Foundational Chemistry Vocabulary Zumdahl Chemistry Wheaton Academy (Regular and Honor’s Chemistry)

Elements and their symbols (must have memorized in the first week of school) Aluminum Al Li (Stibium) Sb Mg Ar Mn As (Hydrargyrum) Hg Ba Ne Be Ni Bi N B O Br P Cd Pt (Lime) Ca (Kalium) K C Ra Cesium Cs Rn Cl Rb Cr Si Co (Argentum) Ag (Cuprum) Cu (Natrium) Na F Sr (Aurum) Au (Brimstone) S He (Stannum) Sn H Ti I (Wolfram) W (Ferrum) Fe U Kr Xe (Plumbum) Pb Zn

June 2008 Wheaton Academy Rebecca Drury and Kirsten Bell Chapter 1: Chemistry—the science that deals with the materials of the universe and the changes that these materials undergo. Scientific Method—a process of studying natural phenomena that involves making observations, forming laws and theories, and testing theories by experimentation. Measurement—a quantitative observation, involves a number and a unit Theory—a set of tested hypotheses that gives an overall explanation of some part of nature Natural Law—a statement that expresses generally observed behavior

Chapter 2: Matter- the material of the universe Atom – the fundamental unit of which elements are composed Compound- a substance with constant composition that can be broken down into elements by chemical processes Molecule- a bonded collection of two or more atoms of the same element of different elements Element- a substance that cannot be decomposed into simpler substances by chemical or physical means. It consists of atoms all having the same . Graphite- carbon based: material that makes up pencil “lead” Diamond- carbon based: hard gemstone Buckminsterfullerene- carbon based: a third form of elemental carbon Solid- one of the three states of matter; has a fixed shape and volume Liquid- one of the three states of matter; has a fixed volume but takes the shape of its container Gas- one of the three states of matter; has neither fixed shape nor fixed volume Physical Properties- a characteristic of a substance that can change without the substance becoming a different substance. Chemical Properties- the ability of a substance to change to a different substance Physical Change- a change in the form of a substance, but not in its chemical nature; chemical bonds are not broken in a physical change. Chemical Change- the change of substances into other substances through a reorganization of the atoms; a chemical reaction. Reaction- involves a change in the fundamental components of the substance; a given substance changes into a different substance or substances Mixture- a material of variable composition that contains two or more substances. Alloy- a substance that contains a mixture of elements and has metallic properties. Pure Substance- a substance with constant composition Homogeneous Mixture- a mixture that is the same throughout; a solution Solution- a homogeneous mixture Heterogeneous Mixture- a mixture that has different properties in different regions of the mixture. Distillation- a method for separating the components of a liquid mixture that depends on differences in the ease of vaporization of the components. Filtration- a method for separating the components of a mixture containing a solid and a liquid

June 2008 Wheaton Academy Rebecca Drury and Kirsten Bell

Chapter 3: Element Symbols—abbreviations for the chemical elements Law of Constant Composition—a given compound always contains elements in exactly the same proportion by mass Dalton’s Atomic Theory—1. Elements are made of tiny particles called atoms. 2. All atoms of a given element are identical. 3. All atoms of a given element are different from those of any other element. Atom—the fundamental unit of which elements are composed Compound—a substance with constant composition that can be broken down into elements by chemical processes Chemical Formula—a representation of a molecule in which the symbols for the elements are used to indicate the types of atoms present and subscripts are used to show the relative numbers of atoms Electron—a negatively charged particle that occupies the space around the nucleus of an atom Nuclear Atom—the modern concept of the atom as having a dense center of positive charge (the nucleus) and electrons moving around the outside Nucleus—the small, dense center of positive charge in an atom Proton—a positively charged particle in an atomic nucleus Neutron—neutral particle contained in the nucleus of the particle, slightly more massive than a proton but has no charge. —atoms of the same element (the same number of protons) that have different numbers of neutrons. They have identical atomic numbers but different mass numbers. Atomic Number—the number of protons in the nucleus of an atom; each element has a unique atomic number Mass Number—the total number of protons and neutrons in the atomic nucleus of an atom —a chart showing all the elements arranged in columns in such a way that all the elements in a given column exhibit similar chemical properties Groups (of the periodic table)—a vertical column of elements having the same and similar chemical properties. Alkaline —a 1 (first column on left hand side of periodic table) Alkaline Earth Metals—a group 2 metal (2nd column on left hand side of periodic table) —a group 7 element (2nd column from the right on the periodic table) Noble Gases—a group 8 element (last column on right on the periodic table) Transition Metals—several series of elements in which inner orbitals (d or f orbitals) are being filled. Metal—an element that gives up electrons relatively easily and is typically lustrous, malleable, and a good conductor of heat and electricity. —an element that does not exhibit metallic characteristics. Chemically, a typical nonmetal accepts electrons from a metal. (Semi-metals)—elements that have both metallic and non-metallic properties. Diatomic Molecule—a molecule composed of two atoms Ion—an atom or a group of atoms that has a net positive or negative charge. Cation—a positive ion

