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Glossary/Index

A taste of 345 Alcohol Compounds that contain a triprotic. See Triprotic acid hydrocarbon group with one or more Abbreviated electron configuration, of types 250 -OH groups attached. 196, 639. See multi-electron atoms 151–154 weak 251–253 also Methanol, Ethanol, and 2-pro- Absolute zero Zero kelvins (0 K), the Acid-base reaction 348–356 panol lowest possible temperature, equiva- strong acid with base bonds and 531 lent to -273.15 °C. It is the point 349–353 Aldehyde A compound that has a hy- beyond which motion can no longer uses 348 drogen atom or a hydrocarbon group be decreased. 18 writing equations 351 connected to a -CHO group. 641 Accuracy How closely a measured Acidic paper, preserving books with 355 Aldol, molecular structure of 645 value approaches the true value of the Acidic solution A solution with a sig- Alka-Seltzer 502 property. 20 nificant concentration of Alkali metals Group 1 (or 1A) on the Acetaldehyde, determining Lewis struc- + , H3O . 248, 340 periodic table; See also Lithium, So- ture 206–207 Acid rain 255 dium, Potassium, and Cesium 85 Acetamide 644 pH and 346 charges of 182–183 ion, solubility of compounds Acrylamide 597 Alkaline earth metals Group 2 (or 2A) with 317 Activated complex 587 on the periodic table; See also Beryl- Acetic acid 250–253, 640 Activation energy The minimum lium, Magnesium, and Calcium 85 dissolved in water 252 energy necessary for reactants to reach ion charges of 183 formulas 250 the activated complex and proceed to Alkane A hydrocarbon (a compound freezing point of 250 products. 588 composed of carbon and hydrogen) in glacial 250 Active site A specific section of the pro- which all of the carbon-carbon bonds molecular structure of 250 tein structure of an enzyme in which are single bonds. 637 as organic acid 250 the substrate fits and reacts. 66 6 Alkene A hydrocarbon that has one or production 504, 630 Actual yield The amount of product more carbon-carbon double bonds. solubility in water 569 that is actually obtained in a chemical 638 taste of 248 reaction. 428 Alkyne A hydrocarbon that has one or uses 250, 630 Adams, Mike 650 more carbon-carbon triple bonds. as weak acid 251 Addition, rounding off for 4 5–46 638 Acetone 642 Addition polymer A polymer that con- Alpha emission The process of releas- boiling point of 522 tains all of the atoms of the original ing an alpha particle by atoms that evaporation of 512 reactant in its structure. This category have too many protons to be stable. use 543 includes polyethylene, polypropylene, 696 vapor pressure of 516 and poly(vinyl ). 669–670 nuclear equations for 699–701 Acetylene 192, 638 Adipic acid 276 Alpha helix 656–657 molecular structure of 192 Adults Alpha particle The emission from ra- water solubility of 556 effects of ionizing radiation on 70 6 dioactive nuclides that is composed of Acid. See also Arrhenius acid fingerprints of 51 7 two protons and two neutrons in the binary. See Binary acid Aerosol can 517 form of a helium nucleus. 696 bleach and 356 Agent Orange 295 effects on body 70 6–707 Brønsted-Lowry 356–360 Aging, oxidizing agents and 376 penetration of the body 707 conjugate acids and bases 357 Agitation, rate of solution and 566–567 Alternate Synthetic Pathways Award 597 carboxylic acid. See Carboxylic acid AIDS 649 Alum. See Aluminum characteristics 248 Air 485–486 Aluminum 86 classification of strong or weak 25 4, density of 48 ion formation 91, 183 344–345 gases in 486 Aluminum , production and use defined 35 6 in lungs 469 399 diprotic. See Diprotic acid internal combustion engine and Aluminum chloride 243 identifying 344–345 468 Aluminum fluoride, production and use monoprotic. See Monoprotic acid Air bags 502 447 names and formulas of 256–258 Air pollution Aluminum hydroxide, dissolving in acid . See Oxyacid catalytic converters and 385 352 pH 346–347 volatile organic solvents and 490 Aluminum 306 polyprotic. See Polyprotic acid Alanine (Ala, A) Aluminum sulfate in saliva 345 silk and 666 old books and 355 strong 253, 340 structure of 654 production and use 456 Study Sheet, indentifying 344 Alar 292 water purification 42 0 G-1 G-2 Glossary/Index

Americium-241 and smoke detectors Androstenedione 662, 663 Arrhenius base A substance that 711 Aniline, production and use 445, 448 produces hydroxide ions, OH-, Amide A compound with the general Animal fat 561 when added to water. 342–346. See formula RCONR, in which each R Anion An ion formed from an atom also Base represents hydrogen atoms or hydro- that has gained one or more elec- compared to Brønsted/Lowry bases carbon groups. 644 trons and thus has become negatively 356–360 in digestion 665 charged. 91 defined 34 1 as peptide bond 656 formation 182–183 reactions with acids 348–355 Amine A compound with the general in batteries 389–390 strong and weak 341–344 formula R3N, in which R represents in classifying types of compounds Arsenic (As) a hydrogen atom or a hydrocarbon 180 bonding patterns of 193 group (and at least one R group being in ionic bond formation 177–178 Asparagine (Asn, N), structure of 655 a hydrocarbon group). 643–644 monatomic 183 Aspartame 681, 687 Amino acid The monomer that forms naming 236–237, 239–241 Aspartic acid (Asp, D) the protein polymers. They contain an polyatomic 185–187 in bridges 658 amine and a carbox- structure of ionic compounds 185 structure of 655 ylic acid group separated by a carbon. writing formulas 242–243 Asphalt, London forces in 532–533 654–655 Anode The electrode at which oxida- Asymmetry, in polar 528, 529 in origin of life 616–618 tion occurs in a voltaic cell. It is the Atmosphere (atm), as unit of pressure protein fomation and 656 source of electrons and is the negative 461 in silk 666 electrode. 389 Atmospheric pressure 461 1-Aminobutane 643 Antacid 300, 482 boiling-point temperature and Aminopeptidase 664 Anti-electron (positron) 155 521–522 341–342 Antimatter 155 Atom The smallest part of the element covalent bond formation 192 Antioxidant, aging and 376 that retains the chemical characteris- hydrogen bonds and 531 Antiparticle 155 tics of the element itself. 88–90 molecular shape of 211 Application, in scientific method 8 –9 atomic numbers of 93 origin of life and 617 Aquamarine 294 chemical bonds between 175–179 pH of 347 Aqueous solution A solution in which in chemical reactions 300–302 production 480, 597 water is the solvent. 309 counting by weighing 100–103 uses 341, 546 Arene (or aromatic compound) A com- electron 90 weak base 341–342 pound that contains the benzene ring. electron configuration 14 2 , use 629 638–639 electron configurations and orbital Ammonium chloride, crystal structure Arginine (Arg, R), structure of 655 diagrams 149, 198 of 186 Argon excited and ground state 138 Ammonium ion in air 486 as formula unit 264 covalent bond formation 192 in incandescent light bulbs 472 mass numbers of 93–94 solubility of compounds with 316 in neon lights 485 molar mass of 104–105 Ammonium , in cold packs 322 Aromatic. See Arene A compound that nuclear reactions of 696–700 Ammonium , space shuttle nuclear stability of 694 contain the benzene ring. and 409 orbital diagram 142 Aromatic compounds Compounds that Ammonium , fertilizers and oxidation numbers of 377–384 contain the benzene ring.. See Arene 377 protons, neutrons, and electrons 89 Arrhenius, Svante August 248 Ammonium , use 24 3 radioactive decay of 696–700 Arrhenius acid According to the Amount of substance, base unit of 10 size of 89 Arrhenius theory, any substance that Amphere, as unit of measure 11 size of nucleus 89 generates hydronium ions, H O+, Amphetamine 558 3 structure of 88–92 when added to water. 248–255, Amphoteric substance A substance Atomic mass The weighted average of 340–347. See also Acid that can act as either a Bronsted- the masses of the naturally occurring binary acid 250 Lowry acid or a Bronsted-Lowry base, isotopes of an element. compared to Brønsted/Lowry acids depending on the circumstances. 359 calculations 105 356–360 Amylase 664 defined 10 2 defined 24 8, 340 Amylopectin 652–653 relative 102 names and formulas for 256–258 Amylose 652–653 Atomic mass unit (u or amu) One- organic (or carbon-based) acid 250 Analogies, to electron behavior 132 twelfth the mass of an atom of 250 Anastas, Paul T. 5 carbon-12. Carbon-12 is the isotope reactions with bases 348–355 Anderson, Carl 155 of carbon that contains 6 protons, Glossary/Index G-3

6 neutrons, and 6 electrons. 89, and sticks for covalent bonds. 96 Benzene 276 101–102 of acetic acid 250 Berkelium (Bk) 701 Atomic number The number of pro- for acetylene 214 Beryllium (Be) tons in an atom’s nucleus. It estab- for boron trifluoride 21 3 electron configuration and orbital lishes the element’s identity. 93 for ethane 213 diagram 144 in nuclear equations 698–702 for organic molecules 636 formation of 718 in nuclides 692–693 of methane 211 Beta emission The conversion of a Atomic orbitals of water 212, 308 neutron to a proton, which stays in 1s 134–136 Band of stability On a graph of the the nucleus, and an electron, called a 2p 139 numbers of neutrons versus protons beta particle in this context, which is 2s 137–138 in the nuclei of atoms, the portion ejected from the atom. 696 3d 140 that represents stable nuclides. 695 nuclear equations for 699–701 electron cloud 136 Barium ion, solubility of compounds Beta particle A high-velocity electron electron spin and 144 with 317 released from radioactive nuclides that for first 10 elements 14 5 Barium sulfate 319 have too many neutrons. 696 order of filling 14 3, 146–148 Barnes, Randy 663 effects on body 70 6–707 probability and 136 Base 341–345 See also Arrhenius base penetration of the body 707 relative energies 138 Arrhenius 342 Beta sheet 656 shapes 137 Brønsted-Lowry 356–360 Big Bang 718 Atomic weight See also Atomic mass carbonate 343 Binary acid Substances that have the 102 classification of strong or weak general formula of HX(aq), where Attraction. See also Gravitational attrac- 344–345 X is one of the first four halogens: tion; Electrostatic attraction; Strong conjugate 358 HF(aq), HCl(aq), HBr(aq), and force; Particle-particle attractions defined 34 1 HI(aq). 250 between gas particles 460 identifying 343–344 formulas 256 between liquid particles 510 in acid-base reactions 348–356 naming 256 intermolecular 523–533 pH 346–347 Binary covalent compound A com- particle-particle attraction 523–538 strong 341 pound that consists of two - Aurum 83 Study Sheet, indentifying 344 lic elements. Automobile Exhaust 173 weak 342–343 memorized names 244 Average, weighted 100 Base units The seven units from which names without prefixes 24 6 Avogadro’s Law Volume and the all other units in the SI system of naming 244–245 number of gas particles are directly measurement are derived. 10–11 prefixes used to name 24 5 proportional if the temperature and table of 11 recognizing from formulas 244 Basic solution pressure are constant. 467 A solution with a recognizing from names 246 significant concentration of hydroxide systematic names 244–246 Avogadro’s number The number of - atoms in 12 g of carbon-12. To four ions, OH . 341 writing formulas 246–247 Battery A device that has two or more Binary An ionic significant figures, it is 6.022× 1023. voltaic cells connected together. The compound whose formula contains 102–103 term is also used to describe any one symbol for a metal and one sym- B device that converts chemical energy bol for a nonmetal. 239 into electrical energy using redox reac- Binding energy The amount of energy Bacon, Roger 33 tions. 388–393. See also Voltaic cell released when a nucleus is formed. Bacteria 400 defined 38 8, 389 713 tooth decay and 354 dry cell 390–391 Biocatalyst 597 Baking powder 175 nickel-cadmium batteries 392 Biochemistry The of biologi- Balance, electronic 23, 46 rechargeable 392 cal systems. 650–663 Balanced chemical equation zinc-air 393 Biomolecule 650–663 coefficient30 1 Beef fat 560–561 amino acids and protein 654–658 coefficients to conversion factors Bends, the 572 carbohydrate 650–653 415–416 Benitoite 294 how form 616–618 in equation stoichiometry 414–421 Bent geometry The molecular geom- steroid 661–662 Balancing chemical equations 302–307 etry formed around an atom with two triglycerides 659 steps in 303 bond groups and two lone pairs or Bismuth, in the creation of element 111 Study Sheet 303 two bond groups and one lone pair. 94 Ball-and-stick model A representation 212 Bitter taste 345 of a molecule that uses balls for atoms Benzedrine 558 Blake, William 119 G-4 Glossary/Index

