Download Chemistry University: C1

MEANINGS
TERMS
1. an orbital lower in energy than the atomic orbitals of which it
is composed. (14.2)
A. Addition reaction:
2. an atom with more than one electron. (12.11)
B. Aldehyde:
3. an equivalence statement between units used for converting
from one unit to another. (A2.2)
C. Atomic radius:
4. the study of carbon-containing compounds (typically chains
of carbon atoms) and their properties. (22)
D. Bonding molecular orbital:
5. the force exerted on an object by gravity.
E. Bonding pair:
6. a type of particle accelerator in which a changing electric field
is used to accelerate a positive ion along a linear path. (21.3)
F. Glass:
7. an organic compound containing the carbonyl group bonded
to at least one hydrogen atom. (22.4)
G. Kinetic energy:
8. the process by which a substance goes directly from the solid
to the gaseous state without passing through the liquid state.
(16.10)
9. (-^ mv2) energy resulting from the motion of an object;
dependent on the mass of the object and the square of its
velocity. (9.1)
10. the square root of the average of the squares of the
individual velocities of gas particles. (5.6)
H. Lanthanide contraction:
11. a reaction in which atoms add to a carbon-carbon multiple
bond. (22.2)
K. Model (theory):
12. the potential energy of a particular nucleus as compared
with the sum of the potential energies of its component protons
and neutrons. (21.1)
13. the decrease in the atomic radii of the lanthanide series
elements, going from left to right in the periodic table. (20.1)
L. Organic chemistry:
14. the change in the number of radioactive nuclides in a
sample per unit time. (21.2)
N. Polyelectronic atom:
15. half the distance between the nuclei in a molecule
consisting of identical atoms. (12.15)
O. Rate of decay:
16. an amorphous solid obtained when silica is mixed with other
compounds, heated above its melting point, and then cooled
rapidly. (16.5)
17. an electron pair found in the space between two atoms.
(13.9)
P. Root mean square velocity:
18. a model that assumes that a molecule is composed of
atoms that are bound together by sharing pairs of electrons
using the atomic orbitals of the bound atoms. (13.9)
19. 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. (1.3)
20. the SI unit of pressure; equal to newtons per meter squared.
(5.1)
R. Thermodynarnic stability (nuclear):
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I. Linear accelerator:
J. Localized electron (LE) model:
M. Pascal:
Q. Sublimation:
S. Unit factor:
T. Weight:
MEANINGS
TERMS
1. an organic molecule that contains one or more elements in
addition to carbon and hydrogen. (22.4)
A. Avogadro's number.
2. atoms of the same element (the same number of protons)
with different numbers of neutrons. They have identical atomic
numbers but different mass numbers. (2.6)
3. a device for measuring the pressure of a gas in a container.
(5.1)
B. Beta-particle production:
4. One mole represents 6.022 X 1023 units. (3.2)
D. Equilibrium (thermodynamic
definition):
5. the SI unit of pressure; equal to newtons per meter squared.
(5.1)
E. Formal charge:
6. the two parts of an oxidation-reduction reaction, one
representing oxidation, the other reduction. (4.11;11.1)
F. Half-reactions:
7. a neutral molecule or ion having a lone pair of electrons that
can be used to form a bond to a metal ion; a Lewis base. (20.3)
G. Heat of vaporization:
8. the energy required to vaporize one mole of a liquid at a
pressure of one atmosphere. (16.10)
H. Hess's law:
9. in going from a particular set of reactants to a particular set of
products, the enthalpy change is the same whether the reaction
takes place in one step or in a series of steps; in summary,
enthalpy is a state function. (9.5)
10. a radioactive nuclide, introduced into an organism for
diagnostic purposes, whose pathway can be traced by
monitoring its radioactivity. (21.4)
11. radioactive damage to an organism resulting in its sickness
or death. (21.7)
I. Hydrocarbon derivative:
12. a nuclear reactor in which fissionable fuel is produced while
the reactor runs. (21.6)
L. Ligand:
13. the position where the free energy of a reaction system has
its lowest possible value. (10.11)
M. Manometer:
14. the average distance a molecule in a given gas sample
travels between collisions with other molecules. (5.6; 5.9)
N. Mean free path:
15. the certain digits and the first uncertain digit of a
measurement. (A1.5)
O. Partial pressures:
16. the resistance of a liquid to an increase in its surface area.
