Vocabulary Words are cumulative and must be hand written using blue/black ink pen in the notebook and picture is written/drawn with each definition for credit! If you are absent you can ask Mrs. Chaillou or a student for an example of a picture shared in class. Scroll down for most recent vocabulary words added in class.
1. chemistry - the study of the composition, structure, properties of matter, the processes that matter undergoes, and the energy changes that accompany these processes.
2. chemical - any substance that has a definite composition
3. matter - anything that has mass and volume
4. pure substance - a sample of matter , either a single element or a single compound, that has definite chemical and physical properties
5. element - a pure substance that cannot be broken down into simpler, stable substances and is made of one type of atom
6. compound - a substance made from the atoms of two or more elements chemically bonded that can be broken down into simple stable substances
7. physical property - a characteristic that can be observed or measured without changing the identity of the substance
8. chemical property - a characteristic related to a substance's ability to undergo changes that transform it into different substances
9. physical change - a change that does not involve a change in the identity of the substance
10. chemical change (reaction) - a change in which one or more substances are converted into different substances
11. significant figures - a measurement that consists of all the digits known with certainty plus one final digit which is somewhat uncertain or estimated
12. uncertain digit - an estimated digit that should be included in ALL measurements taken in the lab; number of digits in a measurement tells how confident you are in that measurement.
13. density - the ratio of mass to volume or mass divided by volume.
14. Archimedes' Principle - states that the upward force exerted on a body immersed in a fluid, whether fully or partially, is equal to the weight of the fluid that the body displaces.
15. derived units - combination of SI units;produced by multiplying or dividing units
16. dimensional analysis - a mathematical technique that allows you to solve problems involving measurements
17. Law of Conservation of Mass - states that mass is neither created nor destroyed during ordinary chemical reactions or physical changes
18. Law of Definite Proportions - states that a chemical compound contains the same elements in exactly the same proportions regardless of the size of the sample or source of the compound
19. Law of Multiple Proportions - states that if two or more compounds are comprised of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first is always a ratio of small whole numbers
20.atomic number - the number of protons in each atom of the element
21. mass number - the total number of protons and neutrons that make up the nucleus of an atom (isotope)
22. isotope - atom of the same element with different number of neutrons which results in different masses
23. decay series - a series of radioactive nuclides produced by successive radioactive decay until a stable nuclide is formed
24. parent nuclide - the heaviest nuclide of each decay series
25. daughter nuclide - the nuclides produced by the decay of the parent nuclides
26. nucleons - protons and neutrons collectively that make up atomic nuclei
27. nuclear binding energy - the energy released when a nucleus is formed from nucleons; energy required to break apart nucleus
28. hydrate - an ionic compound that has water trapped inside the structure of the compound; the water is physically trapped not chemically bonded
29. electromagnetic radiation - a form of energy that exhibits wavelike behavior as it travels through space
30. electromagnetic spectrum - all of the frequencies or wavelengths of electromagnetic radiation
31. quantum - the minimum quantity of energy that can be gained or lost by an atom
32. photon - a particle of EM radiation having zero mass and carrying a quantum of energy; energy depends on frequency of the radiation
33. ground state - lowest energy state of an atom
34. excited state - a state in which an atom has a higher potential energy than its ground state
35. valence electron -an electron that is found in the outermost shell of an atom and that determines the atom's chemical properties
36. main-group element - an element in the s-block or p-block of the periodic table
37. principal quantum number - indicates the main energy level occupied by the electron
38. angular momentum quantum number - indicates the shape/sublevel of the orbital
39. magnetic quantum number - indicates the orientation of an orbital around the nucleus
40. spin quantum number - indicates the two fundamental spin states of an electron in an orbital
41. atomic radius - one-half the distance between the nuclei of identical atoms that are bonded together
42. ion - an atom or group of atoms that have a positive or negative charge
43. ionization - any process that results in the formation of an ion
44. chemical bond - a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together