June 2008 Wheaton Academy Rebecca Drury and Kirsten Bell Anion—a negative ion Ionic Compound—a compound that results when a metal reacts with a nonmetal to form cations and anions.

Chapter 4: Binary Compound- a two-element compound Binary Ionic Compound- contain a positive ion, and negative ion Polyatomic Ion- an ion containing two or more atoms Oxyanion- several series of polyatomic anions exist that contain an atom of a given element and different numbers of oxygen atoms Acid- a substance that produces hydrogen ions in aqueous solution; a proton donor.

Chapter 5: Measurement—a quantitative observation Scientific Notation—expresses a number in the form n x 10^m; a convenient method for representing a very large or very small number and for easily indication the number of significant figures. Units—tells us what scale or standard is being used to represent the results of the measurement. English System—units system used in the United States Metric System—units system used in most of the industrialized world. It is preferred for scientific work. SI Units—International System of units based on the metric system and on units derived from the metric system. Volume—the amount of three-dimensional space occupied by a substance. Liter—1 dm3 Milliliter—1 cm3 Kilogram—fundamental SI unit of mass Gram—the prefixes for various mass units are based on the gram.1/1000 of a kilogram. Mass—the quantity of matter in an object Significant Figures—the certain digits and the first uncertain digit of a measurement Rounding Off—in a series of calculations, carry the extra digits through to the final result and then round off. Conversion Factor—a ratio of the two parts of the statement that relates the two units. Equivalence Statement—equivalents between the English and metric systems Dimensional Analysis—changing from one unit to another via conversion factors (based on the equivalence statements between the units) Fahrenheit Scale—temperature scale widely used in the United States and Great Britain, and it is the scale employed in most of the engineering sciences. Celsius Scale—temperature scale used in Canada and Europe and in the physical and life sciences in most countries Kelvin scale—another temperature scale used in the sciences Density—a property of matter representing the mass per unit volume Specific Gravity—the ratio of the density of a given liquid to the density of water at 4 degrees Celsius.

June 2008 Wheaton Academy Rebecca Drury and Kirsten Bell Chapter 6: Atomic Mass Unit- smaller unit of mass; 1 amu = 1.66 X 10^-24 g Average Atomic Mass- average mass of an element Mole- the number equal to the number of carbon atoms in exactly 12 grams of pure 12C: Avogadro’s number. One mole represents 6.022 X 10^23 units. Avogadro’s number- the number of atoms in exactly 12 grams of pure 12C, equal to 6.002 X 10^23. Molar Mass- the mass in grams of one mole of a compound Mass Percent- the percent by mass of a component of a mixture or of a given element in a compound Empirical Formula- the simplest whole-number ratio of atoms in a compound Molecular Formula- the exact formula of a molecule, giving the types of atoms and the number of each type

Chapter 7: Chemical Reaction—a chemical changed always involves a rearrangement of the ways in which the atoms are grouped. Chemical Equation—a representation of a chemical reaction showing the relative numbers of reactant and product molecules Reactant—a starting substance in a chemical reaction. It appears to the left of the arrow in a chemical equation. Product—a substance resulting from a chemical reaction. It is shown to the right of the arrow in a chemical equation Balancing a Chemical Equation—there must be the same number of each type of atom on the product side as on the reactant side of the arrow. Making sure that the equation for a reaction obeys this rule is called balancing the chemical equation. Coefficient—the accepted convention is that the “best” balanced equation is the one with the smallest integers (whole numbers). These integers are called the coefficients.

Chapter 8: Precipitation- the formation of a solid; one driving force for a chemical reaction Precipitate- the solid that forms Precipitation Reaction- a reaction in which an insoluble substance forms and separates from the solution as a solid. Strong Electrolyte- a material that, when dissolved in water, dissociates (ionizes) completely and gives a solution that conducts an electric current very efficiently Soluble Solid-a solid that readily dissolves in water Insoluble- a solid where such a tiny amount dissolves in water that it is undetectable with the naked eye Molecular Equation- an equation representing a reaction in solution and showing the reactants and products in undissociated form, whether they are strong or weak electrolytes. Complete Ionic Equation- an equation that shows as ions all substances that are strong electrolytes. Spectator Ions- ions present in solution that do not participate directly in a reaction.

June 2008 Wheaton Academy Rebecca Drury and Kirsten Bell Net Ionic Equation- an equation for a reaction in solution, representing strong electrolytes as ions and showing only those components that are directly involved in the chemical change. Acid- a substance that produces hydrogen ions in aqueous solution; s proton donor. Strong Acid- an acid that completely dissociates (ionizes) to produce H+ ion and the conjugate base Base- a substance that produces hydroxide ions in aqueous solution; a proton acceptor Strong Base- a metal hydroxide compound that completely dissociates into its ions in water. Salt- an ionic compound Oxidation Reduction Reaction- a reaction in which one or more electrons are transferred Double Replacement Reaction- double exchange; AB + CD  AD + CB Acid Base Reaction- reaction that involves and H+ ion that ends up in the product water; HCl(aq) + KOH(aq)  H2O(l) + KCl(aq) Single Replacement Reaction- single exchange; A + B  B + AC Combustion Reaction- the vigorous and exothermic oxidation-reduction reaction that takes place between certain substances (particularly organic compounds) and oxygen Synthesis Reaction- when a given compound is formed from simpler materials Decomposition Reaction- when a compound is broken down into simpler compounds or all the way to the component elements.

Chapter 9: Mole Ratio—the ratio of moles of one substance to moles of another substance in a balanced chemical equation Stoichiometry—the process of using a chemical equation to calculate the relative masses of reactants and products involved in a reaction Limiting Reactant—the reactant that is completely consumed when a reaction is run to completion. Theoretical Yield—the maximum amount of a given product that can be formed when the limiting reactant is completely consumed Percent Yield—the actual yield of a product as a percentage of the theoretical yield

Chapter 10: Energy—the capacity to do work or to cause the flow of heat Law of Conservation of Energy—energy can be converted from one form to another but can be neither created nor destroyed. Potential energy—energy due to position of composition Kinetic Energy—(1/2mv^2) energy due to the motion of an object; dependent on the mass of the object and the square of its velocity. Work—force acting over a distance. State Function—a property that is independent of the pathway. Temperature—measure of the random motions (average kinetic energy) of the components of a substance. Heat—energy transferred between two objects because of a temperature difference between them. System—that part of the universe on which attention is to be focused.