(16.2)
P. Pascal:
17. the charge assigned to an atom in a molecule or polyatomic
ion derived from a specific set of rules. (13.12)
Q. Radiotracer:
18. a decay process for radioactive nuclides in which the mass
number remains constant and the atomic number changes. The
net effect is to change a neutron to a proton. (21.1)
19. the independent pressures exerted by different gases in a
mixture. (5.5)
R. Significant figures:
20. energy can be converted from one form to another but can
be neither created nor destroyed. (9.1)
T. Surface tension:
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C. Breeder reactor:
J. Isotopes:
K. Law of conservation of energy:
S. Somatic damage:
MEANINGS
TERMS
1. an equation representing a reaction in solution showing the
reactants and products in undissociated form, whether they are
strong or weak electrolytes. (4.6)
2. an electron pair found in the space between two atoms.
(13.9)
A. Bonding pair:
3. synthetic gas, a mixture of carbon monoxide and hydrogen,
obtained by coal gasification. (9.8)
C. Element:
4. a material that, when dissolved in water, gives a solution that
conducts an electric current very efficiently. (4.2)
D. Fission:
5. the forces, existing among noble gas atoms and nonpolar
molecules, that involve an accidental dipole that induces a
momentary dipole in a neighbor. (16.1)
6. a model whose main postulate is that the structure around a
given atom in a molecule is determined principally by
minimizing electron-pair repulsions. (13.13)
7. an instrument used to determine the relative masses of
atoms by the deflection of their ions in a magnetic field. (3.1)
E. Law of mass action:
8. the study of carbon-containing compounds (typically chains
of carbon atoms) and their properties. (22)
H. Mass spectrometer:
9. a nonmetallic material made from clay and hardened by firing
at high temperature; it contains minute silicate crystals
suspended in a glassy cement. (16.5)
10. a bonded collection of two or more atoms of the same or
different elements. (2.7)
I. Molarity:
11. a U-tube containing an electrolyte that connects the two
compartments of a galvanic cell, allowing ion flow without
extensive mixing of the different solutions. (11.1)
12. the force exerted on an object by gravity.
K. Molecule:
13. an atomic solid containing strong directional covalent bonds.
(16.5)
M. Organic chemistry:
14. in any spontaneous process, there is always an increase in
the entropy of the universe. (10.5)
N. Salt bridge:
15. a substance that cannot be decomposed into simpler
substances by chemical or physical means. (2.1)
O. Scientific method:
16. the percent by mass of a component of a mixture (17.1) or
of a given element in a compound. (3.4)
P. Second law of thermodynamics:
17. the process of studying natural phenomena, involving
observations, forming laws and theories, and testing of theories
by experimentation. (1.3)
18. moles of solute per volume of solution in liters. (4.3; 17.1)
Q. Strong electrolyte:
19. the process of using a neutron to split a heavy nucleus into
two nuclei with smaller mass numbers. (21.6)
S. Valence shell electron-pair repulsion
(VSEPR) model:
20. a general description of the equilibrium condition; it defines
the equilibrium constant expression. (6.2)
T. Weight:
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B. Ceramic:
F. London dispersion forces:
G. Mass percent:
J. Molecular equation:
L. Network solid:
R. Syngas:
MEANINGS
TERMS
1. the vapor pressure of a solution is directly proportional to the
mole fraction of solvent present. (17.4)
A. Activated complex (transition state):
2. the spontaneous rising of a liquid in a narrow tube. (16.2)
B. Alloy:
3. an error that has an equal probability of being high or low.