45. ionic bonding - chemical bonding that results from electrical attraction between cations and anions; metals and nonmetals
46. covalent bonding - chemical bonding that results from the sharing of electron pairs between two atoms; nonmetals and nonmetals
47. molecule - a molecule is a group of two or more atoms covalently bonded that form the smallest identifiable unit into which a pure substance can be divided and still retain composition; forms neutral compound
48. chemical formula - indicates the relative number of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts
49. molecular formula - shows the types and numbers of atoms combined in a single molecule of a molecular compound
50. Nonpolar covalent bond – a covalent bond in which the bonding electrons are equally attracted to both bonded atoms
51. Polar covalent bond – a covalent bond in which the bonded atoms have an unequal attraction for the shared electrons
52. dipole - a molecule that has two poles, or regions, with opposite charges
53. diatomic molecule - a molecule containing only two atoms
54. polyatomic ion -a charged group of covalently bonded atoms
55. Lattice energy - the energy released when one mole of an ionic crystalline compound is formed from gaseous ions
56. VSEPR theory - Valence Shell Electron Pair Repulsion - states that repulsion between the sets of valence level electrons surrounding an atom causes these sets to be oriented as far apart as possible
57. hybridization - the mixing of two or more atomic orbitals of similar energies on the same atom to produce new hybrid orbitals of equal energies
58. hybrid orbitals -orbitals of equal energy produced by the combination of two or more orbitals on the same atom
59. resonance - refers to bonding of molecules or ions that cannot be correctly represented by a single Lewis structure
60. intermolecular forces (IMF) - the forces of attraction between molecules
61. monatomic ions - ions formed from single atoms
62. nomenclature - a naming system
63. oxyanions - polyatomic ions that contain oxygen
64. oxidation number -a positive or negative number assigned to an atom to indicate its degree of oxidation or reduction; the oxidation number for an uncombined atom is zero
65. salt - an ionic compound composed of a cation and an anion from an acid and a base
66. formula mass - the sum of the average atomic masses of all atoms present in the chemical formulas of any molecule, formula unit, or ion
67. percentage composition - the percentage by mass of each element in a compound
68. binary compound - compounds composed of two elements
69. ternary compounds - compounds composed of at least 3 different elements
70. empirical formula - a chemical formula that represents the simplest whole number ratios of atoms
71. molecular formula - a chemical formula that shows the actual number of each type of atoms In a compound (true formula) - empirical and molecular may be the same formula (ex. water)
72. chemical equation - an equation that represented with symbols and formulas and the identities and relative molecular or molar amounts of the reactants and products in the reaction
73. word equation - an equation in which the reactants and products in a chemical equation are represented by words
74. precipitate - a solid substance that is produced as a result of a chemical reaction
75. activity series - a series of elements that have similar properties and that are arranged in descending order of chemical activity
76. electrolysis - the decomposition of a substance by an electric current
77. coefficient - a small whole number that appears as a factor in front of a chemical formula or symbol in a chemical equation
78. composition stoichiometry - deals with the mass relationships of elements in compounds
79. reaction stoichiometry - involves the mass relationships between reactants and products in a chemical reaction
80. mole ratio - a conversion factor that relates the amounts in moles of any two substances involved in a chemical reaction
81. limiting reactant (LR)- the reactant that limits the amount of product that can form in a chemical reaction
82. excess reactant(ER) - the reactant that is not used up completely in a chemical reaction
83. theoretical yield - the maximum amount of product that can be produced from a given amount of reactant
84. actual yield - the measured amount of a product obtained from a reaction
85. percentage yield - the ratio of the actual yield to the theoretical yield
86. kinetic-molecular theory - based on the idea that particles of matter are always in motion; explains properties of solids, liquids, and gases in terms of energy of particles and forces between them
87. ideal gas - a hypothetical gas that perfectly fits all the assumptions of the kinetic molecular theory
88. real gas - a gas that does not behave completely according to the assumptions of the KMT
89. volatile liquids - liquids that evaporate readily, have relatively weak forces of attraction between their particles
90. capillary action - the attraction of the surface of the liquid to the surface of a solid
91. diffusion - spontaneous mixing of two substances caused by their random motion