June 2008 Wheaton Academy Rebecca Drury and Kirsten Bell Surroundings—everything in the universe surrounding a thermodynamic system. Exothermic—refers to a reaction in which energy (as heat) flows out of the system Endothermic—refers to a reaction in which energy (as heat) flows into a system Thermodynamics—a study of energy and its interactions First Law of Thermodynamics—a law stating that the energy of the universe is constant Internal Energy—the sum of the kinetic and potential energies of all components of an object. Calorie—a unit of measurement for energy Joule—a unit of measurement for energy; 1 calorie =4.184 joules. Specific Heat Capacity—the amount of energy required to raise the temperature of one gram of a substance by one Celsius degree. Enthalpy—at constant pressure, the change in enthalpy equals the energy flow as heat. Calorimeter—measures heat flow Hess’ Law—in going from a particular set of reactants to a set of products, the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps. Fossil Fuel—a fuel that consists of carbon-based molecules derived from decomposition of once-living organisms; coal, petroleum, or natural gas Petroleum—a thick, dark liquid composed mostly of hydro-carbon compounds Natural Gas—consists of mostly methane and is associated with petroleum deposits Coal—formed from the remains of plants that were buried and subjected to high pressure and heat over long periods of time. Greenhouse Effect—a warming effect exerted by certain molecules in the earth’s atmosphere (particularly carbon dioxide and water) Energy Spread—in a given process, concentrated energy is dispersed widely. Matter Spread—the molecules of a substance are spread out and occupy a larger volume

Chapter 11: Electromagnetic radiation—radiant energy that exhibits wave-like behavior and travels through space at the speed of light in a vacuum. Wavelength—the distance between two consecutive peaks or troughs in a wave Frequency—the number of waves (cycles) per second that pass a given point in space Photon—a “particle” of electromagnetic radiation Quantized energy level—only certain values of energy levels are allowed. Wave mechanical model—general picture of this model Orbital—a representation of the space occupied by an electron in an atom; the probability distribution for the electron. Principal energy levels—hydrogen atoms have discrete energy levels. Sublevel—each of these levels is subdivided into sublevels Pauli Exclusion Principle—an atomic orbital can hold a maximum of two electrons, and those two electrons must have opposite spins. Electron configuration—electron arrangement Orbital (box) diagram—orbitals are represented by boxes grouped by sublevel with small arrows indicating the electrons. Valence electrons—the electrons in the outermost occupied principal quantum level of an atom

June 2008 Wheaton Academy Rebecca Drury and Kirsten Bell Core electron—an inner electron in an atom; one that is not in the outermost (valence) principal quantum level series—a group of fourteen elements following on the periodic table, in which the 4f orbitals are being filled. series—a group of fourteen elements following on the periodic table, in which the 5f orbitals are being filled. Main-group (representative) elements—elements in the groups labeled 1,2,3,4,5,6,7, and 8 on the periodic table. The group number gives the sum of the valence s and p electrons. Metals—an element that gives up electrons relatively easily and is typically lustrous, malleable, and a good conductor of heat and electricity. Nonmetal—an element that does not exhibit metallic characteristics. Chemically, a typical nonmetal accepts electrons from a metal. —an element that has both metallic and non-metallic properties. Atomic size— Ionization energy—the quantity of energy required to remove an electron from a gaseous atom or ion.

Chapter 12: Bond- the force that holds two atoms together in a compound Bond energy- the energy required to break a given chemical bond Ionic bonding- the attraction between oppositely charged ions Ionic compound- a compound that results when a metal reacts with a nonmetal to from cations and anions Covalent bonding- a type of bonding in which atoms share electrons Polar covalent bond- a covalent bond in which the electrons are not shared equally because one atom attracts them more strongly than the other. – the tendency of an atom in a molecule to attract shared electrons to itself Dipole moment- a property of a molecule whereby the charge distribution can be represented by a center of positive charge and a center of negative charge. Lewis structure- a diagram of a molecule showing how the valence electrons are arranged among the atoms in the molecule Duet rule- hydrogen atoms only require two electrons in a molecule to form a stable molecule Octet rule- the observation that atoms of form the most stable molecules when they are surrounded by eight electrons (to fill their valence orbitals) Bonding pair- an electron pair found in the space between two atoms. Lone (unshared) pair- an electron pair that is localized on a given atom; an electron pair not involved in bonding Single bond- a bond in which two atoms share one pair of electrons Double bond- a bond in which two atoms share two pairs of electrons Triple bond- a bond in which two atoms share three pairs of electrons Resonance- a condition occurring when more than one valid Lewis structure can be written for a particular molecule. The actual electronic structure is represented not by any one of the Lewis structures but by the average of all of them.