Bleach Bromine (Br) Calcium dihydrogen phosphate, produc- dangerous combination with acid structure 97 tion and use 453 356 use 546 Calcium hydrogen , production pH of 347 Bromomethane, and threshold limit and use 407 Blocks, in periodic table 146–147 value, or TLV 498 Calcium nitrate 243, 312–313 Blood Brønsted-Lowry acid A substance that Calcium phosphide (or photophor), pH of 347 donates protons, H+, in a Bronsted- empirical formula for 273 Blue litmus paper, detecting acids with Lowry acid-base reaction. See Acid, Calorie (with an uppercase C), Cal 348 Brønsted-Lowry The dietary calorie. In fact, a Calorie Boiling The conversion of liquid to va- Brønsted-Lowry acid-base reaction A is a kilocalorie or 4184 joules. 127 por anywhere in the liquid rather than chemical reaction in which a proton, calorie (with a lowercase c), cal A just at the top surface. 518–522 H+, is transferred. See Acid-base reac- common energy unit. Equivalent to defined 52 0 tion, Brønsted-Lowry 4.184 joules. 127 how bubbles form 518–520 Brønsted-Lowry base A substance that Cancer, boron fusion and 717 Boiling-point temperature The accepts protons, H+, in a Bronsted- Capsaicin 559 temperature at which a liquid boils. Lowry acid-base reaction. See Base, Carbohydrate Sugar, starch, and It is also the temperature at which Brønsted-Lowry cellulose. Also called saccharides. the equilibrium vapor pressure of the Bubbles 650–653 liquid becomes equal to the external in boiling liquid 520 Carbon (C) 90 pressure acting on the liquid. 520 how form in liquid 518–520 combustion and 383 effect of external pressure 52 0–522 in soft drinks 572 covalent bond formation 190–191 strengths of attractions and 522 Bunsen burner, hottest part of flame 6 0 diamond as 89 Bond. See Chemical bond Bureau International des Poids et electron configuration and orbital Bond angle The angle formed by Mesures (BIPM) 11 diagram 144–145 straight lines (representing bonds) Butadiene 500 in heavy-ion therapy 94 connecting the nuclei of three adja- Butane, molecular structure of 191 isotopes of 102 cent atoms. 210 1,4-Butanediol (BD) 279 medical use 94 Bond dipole A polar covalent bond, Butanoic acid in pig iron 485 which has an atom with a partial posi- molecular structure of 559, 640 Carbon-13 709 tive charge and an atom with a partial solubility of 559 Carbon-14, radioactive decay of 709 negative charge. 525 2-Butanone 642 Carbon-14 dating The process of Bond polarity, predicting 524–528 Butylated hydroxytoluene (BHT) 638 determining the age of an artifact that Books, preserving 355 Butyl ethyl ether 636 contains material from formerly living Boron (B) Butyric acid 640 plants or animals by analyzing the brain cancer treatment and 717 ratio of carbon-14 to carbon-12 in the covalent bond formation 194 C object. 709–710 covalent bonding pattern 195 Carbonate ion 343 electron configuration and orbital Cadaverine 643 reaction with acids 353 diagram 144 Cadmium (Cd) solubility of compounds with 317 nuclear power plant control rods in nickel-cadmium batteries 392 in weak bases 343 and 716 nuclear plant control rods and 716 Carbon black 427 Boron trifluoride 19 4 Caffeine 57 3 Carbon dioxide Bovine pancreatic trypsin inhibitor removal from coffee 49 1 as dry ice 125 (BPTI) 656–658 taste of 339 in automobile exhaust 173 Boyle’s Law The pressure of a gas is in- Calamine 296 catalytic converter and 385 versely proportional to the volume it Calcium (Ca), ion formation 183 in combustion reactions 383 occupies if the number of gas particles Calcium , production 448 decaffeinating coffee and49 1 and the temperature are constant. Calcium carbonate 300, 322, 592 global warming and 430 462–463 acid rain and 255 greenhouse gas 573 Brain, intoxicating liquids and 214 as antacid 482 polarity 528 Brain cancer, treatment for 717 formation in pipes of 320 in soft drinks 572 Brandes, Jay A. 617 in limestone caverns 368 solid to gas 552 Breathing 469 natural sources of 320 solubility in water 569 Bristlecone pines and carbon-14 dating oil production and 354 spray painting and 490 710 precipitation reaction 312–315 supercritical 490 Bromide ion, solubility of compounds solubility in water 569 Carbon dioxide torpedos 573 with 317 Calcium chloride 300 Carbonic acid 573 Glossary/Index G-5

Carbon monoxide its structure. This category includes elements in the compound by their catalytic converters and 385 polyethylene, polypropylene, and symbols and indicates the relative covalent bond formation 193 poly(vinyl chloride). 669 number of atoms of each element in hydrogen gas production 598 Chain reaction A process in which one with subscripts. 172–173. See incomplete combustion and 385 of the products of a reaction initiates also Lewis structure of 193 another identical reaction. 715 for acids 256–258 as pollutant 385 Chapter Objectives 6 for binary covalent compounds 246 in synthesis gas 598 Charge in chemical equations 301 Carbon tetrachloride, use and produc- in atoms 89 conversion factors from 267–270 tion 502 in chemical bonds 178, 524–527 for monatomic ions 236 Carboxylic acid A compound that have in HCl molecules 176 of polyatomic ions 238 a hydrogen atom or a hydrocarbon in hydrogen bonds 529 of polymers 667–670 group connected to a -COOH (or of ions 182–185 Chemical nomenclature -CO2H) group. 250, 353, 640 in London forces 532 binary acids 256 in acid-base reactions 353 in molecules 528–529 binary covalent compounds forming name of 257 in water molecules 212, 307 244–248 Carboxypeptidase, in digestion 664 Charge cloud, for electrons 90, 136–139 memorized Names 244 Carnegie Institution 617 Charles’ Law The pressure of a gas is names without prefixes 24 6 Carothers, W. H. 667 inversely proportional to the vol- naming 244–245 Catalyst A substance that speeds a ume it occupies if the number of prefixes used to name 24 5 chemical reaction without being per- gas particles and the temperature are recognizing from formulas 244 manently altered itself. 594–597, 597 constant. 465 recognizing from names 246 automobile catalytic converter 385 Chemical bond An attraction between systematic names 244–246 equilibrium and 614–615 atoms or ions in chemical com- ionic 239–243 green chemistry and 597 pounds. Covalent bonds and ionic oxyacids 257 homogeneous and heterogeneous bonds are examples. 175–179. See summary 259–260 596–597 also Ionic bond; Covalent bond Chemical reaction The conversion of in producing hydrogen gas 598 angles between 210–212 one or more pure substances into one Catalytic converter 385, 596–597 energy and 123–124 or more different pure substances. Cathode The electrode at which reduc- ionic bond 177–179 300 tion occurs in a voltaic cell. It is the nonpolar covalent 176 acid-base 348–357 positive electrode. 389 polar covalent 176 chemical equations for 300–302 Cation An ion formed from an atom predicting bond type 179–181, collision theory for 586 that has lost one or more electrons 524–525 combination 382 and thus has become positively summary 178 combustion 383–385 charged. 91 Chemical change. See Chemical reaction completion 252 formation of 181, 182–183 . See Compound converting to names 259–260 monatomic Chemical Elements. See Element decomposition 383 naming 236 Chemical engineering 585 double-displacement 312 roles in body 185 Chemical equation 300–307 endothermic 322–323 names 240 for acid-base reactions 351–355 energy and 321–323 produced by ionizing radiation 706 balancing 302–307 equilibrium constants for 602–607 Celgene Corporation 649 polyatomic ions 303, 306 exothermic 321–322 Cellulose 650, 652–653 Study Sheet 303 general process, collision theory molecular structure of 653 chemical calculations and 413 586–592, 634–640, 650–656, Celsius scale 18–19 complete 316 664–670, 666–672, 692–698 Celsius to Fahrenheit conversion complete ionic 315 neutralization 348–355 58–60 heat and 302 oxidation-reduction 372–375 Celsius to Kelvin conversion 58–60 interpreting 300–302 precipitation 312–318. See Cesium (Cs), electron configuration of molecular 316 also Precipitation reaction 152 net ionic 316 predicting extent of 602–605 Cesium-137 706 physical states and 301 rate 592–596 Cesium chloride, crystal structure of special conditions and 301–302 concentration effect 59 3–594 186–187 Chemical equilibrium. See Equilibrium temperature effect 59 2–593 Chain-growth (or addition) poly- A concise written reversible 251, 597–598 mers A polymer that contains all of description of the components of a reversible reaction and equilibrium the atoms of the original reactant in chemical compound. It identifies the 597–601 G-6 Glossary/Index

single-displacement 386 377–380, 382–385, 388–391 Completion reaction 252 synthesis 382 mixture 173 Compound A substance that contains types of 382–388 pure substance 173 two or more elements, the atoms of Chemistry The structure and behavior Study Sheet 174, 476, 483, 488, these elements always combining in of matter. 4. See also Organic chem- 526 the same whole-number ratio. 172 istry; Biochemistry Classifying compounds 180 binary covalent 244 combinatorial 649 Clean Air Act of 1967 499 binary ionic 239 Green. See Green Chemistry Cleaning with soap and detergent classification 18 0 nuclear 691–701 562–563 element versus 172 organic 633–648 Clinton, Bill 5 ionic 180 suggestions for studying 5 Coal, acid rain and 255 molar masses of 261–265, 267–271 Chemists 4 Cobalt-60 molecular 180 Children cancer radiation treatment and 707 as pure substance 172–175 effects of ionizing radiation on 70 6 food irradiation and 711 Computer-based tools that accompany fingerprints of 51 7 gamma ray emission and 698 this text 7 Chili peppers 559 Coefficients The numbers in front Concentration The number of particles Chloral hydrate 206 of chemical formulas in a balanced per unit volume. For gases, it is usu- Chloride ion 91 chemical equation. 301 ally described in terms of moles of gas in sodium chloride 172 Coffee particles per liter of container. Sub- solubility of compounds with 317 pH of 347 stances in solution are described with (Cl) removing caffeine 49 1 molarity (moles of solute per liter of as anion 177–178 Cold-start emissions, catalytic converters solution). 593 bleach and 356 and 385 disruption of equilibrium and 610 catalyst for ozone destruction Cold packs 322 equilibrium constants and 602–605 594–596 Collision theory A model for the rate of reaction and 593–594 diatomic molecules of 97 process of chemical change. 586– Condensation The change from vapor electrolysis and 391 592, 634–640, 650–656, 664–672, to liquid. 510 ion formation 182 692–698 dynamic equilibrium between in ionic bonds 177 orientation 591 evaporation and 513–515 product of the electrolysis of salt 81 steps 586–588 rate of 513 reaction with alkali metals 84 summary 591–592 Condensation (or step-growth) poly- structure 97 Combination (or synthesis) reaction mer A polymer formed in a reaction threshold limit value, or TLV, and The joining of two or more elements that releases small molecules, such as 498 or compounds into one product. 382 water. This category includes nylon use and production 501, 580 Combinatorial chemistry 649 and polyester. 667 valence electrons 198 Combined gas law equation 476 Condensation reaction A chemical Chlorine-36 710 Combustion analysis, empirical and reaction in which two substances Chlorobutane, formation of 428 molecular formulas from 278 combine to form a larger molecule 1-Chloropropane, melting point of 59 Combustion reaction Rapid oxida- with the release of a small molecule, Chocolate, taste of 345 tion accompanied by heat and usually such as water. 656 Cholesterol, structure of 661–662 light. 383–384 Condensed formula 635 Chromite 430 incomplete 385 Confirmation, in scientific method9 (Cr), sources of 297 Study Sheet 384 The molecule or ion Chromium(III) oxide 243 Complete (or molecular) equation A that forms when one H+ ion is added as catalyst 598 chemical equation that includes to a molecule or ion. 357 catalytic converter and 385 uncharged formulas for all of the Conjugate acid-base pair Two mol- empirical formula of 271 reactants and products. The formulas ecules or ions that differ by one +H production and use 447, 454 include the spectator ions, if any. 316 ion. 357–358 Chyme 664 Complete combustion 383–384 Conjugate base The molecule or ion Chymotrypsin, in digestion 664 Complete electron configuration that forms when one H+ ion is re- Citric acid 248 148–150 moved from a molecule or ion. 358 taste of 345 Complete ionic equation A chemi- Conservation of Energy, Law of 122 Citrine 294 cal equation that describes the actual Control rods Rods containing sub- Clark, Desmond 709 form for each substance in solution. stances such as cadmium or boron Classification of Matter 12 0–123, For example, ionic compounds that (which are efficient neutron absorb- 172–175, 256–259, 300–303, 321– are dissolved in water are described as ers), used to regulate the rate of 327, 346–351, 356–359, 372–375, separate ions. 315 nuclear fission in a power plant and Glossary/Index G-7

to stop the fission process if necessary. Dead Sea Scrolls 710 359 716 Decaffeination 49 1 Dimensional analysis. See Unit analysis Conversion factor A ratio that de- Decimal place Dimethyl ether, Lewis structure for 206 scribes the relationship between two calculators and 40 Dipole A molecule that contains an units. 34–36 measurements and 39 asymmetrical distribution of positive atomic mass as 104 rounding for addition and subtrac- and negative charges. density as 49 tion and 45 bond 525 English-metric 38 Decomposition reaction The conver- induced 532–533 in equation stoichiometry 418 sion of one compound into two or instantaneous 532–533 formula mass as 265 more simpler substances. 383 Dipole-dipole attraction The intermo- from percentage 52 Denature To change the tertiary struc- lecular attraction between the partial metric-metric 35 ture of a protein, causing it to lose its negative end of one polar molecule molecular mass as 262 natural function. 665 and the partial positive end of another percentage 52 Density, mass Mass divided by volume. polar molecule. 523 Cooling, in evaporation 512–513 47–51 hydrogen bonds and 530 Copper(II) ion, voltaic cells and 388– calculating for gases 474 London forces and 532 390 of common substances 48 Diprotic acid An acid that can donate Copper(II) oxide, in catalytic converter definition 4 7 two hydrogen ions per molecule in a 385 determination of 50–51 reaction. 250 Copper sulfate, reaction with zinc substance identification and 4 8 Dirac, Paul Adrien 155 386–387 temperature and 47 Direct-contact method 491 Corliss, Jack 617 units of 48 Disaccharide Sugar molecule composed Corundum 290 Designing Safer Chemicals Award 5 of two monosaccharide units. 652 Counting by weighing 100–102 Detergent 563 digestion products 664 Covalent bond A link between atoms cleaning with 562–563 Dispersion forces. See London forces that results from their sharing two pH and 347 Disproof, in scientific method 9 electrons. 96 Deuterium 92–93 Disruption of equilibrium 610–616 common bonding patterns 195 in heavy water 59 catalysts and 614–615 formation of 176 DEZ treatment 355 concentrations and 610–613 polar or nonpolar 524 Diamond 89 Le Chatelier’s Principle 614–616 Covalent bonding patterns 195–196 atoms in 90, 103 Distance, between particles of gases 460 Creatine 663 London forces in 534–535 Distillation, of salt water 81 Critical temperature 490 Diatomic Composed of paired atoms. Disulfide bond A covalent bond Cronenberg, David 7 The diatomic elements are 2H , N2, between two atoms on cysteine Crude oil 532–533 O2, F2, Cl2, Br2, and I2. 97 amino acids in a protein structure. Crystals Solid particles whose compo- Dichlorine monoxide, production and 658 nent atoms, ions, or molecules are use 411 Division, rounding off for 4 0 arranged in an organized, repeating Dichloromethane, in decaffeinating cof- DNA (deoxyribonucleic acid) pattern. 314 fee 491 aging and 376 Cubic centimeter 15 Dietary calorie, Cal Equivalent to 4.184 hydrogen bonding in 530 Cubic meter 12 kJ 127 Dolomite rock, hard water and 320 ion, determing Lewis structure Dietary Supplement and Health Act of Dopamine, Parkinson’s disease and 8 203–204 1994 663 Double-displacement reaction A Cycle, in electromagnetic radiation 130 Diethyl ether, structure of 641 chemical reaction that has the form: Cyclopropane 689 Diethyl zinc (DEZ), in book preserva- AB + CD to AD + CB 312 Cysteine (Cys, C) tion 355 acid-base 352 disulfide bonds between 65 8 Difference in electronegativity, in precipitation 312–315 structure of 655 predicting bond type and polarity Double-exchange reaction. See Double- 524–525 displacement reaction D Digestion The process of converting Double-replacement reaction. See Dou- d block, on periodic table 146–147 large molecules into small molecules ble-displacement reaction Dacron, as polyester 669 that can move into the blood stream Double bond A link between atoms Dalton’s Law of Partial Pressures The to be carried throughout the body. that results from the sharing of four total pressure of a mixture of gases is 664–666 electrons. It can be viewed as two 2- equal to the sum of the partial pres- Digestive enzymes 664–666 electron covalent bonds. 192 sures of each gas. 485–489, 523–527, Digital readouts 23 Drug design 649 597–601 Dihydrogen phosphate, as amphoteric Dry cell battery, chemistry of 390–391 G-8 Glossary/Index

Dry ice 552 elemental symbol surrounded by dots naturally occurring isotopes 93 Dynamic equilibrium A system that representing its valence electrons. 189 85 has two equal and opposing rates of Electron capture In radioactive nu- nuclear stability of 694–695 change, from state A to state B and clides that have too few neutrons, the in ordinary substances 171 from state B to state A. There are combination of an electron with a origin of 718 constant changes between state A proton to form a neutron, which stays oxidation numbers of 377–382 and state B but no net change in the in the nucleus. 697 particle interactions 534 amount of components in either state. nuclear equations for 699–701 periodic table of 84–88 See Equilibrium Electron cloud 90, 136 as pure substances 173 Electron configuration A description solids, liquids, and gases 87 E of the complete distribution of an structure of 88–99 element’s electrons in atomic orbitals. symbols for 83 E.I. Du Pont de Nemours and Company 142, 144–145 table of percent abundances in 667 abbreviated 151–154 Earth’s crust, waters, and atmo- Earth, elemental composition of 719 Study Sheet 149, 198 sphere 719 Electric cars, zinc-air batteries in 393 Electronegativity A measure of the Element 111, creation of 94 Electric current, base unit of 11 electron attracting ability of an atom Element 114, creation of 94 Electric field, in electromagnetic radia- in a chemical bond. 524–527 Emerald 294 tion 130 Study Sheet 526 Empirical formula A chemical formula Electric power plant, using nuclear fis- Electron group geometry A descrip- that includes positive integers that de- sion 714–717 tion of the arrangement of all the scribe the simplest ratio of the atoms Electrode A electrical conductor placed electron groups around a central atom of each element in a compound. 271 in the half-cells of a voltaic cell. 389 in a molecule or polyatomic ion, calculating 271–275 Electrolysis The process by which a including the lone pairs. 212 converting to molecular formula redox reaction is pushed in the non- Electron sharing, in chemical bonds 176 275–278 spontaneous direction or the process Electron spin 142, 144 Shudy Sheet 273 of applying an external voltage to a Electron transfer, in chemical bond Enamel 354 voltaic cell, causing electrons to move formation 177–178 Endergonic changes Changes that from what would normally be the Electron volt (eV) An energy unit absorb energy 123 cell’s cathode toward its anode. 391 equivalent to 1.6 × 10-19 joules. It is energy diagram 590–591 Electrolyte The portion of a voltaic cell often used to describe the energy as- Endothermic change A change that that allows ions to flow. 39 0 sociated with nuclear changes. 713 leads a system to absorb heat energy Electron A negatively charged particle Electroplating 391 from the surroundings. 323 found outside the nucleus of an atom. Electrostatic force (or electromagnetic Energy The capacity to do work. 90, 132–136 force) The force between electrically activation 588–590 in atoms 90–92 charged particles. 694 chemical bonds and 123–124 in batteries 388 Element A substance that cannot be chemical changes and 321–323 as beta decay 696–697 chemically converted into simpler endergonic (or endogonic) changes in chemical bonds 176, 187–193 substances; a substance in which all 123 constructing Lewis structures and of the atoms have the same number of events 128 198 of protons and therefore the same exergonic (or exogonic) changes electronegativity and 524 chemical characteristics. 80–99 124 in ions 90–92 atomic mass of 104 exothermic 322 in isotopes 92–93 compound versus 172–173 in food 128 like guitar strings 132–134 diatomic 97 heat 128–129 in metallic elements 98 electron configurations and orbital nuclear 713–718 in multi-electron atoms 142 diagrams 149, 198 of photons 130–132 octets of 189 electronegativities of 524 potential 122–123 in oxidation-reduction reactions isotopes of 92–93 radiant 130–132 372–375 list of common 83 storage in the body 650 particle interpretation of the wave magic numbers for 713 units of 127 character 136 making new elements 94 water formation and 127 as standing wave 134 metallic 98–99 Energy diagram 590–591 valence 188 metalloids or semimetals 86 Energy level. See Principal energy level waveform of 134 metals 85 Engineering, chemical 585 Electron-dot symbol A representa- molar masses of 104–105 English-metric unit conversion factors tion of an atom that consists of its names of 82, 83–84 38, 415 Glossary/Index G-9

English system, metric system versus 14, Equilibrium vapor pressure The par- 385 37 tial pressure of vapor above a liquid in Exothermic change A change that leads Environment, chemistry and 4 a closed system with a dynamic equi- to heat energy being released from the Environmentally Benign Chemistry. librium between the rate of evapora- system to the surroundings. 322 See Green Chemistry tion and the rate of condensation. Expansion, of solids 77 Environmental Protection Agency 5, 515–516 Experimentation, in scientific method 704 in bubble formation 519–520 8–9 Enzyme A naturally occurring catalyst. temperature and 516 External kinetic energy 128 594, 664–666 Ester A compound with two hydrocar- digestive 664–666 bon groups surrounding an F metallic cations in 185 atom. 642–643 f block, of elements 147 why specific 66 6 in fingerprints 51 7 Fahrenheit scale 18–19 Epictetus 34 olestra as 660–661 Fahrenheit to Celsius conversion Epinephrine 558 Estradiol, structure of 662 58–59 Equation. See Chemical equation, Ethanamide 644 Family All the elements in a given col- Nuclear equation; Ideal gas equation Ethane 191 umn on the periodic table; also called Equation stoichiometry Calculations solubility in hexane 557 group. 85 that make use of the quantitative 1,2-Ethanediol 639 Fat 659 relationships between the substances Ethanoic acid 640 digestion products 664 in a chemical reaction to convert Ethanol (or ethyl alcohol) the amount of one substance in the in combustion reactions 383 Fertilizer chemical reaction to the amount of density of 47 ammonia and 597 a different substance in the reaction hydrogen bonds in 530–531 nitric acid and 472 417–421 as intoxicating liquid 214 Feynman, Richard 136 ideal gases and 478–485 Lewis structure 196 15-minute rule 6, 7 molarity and 434–438 mixing with water 552–553 Fingerprints 517 Study Sheet 437 production of 604 Fire extinguishers, sodium carbonate in Equilibrium 597–598 solubility in water 569 343 disruption of 610–616 Ethene. See Ethylene Fireworks dynamic 514–516 Ether A compound with two hydrocar- calcium nitrate in 243 effect of catalyst 61 4–615 bon groups surrounding an oxygen light emitted from 139 effect on changing concentrations atom. 641 Fission Nuclear reaction that yields en- 610–613 Ethyl alcohol. See Ethanol ergy by splitting larger atoms to form gas solutions and 570–571 Ethyl butanoate 643 more stable, smaller atoms. 714–715 heterogeneous 606–607 Ethylene (or ethene) 192 Flame retardant, in 238 homogeneous 600 polyethylene formation and 669 Flashtubes 499 Le Chatelier’s Principle and 614– Ethylene glycol 639 Flerov Laboratory of Nuclear Reactions 616 in polyester formation 668 94 reversible reactions and 597–609 Ethylene oxide, use and production 503 Fluorapatite, tooth decay and 354 saturated solution and 568–569 Ethyne. See Acetylene Fluoride ion, tooth decay and 354 ski shop analogy for 601 Evaporation The conversion of a liquid Fluorine (F) Equilibrium constant A value that de- to a gas. 79, 511–512 covalent bond formation 188–189 scribes the extent to which reversible cooling and 512 diatomic molecules of 97 reactions proceed toward products be- rate of. See Rate of evaporation electron configuration and orbital fore reaching equilibrium. 602–605 Exact numbers, significant figures and diagram 145 calculating values for 603–604 41 how made 297 extent of reaction and 605 Examples, in this book 6 hydrogen bonds and 529 with heterogeneous equilibria Excited state The condition of an atom oxidation numbers and 378 606–608 that has at least one of its electrons in production of 442–443 table of 604 orbitals that do not represent the low- structure of 97 temperature and 608–609 est possible potential energy. 138 valence electrons of 188 writing expressions for 602–603 Exercises, in this book 6 Fluorine-18 Equilibrium constant expression An Exergonic changes Changes that positron emission tomography and expression showing the ratio of the release energy. 124 708 concentrations of products to the con- energy diagram 590 Food centrations of reactants for a reversible Exhaust 173 Calories in 128 reaction at equilibrium. 602 Exhaust systems, catalytic converters and digestion of 664–666 G-10 Glossary/Index

food, important substances in 650–661 easily change shape and volume. 76, temperature 465 Food and Drug Administration (FDA) 79–80. relationships between properties 491 Avogadro’s Law 467 460–467 Food irradiation 711 in book preservation 355 solubility of 570–571 Force, weight as 16 breathing and 469 typical particle velocities 460 Forensic chemistry 517 calculations universal gas constant 470 628, 641 equation stoichiometry 478 vapor as 510 determing Lewis structure 202–203 Study Sheet 483–484 volume occupied by particles 460 in herbicide formation 597 using the combined gas law Gaseous elements 87 production and use 401, 629 equation 476–478 Gasoline 385, 637 Formic acid, molecular structure of 640 Study Sheet 476 in catalytic converters 385 Formula mass The weighted average of using the ideal gas equation combustion of 383 the masses of the naturally occurring 470–475 composition of 191 formula units of the substance. It is Study Sheet 471 in internal combustion engines 468 the sum of the atomic masses of the using the molar volume at STP Gas pressure. See also Gas atoms in a formula unit. 265–266 479 boiling-point temperature and exter- calculations 266 Charles’ Law 465 nal 518–520 Formula unit A group represented by concentration effect on reaction breathing and 469 a substance’s chemical formula, that rates 593 in bubble formation 518–520 is, a group containing the kinds and Dalton’s Law of Partial Pressures in combined gas law equation numbers of atoms or ions listed in the 485–489, 523–527 476–478 chemical formula. 264 Study Sheet 488 Dalton’s Law of partial pressures Fortrel (registered trademark) 669 densities of 48 485–489 Fractional charge, in chemical bonds equilibrium constants and 602–603 equilibrium vapor 515–517 176 expansion 551 in gas stoichiometry 478–485 France, zinc-air batteries in 393 Gay-Lussac’s Law 464 in ideal gas equation 470 Free radicals Particles with unpaired greenhouse gases 430–431 internal combustion engine and electrons. 706 heterogeneous equilibria and 468 Fructose 650–651 606–608 number of gas particles and 466 Functional group A small section of an ideal 461 standard 479 organic molecule that to a large extent ideal gas calculations 470–478 temperature and 464 determines the chemical and physical instrument-carrying balloons and volume and 462–463 characteristics of the molecule. 638 469 Gas stoichiometry 478–485 Furnace method 414 internal combustion engine and Gastric juice 482 Fusion Nuclear reaction that yields 468 pH and 347 Gay-Lussac’s Law energy by combining smaller atoms to liquids changing from and into The pressure of a make larger, more stable ones. 714, 510–512 gas is inversely proportional to the model 460 volume it occupies if the number of 718 molar volume 479 gas particles and the temperature are G noble 85 constant. 464 partial pressure of 485–489, 571 Geometric sketch 210 Galactose 650–651 particle collisions 460 Geometry 209–213. See Molecular Galapagos Islands, global warming ex- pressure 461 shape periments at 431 pressure and industrial safety Study Sheet 215 Galileo Galilei 9 477–478 German Cancer Research Center 94 Gallium-67, radioactive decay of 700 properties of 461 Gesellschaft fur Schwerionenforschung Galvanizing nails 306 race cars and air density 475 (GSI) 94 Gamma aminobutanoic acid, gamma real 460 Gide, Andre 75 aminobutyric acid, or GABA 645 relationship between number of gas Giga (G) prefix 1 3 intoxicating liquids and 214 particles and pressure 466 Girard, Georges 11 Gamma ray A stream of high-energy relationship between number of gas Glacial acetic acid 250 photons. 131, 698 particles and volume 467 Glioma 717 antimatter and 155 relationship between pressure and Global warming 430–431, 573, 597, harmful effects of 70 6–707 temperature 464 649, 663, 717 penetration of the body 707 relationship between volume and Glucose 650–651 in radioactive decay 698 pressure 462–463 empirical and molecular formulas Gas The state in which a substance can relationship between volume and of 271 Glossary/Index G-11

Glutamic acid, structure of 655 in chemical equations 302 solubility of 555 Glutamine, structure of 655 in endothermic reactions 323–324, Hydrochloric acid 248–249, 597 Glycerol or glycerin 639 590–591 as binary acid 250 Glycine, structure of 654 as energy 129 dissolving basic 352 Glycogen 652–653 transfer 129–130 dissolving in water 248 Gold (Au) Heat of reaction 322 dissolving limestone 354 atom of 89 Heavy-ion therapy 94 in formation of magnesium chloride as malleable 85 Heavy water, freezing point of 59 411 origin of name 83 Heidelberg Radiology Clinic 94 forming name of 256 scanning tunneling microscope im- Helium in gastric juices 482 age of 88 to avoid the bends 572 in processing corn syrup 235 Gold-198, radioactive decay of 700 formation 718 production and use 71, 176, 249, Graduated cylinder 21 Helium-4, in treating brain cancer 717. 400, 501 Gravitational attraction, weight and 16 See also Alpha particles reaction with calcium carbonate Green Chemistry 5 Hematite 294 300 decaffeinating coffee and49 1 Hemoglobin 385 as strong acid 251, 253, 254, 340 Designing Safer Chemicals Award 5 carbon monoxide poisoning and Hydrofluoric acid development of new and better 385 forming name of 254 catalysts 597, 649, 663, 717 iron ions in 185 light bulbs and 401 Green Chemistry Challenge Awards Heptane, octane rating and 637 used to make CFCs 400 5 Heterogeneous catalyst A catalyst that Hydrogen (H) Green Chemistry Program 5 is in the same phase as the reactants in acid-base reactions 348–360 Making Chemicals from Safer Reac- (so that all substances are gases or all acids and 248–253 tants 276 are in solution). 596 atomic orbitals 134–141 Sea-Nine antifoulant and 5 Heterogeneous equilibrium An from Big Bang 718 spray paint and 490 equilibrium in which the reactants in Brønsted-Lowry acids and bases Greenhouse gases 430, 573 and products are not all in the same 356–358 Greenspan, Alan 90 phase (gas, liquid, solid, or aqueous). combustion 300, 321, 383 Ground state The condition of an atom 606–607 covalent bond formation 190 whose electrons are in the orbitals that Hexane, solubility in 554–557 electronegativity of 524 give it the lowest possible potential 1-Hexanol 636 formation from water 383 energy. 138 3-Hexanol, molecular structure of 636 formation of hydrogen molecules Group All the elements in a given col- High-density polyethylene (HDPE) 669 190 umn on the periodic table; also called Histidine, structure of 655 in formation of water 300–301 Homogeneous catalyst family. 85 A catalyst that ion formation 182 Guitar strings, like electrons 132–134 is in the same phase as the reactants isotopes of 92–93 (so that all substances are gases or all nuclear fusion of 718 H are in solution). 596 oxidation number of 378 Homogeneous equilibrium An equi- position on preiodic table 87 Half-life The time it takes for one-half librium system in which all of the production and use 408, 597–600 of a sample to disappear. 702–704 components are in the same phase structure 96 Half-reaction Separate oxidation or (gas, liquid, solid, or aqueous). 600 in synthesis gas 598 reduction reaction equation in which Hormone 661 Hydrogenation A process by which electrons are shown as a reactant or Huber, Claudia 617 hydrogen is added to an unsaturated product. 374 Hydrazine, production and use 456 triglyceride to convert double bonds Halogen Hydride ion 236 to single bonds. This can be done by covalent bond formation 194 Hydriodic acid combining the unsaturated triglycer- ion formation 182 forming name of 256 ide with hydrogen gas and a platinum London forces in 532–533 production and use 453, 630 catalyst. 659 in periodic table 85 Hydrobromic acid, forming name of Hydrogen atom, electron wavesforms in Hard water, soaps and detergents in 563 256 134–141 Hearst, William Randolph 255 Hydrocarbon Compounds that contain The intermolecular Heat The energy that is transferred only carbon and hydrogen. 191, 533 attraction between a , oxygen, from a region of higher temperature catalytic converters and 385 or fluorine atom of one molecule to a region of lower temperature as in combustion reactions 383 and a hydrogen atom bonded to a a consequence of the collisions of in internal combustion engines 468 nitrogen, oxygen, or fluorine atom in particles. 129 London forces among 532–533 another molecule. 529–531 G-12 Glossary/Index

in ethanol/water solutions 552 Hydroxyapatite, in tooth enamel 354 London forces and 532 predicting existence of 535 3-Hydroxybutanal 645 name of 83 in proteins 658 17-Hydroxyprogesterone, molecular production and use 399 Hydrogen bromide, threshold limit structure of 662 structure of 97 value, or TLV 498 ion tincture of 532 Hydrogen carbonate ion in bleach 356 Iodine-125 as amphoteric 359 sunlight and swimming pools 405 electron capture by 712 as weak base 343 Hypothesis, in scientific method 8 –9 radioactive decay of 697 Hydrogen chloride 176 iodine-131 706–707 chemical bonds in 176 I Iodine pentafluoride, production and use dipole-dipole attractions 523 407, 451 Ideal Gas A gas for which the ideal gas dissolved in water 248 Ion Any charged particle, whether posi- model is a good description. 461 solubility in water 569 tively or negatively charged. 90–92 calculations involving 470–478 Hydrogen cyanide 597 anion 91. See also Anion equation stoichiometry and molecular geometry of 213 cation 91. See also Cation 478–483 Hydrogen fluoride charges on monatomic 184 Ideal gas constant (R) 470 hydrogen bonds and 529 formation of 177 Ideal Gas Equation 470–475 Hydrogen halides, as polar molecules monatomic anion charges 182 combined gas law equation and 476 529 monatomic anion names 236 equation stoichiometry and Hydrogen peroxide monatomic cation. See Cation, aging and 376 480–485 monatomic Ideal gas model composition of 175 The model for gases polyatomic. See Polyatomic ion dark bottles and 407 that assumes (1) the particles are predicting charges 182–185 empirical and molecular formulas point-masses (they have mass but no size of 185 of 271 volume) and (2) there are no attrac- spectator 315–316 as oxidizing agent 376 tive or repulsive forces between the symbols for 91 Hydrogen sulfate ion 356 particles. 461 Ionic bond The attraction between a as cleaning agent 356 Incandescent light bulbs 472 cation and an anion. 177–179 as weak acid 254, 340 Induced dipole 532 in ionic compounds 180 Hydrogen sulfide Industrial chemistry 4, 5 predicting existence of 524–527 threshold limit value, or TLV 498 Infrared (IR) radiation 131 Ionic compound A compound that Hydrolysis A chemical reaction in Inner transition metals The 28 ele- consists of ions held together by ionic which larger molecules are broken ments at the bottom of the periodic bonds. 180, 236–250 down into smaller molecules by a table. 86 as bases 343 reaction with water in which a water Insoluble substances 316–317, 554–557 binary 239, 242, 372–374 molecule is split in two, each part Instantaneous dipole 532 formula mass of 265–266 joining a different product molecule. Intermolecular attraction Attraction formulas to names 239–241 665 between molecules. 529–533 names to formulas 242–243 + Hydronium ion H3O 248–249, dipole-dipole attraction 523 polyatomic ions is 185–187 340–341 hydrogen bonds 529–531 reactions of acids with 349 in acid-base reactions 348–353 London forces 532–533 recognizing from formulas 239 acids and 248–254 Internal combustion engine 468 solutility of 317 pH and 346–348 effects of weather on 47 4 solution of 309–311 Hydrophilic (“water loving”) A polar gases and 468 as strong and weak bases 343 molecule or ion (or a portion of a International System of Measurement structure of 185–187 molecule or polyatomic ion) that is 10–19 types of 239 attracted to water. 558 abbreviations 13 uses of 181, 186 Hydrophobic (“water fearing”) A metric prefixes 1 2–13 Ionizing radiation Alpha particles, beta nonpolar molecule (or a portion of a units derived from base units 12 particles, and gamma photons, which molecule or polyatomic ion) that is Intestines 665 are all able to strip electrons from not expected to mix with water. 558 Intoxicating liquids 214 atoms as they move through matter, Hydrothermal vent 617–618 ion, solubility of compounds with leaving ions in their wake. 706 Hydroxide ion 317 Iridium (Ir), in catalytic converter 385 covalent bond formation 193 Iodine (I) Iridium-192, checking pipe joints and solubility of compounds with 317 beta emission and 696 711 Hydroxides Compounds that contain diatomic molecules of 97 Iron (Fe) hydroxide ions. 341 electron capture and 697 electron configuration and orbital Glossary/Index G-13

diagram for 150 Kilojoule (kJ) 128 elemental symbol for each atom in formation of 719 Kilometer (km) 13 the molecule, lines to show covalent formation of pig 382, 485 Kilopascal (kPa) 461 bonds, and pairs of dots to indicate global warming and 430–431 Kinetic energy, KE The capacity to do lone pairs. 190–194, 195–205 as limiting reactant in global warm- work resulting from the motion of an general steps for drawing 200, 460 ing 430 object. 121 and 207–209 Iron(II) sulfate, in global warming ex- chemical reactions and 321–322 simple procedure 196–198 periments 431 in formation of water 321 Study Sheet 198–199 Iron(III) sulfate, formula mass calcula- internal and external 129 Libraries, of drugs 649 tions for 266, 268 mass and 121 Life Iron-59 712 of reactant molecules 587–588 hydrogen bonds and 530 Island of stability, of nuclides 695 solution of ammonium nitrate and origin of 616–617 Isobutene, use 638 322 Light bulbs Isoleucine (Ile, I), molecular structure velocity and 121 argon gas in 488 of 654 Kinetic molecular theory. See Particle filament evaporation in 47 2, 475 Compounds that have the nature of matter flash tubes 49 9 same molecular formula but different Knockout drops 206 fluorescent 49 7 molecular structures. 206 , light bulbs and 475 “Like dissolves like” guideline, for solu- Lewis structures of 206–207 Krypton-81 693, 710 bility 554–557 of organic compounds 634 Lime 409 Isooctane 637 L Limestone 354, 592 Isopropyl alcohol. See 2-propanol acid rain and 255 Lactase, in digestion 664 Isotopes Atoms that have the same increasing permeability of 249 Lactic acid, in cosmetic lotion 368 number of protons but different num- Limestone caverns 368 Lactose, or milk sugar 652 bers of neutrons. They have the same Limiting reactant The reactant that Laskowski, Edweard R. 663 atomic number but different mass runs out first and limits the amount Latent fingerprints 51 7 numbers. 92–94 of product that can form. 422–427 Law of Conservation of Energy atomic numbers of 93 global warming and 430–431 Energy can be neither created nor de- of carbon 102 how chosen 422–423 stroyed, but it can be transferred from mass numbers of 93 Study Sheet 426 one system to another and changed in nuclear reactions 698 Linear geometry The geometric ar- symbol for 692–693 from one form to another. 122 rangement that keeps two electron Isovaleraldehyde 641–642 Lawrence Laboratory 701 groups as far apart as possible. It leads L-dopa 8 to angles of 180° between the groups. J Lead(II) ion, solubility of compounds 213 with 317 Linear molecules 213, 215 Jeans, James Hopwood 90 Lead (Pb) Line drawing 558, 635 Jesus of Nazareth 710 in creating elements 110 94 Ling Po 7 Jewelry, elements in 83 density of 47 Liquid The state in which a substance Joule, J The accepted SI unit for energy. gasoline and 408 has a constant volume at a constant 127 lead-206, in radioactive decay series 705 temperature but can change its shape. K Lead-acid batteries, chemistry of 393 76, 78 Lebowitz, Fran 33 boiling 518–520 Kaposi’s sarcoma 649 Le Chatelier’s principle If a system at dissolving gases in 570 Kelvin, a temperature unit 19 equilibrium is altered in a way that dissolving solids in 564–569 Kelvin scale 11, 18–19 disrupts the equilibrium, the system dynamic equilibrium between va- gas temperature and 461 will shift so as to counter the change. pors and 571 temperature conversions for 58–60 614–616 heterogeneous equilibria and Kerosene, London forces and 532 Leclanché cell 390–391 606–607 Ketone A compound that have a hy- Length 14–15 Liquid-liquid solutions 311 drogen atom or a hydrocarbon group range of 15 Liquid elements 87 connected to a -CHO group. 642 Leucine (Leu, L), structure of 654 Liter 12 Kettering, Charles F. 132 Levi, Primo 3 Lithium (Li) Khirbat Qumrân 710 Levocarbidopa, in Parkinson’s disease 8 from Big Bang 718 Kilo (k) prefix 1 3 Levodopa, in Parkinson’s disease 8 electron configuration and orbital Kilocalorie (kcal, Cal) 127 Lewis structure A representation diagram 144 Kilogram (kg) 11 of a molecule that consists of the formation of 718 G-14 Glossary/Index

Lithium-7, in treating brain cancer 717 Marble, acid rain and 255 Metallic bond The attraction between Lithium batteries 393 Margarine 659 the positive metal cations that form Lithium hydroxide, uses 341 Martin, John 430–431 the fundamental structure of a solid Litmus, detecting acids and bases with Mass The amount of matter in an metal and the negative charge from 348 object. Mass can also be defined as the mobile sea of electrons that sur- London forces The attractions pro- the property of matter that leads to round the cations. 534 duced between molecules by instanta- gravitational attractions between Metallic elements 86 neous and induced dipoles. 532–533 objects and therefore gives rise to attractive forces in 534–535 molecular size and 532 weight. 16–17 ion charges of 182–184 Lone pair Two electrons that are base unit of 11 Metalloids or semimetals The ele- not involved in the covalent bonds density and 47–49 ments that have some but not all of between atoms but are important for of elements and compounds the characteristics of metals. 86 explaining the arrangement of atoms 267–271 bonding patterns of 199 in molecules. They are represented by English-metric unit conversions of in periodic table 86 pairs of dots in Lewis structures. 189 55 Metals The elements that (1) have a Low-density polyethylene (LDPE) 669 kinetic energy and 121 metallic luster, (2) conduct heat and Lucretius 345 measuring 16–17 electric currents well, and (3) are mal- Luminous intensity, base unit for 11 percentage by 52–53 leable. 85, 98–99 Luminous tubes 477 range of 17 electrolysis to purify 391 Lungs, gases in 469 weight and 16–17 forming cations 181 Lye. See Sodium hydroxide weighted average 100 sea of electrons model 99 Lye soap 562 Mass density Mass divided by volume Meter 10, 11 Lysine (Lys, K) (usually called density). 47–51 Methamphetamine, molecular structure molecular structure of 655 as conversion factor 49–51 of 558–559 in salt bridges 658 Mass number The sum of the number Methamphetamine hydrochloride of protons and neutrons in an atom’s 558–559 M nucleus. 93 Methane 187, 191 binding energy versus 714 combustion of 120 “Mickey Finn” sedative 206 in nuclear equations 699 covalent bond formation 191 Magic numbers and nuclear stability 94, in nuclides 692 in hydrogen gas production 713 Mass percentage 52 597–600 Magnesium (Mg), meals ready to eat Matches, chemicals in 305 molecular shape 210–211 (MREs) and 549 Matter Anything that has mass and solubility in water 569 Magnesium chloride, production and takes up space. 16 Methanethiol, in natural gas 383 use 411 chemistry and 4 Methanoic acid 640 Magnesium oxide 241 classification of 17 2–175 Methanol 187 Magnetic field, in electromagnetic radia- existence of 155 density of 50 tion 130 origin of 718 hydrogen bonds and 531 Magnetic resonance imaging (MRI) 708 as solid, liquid, or gas 76–80 as polar molecule 529 Main-group element The elements in Mayo Clinic 663 production and use 408, 503, 603 groups 1, 2, and 13 through 18 (the Meals ready to eat (MRE) 549 water solubility of 556 “A” groups) on the periodic table; also Measurement 9, 9–23 Methionine (Met, M), structure of 655 called representative elements. 86 digital readouts 23 Methyl alcohol 196. See also Methanol Malleable Capable of being extended International System of 10–11 Methyl bromide or shaped by the blows of a hammer. reporting values from 20 determing Lewis structure 200–201 85 trailing zeros and 22 ozone layer and 3 Maltase, in digestion 664 uncertainty in 20–23, 39 threshold limit value, or TLV, and Maltose, molecular structure of 652 Medicine, uses of radioactive substances 498 Manganese (Mn) in 707–708 3-Methylbutanal 641–642 in dry cell batteries 390–391 Mega (M) prefix 1 3 Methyl cyanoacrylate, molecular struc- how made 292 Meitner, Lise 82 ture of 216 Manganese(II) oxide, naming 240 Meniscus, in measurement 21 Methylene chloride, in decaffeinating Manganese(II) phosphate Menstrual cycles, hormones in 662 coffee 49 1 production and use 406 Menthol 560 Methyl ethyl ketone or MEK, molecular uses 368 Metal-nonmetal compounds structure of 642 Manganese dioxide, in dry cell batteries bonds in 525 2-Methylpropene 638 390–391 formulas and names of 239 Metric-metric unit conversions 35–37 Glossary/Index G-15

Metric prefixes 1 2–13 composed of molecules. In such charges 182 table of 13 compounds, all of the bonds between naming 236 Metric system 10. See also International atoms are covalent bonds. 180 Monatomic cation Positively charged System of Measurement attractive forces in 535 particles, such as Na+, Ca2+, and MeV (million electron volts) 713 in oxidation-reduction reactions Al3+, that contain single atoms with micro (mu) prefix 1 3 375 a positive charge. 183. See also Cat- Microwaves 131 water solubility of 555 ion, monatomic Mifepristone 681 Molecular dipole A molecule with an formation 182–183 Milk, pH of 347 asymmetrical distribution of positive naming 236 milli (m) prefrix 13 and negative charge. 523 roles in body 185 Millimeter of (mmHg), as unit Molecular equation. See Complete equa- Monatomic ion, charges 184 of pressure 461 tion Monoethanolamine 613 Miscible Can be mixed in any propor- Molecular formula The chemical Monomer The repeating unit in a poly- tion without any limit to solubility. formula that describes the actual mer. 652 552 numbers of atoms of each element in in addition polymers 669 Mixture A sample of matter that con- a molecule of a compound. 271 in polysaccharides 652–653 tains two or more pure substances and from empirical formula 275–278 in proteins 654 has variable composition. 173 empirical formulas versus 271 Monoprotic acid An acid that donates of gases 485 Study Sheet 277 one hydrogen ion per molecule in a Model A simplified approximation of Molecular geometry The description reaction. 250, 340 reality. See also Scientific model of the arrangement of all the atoms Monosaccharide Sugar molecule with calculating 433 around a central atom in a molecule one saccharide unit. 650 collision theory as 586–592 or polyatomic ion. This description Monosodium glutamate (MSG), taste of gases 79 does not consider lone pairs. 209– and 345 ideal gas 461 216. See also Geometry Monsanto Company 597 of liquids 78 Molecular mass The weighted aver- Moss Landing Marine Laboratories 430 of metallic elements 98 age of the masses of the naturally Mount Everest, atmospheric pressure at of solids 76–77 occurring molecules of a molecular the top 521 strengths and weaknesses of 187 substance. It is the sum of the atomic MTBE 641 valence-bond 188–193 masses of the atoms in a molecule. Multiplication Moderator A substance in a nuclear 262–263 rounding off for 4 0–45 reactor that slows neutrons as they calculating 263 significant figures for4 0–45 pass through it. 716 in calculating molecular formulas Mylar, as polyester 669 Molarity (abbreviated M) Moles of 275–276 solute per liter of solution. 433–438 Molecular models 96 N equation stoichiometry and Molecular polarity, predicting 528 434–438 Molecular Shape 209–211 Names Molar mass The mass in grams of one ball-and-stick model 210 for acids 256–258 mole of substance. 104–107 geometric sketch 210 for binary covalent compounds 235 from atomic mass 104 space-filling model 21 0 for chemical compounds 259–260 calculations using atomic mass 105 Molecular size, London forces and for elements 82–83 calculations using ionic formula 532–533 for ionic compounds 236–244 mass 266 Molecule An uncharged collection of for organic compounds 637 calculations using molecular mass atoms held together with covalent Nano (n) prefix 1 3 263 bonds. 96 Natrium 83 in equation stoichiometry 416–420 diatomic 97 Natural gas 187 in ideal gas equation 471 as formula unit 264 Nature, elements found in 82 from ionic formula mass 265 of hydrogen 96 Neon (Ne) from molecular mass 262–263 in molar mass 262 electron configuration and orbital Molar volume at STP 479 shapes of 209–216 diagram 145 Mole (mol) The amount of substance Momentum, of particles in evaporation luminous tubes and 477 that contains the same number of 511 in neon lights 477, 489 particles as there are atoms in 12 g of Monatomic anions Negatively charged Nerve cells carbon-12. 11, 102–103 particles, such as Cl-, O2-, and N3-, intoxicating liquids and 214 in equation stoichiometry 478–485 that contain single atoms with a nega- taste and 345 in ideal gas equation 479 tive charge. 182. See also Anion, Net ionic equation A chemical equa- Molecular compound A compound monatomic tion for which the spectator ions have G-16 Glossary/Index

been eliminated, leaving only the oxidation-reduction and 375 Nuclear power plant 716–717 substances actively involved in the Nitrogen narcosis 572 Nuclear reaction A process that results reaction. 316 Nitrogen in a change in an atomic nucleus (as Net rate of solution 565–567 in automobile exhaust 127 opposed to a chemical reaction, which Neutralization reaction A chemical Nitroglycerine, in decomposition reac- involves the loss, gain, or sharing of reaction between an acid and a base. tions 383 electrons). 698–702 See Acid-base reaction Nitrosyl chloride, production and use Nuclear reactors 714–717 Neutron An uncharged particle found 631 Nuclear stability 694–695, 713–714 in the nucleus of an atom. 89 Nitrosyl fluoride, molecular geometry Nucleon number The sum of the num- in nuclear fission 71 4–715 216 bers of protons and neutrons (nucle- as nuclear glue 694 Nitrous oxide, formation of 304 ons) in the nucleus of an atom. It is nuclear stability and 694–695 Noble gases, structure 95 also called the mass number. 692 Newton (N), a unit of force 16 Node The locations in a waveform Nucleons The particles that reside in NiCd batteries. See Nickel-Cadmium where the intensity of the wave is the nucleus of atoms (protons and batteries always zero. 133 neutrons). 692 Nickel (Ni), in the creation of elements Nomenclature. See Chemical nomen- Nucleus The extremely small, positively 110 and 111 94 clature charged core of the atom. 89 Nickel-60, gamma ray emission by 698 Nonmetals The elements that do not of atom 89 Nickel-cadmium battery, chemistry of have the characteristics of metals. creation of new elements and 94 392 Some of the nonmetals are gases at electrons around 134–140 Nicotine 293 room temperature and pressure, some of helium atoms 95 Nippoldt, Todd B. 663 are solids, and one is a liquid. Various mass number and 93 Nitrate ion colors and textures occur among the stability of 694 resonance and 207–209 nonmetals. 85 Nuclide A particular type of nucleus solubility of compounds with 317 forming anions 181 that is characterized by a specific Nitric acid Nonpolar covalent bond A covalent atomic number (Z) and nucleon acid rain and 255 bond in which the difference in elec- number (A). 692 formation of 616 tron-attracting ability of two atoms in band of stability of 695 forming name of 257 a bond is negligible (or zero), so the in nuclear equations 698–702 production and use 405 atoms in the bond have no significant radioactive 703 reaction with sodium hydroxide charges. 176 symbol 692–693 349–351, 349–353 predicting existence of 524–527 uses for radioactive (table) 712 solution of 349 Nonpolar molecular substance, solubility Numbers, exact or not 41 as strong acid 253 and 554–555 Nutrients, for phytoplankton 430 Normal boiling-point temperature Nitride ion, forming name of 236 Nylon 667 Nitril hydratase 597 The temperature at which the equi- molecular structure of 667 Nitrogen (N) librium vapor pressure of the liquid production of 275, 667–668 covalent bond formation 192 equals one atmosphere. 521 Nylon-66 275–276 diatomic molecules of 97 Notation, for nuclides 692–693 electron configuration and orbital Nuclear chemistry The study of the O diagram 145 properties and behavior of atomic ion formation 182 nuclei. 691 “Oil rig” mnemonic 373 liquid 127 Nuclear decay series A series of radio- Objectives 6 London forces and 534 active decays that lead from a large Observation, in scientific method 8 –9 structure of 97 unstable nuclide, such as - Octane rating 637 Nitrogen-13, radioactive decay of 700 238, to a stable nuclide, such as lead- Octet of electrons 189–190, 199–200 Nitrogen-14, in radiocarbon dating 702 206. 705 Oil 354, 532–533 Nitrogen dioxide Nuclear energy 713–718 Oil industry 354 acid rain and 255 Nuclear equation The shorthand nota- Olestra 660–661, 718–719 nitric acid and 616 tion that describes nuclear reactions. Oligopeptide 656 threshold limit value, or TLV and It shows changes in the participating Open-chain forms, of monosaccharides 498 nuclides’ atomic numbers (the num- 650–651 Nitrogen molecules, velocities of 460 ber of protons) and mass numbers Orange juice, pH of 347 Nitrogen monoxide 596 (the sum of the numbers of protons Orbital diagram A drawing that uses in acid rain 255 and neutrons). 698–702 lines or squares to show the distribu- catalytic breakdown of 596 Nuclear fission 71 4–715 tion of electrons in orbitals and ar- how made 472 Nuclear fusion 718 rows to show the relative spin of each Glossary/Index G-17

electron. 142, 144–145 defined 37 4 effect on gas solubility 57 1 Study Sheet 149, 198 oxidation numbers and 377–382 equilibrium vapor pressure as Orbitals See Atomic orbitals Oxoacid. See Oxyacid 515–516 Organic acid Carbon-based acids. 250 Oxyacid (oxoacid) Molecular sub- Particle-particle attractions 523, 597 Organic chemistry The branch of stances that have the general formula summary 534–535 chemistry that involves the study HaXbOc. In other words, they contain Particle nature of matter 76–80 of carbon-based compounds. 191, hydrogen, oxygen, and one other ele- gas 76, 79–80 634–648 ment represented by X; the a, b, and c liquid 76, 78 Organic compound 634–648 represent subscripts. 250 solids 76–77 alcohol 639 names for 257 Particles aldehyde 641 as polar molecule 529 in atoms 89 alkane 637 Oxygen (O) attractive forces among 523–536 alkene 638 in combustion reactions 383–385 in collision theory 586 alkyne 638 covalent bond formation 193–194 in condensation 510 amide 644 diatomic molecules of 97 in evaporation 511–512 amine 643–644 electron configuration and orbital in gases 79 arene 638–639 diagram 145 in liquids 78 carboxylic acid 640 electronegativity of 524 radiant energy as 130–131 condensed formula 635 in formation of water 300–301 in solids 76–77 ester 642–643 in internal combustion engines 468 space occupied 79 ether 641 ion formation 182–183 Pascal (Pa), pressure unit 461 how to describe 634–636 oxidation numbers for 378 Pearl ash, empirical formula for 274 ketone 642 structure 97 Pentane line drawing 558, 635 Ozone hexane solubility of 554 table of types 646–647 chlorine catalyzed destruction in solution 311 Organophosphorus compounds 293 594–596 water solubility of 554 Oxalic acid 640 as greenhouse gas 430 Pepper, spiciness of 559 uses 235 process of destruction 586–590 Pepsin, in digestion 664 Oxidation Any chemical change in Peptide A substance that contains two which at least one element loses elec- P or more amino acids linked together trons, either completely or partially. by peptide bonds. 656 372–373, 375 p block, of elements 146–148 how form 616–618 Oxidation-reduction reaction The Paint spraying, preventing air pollution Peptide bond An amide functional chemical reactions in which there 490 is a complete or partial transfer of Palladium, in catalytic converter 385 group that forms when the carboxylic electrons, resulting in oxidation and Pancreatic amylase, in digestion 664 acid group on one amino acid reacts reduction. These reactions are also Pancreatic lipase, in digestion 664 with the amine group of another called redox reactions. 372–375 Paper, saving acidic 355 amino acid. 656 within batteries 388–393 Parkinson’s disease 7–8 Percentage 52–53 half-reaction 374 positron emission tomography and as conversion factor 52 oxidation 372 155 by mass, definition 5 2 oxidation numbers (or states) scientific method and 7 –8 by volume 52 377–382 Partial charge Percentage calculations 52–53, 57 reduction 373 in chemical bonds 176, 524–527 in calculating empirical formulas uses of 371 in hydrogen bonds 529 274 Oxidation number (or state) A tool in London forces 532–533 in calculating molecular formulas for keeping track of the flow of elec- Partial electron transfer in oxidation-re- 278 trons in redox reactions. 377–382 duction reactions 375 Percent yield The actual yield divided assignment of oxidation numbers Partially hydrogenated triglycerides by the theoretical yield times 100. 378 659–660 428–430 Study Sheet 378 Partial pressure The portion of the to- why less than 100% 428–429 . See Oxidation number tal pressure that one gas in a mixture Periodic table of the elements 84–88 Oxidizing agent A substance that gains of gases contributes. Assuming ideal electronegativity and 524 electrons, making it possible for an- gas character, the partial pressure of group number 85 other substance to lose electrons and any gas in a mixture is the pressure group or family 85 be oxidized. 374 that the gas would yield if it were hydrogen, position on periodic table aging and 376 alone in the container. 485 87 G-18 Glossary/Index

metals, nonmetals, and metalloids Pico (p) prefix 1 3 Polyprotic acid An acid that can do- 86 Pig iron, formation of 485 nate more than one hydrogen ion per modern model of the atom and Plastic fingerprints 51 7 molecule in a reaction. 250 146–154 Platinum (Pt) 98 Polysaccharide Molecule with many periods 87 as catalyst 616 saccharide units. 652 representative (or main-group) in catalytic converters 385, 596 digestion products 664 elements, transition metals, and density of 48 Polystyrene 670–671 inner transition metals 86 Plutonium (Pu), in creation of new ele- Positron A high-velocity anti-electron Periods The horizontal rows on the ments 94 released from radioactive nuclides that periodic table. 87 Plutonium-239 have too few neutrons. 155, 697 Peroxides, oxidation numbers of 378 half-life 703 discovery of 155 Petroleum 532–533 in radioactive wastes 704 Positron emission In radioactive nu- pH 346–347 radioactive decay 703 clides that have too few neutrons, the acid rain and 346 Polar covalent bond A covalent bond conversion of a proton to a neutron, Pharmaceuticals 649 in which electrons are shared unequal- which stays in the nucleus, and a Phenylalanine (Phe, F), molecular struc- ly, leading to a partial negative charge positron, which is ejected from the ture of 655 on the atom that attracts the electrons nucleus. 697 Phosgene gas, production and use 631 more and to a partial positive charge nuclear equations for 699–701 Phosphate, production 377 on the other atom. 176 Positron emission tomography (PET) Phosphate ion, solubility of compounds dipole-dipole attractions and 155, 708 with 317 523–524 Potassium-40 Phosphate rock, in furnace method 261 predicting in molecules 524–528 radioactive decay of 697 Phosphide ion 236 Polarity uses for 697 Phosphoric acid 356 of amphetamine and epinephrine Potassium carbonate, empirical formula forming name of 257 558 determination 274 furnace method of preparation 261 of bonds 524–525 Potassium , production and use neutralizing 436 of capsaicin 559 444 production of 414 molecular 528 Potassium hydroxide, production and use reaction with sodium hydroxide predicting in molecules 528–529 341, 409 352 solubility and 554 Potassium nitrate in toilet bowl cleaners 356 Polar molecular substance, solubility and production and use 401 uses 235, 250 554–555 in voltaic cells 390 Phosphorus (P) Polonium-210, radioactive decay of 700 Potassium perchlorate, production and covalent bond formation 193 Polonium-218, in radioactive decay 705 use 445 in furnace method 414 Poly(ethylene terephthalate) 671 Potassium , production ion formation 182 Poly(vinyl chloride), PVC 670–671 and use 447 London forces in 534 Polyatomic ion A charged collection Potato chips 660 in oxidation-reduction reactions of atoms held together by covalent Potential energy (PE) A retrievable, 379 bonds. 185–187 stored form of energy an object pos- in photophor 272 balancing equations and 303, 306 sesses by virtue of its position or state. production of 377, 454 formulas and names 238 122 Phosphorus pentachloride, production with hydrogen 238 chemical reactions and 321–323 and use 410 nonsystematic names 238 electron orbitals and 138 Phosphorus tribromide 429 Polychlorinated biphenyl (PCB) 278 in formation of water 321 Phosphorus trichloride, production and Polyester 668–669 stability and 122–124 use 606 Polyethylene 669 Precipitate A solid that comes out of Photons Tiny, massless packets or par- Polymer A large molecule composed of solution. 312 ticles of radiant energy. 130 repeating units. 652 Precipitation The process of forming a Photophor, empirical formula for 272 addition 669–670 solid in a solution. 312 Physical states, in chemical equations formulas for 667 tooth decay and 354 301 polysaccharides as 652–653 Precipitation reaction A reaction in Physics proteins as 656 which one of the products is insoluble chemistry and 76 synthetic 666–671 in water and comes out of solution as of electrons 132–141 Polypeptide 656. See also Protein a solid. 312–318 origin of matter and 616–617 nylon as 667 of calcium carbonate 312–315 Phytoplankton, global warming and silk as 666 Study Sheet 318 430–431 Polypropylene 670–671 writing equations for 318–319 Glossary/Index G-19