92. elastic collisions - collisions between gas particles and the walls of the container which there is no net loss of total kinetic energy
93. molar enthalpy of vaporization - the amount of energy as heat that is needed to vaporize one mole of liquid at the liquid's boiling point at constant pressure and temperature
94. molar enthalpy of fusion - the amount of energy as heat that is needed to melt one mole of a solid at the solid's melting point at constant pressure and temperature
95. phase diagram - a graph of pressure versus temperature that shows conditions under which the phase of a substance exists
96. supercritical fluid (SCF) - any substance at a temperature and pressure above its critical point where distinct liquid and gas phases do not exist
97. STP - standard temperature and pressure is 0 degrees C and 1 atm
98. pressure - the force per unit area on a surface
99. Newton - the SI unit of force; will increase the speed of a one kilogram mass by one meter per second each second
100. Pascal - the pressure (SI unit) exerted by the force of one newton acting on the area of one square meter
101. standard molar volume of gas - the volume occupied by one mole of a gas at STP
102. mixture - a combination of two or more substances physically mixed; no fixed ratios
103. heterogeneous mixture - a mixture that is not uniformly mixed
104. homogeneous mixture - a mixture that is uniformly mixed
105. soluble - capable of being dissolved
106. solution - a homogeneous mixture of two or more substances in a single phase
107. solute - the substance being dissolved in a solution
108. solvent - the dissolving medium; substance doing the dissolving
109. concentration - the measure of the amount of solute in a given amount of solvent in a solution
110. molarity - the number of moles of solute in one liter of solution
111. molality - the concentration of a solution expressed in moles of solute per kilogram of solvent
112. percent by mass - a process that describes the concentration by comparing the ratio of the mass of the solute to the total mass of the solution
113. dilution - the process of decreasing concentration of a solute in a solution, usually by simply mixing with more solvent like adding more water to the solution
114. solubility - the amount of a substance required to form a saturated solution with a specific amount of solvent at a specified temperature
115. saturated solution - a solution that contains the maximum amount of solute in a solvent at a specific temperature
116. dissociation - the separation of ions that occurs when an ionic compound dissolves
117. ionization - the formation of ions from solute molecules by the action of the solvent
118. boiling point elevation - the difference in temperature between boiling point of a solution and the boiling point of the pure solvent
119. freezing point depression - the difference in temperature between the freezing point of a solution and the freezing point of the pure solvent
120. Arrhenius acid - a substance that increases the concentration of H+ ions in an aqueous solution(ionizes in solution)
121. Arrhenius base - a substance that increases the concentration of OH- in an aqueous solutions (some are ionic hydroxides)
122. Bronsted-Lowry acid - a molecule or ion that is a proton donor
123. Bronsted-Lowry base - a molecule or ion that is a proton acceptor
124. Bronsted-Lowry acid-base reaction - protons are transferred from one reactant (the acid) to another (the base)
125. conjugate acid - the species formed when a Bronsted-Lowry base gains a hydrogen ion (proton)
126. conjugate base - the species that remains when a Bronsted-Lowry acid has donated a hydrogen ion (proton)
127. conjugate acid-base pair - two substances that are related by the loss and gain of a single hydrogen ion (proton)
128. pH - the measure of [H3O+] in a solution, measure of “acidity”
129. pOH - the measure of [OH-] in a solution, measure of "alkalinity"
130. self-ionization of water - two water molecules produce a hydronium ion and a hydroxide ion by transfer of a proton
131. neutralization - the reaction of hydronium ions and hydroxide ions to form water molecules and a salt
132. amphoteric - any species that can react as either an acid or a base
133. endpoint - the point in a titration at which an indicator changes color
134. standard solution - the solution that contains the precisely known concentration of the solute; the "known" solution
135. titration - the controlled addition and measurement of the amount of a solution of known concentration to react completely with a measured amount of a solution of unknown concentration
136. equivalence point - the point at which two solutions used in a titration are present in chemically equivalent amounts
137. thermochemistry - the study of the transfers of energy as heat that accompany chemical reactions and physical changes
138. temperature - a measure of the average kinetic energy of the particles in a sample of matter
139. calorimeter - instrument used to measure the energy absorbed or released as heat in a chemical reaction and physical changes