June 2008 Wheaton Academy Rebecca Drury and Kirsten Bell Molecular (geometric) structure- the three-dimensional arrangement of atoms in a molecule. Linear structure- all atoms in a line (180 degrees between atoms) Trigonal planar structure- 120 degrees between each atom Tetrahedral structure- 109.5 degrees between each atom Valence shell electron pair repulsion- a model the main postulate of which is that the structure around a given atom in a molecule is determined principally by the tendency to minimize electron-pair repulsions. Model- a set of assumptions put forth to explain the observed behavior of matter. The models of chemistry usually involve assumptions about the behavior of individual atoms or molecules. Trigonal pyramid- the molecular structure of ammonia

Chapter 13: Barometer—a device for measuring atmospheric pressure. mm Hg—millimeters of mercury Torr—another name for millimeters of mercury Standard atmosphere—a related unit for pressure to torr, abbreviated as atm Pascal—the SI unit of measurement for pressure; equal to one Newton per square meter. Boyle’s law—the volume of a given sample of gas at constant temperature varies inversely with the pressure. Absolute zero—matter cannot be cooled to temperatures lower than -273 degrees Celsius. Therefore, this temperature is defined as absolute zero on the Kelvin scale. Charles’s law—the volume of a given sample of gas at constant pressures is directly proportional to the temperature in Kelvin Avogadro’s law—equal volumes of gases at the same temperature and pressure contain the same number of particles (atoms or molecules). Universal gas constant—the combined proportionality constant in the ideal gas law; 0.08206 L atm/K mol, or 8.314 J/K mol. Ideal gas law—an equation relating the properties of an ideal gas, expressed as PV = nRT, where P=pressure, V=volume, n=moles of the gas, R=the universal gas constant, and T=temperature on the Kelvin scale. This equation expresses behavior closely approached by real gases at high temperature and/or low pressure. Ideal gas—a hypothetical gas that exactly obeys the ideal gas law. A real gas approaches ideal behavior at high temperature and/or low pressure. Combined gas law—use when the amount of gas (moles) is held constant Partial pressures—the independent pressures exerted by different gases in a mixture. Dalton’s law of partial pressures—for a mixture of gases in a container, the total pressure exerted is the sum of the pressures that each gas would exert if it were alone. Kinetic molecular theory—a model that assumes that an ideal gas is composed of tiny particles (molecules) in constant motion. Molar volume—the volume of the gas given by the ideal gas law is called the molar volume of an ideal gas. Standard temperature and pressure (STP)—the conditions 0 degrees Celsius, and 1 atm.

Chapter 14:

June 2008 Wheaton Academy Rebecca Drury and Kirsten Bell Intermolecular forces- relatively weak interactions that occur between molecules. Intramolecular forces- interactions that occur within a given molecule. Dipole-dipole attraction- the attraction force resulting when polar molecules line up such that the positive and negative ends are close to each other. Hydrogen bonding- unusually strong dipole-dipole attractions that occur among molecules in which hydrogen is bonded to a highly electronegative atom. London dispersion forces- the relatively weak forces, which exist among atoms and nonpolar molecules, that involve an accidental dipole that induces a momentary dipole in a neighbor. Normal boiling point- the temperature at which the vapor pressure of a liquid is exactly one atmosphere; the boiling temperature under one atmosphere of pressure. Heating/cooling curve- a plot of temperature versus time for a substance, where energy is added at a constant rate. Normal freezing point- the melting/freezing point of a solid at a total pressure of one atmosphere. Molar heat of fusion- the energy required to melt 1 mol of a solid. Molar heat of vaporization- the energy required to vaporize 1 mol of a liquid. Vaporization (evaporation)- the change in state that occurs when a liquid evaporates to form a gas. Condensation- the process by which vapor molecules reform a liquid. Vapor pressure- the pressure of the vapor present at equilibrium with its liquid Crystalline solid- a solid characterized by the regular arrangement of its components. Ionic solid- a solid containing cations and anions that dissolves in water to give a solution containing the separated ions, which are mobile and thus free to conduct an electric current. Molecular solid- a solid composed of small molecules. Atomic solid- a solid that contains atoms at the lattice points Electron sea model- pictures a regular array of metal atoms in a “sea” of valence electrons that are shared among the atoms in a nondirectional way and that are quite mobile in the metal crystal. Alloy- a substance that contains a mixture of elements and has metallic properties Substitutional alloy- where some of the host metal atoms are replaced by other metal atoms of similar sizes Interstitial alloy- formed when some of the interstices (holes) among the closely packed metal atoms are occupied by atoms much smaller than the host atoms

Chapter 20: Organic chemistry—the study of carbon-containing compounds (typically containing chains of carbon atoms) and their properties. Biochemistry—the study of the chemistry of living systems Hydrocarbon—a compound of carbon and hydrogen Saturated—hydrocarbons whose carbon-carbon bonds are all single bonds Unsaturated—hydrocarbons containing carbon-carbon multiple bonds Alkane—a saturated hydrocarbon with the general formula CnH2n+2 Normal Hydrocarbons—alkanes in which the carbon atoms form long “strings” or chains

June 2008 Wheaton Academy Rebecca Drury and Kirsten Bell Structural isomerism—occurs when two molecules have the same atoms but different bonds Petroleum—a thick, dark liquid composed mostly of hydrocarbon compounds Natural gas—consists of mostly methane and is associated with petroleum deposits Combustion reaction—the vigorous and exothermic oxidation-reduction reaction that takes place between certain substances (particularly organic compounds) and oxygen. Substitution reaction—a reaction in which an atom, usually a , replaces a hydrogen atom in a hydrocarbon. Dehydrogenation reaction—hydrogen atoms are removed and the product is an unsaturated hydrocarbon Alkene—an unsaturated hydrocarbon containing a carbon-carbon double bond. The general formula is CnH2n Alkyne—an unsaturated hydrocarbon containing a carbon-carbon triple bond. The general formula is CnH2n-2 Addition reaction—new atoms form single bonds to the formerly involved in the double or triple bonds. Hydrogenation reaction—use H2 as a reactant Halogenation—involves the addition of halogen atoms Polymerization—a process in which many small molecules (monomers) are joined together to form a large molecule. Aromatic hydrocarbon—one of a special class of cyclic unsaturated hydrocarbons, the simplest of which is benzene. Benzene—a six-membered ring of carbon atoms called the benzene ring. It has formula C6H6, and a planar structure in which all of the bond angles are 120 degrees. Phenyl group—the benzene molecule minus one hydrogen atom. Hydrocarbon derivative—unusually strong dipole-dipole attractions that occur among molecules in which hydrogen is bonded to a highly electronegative atom. Functional group—an atom or group of atoms in hydrocarbon derivatives that contains elements in addition to carbon and hydrogen. Alcohol—an organic compound in which the hydroxyl group is a substituent on a hydrocarbon. Phenol—the simplest aromatic alcohol Carbonyl group—aldehydes and ketones contain the carbonyl group Ketone—an organic compound containing the carbonyl group bonded to two carbon atoms. Aldehyde—an organic compound containing the carbonyl group Carboxylic acid—an organic compound containing the carboxyl group Carboxyl group—the –COOH group in an organic acid Ester—an organic compound produced by the reaction between a carboxylic acid and an alcohol. Polymer—a large, usually chain-like molecule built from many small molecules (monomers). Addition polymerization—monomers simply “add together” to form the polymer and there are no other products. Condensation—the process by which vapor molecules reform a liquid

June 2008 Wheaton Academy Rebecca Drury and Kirsten Bell Polymerization—a process in which many small molecules (monomers) are joined together to form a large molecule. Copolymer—two different types of monomers combine to form the chain Homopolymer—results from the polymerizing of a single type of monomer. Dimer—two monomers joined Polyester—Dacron

Chapter 21: Biochemistry- the study of the chemistry of living systems Biotechonology- uses nature’s “machinery” to synthesize desired substances Essential elements- the elements known to be essential to human life Trace elements- metals present only in trace amounts in the human body Cell- the smallest unit in living things that exhibits the properties normally associated with life; life is organized around the function of the cell Protein- a natural polymer formed by condensation reactions between amino acids. Fibrous protein- provide structural integrity and strength for many types of tissue and are the main components of muscle, hair, and cartilage. Globular protein- have roughly spherical shape, are the “worker” molecules of the body a-amino acid- an organic acid in which an amino group, a hydrogen atom, and an R group are attached to the carbon atom next to the carboxyl group. Side chain- also called R groups Dipeptide- Peptide linkage- Polypeptide- Primary structure- the order (sequence) of amino acids in the protein chain Secondary structure- the three dimensional structure of the protein chain (for example, a- helix, random coil, or pleated sheet). a-helix – the spiral staircase structure that gives the protein elasticity and is found in the fibrous proteins in wool, hair, and tendons Pleated Sheet- another type of secondary structure involves joining several different protein chains in a an arrangement; this arrangement is called pleated sheet Tertiary Structure- the overall shape of a protein, long and narrow or globular, maintained by different types of intramolecular interactions. Disulfide Linkage- Denaturation Enzyme- Lock-and-key Model- Substrate- Active Site- Carbohydrate- a polyhydroxyl ketone or polyhydroxyl aldehyde or a polymer composed of these. Monosaccharide (simple sugar)- Disaccharide- a sugar formed from two monosaccharides joined by a glycoside linkage. Sucrose- common table sugar; a disaccharide formed from glucose and fructose Glycoside Linkage- eleimination of water to for a C-O-C bond between the rings Polysaccharide- large polymers containing many monosaccharide units Starch- carbohydrate reservoir in plants

June 2008 Wheaton Academy Rebecca Drury and Kirsten Bell Cellulose- the major structural component of woody plants and natural fivers such as cotton; also a polymer of glucose Glycogen- the main carbohydrate reservoir in animals; found in muscles Deoxyribonucleic Acid- a huge nucleotide polymer having a double-helical structure with complementary bases on the two strands. Its major functions are protein synthesis and the storage and transport of genetic information. Ribonucleic Acid- RNA; DNA’s similar nucleic acids which are found in the cytoplasm outside the cell nucleus, and are much smaller than DNA polymers Nucleotide- the fundamental unit in DNA and RNA Protein Synthesis- one of the major functions of DNA Gene- a given segment of the DNA molecule that contains the code for a specific protein. Messenger RNA (mRNA)- built in the cell nucleus, where a specific section of DNA is used as the pattern, mRNA then migrates from the nucleus into the cytoplasm of the cell, where, with the assistance of the ribosomes, the protein is synthesized. Transfer RNA (tRNA)- small RNA fragments which attach themselves to specific amino acids and bring them to the growing protein chain as dictated by the pattern built into the mRNA Lipid- water-insoluble substances that can be extracted from cells by nonpolar organic solvents. Fat- an ester composed of glycerol and fatty acids. Fatty Acid- a long-chain carboxylic acid. Triglyceride—fats that are esters of glycerol Saponification—triglycerides can be broken down by treatment with aqueous sodium hydroxide. The products are glycerol and the fatty acid salts; the latter are known as soaps. This process is called saponification. Micelle—these aggregates of fatty-acid anions have the water-incompatible tails in the interior; the anionic parts (the polar heads) point outward and interact with the polar water molecules. Surfactant—wetting agent Phospholipids—similar in structure to fats in that they are esters of glycerol. Unlike fats, they contain only two fatty acids. The third group bound to glycerol is a phosphate group. It has the long nonpolar “tail” and the polar substituted-phosphate “head”. Wax—class o f lipids, involve monohydroxy alcohols instead of glycerol. Steroid—a class of lipids that have a characteristic carbon ring structure. Cholesterol—a class of steroids found in virtually all organisms and is the starting material for the formation of the many other steroid-based molecules, such as vitamin D. Adrenocorticoid Hormone—steroid that is synthesized in the adrenal glands and are involved in various regulatory functions. Sex Hormone—a class of steroids Bile Acid—a class of steroids produced from cholesterol in the liver and stored in the gallbladder.

June 2008 Wheaton Academy Rebecca Drury and Kirsten Bell

June 2008 Wheaton Academy Rebecca Drury and Kirsten Bell