Words you must know for the final
Chapters 8 Vocabulary (Covalent bonding)
Sections 1-2
1. Bond dissociation energy: The energy required to break the bond between
two covalently bonded atoms
2. Bond length: The distance between two bonded atoms at their minimum
potential energy
3. Coordinate covalent bond: A covalent bond in which one atom contributes
both bonding electrons
4. Covalent bond: A bond resulting from the sharing of electron pairs
between two atoms
5. Diatomic molecule: A molecule consisting of two atoms
6. Double covalent bond: A bond formed by sharing two pairs of electrons
7. Lewis structures: An indicator in which atomic symbols represent nuclei
and inner-shell electrons, dot-pairs or dashes between two atomic
symbols represent electron pairs in covalent bonds, and dots adjacent to
only one atomic symbol represent unshared electrons
8. Molecular compound: A chemical compound whose simplest units are
molecules
9. Molecular formula: The chemical formula of a molecular compound
10. Molecule: A neutral group of atoms joined together by covalent bonds
11. Polyatomic ion: A positive or negative charged group of covalently bonded
atoms behaving as an unit
12. Resonance structure: A structure that occurs when it is possible to write
two or more valid electron dot formulas that have the same number of
electron pairs for a molecule or ion
13. Structural formula: A formula representing the covalent bonds by dashes
and shows the arrangement of covalently bonded atoms (the same thing
as Lewis structures)
14. Triple covalent bond: A bond formed by sharing three pairs of electrons
15. Unshared pair: The lone pair or nonbonding pair of valence electrons
Sections 3-4
1. Bonding orbital: A molecular orbital that can be occupied by two electrons
of a covalent bond
2. Dipole: Opposite charges that are equal and separated by a short distance
3. Dipole interactions: Forces that occur when polar molecules are attracted
to one another
4. Dispersion forces: The weakest of all molecular interactions, caused by
the movement of electrons, and can also be called London forces
5. Hybridization: The mixing of 2 or more atomic orbitals to produce new
hybrid (changed) atomic orbitals
6. Hydrogen bonds: Forces that hold molecules containing hydrogen
together
7. Molecular orbitals: A model showing atomic overlap when two atoms
combine and applies to the entire molecule
8. Network solids: A solid in which all of the atoms are covalently bonded to
each other
9. Nonpolar covalent bond: Bonding electrons are shared equally by the
bonded atoms, resulting in a balanced distribution of electrical charge
10. pi bond: A bond formed when two atomic orbitals combine and are not
symmetrical forming shapes above and below the bond axis
11. Polar covalent bond: Bonded atoms have an unequal attraction for the
shared electrons
12. Polar molecule: When one end of a molecule is slightly negative and the
other end is slightly positive
13. sigma bond: A bond formed when two atomic orbitals combine to form a
molecular orbital that is symmetrical around the axis connecting two
atomic nuclei, denoted σ
14. Tetrahedral angle: Angles that for 109.5° angles in the geometric shape of
the molecule
15. Van der Waals forces: Forces both dipole and dispersion that are the
weakest attractions between molecules
16. VSEPR theory: When electron pairs repel to take positions to maximize
separation and minimize repulsions
Chapters 9 Vocabulary (Chemical Names and Formulas)
16. Acid: A compound that contains one or more hydrogen atoms and
produces H+ when dissolved in water
17. Base: An ionic compound that produces hydroxide ions when dissolved in
water
18. Binary compound: A compound composed of two elements and can be
either ionic or molecular
19. Empirical formula: The symbols for the elements combined in a
compound, with subscripts showing the smallest whole-number mole ratio
of the different atoms in the compound
20. Law of definite proportions: In samples of any chemical compound, the
masses of the elements are always in the same proportions
21. Law of multiple proportions: Whenever the same two elements form more
than one compound, the different masses of one element that combine
with the same mass of the other element are in the ratio of small whole
numbers
22. Monatomic ions: Ions consisting of a single atom with a positive or
negative charge resulting from the loss or gain of one or more valence
electrons, respectively
23. Nomenclature: The naming of binary compounds
24. Oxidation numbers: The number of electrons that must be added or
removed from an atom in a combined state to convert the atom into the
elemental form
25. Polyatomic ions: Ions composed of more than one atom covalently
bonded
26. Stock system: Uses a Roman numeral to indicate an ion’s charge when
naming chemical ions in a compound
Chapters 10 Vocabulary (Chemical Quantities)
27. Avogadro’s hypothesis: Equal volumes of gases at the same temperature
and pressure contain equal numbers of particles
28. Avogadro’s number: A word representation for the number 6.022 X 10 23
29. Drug testing: A test to identify an abused substance in the body
30. Empirical formula: A ratio giving the lowest whole-number ratio of the
atoms in a compound
31. Gas chromatography: Separates a chemical mixture and identifies its
components using retention time readings
32. Mass spectrometry: Separates a chemical mixture and identifies its
components bases on the components masses
33. Molar mass: The mass of a mole of an element
34. Molar volume: The volume occupied by 1 mole of a gas at standard
temperature and pressure
35. Mole: A unit for measuring the amount of a substance by specifying the
number of particles where 1 mol equals 6.022 X 1023
36. Percent composition: The number of grams of the element divided by the
mass in grams of the compound, multiplied by 100%
37. Representative particle: The species present in a substance, usually
atoms, molecules, or formula units
38. Standard temperature and pressure: A substance having the temperature
0°C and a pressure of 1 atmosphere (atm)
Chapters 11 Vocabulary (Chemical Reactions)
Get Definitions from Blue Modern Chemistry Book Chapter 8
39. Activity Series: A list of elements organized according to the ease with
which the elements undergo certain chemical reactions
40. Chemical equation: A representation with symbols and formulas, the
identities and relative molecular or molar amounts of the reactants and
products in a chemical reaction
41. Coefficient: A small whole number that appears in front of a formula in a
chemical equation
42. Combustion reaction: A reaction when a substance combines with oxygen,
releasing a large amount of energy in the form of light and heat
43. Decomposition reaction: A reaction when a single compound undergoes a
reaction that produces two or more simpler substances
44. Double-displacement reaction: A reaction when the ions of two
compounds exchange places in an aqueous solution to form two new
compounds
45. Electrolysis: The decomposition of a substance by an electric current
46. Formula equation: A representation of the reactants and products of a
chemical reaction that only meets 2 of 3 requirements for a correct
chemical equation
47. Precipitate: A solid that is produced as a result of a chemical reaction in
solution and that separates from the solution
48. Products: The resulting substances of a chemical reaction
49. Reactants: The original substances of a chemical reaction
50. Reversible reaction: A chemical reaction in which the products re-form the
original reactants
51. Single-displacement reaction: A reaction when one element replaces a
similar element in a compound
52. Synthesis reaction: A reaction when two or more substance combine to
form a new compound
53. Word equation: An equation in which the reactants and products in a
chemical reaction are represented by words
Chapters 14 Vocabulary (Behavior of Gases)
54. Boyle’s law
55. Charles’s law
56. Combined gas law
57. Compressibility
58. Dalton’s law of partial pressures
59. Diffusion
60. Effusion
61. Gay-Lussac’s law
62. Graham’s law of effusion
63. Ideal gas
64. Ideal gas constant
65. Ideal gas law
66. Partial pressure
67. Real gas