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2nd Semester Chemistry Terms 1. Atom- the smallest particle of an element that has all of the element’s chemical properties 2. Element- any material that is made up of only one type of atom 3. Periodic table- a chart in which all known elements are listed in order of atomic number 4. Atomic symbol- an abbreviation for an element or atom 5. Atomic nucleus- the core of an atom, consisting of two basic subatomic particles—protons and neutrons 6. Electron- a negatively charged particle in an atom 7. Proton- a positively charged particle in an atomic nucleus 8. Atomic number- the number that designates the identity of an element, which is the number of protons in the nucleus of an atom; in a neutral atom, the atomic number is also the number of electrons in the atom 9. Mass number- the total number of nucleons in an atomic nucleus 10. Neutron- an electrically neutral subatomic particle in an atomic nucleus 11. Nucleon- a nuclear particle; a proton or a neutron in an atomic nucleus 12. Isotopes- different forms of an element whose atoms contain the same number of protons but different number of neutrons 13. Atomic mass- the mass of an element’s atoms listed in the periodic table as an average value based on the relative abundance of the element’s isotopes 14. Atomic mass unit (amu)- the standard unit of atomic mass, which is equal to one-twelfth the mass of the common atom of carbon, arbitrarily given the value of exactly 12 15. Period- a horizontal row in the periodic table 16. Group- a vertical column in the periodic table, also known as the family of elements 17. Physical model- a representation of an object on some convenient scale 18. Conceptual model- a representation of a system that helps in making predictions about how the system behaves 19. Spectroscope- a device that uses a prism or a diffraction grating to separate light into its component colors 20. Atomic spectrum- the pattern of frequencies of electromagnetic radiation emitted by the atoms of an element, considered to be the element’s “fingerprint” 21. Quantum hypothesis- the idea that light energy is contained in discrete packets called quanta 22. Quantum- a small, discrete packet of light energy 23. Principal quantum number, n- an integer that specifies the quantized energy level of an atomic orbital 24. Probability cloud- the pattern of electron positions plotted over time to show the likelihood of an electron’s being at a given position at a given time 25. Atomic orbital- a region of space in which an electron in an atom has a 90 percent chance of being located 26. Shell- a set of overlapping atomic orbitals of similar energy levels 27. Valence electrons- an electron that is located in the outermost occupied shell of an atom and can participate in chemical bonding 28. Radioactivity- the process whereby unstable atomic nuclei break down and emit radiation 29. Alpha particle- the nucleus of a helium atom 30. Beta particle- an electron emitted during the radioactive elements 31. Gamma ray- high-frequency electromagnetic radiation emitted by the nuclei or radioactive atoms 32. Nucleon- a nuclear proton or neutron 33. Half-life- the time required for half the atoms in a sample of a radioactive isotope to decay 34. Transmutation- the conversion of an atomic nucleus of one element into an atomic nucleus of another element through a loss or gain in the number of protons 35. Nuclear fission- the splitting of the nucleus of a heavy atom accompanied by the release of much energy 36. Chain reaction- a self-sustaining reaction in which the products of one reaction event stimulate further reaction events 37. Critical mass- the minimum mass of fissionable material in a reactor or nuclear bomb that will sustain a chain reaction 38. Nuclear fusion- the combining of nuclei of light atoms to form heavier nuclei, with the release of much energy 39. Thermonuclear fusion- nuclear fusion produced by high temperature 40. Basic research- a branch of scientific research that focuses on a greater understanding of how the natural world operates 41. Applied research- a branch of scientific research that focuses on developing applications built upon the principles discovered through basic research 42. Molecule- a submicroscopic particle consisting of a group of atoms 43. Submicroscopic- refers to the realm of atoms and molecules 44. Physical property- any physical attribute of a substance 45. Physical change- a change in which a substance changes one or more of its physical properties without transforming it into a different substance 46. Chemical property- a property that characterizes the ability of a substance to undergo a change that transforms it into a different substance 47. Chemical bond- the force of attraction between two atoms that holds them together 48. Chemical change- a change in which the atoms of one or more substances are rearranged into one or more new substances 49. Chemical reaction- synonymous with chemical change 50. Elemental formula- a notation that uses the atomic symbol and a numerical subscript to denote how atoms of the element are bonded together 51. Compound- a material in which atoms of different elements are bonded to one another 52. Chemical formula- a notation used to indicate the compositions of a compound 53. Chemical equation- a representation of a chemical reaction in which reactants are drawn before an arrow that points to the products 54. Reactants- the reacting substances in a chemical reaction 55. Products- the new materials formed in a chemical reaction 56. Law of mass conservation- matter is neither created nor destroyed during a chemical reaction 57. Mixture- A combination of two or more substances in which each substance retains its properties. 58. Distillation- A purifying process in which a vaporized substance is collected by exposing it to cooler temperatures over a receiving flask, which collects the condensed purified liquid. 59. Pure- Having a uniform composition, or being without impurities. 60. Impure- a material that is a mixture of more than one element or compound. 61. Heterogeneous Mixture – A mixture in which the various components can be seen as individual substances. 62. Homogeneous mixture- A mixture in which the components are so finely mixed that the composition is the same throughout. 63. Solution- A homogeneous mixture in which all components are in the same phase. 64. Suspension- A homogeneous mixture in which the various components are in different phases. 65. Solvent- The component in a solution that is present in the largest amount. 66. Solute- Any component in a solution that is not the solvent. 67. Dissolving- The process of mixing a solute in a solvent to produce a homogeneous mixture. 68. Saturated Solution- A solution containing the maximum amount of solute that will dissolve in its solvent. 69. Unsaturated Solution- A solution that is capable of dissolving additional solute. 70. Concentration- A quantitative measure of the amount of solute in a solution. 71. Mole- The amount of an pure substance that contains as many atoms, molecules, ions, or other elementary units as the number of atoms in 12 grams of Carbon-12. 72. Molarity- A unit of concentration equal to the number of moles of a solute per liter of solution. 73. Semipermeable membrane- A membrane that allows only the passage of molecules small enough to fit through its submicroscopic pores. 74. Osmosis- The diffusion of water or some other fluid through a semipermeable membrane from a solution with a low concentration or solutes to a solution with a higher concentration of solutes. 75. Reverse Osmosis- A technique for purifying water by forcing it through a semipermeable membrane. 76. Valence shell- the outermost occupied shell of an atom 77. Electron-dot structure- a shorthand notation of the shell model of the atom 78. Nonbonding pairs- two paired valence electrons that tend not to participate in a chemical bond 79. Ion- an electrically charged particle created when an atom either loses or gains one or more electrons 80. Polyatomic ion- an ionically charged molecule 81. Ionic bond- a chemical bond in which an attractive electric force holds ions of opposite charge together 82. Ionic compound- any chemical compound containing ions 83. Covalent bond- a chemical bond in which atoms are held together by their mutual attraction for two or more electrons they share 84. Covalent compound- an element or chemical compound in which atoms are held together by covalent bonds 85. Molecule- a group of atoms held tightly together by covalent bonds 86. Dipole- a separation of charge that occurs in a chemical bond because of differences in the electronegativities of the bonded atoms. 87. Electronegativity- the ability of an atom to attract a bonding pair of electrons to itself when bonded to another atom 88. Nonpolar- said of a chemical bond that has no dipole 89. Polar- said of a chemical bond that has a dipole 90. Hydrogen bond- a strong dipole 91. Induced dipole- a dipole temporarily created in an otherwise nonpolar molecule, induced by a neighboring charge 92. Solubility- the ability of a solute to dissolve in a given solvent 93. Soluble- capable of dissolving to an appreciable extent in a given solvent 94. Insoluble- not capable of dissolving to any appreciable extent in a given solvent 95. Precipitate- a solute that has come out of a solution 96. Hard water- water containing large amounts of calcium and magnesium ions 97. Reaction rate- a measure of how quickly the concentration of products in a chemical reaction increases or the concentration of reactants decreases 98. Activation energy- the minimum energy required in order for a chemical reaction to proceed 99. Catalyst- any substance that increases the rate of a chemical reaction without itself being consumed