Precision The closeness in value of a hydrogen bond 658 clide whose numbers of protons and series of measurements of the same primary structure 656 neutrons place it outside the band of entity. The closer the values of the ribbon convention 657 stability. 695 measurements, the more precise they salt bridge 658 Radioactive substances are. 20 secondary structure 656 smoke detectors, pipe joint check, in reporting measured values 39 tertiary structure 657–658 food irradiation, radioactive trac- Prefixes.See Metric prefixes Proton A positively charged particle ers 711 Preserving books 355 found in the nucleus of an atom. 89 uses 707–712 Presidential Green Chemistry Challenge in artificial elements 9 4 Radioactive tracer A radioactive Award 597 in atoms 89–90 nuclide that is incorporated into Pressure Force per unit area. See Gas in Bronsted-Lowry acids and bases substances that can then be tracked pressure; See Gas, pressure 356 through detection of the nuclide’s Pressure cooker 520 in ions 90–91 emissions. 711 Primary battery A battery that is not in isotopes 92–93 Radiocarbon (or carbon-14) dating rechargeable. 392 mass number and 93 The process of determining the age of Primary protein structure The se- MRI and 708 an artifact that contains material from quence of amino acids in a protein nuclear stability and 694–695, 713 formerly living plants or animals by molecule. 656 in nuclides 692–693 analyzing the ratio of carbon-14 to Principal energy level A collection of origin of the elements and 718 carbon-12 in the object. 709–710 orbitals that have the same potential Publication, in scientific method 9 Radio waves 131 energy for a hydrogen atom, except Pure substance A sample of matter that Radium-226 for the first (lowest) principal energy has constant composition. There are half-life 703 level, which contains only one orbital two types of pure substances: ele- radioactive decay 705 (1s). 138 ments and compounds. 173 use 712 Probabilities, electron behavior and 132, Putrescine, molecular structure of 643 Radon-222 136 half-life 703 Products The substances that form in Q lung cancer and 704 a chemical reaction. Their formulas in radioactive decay series 705 Quantum mechanics 155 are on the right side of the arrow in a Rags, in paper 355 Quick lime, formation of 409 chemical equation. 301 Rapture of the deep 572 Progesterone, molecular structure of 662 R Rate of chemical reaction The number Proline (Pro, P), molecular structure of of product molecules that form (per- 655 Race cars and air density 475 haps described as moles of product Propane 191 Radiant energy Energy that can be de- formed) per liter of container per 1,2,3-Propanetriol 639 scribed in terms of oscillating electric second. 592–596 2-Propanol and magnetic fields or in terms of concentration effect 59 3–594 hydrogen bonds in 530 photons. 130–132 temperature and 592–593 Lewis structure 196 spectrum 131 Rate of condensation The number of molecular structure of 530 the wave view 130 particles moving from gas to liquid 2-Propanone 642 wavelength 130 per second. 513 Propionic acid Radiation Rate of evaporation The number of molecular structure of 556 effects on the body 70 6–707 particles moving from liquid to gas water solubility 556 treatment for cancer 707 per second. 511–513, 512–513 Proportionality Radiator coolants 554 strengths of attractions and 512 direct 463 Radioactive decay One of several surface area and 512 inverse 463 processes that transform a radioactive temperature and 513 Propylene nuclide into a more stable product or three factors that determine 512 hexane solubility of 557 products. 695 Rate of solution. See Solution, Rate of in polypropylene 670 effects on body 70 6–707 Ratio Propylene glycol, molecular structure of rates and half-life 702–704 empirical formulas and 271 554 Radioactive decay series 704–705 molar 270 Protein Natural polypeptide. 654–655, Radioactive emissions neutron-to-protons 694–695 656 alpha particle 696 stoichiometric 422 alpha helix 656 beta emission 696 Rational drug design 649 beta sheet 656 gamma rays 698 Reactants The substances that change digestion products 664 positron emission 697 in a chemical reaction. Their formulas disulfide bond 65 8 Radioactive nuclide An unstable nu- are on the left side of the arrow in a G-20 Glossary/Index

chemical equation. 301 Roasting 430 rechargeable battery. 392 equilibrium disruption and 610– Rohm and Haas Company 5 Secondary protein structure The ar- 612 Roman numeral, in naming monatomic rangement of atoms that are close to limiting 423–427 cations 236 each other in a polypeptide chain. Reaction. See Chemical reaction Roots of nonmetal names 236 Examples of secondary structures are Reaction Rate. See Rate of chemical Roscoelite 297 alpha helix and beta sheet. 656–657 reaction Rounding off 3 9–47 Second period elements, electrons in Rechargeable batteries 392 for addition and subtraction 45–47 143–145 Recycling 670 for multiplication and division Selenide ion 236 Red giant stars 719 40–45 Selenium Red litmus paper, detecting bases with Roundup 597 covalent bond formation 194 348 RU-486 681 ion formation 182–183 Redox reaction. See Oxidation-reduction Ruby 290 Semimetals The elements that have reaction some but not all of the characteristics Reducing agent A substance that loses S of metals. 86 electrons, making it possible for an- Serine (Ser, S) s block, on peridoic table 146–147 other substance to gain electrons and hydrogen bonds between 658 Saccharide Sugar, starch, and cellulose. be reduced. 374 molecular structure of 655 Also called carbohydrates. 650–653. Reduction Any chemical change in Shape. See Molecular shape See also Carbohydrate which at least one element gains elec- Shell 138. See also Principal energy trons, either completely or partially. Saliva, tooth decay and 354 level See 373, 375 Salt. Sodium chloride Shroud of Turin 710 Salt bridge Relative atomic mass 102 (in proteins) A covalent Side-chain, in anion acid 654 Relative solubilities 554 bond between two sulfur atoms on Significant figures The number of Representative elements The elements cysteine amino acids in a protein meaningful digits in a value. The in groups 1, 2, and 13 through 18 structure. 658 number of significant figures in a (the “A” groups) on the periodic table; Salt bridge (in voltaic cells) A device value reflects the value’s degree of un- also called main-group elements. 86 used to keep the charges in a voltaic certainty. A larger number of signifi- Research, in scientific method 8 cell balanced. 390 cant figures indicates a smaller degree Research chemist 585 Salt taste 345 of uncertainty. 39–47 Resonance The hypothetical switch- Salt water separation 82 counting the number of 41–42 ing from one resonance structure to San Simeon, California, protection from zeros and 42 another. 207–209 acid rain in 255 Silicon (Si) 300 Resonance hybrid A structure that Saturated solution A solution that has electronics grade 425 represents the average of the reso- enough solute dissolved to reach the metallurgical grade 425 nance structures for a molecule or solubility limit. 568, 568–569 purifying 425–426 polyatomic ion. 208 dynamic equilibrium and 564–569 from silicon dioxide 423 Resonance structures Two or more formation of 568–569 Silicon dioxide Lewis structures for a single molecule Saturated triglyceride A triglyceride citrine as 294 or polyatomic ion that differ in the with single bonds between all of the in furnace method 261 positions of lone pairs and multiple carbon atoms. 659 purifying silicon from 425–426 bonds but not in the positions of the Scale, calcium carbonate in 320 Silk atoms in the structure. 208 Schrodinger, Erwin 134 molecular structure of 666 Reversible reaction A reaction in Science nylon as substitute for 666 which the reactants are constantly chemistry as 7–9 Silver (Ag) forming products and, at the same existence of matter and 155 density of 48 time, the products are reforming the Scientific Method 7 –9 ion charges of 237 reactants. 251, 597–598 Scientific model A simplified approxi- melting point of 60 in chemical equilibrium 597–601 mation of reality. 76, 98, 187 Silver ion, solubility of compounds with disruption of equilibrium for 610 Scientific notation 4 –5 317 equilibrium constants for 602 Scuba diving, gas solubility and 572 Silver nitrate, in precipitation reaction percent yield and 428 Sea-Nine antifoulant 5 318 Review Skills sections 6 Seaborg, Glenn 701 Single-displacement reaction Chemi- Rhodium, in catalytic converter 385 Sea of electrons model for metals 99 cal change in which atoms of one Ribbon convention for proteins 657 Seawater, pH and 347 element displace (or replace) atoms Ring forms, of monosaccharides Second (s), as unit of measurement 11 of another element in a compound. 650–651 Secondary (or storage) battery A 386–387 Glossary/Index G-21

Sinkhole 368 Sodium , production and use senting a molecule to show a some- SI System of Measurement. See Interna- 407 what realistic image of the electron- tional System of Measurement Sodium sulfate, production and use 407, charge clouds that surround the Sixth principal energy level, electron 493 molecule’s atoms. 96, 210 orbitals of 141 Sodium tripolyphosphate, production Spandex (R), synthesis of 278 Slaked lime 409 and use 456 Special conditions, in chemical equations Smelling salts 629 Soft drink, why bubbles form 572 301–302 Smog “Solar system” model of the atom 132 Special topics nitrogen dioxide in 605 Solid The state in which a substance Acid Rain 255 Smoke detectors 711 has a definite shape and volume at a A Greener Way to Spray Paint 490 Soap 560, 562–563 constant temperature. 76–77 Air Pollution and Catalytic Convert- Society for Heavy-Ion Research 94 densities of 47–48 ers 385 Sodium (Na) expansion when heated 77 A New Treatment for Brain Cancer electrolysis and 391 heterogeneous equilibrium and 717 formation from sodium chloride 606–607 Be Careful with Bleach 356 383 Solid acid, in meals ready to eat 549 Big Problems Require Bold Solu- ion 177–178 Solid elements 87, 98–99 tions - Global Warming and ion formation 182 Solubility The maximum amount of Limiting Reactants 430 Sodium aluminum sulfate, in baking solute that can be dissolved in a given Chemistry and Your Sense of Taste powder 175 amount of solvent. 554–560 345 Sodium bromide, use 576 gas 570–571 Chemistry Gets the Bad Guys 517 Sodium carbonate guidelines 554 Gas Solubility, Scuba Diving, and reaction with acid 343 like dissolves like 554–555 Soft Drinks 572 uses 343 soaps and detergents and 562–563 Global Warming, Oceans, and CO2 Sodium chlorate, production and use in water 316–317, 569 Torpedoes 573 408 guidelines 316 Green Chemistry 5 Sodium chloride Solute The gas in a solution of a gas in Green Chemistry - Making Chemi- electrolysis and 391 a liquid. The solid in a solution of a cals from Safer Reactants 276 formation 178 solid in a liquid. The minor compo- Green Chemistry - The Develop- formula mass of 265 nent in other solutions. 311 ment of New and Better Cata- formula unit of 264 gas as 570–571 lysts 597 oxidation-reduction and 372–373 in saturated solution 564 Green Decaf Coffee 49 1 solubility in water 569 Solution A mixture whose particles are Hard Water and Your Hot Water solution in water 309–311 so evenly distributed that the relative Pipes 320 structure of 185, 185–186 concentrations of the components are Harmless Dietary Supplements or taste of 345 the same throughout. Solutions can Dangerous Drugs 663 Sodium chromate 430 also be called homogeneous mixtures. Molecular Shapes, Intoxicating Sodium dichromate, production and use chemical reactions in 549 Liquids, and the Brain 214 446, 454 dynamic equilibrium and 564–569 Olestra and Low-Fat Potato Chips sodium dodecyl sulfate (SDS), as deter- formation of 552–553 660–661 gent 563 of ionic compounds 309–311 Oxidizing Agents and Aging 376 Sodium fluoride, in toothpaste 18 1 molarity and 431–438 Precipitation, Acid-Base Reactions, Sodium hydrogen carbonate rate of 565–568 and Tooth Decay 354 production and use 343, 405 agitation 567 Recycling Synthetic Polymers 670 reaction with acids 343 factors that effect 56 5 Rehabilitation of Old Drugs and Sodium hydrogen sulfate, production surface area 565–566 Development of New Ones 649 and use 453 temperature effect 56 8 Safe and Effective? 27 9 Sodium hydroxide saturated 568–569 Saving Valuable Books 355 aqueous solution of 341 solute and solvent 311 The Big Question - How Did We formation 185 unsaturated 568 Get Here? 616 in neutralizing phosphoric acid 436 why form 550–553 The Origin of the Elements 71 8 reaction with nitric acid 349–353 Solvent The liquid in a solution of a gas Wanted: A New Kilogram 11 uses of 185, 341 in a liquid. The liquid in a solution of Why Create New Elements? 94 Sodium hypochlorite, production 485, a solid in a liquid. The major compo- Why Does Matter Exist, and Why 528, 536, 556, 557 nent in other solutions. 311 Should We Care About This Sodium ions 91 Sour taste 345 Question? 155 taste and 345 Space-filling model A way of repre- Zinc-Air Batteries 393 G-22 Glossary/Index

Spectator ions Ions that play a role in at least one hydroxide ion in solution tions and orbital diagrams for delivering other ions into solution to for every unit of substance added to uncharged atoms 149 react but that do not actively partici- water. 341 writing equations for combustion pate in the reaction themselves. 315 identifying 344 reactions 384 Spectrum, of radiant energy 131–132 reactions of strong acids with Styrene, in polystyrene 670 Spin. See Electron spin 349–353 Sublevel or subshell A given type (or Spinels 291 Strong force The force that draws shape) of orbital available at a given Spodumene 297 nucleons (protons and neutrons) principal energy level. 139 Spray paint 490 together. 694 Sublimation, of dry ice 125, 126 Stability A relative term that describes Strontium-90 706 Subshell, of atomic orbitals 139 the resistance to change. 96, 122– Studying chemistry 5 Substance, base unit of 10–11 124 Study Sheets Substances Standard kilogram 11 abbreviated electron configuration densities of common 48 Standard pressure 479 151–154 equation stoichiometry and Standard temperature 479 assignment of oxidation numbers 414–421 Standard temperature and pressure (STP) 378 hydrophilic and hydrophobic 558 479 balancing chemical equations 303 solubilities of 554–555 gas stoichiometry and 479 basic equation stoichiometry - con- uses for radioactive 707–710 gas stoichiometry for conditions verting mass of one substance Substrate A molecule that an enzyme other than 480–481 in a reaction to mass of another causes to react. 666 Standing waves 132–134 418–419 Subtraction, rounding off and 4 5–47 Starch 650, 652 calculating empirical formulas 273 Sucrase, in digestion 664 Stars, element formation and 719 calculating molecular formulas 277 Sucrose, solubility in water 569 State, physical 301 calculations using unit analysis 54 Sugar 650–652 Stationary wave 133 classification of matter 17 4 rate of solution 566 Steam re-forming 442, 598 combustion reaction 384 taste of 345 Stearic acid converting between mass of element Sulfate ion, solubility of compounds molecular structure of 640 and mass of compound contain- with 317 solubility of 559 ing the element 270 Sulfur 85–86 Step-growth (or condensation) poly- drawing Lewis structures from for- combustion and 383 mer A polymer formed in a reaction mulas 198–199 covalent bond formation 194 that releases small molecules, such as electron configurations and orbital ion formation 182–183 water. This category includes nylon diagrams 149, 198 production 408 and polyester. 667 electronegativity, types of chemical use and production 501 Sterno 187 bonds, and bond polarity 526 Sulfur dioxide Steroid Compounds containing a four- equation stoichiometry 418–419, acid rain and 255 ring structure. 661–662 437, 483–484 air pollution and 499 Stirring, rate of solution and 565–567 equation stoichiometry problems in combustion reactions 383 Stockings 666 437 as pollutant and removal 454 Stoichiometric ratio 422 identification of strong and weak Sulfur hexafluoride, threshold limit Stoichiometry. See Equation acids and bases 344 value, or TLV 498 stoichiometry limiting reactant problems 426 254 Stomach predicting molecular geometry 215 acid rain and 255 hydrochloric acid in 482 predicting precipitation reactions in acrylamide synthesis 597 role in digestion 665 and writing precipitation equa- forming name of 257 Stomach acid 482 tions 318 as oxyacid 250 Storage battery 392 rounding off numbers calculated us- production 402 Strong acid An acid that donates its H+ ing addition and subtraction 45 reaction with sodium hydroxide ions to water in a reaction that goes rounding off numbers calculated 352 completely to products. Such a com- using multiplication and division as strong acid 254, 340 + pound produces close to one H3O 41 uses 254 ion in solution for each acid molecule using Dalton’s Law of Partial Pres- Sulfur trioxide, in acid rain 255 dissolved in water. 251, 253, 340 sures 488 Sun, nuclear fusion and 718 identifying 344 using the combined gas law equa- Supercritical carbon dioxide reactions of strong base with tion 476 decaffeinating coffee and49 1 349–353 using the ideal gas equation 471 spray paint and 490 Strong base A substance that generates writing complete electron configura- Supercritical fluid 49 0 G-23 Glossary/Index

Super glue 216 Tetrahedral The molecular shape that planar) The geometric arrangement Supernovas 719 keeps the negative charge of four that keeps three electron groups as far Surface area, rate of solution and electron groups as far apart as pos- apart as possible. It leads to angles of 565–566 sible. This shape has angles of 109.5° 120° between the groups. 213 Sweet taste 345 between the atoms. 210 Trigonal pyramid The molecular ge- Symbols Tetrahedral molecules 210 ometry formed around an atom with for elements 83 Tetramethylene glycol 279 three bonds and one lone pair. 212 for nuclides 692 Tetrapeptide 656 Trimethylamine 644 Synthesis gas 598 Tetraphosphorus decoxide, in furnace 2,2,4-Trimethylpentane 637 Synthesis reactions 382 method 261 Trinitrotoluene (TNT) 638–639 Synthetic polymers 666–671 Tetraphosphorus trisulfide 30 5 Triple bond A link between atoms that Thalidomide 29 6, 649 results from the sharing of 6 electrons. T Theoretical yield The calculated maxi- It can be viewed as three 2 electron mum amount of product that can covalent bonds. 192 Tanzanite 294 form in a chemical reaction. 428 Triprotic acid An acid that can donate Taste 345 Thermometers 1 8–19 three hydrogen ions per molecule in a Technical University of Munich 617 44 4 reaction. 250, 340 Television waves 131 Thionyl chloride, production and use Tristearin 560 Tellurium (Te), bonding patterns of 199 454 Tritium 92–93 Temperature A measure of the average Thoburn, Steve 3 8 Trypsin 664 internal kinetic energy of an object. Thortveitite 29 6 Tryptophan (Trp, W), molecular struc- 17–19, 129 Threonine (Thr, T), molecular structure ture of 655 absolute zero 18 of 655 Tungsten (W), in light bulb filaments base unit of 11 Threshold limit value, or TLV 49 8 472 boiling-point 520 Time, base unit of 11 Tyrosine (Tyr, Y), molecular structure Celsius scale 18 Tin(II) sulfide, melting point of 6 0 of 655 coldest 19 Tincture of iodine 532 common scales 19 Tin isotopes 93–94 U in condensation 510 Titanium(IV) oxide Ultraviolet radiation 131 critical 490 production 504 Umami taste 345 density and 47 production and use 457 Uncertainty 21 effect on rate of solution 56 8 Titanium (Ti) 98 in measurements 20–22 equilibrium constants and 608–609 production and use 411 significant figures and3 9–47 equilibrium vapor pressure and Titanium carbide 427 Unified mass unit.See Atomic mass unit 516–517 Titanium dioxide 608 Unit A defined quantity based on a in evaporation 512–513 production and use 402 standard. 9–18, 1–3 Fahrenheit scale 18–19 Titration, Web site for 438 abbreviations 1 gases and 461 Tooth decay, acid-base reactions and 354 conversions among 34–60 Kelvin scale 18–19 Tooth enamel, composition of 354 of energy 127 measuring 18 Toothpaste, chemicals in 226 in international system of measure- normal boiling-point 521 Torr, as unit of pressure 461 ment 10–12 pressure and 464 Trailing zeros, measurement uncertainty length 14 range of 19 and 22 mass 16 rate of reaction and 592–594 Transition metals The elements in the importance of putting into equa- rate of solution and 568 groups 3 through 12 (the “B” groups) tions 473 standard 479 on the periodic table. 86 volume 15 volume and 465 as catalysts 596 Unit analysis A general technique for Temperature conversions 58–60 in catalytic converters 385 doing unit conversions. 34–38, 132– Terephthalic acid, in plyester formation in periodic table 86 136, 142–146, 267–275, 414–418, 668 Transition state, in chemical reactions 422–426 Tertiary protein structure The overall 587 equation stoichiometry and 416 arrangement of atoms in a protein Triacylglycerol 560–561 gas stoichiometry and 481 molecule. 657 Triglyceride A compound with three Study Sheet 54–55 Testosterone 662 hydrocarbon groups attached to a summary of 54–58 Tetraboron carbide, production and use three carbon backbone by ester func- Unit conversions 34–38, 132–136, 446, 447 tional groups. 560–561, 659–661 142–146, 267–271, 271–275, Tetrachloroethene 421 Trigonal planar (often called triangular 414–418, 422–426 G-24 Glossary/Index

“something per something” 57 or calculation. 10 W common 54–58 Vanadium(V) oxide, in catalytic con- density and 49, 56, 477, 479–482, verter 385 Wächtershäuser, Günter 617 527 Vapor A gas derived from a substance Water 172 English-metric 37–38, 56 that is liquid at normal temperatures acids and 248–249, 251–252, metric-metric 35–37, 56 and pressures. It is also often used to 340–341 percentage and 53, 57 describe gas that has recently come ammonia and 341–342 Universal gas constant, R The constant from a liquid. 510 attractions 308 in the ideal gas equation. 470 Vaporization The conversion of a bases and 341 in gas stoichiometry 481–485 liquid to a gas. 79 boiling point of 18–19, 521 in ideal gas equation 470–475 Vapor pressure. See Equilibrium vapor as compound 173 Universe pressure condensation of 510–511 hottest temperatures in 19 Vegetable oil 561 in condensation reactions 665 origin of elements in 718–719 Velocity covalent bond formation 193 University of California, Berkeley 701 of gas particles 460 density of 48 dissolving sodium chloride in University of Regensberg 617 kinetic energy and 121 310–311 Unpaired electrons 190 of particles in evaporation 511 evaporation of 511 in valence-bond model 188 Vinegar hard 320 Unsaturated solution A solution that acetic acid in 250 heavy 59 has less solute dissolved than is pre- taste of 345 hydrogen bonds in 530 dicted by the solubility limit. 568 Vinyl chloride, in poly(vinyl chloride) ionizing radiation and 706–707 Unsaturated triglyceride A triglyceride 670 liquid 308–309 that has one or more carbon-carbon Visible fingerprints 51 7 melting point of 18–19 double bonds. 659 Visible light 131 mixing with ethanol 552–553 Uranium 427 Vitamin C, aging and 376 molecular shape 307–308 alpha emission 696 Vitamin E, aging and 376 in nylon formation 667 production 448 Volatile organic compounds (VOCs) pH of 347 uranium-238 decay series 705 490 as polar molecule 308, 529 Uranium(IV) oxide 427 Voltage 391 producing hydrogen gas from Uranium-234 716 Voltaic cell A system in which two 597–599 Uranium-235 716 half‑reactions for a redox reaction in protein formation 656 enrichment 427 are separated, allowing the electrons rate of solution in 565–569 in fission reactors 71 6 transferred in the reaction to be solubility in 554–559 half-life 703 passed between them through a wire. Water dissociation constant (K ) The Uranium-238 388–393 w equilibrium constant for the reaction: in fission reactors 71 6 anode 389 H O(l ) H+(aq) + OH-(aq) 608 half-life 703 cathode 389 2 common examples 393 Water purification 42 0 nuclide symbol 693 electrode 389 Water solubility 316–317 radioactive decay series 705 electrolyte 390 Water treatment 366 Uranium-239 primary battery 392 Wave in nuclear reactors 716 salt bridge 390 electrons as 134–141 in nuclear fission 71 4 secondary battery 392 for guitar strings 132 Uranium hexafluoride 41 3, 427 zinc-air batteries 393 radiant energy as 130–132 Urea 457 Volume (V) 15–16 standing 132–133 use and production 502, 630 density and 47 Waveform A representation of the V English-metric conversion factors shape of a wave. for 38 of electron 134 Valence-bond model 188–193 of gases 461 of guitar strings 133 Valence electrons The electrons that are of ideal gas particles 461 Wavelength The distance in space over most important in the formation of measurement, graduated cylinder which a wave completes one cycle of chemical bonds. The highest energys 21 its repeated form. 130–131 and p electrons for an atom. 188 number of gas particles and 467 Weak acid A substance that is incom- Valine (Val, V), molecular structure of pressure and 462–463 pletely ionized in water due to the 654 range of 16 reversibility of the reaction that forms + Value A number and unit that together temperature and 465 hydronium ions, H3O , in water. represent the result of a measurement Volume unit, liter 12 Weak acids yield significantly less G-25 Glossary/Index

+ than one H3O ion in solution for attractions 536 each acid molecule dissolved in water. for resonance 209 251, 252, 340 for temperature effect on solid and Weak base A substance that produces fewer hydroxide ions in water solution gas solubility 569, 573 than particles of the substance added. for writing complete ionic and net 342–343 ionic equations 319 ammonia as 341–342 Weight A measure of the force of gravi- identifying 344 tational attraction between an object Weather balloon 478 Web site and a significantly large object, such for acid-base titration 438 as the earth or the moon. 16 for acid nomenclature 257 Weighted average A mass calculated for animation of acid-base reaction by multiplying the decimal fraction 353 of each component in a sample by its for animation of a single-displace- ment reaction 386 mass and adding the results of each for animation of dissolving ethanol multiplication together. 100 in water 553 Wine for animation of element structure pH of 347 98 sediment formation 555 for animation of precipitation reac- tion 316 Work What is done to move an object for animation of solution of sodium against some sort of resistance. 120 chloride 310 for animation of strong and weak X acids 254 for animation of the particle nature X-ray crystallography 649 of matter 80 X-rays 131 for animation of water structure Xenon (Xe), reactions 406 309 Xenon difluoride 44 3 for balancing redox equations 382, 386 Y for calculating element percentages 271 Yield. See Actual yield, Theoretical yield, for changing volume and gas reac- and Percent yield tions 613 for combustion analysis 278 Z for conversion between element names and formulas 83 Zeros and significant figures4 2 for different electron configurations Zinc (Zn) 98 154 batteries and 388–391 for enzyme mechanism 666 for equilibrium calculations, includ- reaction with copper sulfate ing pH 609 386–387 for isotope notation 94 single-displacement reaction and for gas stoichiometry shortcut 482 386–387 for how addition polymers are made voltaic cells and 388–390 669 for London forces and polar mol- Zinc-air batteries 393 ecules 534 Zinc oxide for mixtures and equation in book preservation 355 stoichiometry 421 oxidation-reduction and 372–373 for polyatomic ions 238 for predicting molecular polarity in zinc-air batteries 393 529 Zinc phosphate 306 for predicting relative strengths of G-26 Glossary/Index