140. enthalpy change - the amount of energy absorbed/released by a system as heat during a process at constant pressure
141. thermochemical equation - an equation that includes the quantity of energy released or absorbed as heat during that reaction as written
142. joule - the SI unit of heat as well as other forms of energy
143. entropy - a measure of the degree of randomness/disorder of the particles, such as molecules in a system
144. entropy change - a measure of the difference between entropy of the products and the reactants
145. free energy - the energy available to do work
146. free energy change - the difference between the enthalpy and the product of the Kelvin temperature, and the entropy change at constant temperature and pressure
147. activated complex - a transitional structure that results from an effective collision and that persists while old bonds are breaking and new bonds are forming
148. reaction rate - the change in concentration of the reactants per unit of time as the reaction proceeds
149. reaction mechanism - the step-by-step sequence of reactions by which the overall chemical change occurs
150. intermediate - species that appear in some steps but not in the net equation
151.chemical equilibrium - a reversible reaction that occurs when the rate of its forward reaction equals the rate of its reverse reaction and the concentration of the products and the reactants remain unchanged
152. equilibrium constant - the ratio of the mathematical product of the concentrations of substances formed at equilibrium to the mathematical product of the concentrations of reacting substances; each concentration is raised to a power equal to the coefficients of that substance
153. acid ionization constant- constant for a specified temperature but has a new value for each new temperature
154. Le'Chatelier's Principle - states if a system at equilibrium is subjected to a stress, the equilibrium is shifted in the direction that tends to relieve the stress
155. solubility product constant - is the product of the molar concentration of its ions in a saturated solution, each raised to the power that is the coefficient of that ion in the balanced chemical equation.
156. anion hydrolysis - salts formed from weak acids and its strong conjugate base react with water to produce solutions that are basic
157. cation hydrolysis - salts formed from weak bases and its strong conjugate acid react with water to produce solutions that are acidic
158. oxidation - processes in which the atoms or ions of an element experience an increase in oxidation numbers due to electron loss
159. oxidized - refers to what happens to a species whose oxidation number increases
160. reduction - processes in which the atoms or ions of an element experience a decrease in oxidation numbers due to electron gain
161. reduced - refers to what happens to a species whose oxidation number decreases
162. oxidizing agent - a substance that has the potential to cause another substance to be oxidized (gains e-)
163. reducing agent - a substance that has the potential to cause another substance to be reduced (loses e-)
164. Disproportionation - a process in which a substance acts as both an oxidizing and reducing agent; self-oxidizing and self-reducing
165. half-reaction - the part of the reaction involving oxidation or reduction alone; overall equation is the sum of the two reactions
1. chemistry - the study of the composition, structure, properties of matter, the processes that matter undergoes, and the energy changes that accompany these processes.
2. chemical - any substance that has a definite composition
3. matter - anything that has mass and volume
4. pure substance - a sample of matter , either a single element or a single compound, that has definite chemical and physical properties
5. element - a pure substance that cannot be broken down into simpler, stable substances and is made of one type of atom
6. compound - a substance made from the atoms of two or more elements chemically bonded that can be broken down into simple stable substances
7. physical property - a characteristic that can be observed or measured without changing the identity of the substance
8. chemical property - a characteristic related to a substance's ability to undergo changes that transform it into different substances
9. physical change - a change that does not involve a change in the identity of the substance
10. chemical change (reaction) - a change in which one or more substances are converted into different substances
11. significant figures - a measurement that consists of all the digits known with certainty plus one final digit which is somewhat uncertain or estimated
12. uncertain digit - an estimated digit that should be included in ALL measurements taken in the lab; number of digits in a measurement tells how confident you are in that measurement.
13. density - the ratio of mass to volume or mass divided by volume.
14. Archimedes' Principle - states that the upward force exerted on a body immersed in a fluid, whether fully or partially, is equal to the weight of the fluid that the body displaces.
15. derived units - combination of SI units;produced by multiplying or dividing units
16. dimensional analysis - a mathematical technique that allows you to solve problems involving measurements
17. Law of Conservation of Mass - states that mass is neither created nor destroyed during ordinary chemical reactions or physical changes
18. Law of Definite Proportions - states that a chemical compound contains the same elements in exactly the same proportions regardless of the size of the sample or source of the compound
19. Law of Multiple Proportions - states that if two or more compounds are comprised of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first is always a ratio of small whole numbers
20.atomic number - the number of protons in each atom of the element
21. mass number - the total number of protons and neutrons that make up the nucleus of an atom (isotope)
22. isotope - atom of the same element with different number of neutrons which results in different masses
23. decay series - a series of radioactive nuclides produced by successive radioactive decay until a stable nuclide is formed
24. parent nuclide - the heaviest nuclide of each decay series
25. daughter nuclide - the nuclides produced by the decay of the parent nuclides
26. nucleons - protons and neutrons collectively that make up atomic nuclei
27. nuclear binding energy - the energy released when a nucleus is formed from nucleons; energy required to break apart nucleus
28. hydrate - an ionic compound that has water trapped inside the structure of the compound; the water is physically trapped not chemically bonded
29. electromagnetic radiation - a form of energy that exhibits wavelike behavior as it travels through space
30. electromagnetic spectrum - all of the frequencies or wavelengths of electromagnetic radiation
31. quantum - the minimum quantity of energy that can be gained or lost by an atom
32. photon - a particle of EM radiation having zero mass and carrying a quantum of energy; energy depends on frequency of the radiation
33. ground state - lowest energy state of an atom
34. excited state - a state in which an atom has a higher potential energy than its ground state
35. valence electron -an electron that is found in the outermost shell of an atom and that determines the atom's chemical properties
36. main-group element - an element in the s-block or p-block of the periodic table
37. principal quantum number - indicates the main energy level occupied by the electron
38. angular momentum quantum number - indicates the shape/sublevel of the orbital
39. magnetic quantum number - indicates the orientation of an orbital around the nucleus
40. spin quantum number - indicates the two fundamental spin states of an electron in an orbital
41. atomic radius - one-half the distance between the nuclei of identical atoms that are bonded together
42. ion - an atom or group of atoms that have a positive or negative charge
43. ionization - any process that results in the formation of an ion
44. chemical bond - a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together
45. ionic bonding - chemical bonding that results from electrical attraction between cations and anions; metals and nonmetals
46. covalent bonding - chemical bonding that results from the sharing of electron pairs between two atoms; nonmetals and nonmetals
47. molecule - a molecule is a group of two or more atoms covalently bonded that form the smallest identifiable unit into which a pure substance can be divided and still retain composition; forms neutral compound
48. chemical formula - indicates the relative number of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts
49. molecular formula - shows the types and numbers of atoms combined in a single molecule of a molecular compound
50. Nonpolar covalent bond – a covalent bond in which the bonding electrons are equally attracted to both bonded atoms
51. Polar covalent bond – a covalent bond in which the bonded atoms have an unequal attraction for the shared electrons
52. dipole - a molecule that has two poles, or regions, with opposite charges
53. diatomic molecule - a molecule containing only two atoms
54. polyatomic ion -a charged group of covalently bonded atoms
55. Lattice energy - the energy released when one mole of an ionic crystalline compound is formed from gaseous ions
56. VSEPR theory - Valence Shell Electron Pair Repulsion - states that repulsion between the sets of valence level electrons surrounding an atom causes these sets to be oriented as far apart as possible
57. hybridization - the mixing of two or more atomic orbitals of similar energies on the same atom to produce new hybrid orbitals of equal energies
58. hybrid orbitals -orbitals of equal energy produced by the combination of two or more orbitals on the same atom
59. resonance - refers to bonding of molecules or ions that cannot be correctly represented by a single Lewis structure
60. intermolecular forces (IMF) - the forces of attraction between molecules
61. monatomic ions - ions formed from single atoms
62. nomenclature - a naming system
63. oxyanions - polyatomic ions that contain oxygen
64. oxidation number -a positive or negative number assigned to an atom to indicate its degree of oxidation or reduction; the oxidation number for an uncombined atom is zero
65. salt - an ionic compound composed of a cation and an anion from an acid and a base
66. formula mass - the sum of the average atomic masses of all atoms present in the chemical formulas of any molecule, formula unit, or ion
67. percentage composition - the percentage by mass of each element in a compound
68. binary compound - compounds composed of two elements
69. ternary compounds - compounds composed of at least 3 different elements
70. empirical formula - a chemical formula that represents the simplest whole number ratios of atoms
71. molecular formula - a chemical formula that shows the actual number of each type of atoms In a compound (true formula) - empirical and molecular may be the same formula (ex. water)
72. chemical equation - an equation that represented with symbols and formulas and the identities and relative molecular or molar amounts of the reactants and products in the reaction
73. word equation - an equation in which the reactants and products in a chemical equation are represented by words
74. precipitate - a solid substance that is produced as a result of a chemical reaction
75. activity series - a series of elements that have similar properties and that are arranged in descending order of chemical activity
76. electrolysis - the decomposition of a substance by an electric current
77. coefficient - a small whole number that appears as a factor in front of a chemical formula or symbol in a chemical equation
78. composition stoichiometry - deals with the mass relationships of elements in compounds
79. reaction stoichiometry - involves the mass relationships between reactants and products in a chemical reaction
80. mole ratio - a conversion factor that relates the amounts in moles of any two substances involved in a chemical reaction
81. limiting reactant (LR)- the reactant that limits the amount of product that can form in a chemical reaction
82. excess reactant(ER) - the reactant that is not used up completely in a chemical reaction
83. theoretical yield - the maximum amount of product that can be produced from a given amount of reactant
84. actual yield - the measured amount of a product obtained from a reaction
85. percentage yield - the ratio of the actual yield to the theoretical yield
86. kinetic-molecular theory - based on the idea that particles of matter are always in motion; explains properties of solids, liquids, and gases in terms of energy of particles and forces between them
87. ideal gas - a hypothetical gas that perfectly fits all the assumptions of the kinetic molecular theory
88. real gas - a gas that does not behave completely according to the assumptions of the KMT
89. volatile liquids - liquids that evaporate readily, have relatively weak forces of attraction between their particles
90. capillary action - the attraction of the surface of the liquid to the surface of a solid
91. diffusion - spontaneous mixing of two substances caused by their random motion
92. elastic collisions - collisions between gas particles and the walls of the container which there is no net loss of total kinetic energy
93. molar enthalpy of vaporization - the amount of energy as heat that is needed to vaporize one mole of liquid at the liquid's boiling point at constant pressure and temperature
94. molar enthalpy of fusion - the amount of energy as heat that is needed to melt one mole of a solid at the solid's melting point at constant pressure and temperature
95. phase diagram - a graph of pressure versus temperature that shows conditions under which the phase of a substance exists
96. supercritical fluid (SCF) - any substance at a temperature and pressure above its critical point where distinct liquid and gas phases do not exist
97. STP - standard temperature and pressure is 0 degrees C and 1 atm
98. pressure - the force per unit area on a surface
99. Newton - the SI unit of force; will increase the speed of a one kilogram mass by one meter per second each second
100. Pascal - the pressure (SI unit) exerted by the force of one newton acting on the area of one square meter
101. standard molar volume of gas - the volume occupied by one mole of a gas at STP
102. mixture - a combination of two or more substances physically mixed; no fixed ratios
103. heterogeneous mixture - a mixture that is not uniformly mixed
104. homogeneous mixture - a mixture that is uniformly mixed
105. soluble - capable of being dissolved
106. solution - a homogeneous mixture of two or more substances in a single phase
107. solute - the substance being dissolved in a solution
108. solvent - the dissolving medium; substance doing the dissolving
109. concentration - the measure of the amount of solute in a given amount of solvent in a solution
110. molarity - the number of moles of solute in one liter of solution
111. molality - the concentration of a solution expressed in moles of solute per kilogram of solvent
112. percent by mass - a process that describes the concentration by comparing the ratio of the mass of the solute to the total mass of the solution
113. dilution - the process of decreasing concentration of a solute in a solution, usually by simply mixing with more solvent like adding more water to the solution
114. solubility - the amount of a substance required to form a saturated solution with a specific amount of solvent at a specified temperature
115. saturated solution - a solution that contains the maximum amount of solute in a solvent at a specific temperature
116. dissociation - the separation of ions that occurs when an ionic compound dissolves
117. ionization - the formation of ions from solute molecules by the action of the solvent
118. boiling point elevation - the difference in temperature between boiling point of a solution and the boiling point of the pure solvent
119. freezing point depression - the difference in temperature between the freezing point of a solution and the freezing point of the pure solvent
120. Arrhenius acid - a substance that increases the concentration of H+ ions in an aqueous solution(ionizes in solution)
121. Arrhenius base - a substance that increases the concentration of OH- in an aqueous solutions (some are ionic hydroxides)
122. Bronsted-Lowry acid - a molecule or ion that is a proton donor
123. Bronsted-Lowry base - a molecule or ion that is a proton acceptor
124. Bronsted-Lowry acid-base reaction - protons are transferred from one reactant (the acid) to another (the base)
125. conjugate acid - the species formed when a Bronsted-Lowry base gains a hydrogen ion (proton)
126. conjugate base - the species that remains when a Bronsted-Lowry acid has donated a hydrogen ion (proton)
127. conjugate acid-base pair - two substances that are related by the loss and gain of a single hydrogen ion (proton)
128. pH - the measure of [H3O+] in a solution, measure of “acidity”
129. pOH - the measure of [OH-] in a solution, measure of "alkalinity"
130. self-ionization of water - two water molecules produce a hydronium ion and a hydroxide ion by transfer of a proton
131. neutralization - the reaction of hydronium ions and hydroxide ions to form water molecules and a salt
132. amphoteric - any species that can react as either an acid or a base
133. endpoint - the point in a titration at which an indicator changes color
134. standard solution - the solution that contains the precisely known concentration of the solute; the "known" solution
135. titration - the controlled addition and measurement of the amount of a solution of known concentration to react completely with a measured amount of a solution of unknown concentration
136. equivalence point - the point at which two solutions used in a titration are present in chemically equivalent amounts
137. thermochemistry - the study of the transfers of energy as heat that accompany chemical reactions and physical changes
138. temperature - a measure of the average kinetic energy of the particles in a sample of matter
139. calorimeter - instrument used to measure the energy absorbed or released as heat in a chemical reaction and physical changes
140. enthalpy change - the amount of energy absorbed/released by a system as heat during a process at constant pressure
141. thermochemical equation - an equation that includes the quantity of energy released or absorbed as heat during that reaction as written
142. joule - the SI unit of heat as well as other forms of energy
143. entropy - a measure of the degree of randomness/disorder of the particles, such as molecules in a system
144. entropy change - a measure of the difference between entropy of the products and the reactants
145. free energy - the energy available to do work
146. free energy change - the difference between the enthalpy and the product of the Kelvin temperature, and the entropy change at constant temperature and pressure
147. activated complex - a transitional structure that results from an effective collision and that persists while old bonds are breaking and new bonds are forming
148. reaction rate - the change in concentration of the reactants per unit of time as the reaction proceeds
149. reaction mechanism - the step-by-step sequence of reactions by which the overall chemical change occurs
150. intermediate - species that appear in some steps but not in the net equation
151.chemical equilibrium - a reversible reaction that occurs when the rate of its forward reaction equals the rate of its reverse reaction and the concentration of the products and the reactants remain unchanged
152. equilibrium constant - the ratio of the mathematical product of the concentrations of substances formed at equilibrium to the mathematical product of the concentrations of reacting substances; each concentration is raised to a power equal to the coefficients of that substance
153. acid ionization constant- constant for a specified temperature but has a new value for each new temperature
154. Le'Chatelier's Principle - states if a system at equilibrium is subjected to a stress, the equilibrium is shifted in the direction that tends to relieve the stress
155. solubility product constant - is the product of the molar concentration of its ions in a saturated solution, each raised to the power that is the coefficient of that ion in the balanced chemical equation.
156. anion hydrolysis - salts formed from weak acids and its strong conjugate base react with water to produce solutions that are basic
157. cation hydrolysis - salts formed from weak bases and its strong conjugate acid react with water to produce solutions that are acidic
158. oxidation - processes in which the atoms or ions of an element experience an increase in oxidation numbers due to electron loss
159. oxidized - refers to what happens to a species whose oxidation number increases
160. reduction - processes in which the atoms or ions of an element experience a decrease in oxidation numbers due to electron gain
161. reduced - refers to what happens to a species whose oxidation number decreases
162. oxidizing agent - a substance that has the potential to cause another substance to be oxidized (gains e-)
163. reducing agent - a substance that has the potential to cause another substance to be reduced (loses e-)
164. Disproportionation - a process in which a substance acts as both an oxidizing and reducing agent; self-oxidizing and self-reducing
165. half-reaction - the part of the reaction involving oxidation or reduction alone; overall equation is the sum of the two reactions