by the reaction 100. Exothermic- a term that describes a chemical reaction in which there is a net release of energy 101. Endothermic- a term that describes a chemical reaction in which there is a net absorption of energy 102. Bond energy- the amount of energy that is either absorbed as a chemical bond breaks or is released as a chemical bond forms 103. Formula mass- the sum of the atomic masses of the atoms in a chemical compound or element 104. Avogadro’s number- the number of particles- 6.02 X 1023 -containing in 1 mole of anything 105. Molar mass- the mass of 1 mole of a substance 106. Acid- donates a hydrogen ion 107. Base- accepts a hydrogen ion 108. Hydronium ion- a water molecule after accepting a hydrogen ion 109. Hydroxide ion- a water molecule after loosing a hydrogen ion 110. Salt- an ionic compound formed from the reaction between an acid and a base 111. Neutralization- a reaction in which an acid and base combine to form a salt 112. Amphoteric- a description of a substance that can behave either as an acid or as a base 113. Acidic solution- a solution in which the hydronium-ion concentration is higher than the hydroxide-ion concentration 114. Basic solution- a solution in which the hydroxide-ion concentration is higher than the hydronium-ion concentration 115. Neutral solution- a solution in which the hydronium-ion concentration is equal to the hydroxide-ion concentration 116. pH- a measure of the acidity of a solution, equal to the negative of the base-10 logarithm of the hydronium-ion concentration 117. Buffer solution- A solution that resists large changes in pH. 118. Oxidation- The process whereby a reactant loses one or more electrons. 119. Reduction- The process whereby a reactant gains one or more electrons. 120. Half reaction – One proportion of an oxidation-reduction reaction, represented by an equation showing electrons as either reactants or products. 121. Electrochemistry- The branch of chemistry concerned with the relationship between electrical energy and chemical change. 122. Electrode- Any material that conducts electrons into or out of a medium in which electrochemical reactions are occurring. 123. Cathode- the electrode where reduction occurs. 124. Anode- The electrode where oxidation occurs. 125. Electrolysis- The use of electrical energy to produce chemical change. 126. Corrosion – The deterioration of a metal, to produce chemical change. 127. Combustion- An exothermic oxidation-reduction reaction between a nonmetallic material and molecular oxygen. 128. Organic chemistry- The study of carbon-containing compounds. 129. Hydrocarbon- A chemical compound containing only carbon and hydrogen atoms. 130. Structural isomers- Molecules that have the same molecular formula but different chemical structures. 131. Conformation- One of the possible spatial orientations of a molecule. 132. Saturated Hydrocarbon- A hydrocarbon containing no multiple covalent bonds, with each carbon atom bonded to four other atoms. 133. Unsaturated Hydrocarbon- A hydrocarbon containing at least one multiple covalent bond. 134. Aromatic Compound- Any organic molecule containing a benzene ring. 135. Heteroatom- Any atom other than carbon or hydrogen in an organic molecule. 136. Functional Group- A specific combination of atoms that behaves as a unit in an organic molecule. 137. Alcohol- An organic molecule that contains a hydroxyl group bonded to a saturated carbon. 138. Phenol- An organic molecule in which a hydroxyl group is bonded to a benzene ring. 139. Ether- An organic molecule containing an oxygen atom bonded to two carbon atoms. 140. Amine- An organic molecule containing a nitrogen atom bonded to one or more saturated carbon atoms. 141. Carbonyl Group- A carbon atom double-bonded to an oxygen atom; found in ketones, aldehydes, amides, carboxylic acids, and esters. 142. Ketone- An organic molecule containing a carbonyl group, the carbon of which is bonded to two carbon atoms. 143. Aldehyde- An organic molecule containing a carbonyl group, the carbon of which is bonded either to one carbon atom and one hydrogen atom or two hydrogen atoms. 144. Amide- An organic molecule containing a carbonyl group, the carbon of which is bonded to a nitrogen atom. 145. Carboxylic Acid- An organic molecule containing a carbonyl group, the carbon of which is bonded to a hydroxyl group. 146. Ester- An organic molecule containing a carbonyl group, the carbon of which is bonded to one carbon atom and one oxygen atom bonded to another carbon atom. 147. Polymer- A long organic molecule made of many repeating unites. 148. Monomers- The small molecular unites form which a polymer is formed. 149. Addition Polymer- A polymer formed by the joining together of monomer units with no atoms being lost as the polymer forms. 150. Condensation Polymer- A polymer formed by the joining together of monomer units accompanied by the loss of small molecules, such as water.