(A1.5)
C. Atomic radius:
4. the series of elementary steps involved in a chemical
reaction. (15.6)
D. Basic oxide:
5. a given compound always contains exactly the same
proportion of elements by mass. (2.2)
E. Capillary action:
6. a natural high-molecular-weight polymer formed by
condensation reactions between amino acids. (22.6)
F. Ceramic:
7. a substance that contains a mixture of elements and has
metallic properties. (16.4)
G. Endpoint:
8. a condition occurring when more than one valid Lewis
structure can be written for a particular molecule. The actual
electronic structure is not represented by any one of the Lewis
structures but by the average of all of them. (13.11)
9. an instrument that measures the rate of radioactive decay
based on the ions and electrons produced as a radioactive
particle passes through a gas-filled chamber. (21.4)
10. the process of transforming N3 to nitrogen-containing
compounds useful to plants. (19.2)
H. Geiger-Muller counter (Geiger
counter):
11. an ionic oxide that dissolves in water to produce a basic
solution. (18.4)
K. Monodentate (unidentate) ligand:
12. one or more assumptions put forth to explain the observed
behavior of nature. (1.3)
L. Nitrogen fixation:
13. the arrangement of atoms found at the top of the potential
energy barrier as a reaction proceeds from reactants to
products. (15.8)
14. an atom with more than one electron. (12.11)
M. Normal melting point:
15. half the distance between the nuclei in a molecule
consisting of identical atoms. (12.15)
O. Protein:
16. the point in a titration at which the indicator changes color.
(4.9)
P. Random error:
17. in any spontaneous process, there is always an increase in
the entropy of the universe. (10.5)
Q. Raoult's law:
18. the temperature at which the solid and liquid states have the
same vapor pressure under conditions where the total pressure
on the system is one atmosphere. (16.10)
19. a nonmetallic material made from clay and hardened by
firing at high temperature; it contains minute silicate crystals
suspended in a glassy cement. (16.5)
20. a ligand that can form one bond to a metal ion. (20.3)
R. Reaction mechanism:
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I. Hypothesis:
J. Law of definite proportion:
N. Polyelectronic atom:
S. Resonance:
T. Second law of thermodynamics:
MEANINGS
TERMS
1. a spectrum showing only certain discrete wavelengths. (12.3)
A. Antibonding molecular orbital:
2. the interaction between solute particles and water molecules.
(4.1)
B. Atomic number:
3. a thermodynamic function that measures randomness or
disorder. (10.1)
C. Ball-and-stick model:
4. a ligand that can form one bond to a metal ion. (20.3)
D. Ceramic:
5. a species that is neither a reactant nor a product but that is
formed and consumed in the reaction sequence. (15.6)
E. Entropy:
6. the enthalpy change that occurs to melt a solid at its melting
point. (16.10)
F. Haber process:
7. an organic molecule that contains one or more elements in
addition to carbon and hydrogen. (22.4)
G. Heat of fusion:
8. an orbital higher in energy than the atomic orbitals of which it
is composed. (14.2)
H. Hydration:
9. a compound that results when a metal reacts with a nonmetal
to form a cation and an anion. (13.1)
I. Hydrocarbon derivative:
10. quantities of reactants mixed in exactly the correct amounts
so that all are used up at the same time. (3.9)
J. Intermediate:
11. the manufacture of ammonia from nitrogen and hydrogen,
carried out at high pressure and high temper-ature with the aid
of a catalyst. (3.9; 6.1; 19.2)
12. the number of equivalents of a substance dissolved in a liter
of solution. (17.1)
K. Ionic compound (binary):
13. the separation and identification of individual ions from a
mixture. (4.7; 8.9)
M. Molality:
14. the number of moles of solute per kilogram of solvent in a
solution. (17.1)
N. Monodentate (unidentate) ligand:
15. the proportionality constant in the relationship between
reaction rate and reactant concentrations. (15.2)
O. Normality:
16. a molecular model that distorts the sizes of atoms, but
shows bond relationships clearly. (2.7)
P. Qualitative analysis:
17. the number of protons in the nucleus of an atom. (2.6)
Q. Rate constant:
18. a nonmetallic material made from clay and hardened by
firing at high temperature; it contains minute silicate crystals
suspended in a glassy cement. (16.5)
19. the certain digits and the first uncertain digit of a
measurement. (A1.5)
R. Significant figures:
20. a reaction step involving only one molecule. (15.6)
T. Unimolecular step:
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L. Line spectrum:
S. Stoichiometric quantities: