–593 Molecular Shapes, Intoxicating sodium dodecyl sulfate (SDS), as deter- formation of 576–577 Liquids, and the Brain 89 gent 587 of ionic compounds 133–135 Olestra and Low-Fat Potato Chips Sodium fluoride, in toothpaste 9 5 molarity and 385–392 684–685 Sodium hydrogen carbonate rate of 589–592 Other Ozone-Depleting Chemicals production and use 175, 241 agitation 591 272 reaction with acids 175 factors that effect 58 9 Oxidizing Agents and Aging 212 Sodium hydrogen sulfate, production surface area 589–590 Precipitation, Acid-Base Reactions, and use 407 temperature effect 59 2 and Tooth Decay 186 Sodium hydroxide saturated 592–593 aqueous solution of 173 solute and solvent 136 Recycling Synthetic Polymers 694 formation 101 unsaturated 592 Rehabilitation of Old Drugs and in neutralizing phosphoric acid 390 why form 574–577 Development of New Ones 673 reaction with nitric acid 181–185 Solvent The liquid in a solution of a gas Safe and Effective? 35 4 uses of 101, 173 in a liquid. The liquid in a solution of Saving Valuable Books 187 Sodium hypochlorite, production 509, a solid in a liquid. The major compo- The Big Question - How Did We 552, 560, 580, 581 nent in other solutions. 136 Get Here? 640 Sodium ions 49 Sour taste 177 The Origin of the Elements 74 2 taste and 177 Space-filling model A way of repre- Wanted: A New Kilogram 11 Sodium , production and use senting a molecule to show a some- Why Create New Elements? 52 243 what realistic image of the electron- Why Does Matter Exist, and Why Sodium sulfate, production and use 243, charge clouds that surround the Should We Care About This 517 molecule’s atoms. 54, 86 Question? 437  Sodium tripolyphosphate, production Spandex , synthesis of 353 Zinc-Air Batteries 229 and use 410 Special conditions, in chemical equations Spectator ions Ions that play a role in Soft drink, why bubbles form 596 127–128 delivering other ions into solution to “Solar system” model of the atom 414 Special topics react but that do not actively partici- Solid The state in which a substance Acid Rain 167 pate in the reaction themselves. 139 has a definite shape and volume at a Air Pollution and Catalytic Convert- constant temperature. 34–35 ers 221 Spectrum, of radiant energy 261–262 densities of 301–302 A Greener Way to Spray Paint 514 Spin. See Electron spin expansion when heated 35 A New Treatment for Brain Cancer Spinels 359 heterogeneous equilibrium and 741 Spodumene 365 630–631 Be Careful with Bleach 188 Spray paint 514 Solid acid, in meals ready to eat 573 Big Problems Require Bold Solu- Stability A relative term that describes Solid elements 45, 56–57 tions - Global Warming and the resistance to change. 54, 252– Solubility The maximum amount of Limiting Reactants 384 254 solute that can be dissolved in a given Chemistry and Your Sense of Taste Standard kilogram 11 amount of solvent. 578–584 177 Standard pressure 503 gas 594–595 Chemistry Gets the Bad Guys 541 Standard temperature 503 guidelines 578 Gas Solubility, Scuba Diving, and Standard temperature and pressure (STP) like dissolves like 578–579 Soft Drinks 596 503 soaps and detergents and 586–587 Global Warming, Oceans, and CO2 gas stoichiometry and 503 in water 140–141, 593 Torpedoes 597 gas stoichiometry for conditions guidelines 141 Green Chemistry 5 other than 504–505 Solute The gas in a solution of a gas in Green Chemistry - Making Chemi- Standing waves 414–416 a liquid. The solid in a solution of a cals from Safer Reactants 351 solid in a liquid. The minor compo- Green Chemistry - Substitutes for Starch 674, 676 nent in other solutions. 136 Chlorofluorocarbons 27 2 Stars, element formation and 743 gas as 594–595 Green Chemistry - The Develop- State, physical 127 in saturated solution 588 ment of New and Better Cata- Stationary wave 415 Solution A mixture whose particles are lysts 621 Steam re-forming 396, 622 so evenly distributed that the relative Green Decaf Coffee 51 5 Stearic acid concentrations of the components are Hard Water and Your Hot Water molecular structure of 664 the same throughout. Solutions can Pipes 144 solubility of 583 G-23 Glossary/Index

Step-growth (or condensation) poly- calculating molecular formulas 352 Sucrase, in digestion 688 mer A polymer formed in a reaction calculations using unit analysis 308 Sucrose, solubility in water 593 that releases small molecules, such as classification of matter 7 2 Sugar 674–676 water. This category includes nylon combustion reaction 220 rate of solution 590 and polyester. 691 converting between mass of element taste of 177 Sterno 447 and mass of compound contain- Sulfate ion, solubility of compounds Steroid Compounds containing a ing the element 345 with 141 four-ring structure. 685–686 drawing Lewis structures from for- Sulfur 43–44 Stirring, rate of solution and 589–591 mulas 456–457 bonding pattern 81 Stockings 690 electronegativity, types of chemical combustion and 219 Stoichiometric ratio 376 bonds, and bond polarity 550 covalent bond formation 453 Stoichiometry. See Equation electron configurations and orbital ion formation 95–96 stoichiometry diagrams 431, 456 most common bonding pattern 455 Stomach equation stoichiometry 372–373, production 244 hydrochloric acid in 506 391, 507–508 use and production 525 role in digestion 689 equation stoichiometry problems 166 Stomach acid 506 391 acid rain and 167 Storage battery 228 identification of strong and weak in acrylamide synthesis 621 Stratosphere The second layer of the acids and bases 176 forming name of 169 earth’s atmosphere. It extends from limiting reactant problems 380 as oxyacid 162 about 10 km to about 50 km above predicting molecular geometry 472 production 238 sea level. 268 predicting precipitation reactions reaction with sodium hydroxide destruction of ozone in 269–271 and writing precipitation equa- 184 ozone hole in 271 tions 142 as strong acid 166 removal of UV radiation in 269 rounding off numbers calculated uses 166 + Strong acid An acid that donates its H using addition and subtraction Sulfur dioxide ions to water in a reaction that goes 299 acid rain and 167 completely to products. Such a com- rounding off numbers calculated air pollution and 523 + pound produces close to one H3O using multiplication and division in combustion reactions 219 ion in solution for each acid molecule 295 as pollutant and removal 408 dissolved in water. 163, 165 using Dalton’s Law of Partial Pres- Sulfur hexafluoride, threshold limit identifying 176 sures 512 value, or TLV 522 reactions of strong base with using the combined gas law equa- Sulfur trioxide, in acid rain 167 181–185 tion 500 Sun, nuclear fusion and 742 Strong base A substance that generates using the ideal gas equation 495 Supercritical carbon dioxide at least one hydroxide ion in solution writing complete electron configura- decaffeinating coffee and51 5 for every unit of substance added to tions and orbital diagrams for spray paint and 514 uncharged atoms 431 water. 173 Supercritical fluid 51 4 writing equations for combustion identifying 176 Supernovas 743 reactions 220 reactions of strong acids with Super glue 473 Styrene, in polystyrene 694 181–185 Surface area, rate of solution and Strong force Sublevel or subshell Orbitals that have The force that draws 589–590 nucleons (protons and neutrons) the same potential energy, same size, Sweet taste 177 together. 718 and same shape. 421 Symbols Strontium-90 730 Sublimation, of dry ice 255, 256 for elements 41 Studying chemistry 5 Subshell, of atomic orbitals 421 for nuclides 716 Study Sheets Substance, base unit of 10–11 Synthesis gas 622 abbreviated electron configuration Substances Synthesis reactions 218 433–436 densities of common 302 Synthetic polymers 690–695 assignment of oxidation numbers equation stoichiometry and s block, on peridoic table 428–429 214 368–375 balancing chemical equations 129 hydrophilic and hydrophobic 582 T basic equation stoichiometry - con- solubilities of 578–579 verting mass of one substance uses for radioactive 731–734 Tanzanite 363 in a reaction to mass of another Substrate A molecule that an enzyme Taste 177 372–373 causes to react. 690 Technical University of Munich 641 calculating empirical formulas 348 Subtraction, rounding off and 29 9–301 Television waves 262 G-24 Glossary/Index

Tellurium (Te), bonding patterns of 457 408 Tristearin 584 Temperature A measure of the average Thoburn, Steve 29 2 Tritium 50–51 internal kinetic energy of an object. Thortveitite 36 4 Troposphere The lowest layer of the 17–19, 259 Threonine (Thr, T), molecular structure earth’s atmosphere. It extends from absolute zero 18 of 679 the surface of the earth to about 10 base unit of 11 Threshold limit value, or TLV 52 2 km above the earth. 268 boiling-point 544 Time, base unit of 11 Trypsin 688 Celsius scale 18 Tin(II) sulfide, melting point of 31 4 Tryptophan (Trp, W), molecular struc- coldest 19 Tincture of iodine 556 ture of 679 common scales 19 Tin isotopes 51–52 Tungsten (W), in light bulb filaments in condensation 534 Titanium(IV) oxide 496 critical 514 production 528 Tyrosine (Tyr, Y), molecular structure density and 301 production and use 411 of 679 effect on rate of solution 59 2 Titanium (Ti) 56 equilibrium constants and 632–633 production and use 247 U equilibrium vapor pressure and Titanium carbide 381 Ultraviolet radiation 262 540–541 Titanium dioxide 632 Umami taste 177 in evaporation 536–537 production and use 238 Uncertainty 21 Fahrenheit scale 18–19 Titration, Web site for 392 in measurements 20–22 gases and 485 Toothpaste, chemicals in 116 Kelvin scale 18–19 Tooth decay, acid-base reactions and 186 significant figures and29 3–301 See measuring 18 Tooth enamel, composition of 186 Unified mass unit. Atomic mass unit Unit normal boiling-point 545 Torr, as unit of pressure 485 A defined quantity based on a pressure and 488 Trailing zeros, measurement uncertainty standard. 9–18, 1–3 range of 19 and 22 abbreviations 1 rate of reaction and 616–618 Transition metals The elements in conversions among 288–314 rate of solution and 592 groups 3 through 12 (the “B” groups) of energy 257 standard 503 on the periodic table. 44 in international system of measure- volume and 489 as catalysts 620 ment 10–12 Temperature conversions 312–314 in catalytic converters 221 length 14 Terephthalic acid, in plyester formation in periodic table 44 mass 16 692 Transition state, in chemical reactions the importance of putting into equa- Tertiary protein structure The overall 611 tions 497 arrangement of atoms in a protein Triacylglycerol 584–585 volume 15 molecule. 681 Triangular planar. See Trigonal planar United States, ozone concentrations in Testosterone 686 Triglyceride A compound with three 267 Tetraboron carbide, production and use hydrocarbon groups attached to a Unit analysis A general technique for 400, 401 three carbon backbone by ester func- doing unit conversions. 288–292, Tetrachloroethene 375 tional groups. 584–585, 683–685 330–334, 342–350, 368–372, 376– Tetrahedral molecules 86, 468–469 Trigonal planar (often called triangular 380, 414–418, 424–428, 448–452 Tetrahedral The molecular shape that planar) The geometric arrangement equation stoichiometry and 370 keeps the negative charge of four that keeps three electron groups as far gas stoichiometry and 505 electron groups as far apart as pos- apart as possible. It leads to angles of Study Sheet 308–309 sible. This shape has angles of 109.5° 120° between the groups. 470 summary of 308–312 between the atoms. 86 Trigonal pyramid The molecular ge- Unit conversions 288–292, 330–334, Tetramethylene glycol 354 ometry formed around an atom with 342–346, 346–350, 368–372, 376– Tetrapeptide 680 three bonds and one lone pair. 469 380, 414–418, 424–428, 448–452 Tetraphosphorus decoxide, in furnace Trimethylamine 668 “something per something” 311 method 330 2,2,4-Trimethylpentane 661 common 308–312 Tetraphosphorus trisulfide 13 1 Trinitrotoluene (TNT) 662–663 density and 303, 310, 501-506, Thalidomide 36 4, 673 Triple bond A link between atoms 551 Theoretical yield The calculated maxi- that results from the sharing of six English-metric 291–292, 310 mum amount of product that can electrons. It can be viewed as three 2- metric-metric 289–291, 310 form in a chemical reaction. 382 electron covalent bonds. 83, 451 percentage and 307, 311 Thermometers 1 8–19 Triprotic acid An acid that can donate Universal gas constant, R The constant 39 8 three hydrogen ions per molecule in a in the ideal gas equation. 494 Thionyl chloride, production and use reaction. 163 in gas stoichiometry 505–509 G-25 Glossary/Index

in ideal gas equation 494–499 and p electrons for an atom. 79, 449 measurement, graduated cylinder Universe electron dot symbol 79–80 21 hottest temperatures in 19 Valine (Val, V), molecular structure of number of gas particles and 491 origin of elements in 742–743 678 pressure and 486–487 University of California, Berkeley 725 Value A number and unit that together range of 16 University of Regensberg 641 represent the result of a measurement temperature and 489 Unpaired electrons 79 or calculation. 10 Volume unit, liter 12 in valence-bond model 449 Vanadium(V) oxide, in catalytic con- Unsaturated solution A solution that verter 221 W has less solute dissolved than is pre- Vapor A gas derived from a substance dicted by the solubility limit. 592 that is liquid at normal temperatures Wächtershäuser, Günter 641 Unsaturated triglyceride A triglyceride and pressures. It is also often used to Water 70 that has one or more carbon-carbon describe gas that has recently come acids and 160–161, 163–164 double bonds. 683 from a liquid. 534 ammonia and 173–174 Uranium 381 Vaporization The conversion of a attractions 88 alpha emission 720 liquid to a gas. 37 bases and 173 production 402 Vapor pressure. See Equilibrium vapor boiling point of 18–19, 545 uranium-238 decay series 729 pressure as compound 71 Uranium(IV) oxide 381 Vegetable oil 585 condensation of 534–535 Velocity Uranium-234 740 in condensation reactions 689 Uranium-235 740 of gas particles 484 covalent bond formation 452 enrichment 381 kinetic energy and 251 density of 302 in fission reactors 74 0 of particles in evaporation 535 dissolving sodium chloride in half-life 727 Vinegar Uranium-238 acetic acid in 162 134–135 in fission reactors 74 0 taste of 177 evaporation of 535 half-life 727 Vinyl chloride, in poly(vinyl chloride) hard 144 nuclide symbol 717 694 heavy 313 radioactive decay series 729 Visible fingerprints 54 1 hydrogen bonds in 554 Uranium-239 Visible light 262 ionizing radiation and 730–731 in nuclear reactors 740 Vitamin C, aging and 212 Lewis structure 81 in nuclear fission 73 8 Vitamin E, aging and 212 liquid 88–89 Uranium hexafluoride 36 7, 381 Volatile organic compounds (VOCs) melting point of 18–19 Urea 411 514 mixing with ethanol 576–577 use and production 526, 654 Voltage 227 molecular shape 87–88, 469 Voltaic cell UV-A Ultraviolet radiation in the range A system in which two in nylon formation 691 half‑reactions for a redox reaction of about 320 to 400 nm wavelengths. pH of 179 are separated, allowing the electrons This is the part of the ultraviolet as polar molecule 88, 553 spectrum that reaches the earth and transferred in the reaction to be producing hydrogen gas from provides energy for the production of passed between them through a wire. 621–623 vitamin D. 268 224–229 in protein formation 680 UV-B Ultraviolet radiation in the range anode 225 of about 290 to 320 nm wavelengths. cathode 225 rate of solution in 589–593 Most of this radiation is filtered out common examples 229 solubility in 578–583 by the earth’s atmosphere, but some electrode 225 structure of 87–88 reaches the surface of the earth. 268 electrolyte 226 Water dissociation constant (Kw) The UV-C Ultraviolet radiation in the range primary battery 228 equilibrium constant for the reaction: + - of about 40 to 290 nm wavelengths. salt bridge 226 H2O(l ) H (aq) + OH (aq) 632 Almost all UV‑C is filtered out by our secondary battery 228 Water purification 37 4 atmosphere. 268 zinc-air batteries 229 Water solubility 140–141 Volume (V) 15–16 Water treatment 202 V density and 301 Wave English-metric conversion factors electrons as 416–423 Valence-bond model 449–454 for 292 Valence electrons for guitar strings 414 The electrons that are of gases 485 radiant energy as 260–262 most important in the formation of of ideal gas particles 485 chemical bonds. The highest energys standing 414–415 G-26 Glossary/Index

Waveform A representation of the for gas stoichiometry shortcut 506 shape of a wave. for how addition polymers are made of electron 416 693 of guitar strings 415 for London forces and polar mol- Wavelength The distance in space over ecules 558 which a wave completes one cycle of for mixtures and equation its repeated form. 261–262 stoichiometry 375 Weak acid A substance that is incom- for polyatomic ions 103 pletely ionized in water due to the for predicting molecular polarity reversibility of the reaction that forms 553 + hydronium ions, H3O , in water. for predicting relative strengths of Weak acids yield significantly less attractions 560 + than one H3O ion in solution for for resonance 467 each acid molecule dissolved in water. for temperature effect on solid and 163, 164 gas solubility 597 Weak base A substance that produces for writing complete ionic and net fewer hydroxide ions in water solution ionic equations 143 than particles of the substance added. Weight A measure of the force of gravi- 174–175 tational attraction between an object ammonia as 173–174 and a significantly large object, such identifying 176 as the earth or the moon. 16 Weather balloon 502 Weighted average A mass calculated Web site by multiplying the decimal fraction for acid-base titration 392 of each component in a sample by its for acid nomenclature 169 mass and adding the results of each for animation of acid-base reaction multiplication together. 331 185 Wine for animation of a single-displace- pH of 179 ment reaction 222 sediment formation 579 for animation of dissolving ethanol Work What is done to move an object in water 577 against some sort of resistance. 250 for animation of element structure 56 X for animation of precipitation reac- X-rays 262 tion 140 X-ray crystallography 673 for animation of solution of sodium Xenon (Xe), reactions 242 chloride 136 Xenon difluoride 39 7 for animation of strong and weak acids 166 Y for animation of the particle nature See of matter 38 Yield. Actual yield; Theoretical yield; for animation of water structure 89 Percent yield for balancing redox equations 218, Z 222 for calculating element percentages Zeros and significant figures29 6 346 Zinc-air batteries 229 for changing volume and gas reac- Zinc (Zn) 56 tions 637 batteries and 224–227 for combustion analysis 353 reaction with copper sulfate for conversion between element 222–223 names and formulas 41 single-displacement reaction and for different electron configurations 222–223 436 voltaic cells and 224–226 for enzyme mechanism 690 Zinc oxide for equilibrium calculations, includ- in book preservation 187 ing pH 633 oxidation-reduction and 208–209 for isotope notation 52 in zinc-air batteries 229