Quarterly 4 review Flashcards
1
Q
(Ch 1) chemistry is the study of the …, …, and … of matter and the changes that matter undergoes
A
composition; structure; properties
2
Q
(Ch 1) a chemical is any substance that has a
A
definite composition or is used or produced in a chemical process
3
Q
(Ch 1) basic research is carried out for the sake of
A
increasing knowledge
4
Q
(Ch 1) applied research is carried out to
A
solve practical problems
5
Q
(Ch 1) technological development involves the use of existing knowledge to
A
make life easier or more convenient
6
Q
(Ch 1) all matter has … and …
A
mass; takes up space
7
Q
(Ch 1) mass is one measure of the
A
amount of matter
8
Q
(Ch 1) chemical properties refer to a substance’s ability to
A
undergo changes that alter its composition and identity
9
Q
(Ch 1) an element is composed of one kind of
A
atom
10
Q
(Ch 1) compounds are made from two or more
A
elements in fixed proportions
11
Q
(Ch 1) all substances have characterisitc properties that enable chemists to tell the
A
substances apart and to separate the substances
12
Q
(Ch 1) physical changes do not involve changes in
A
identity of a substance
13
Q
(Ch 1) the three major states of matter are
A
solid, liquid, and gas
14
Q
(Ch 1) changes of state, such as melting and boiling, are
A
physical changes
15
Q
(Ch 1) in a chemical change (chemical reaction) the
A
identity of the substance changes
16
Q
(Ch 1) energy changes accompany
A
physical and chemical changes
17
Q
(Ch 1) energy may be released or absorbed, but it is neither
A
created nor destroyed
18
Q
(Ch 1) matter can be classified into
A
mixtures and pure substances
19
Q
(Ch 1) each element has a
A
unique symbol
20
Q
(Ch 1) the periodic table shows the elements organized by their
A
chemical properties
21
Q
(Ch 1) columns on the table respresent .. or … of elements that have similar …
A
groups; families; chemical properties
22
Q
(Ch 1) properties vary across the rows, or
A
periods
23
Q
(Ch 1) the elements can be classified as …, …, …, and …
A
metals, nonmetals, metalloids, noble gases
24
Q
(Ch 1) these classes occupy different areas of the periodic table. metals tend to be, …., …, and … and tend to be good….
A
shiny; malleable; ductile; conductors
25
(Ch 1) nonmetals tend to be ... and tend to be poor..
brittle; conductors
26
(Ch 1) metalloids are intermediate in properties between .. and ...., and they tend to be ... of electricity
metals; nonmetals; semiconductors
27
(Ch 1) the noble gases are generally
unreactive elements
28
(Ch 1) extensive properties depend on the amount of matter that is
present
29
(Ch 1) intensive properties do not depend on the
amount of matter present
30
(Ch 1) a physical property is a characteristic that can be observed or measured without changing the
identity of the substance
31
(Ch 1) a chemical proeprty relates to a substance's ability to undergo changees that transform it into
different substances
32
(ch 2) the scientific method is a logical approach to
solving problems that lend themselves to investigation
33
(ch 2) a hypothesis is a testable statemtn that serves as the
basis for predictions and further experiments
34
(ch 2) a theory is a broad generalization that explains a body of
known facts or phenomena
35
(ch 2) the result of nearly every measurement is a
number and a unit
36
(ch 2) the SI system of measurement has seven base units:
```
meter (length)
kilogram (mass)
second (time)
kelvin (temperature)
mole (amount of substance)
ampere (electric current)
candela (luminous intensity)
```
37
(ch 2) weight is a measure fo the
gravitational pull on matter
38
(ch 2) derived Si units include the ... and the ...
square meter (area); cubic meter (volume)
39
(ch 2) density is the ratio of
mass to volume
40
(ch 2) conversion factors are used to convert from
one unit to another
41
(ch 2) accuracy refers to the closeness of a measurement to the
correct or accepted value
42
(ch 2) precision refers to the closeness of values for a
set of measurements
43
(ch 2) percentage error is the difference between the experimental and the accepted value that is
divided by the accepted value and then multiplied by 100
44
(ch 2) the significant figures in a number consist of all digits known with certainty plus
one final digit, which is uncertain
45
(ch 2) after addition or subtraction, the answer should be rounded so that it has no more digits to the right of the decimal point that there are in the measurement that has the
smallest number of digits to the right of the decimal point
46
(ch 2) after multiplication or division, the answer should be rounded so that it has no more significant figures than there are in the measurement that has
the fewest number of significant figures
47
(ch 2) exact conversion factors are completely certain and do not limit the number of
digits in a calculation
48
(ch 2) a number written in scientific notation is of the form ... in which M is greater than or equal to 1 but less than 10 and n is an integer
M x 10^n
49
(ch 2) two quantities are directly proportional to each other if dividing one by the other
yields a constant value
50
(ch 2) two quantities are inversely proportional to each other if their product has a
constant value
51
(ch 2) a system is a specific portion of matter in a given region of space that has been selected for study
during an experiment or observation
52
(ch 2) a model in science is more than a physical object; it is often an explanation of how phenomena occur and how
data or events are related
53
(ch 2) a quantity is something that has
magnitude, size, or amount
54
(ch 2) dimensional analysis is a mathematical technique that allows you to use units to
solve problems involving measurements
55
(ch 3) john dalton proposed a scientific theory of atoms that can still be used to explain
properties of most chemicals today
56
(ch 3) matter and its mass cannot be ... or .... in chemical reactions
created; destroyed
57
(ch 3) the mass ratios of the elements that make up a given compound are always the ..., regardless of how much of the compound there ... or how it ...
same; is; was formed
58
(ch 3) if two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element can be expressed as
a ratio of small whole numbers
59
(ch 3) cathode-ray tubes supplied evidence of the existence of
electrons
60
(ch 3) electrons are negatively charged subatomic particles that have relatively
little mass
61
(ch 3) rutherford found evidence for the existence of the atomic nucleus by bombarding gold foil with a
beam of positively charged particles
62
(ch 3) atomic nuclei are composed of ..., which have an electric charge of ..., and (in all but one case) neutrons, which have .. electric charge
protons; +1; no
63
(ch 3) atomic nuclei have radii of about ...., and atoms have radii of about ...
.001 pm; 40-270 pm
64
(ch 3) the atomic number of an element is equal to the number of
protons of an atom of that element
65
(ch 3) the mass number is equal to the total number of protons and neutrons that make up the
nucleus of an atom of that element
66
(ch 3) the relative atomic mass unit (amu) is based on the ... atom and is a convenient unit for measuring the ... of atoms
carbon-12; mass
67
(ch 3) the average atomic mass of an element is found by calculating the .... of the atomic masses of the naturally occuring ... of the element
weighted average; isotopes
68
(ch 3) avogadro's number is equal to approximately.... a sample that contains a number of particles equal to Avogadro's number contains a ... of those particles
6.022 x 10^23; mole
69
(ch 3) atom is the smallest particle of an element that retains the
chemical properties of that element
70
(ch 3) nuclear forces are short range ..., ...., and ... forces that hold the nuclear particles ...
proton-neutron, proton-proton, and neutron-neutron; together
71
(ch 3) isotopes are atoms of the same element that have
different masses
72
(ch 3) nuclide is a general term for a specific
isotope of an element
73
(ch 3) a mole is the amount of a substance that contains as many particles as there are atoms in exactly
12 g of carbon-12
74
(ch 3) molar mass is the mass of ... of a pure substance
one mole
75
(ch 4) in the early 20th century, light was determined to have a dual
wave-partticle nature
76
(ch 4) quantum theory was developed to explain observations such as the ... and the .... of hydrogen
photoelectric effect; line-emission spectrum
77
(ch 4) quantum theory states that electrons can exist only at specific
atomic energy levels
78
(ch 4) when an electron moves from one main energy level to a main energy level of lower energy, a .... is emitted. the ... energy equals the energy difference between ....
photon; photon's; the two levels
79
(ch 4) an electron in an atom can move from one main energy level to a higher main enrgy level only by absorbing an amount of energy exactly equal to the
difference between the two levels
80
(ch 4) electrons were determined to have a dual
wave-particle nature
81
(ch 4) the heisenberg uncertainty principle states that it is impossible to determine simultaneously the ... and ... of an ... or any other ...
velocity; position; electron; particle
82
(ch 4) quantization of electron energies is a natural outcome of othe .... which describes the properties of an atom's ...
Schrodinger wave equation; electrons
83
(ch 4) an orbital, a....., shows the regin in space where an electron is most likely to be ...
3d region around the nucleus; found
84
(ch 4) the four quantum numbers that describe the properties of electrons in atomic orbitals are the:
principal quantum number
angular momentum quantum number:
magnetic quantum number
spin quantum number
85
(ch 4) the ground-state electron configuration of an atom can be written by using the:
aufbau principle
hund's rule
pauli exclusion principle
86
(ch 4) electron configurations can be depicted by using different types of notation such as:
orbital notation
electron-configuration notation
noble-gas notation
87
(ch 4) electron configurations of some atoms, such as Cr, deviate from the predictions of the Aufbau principle, but the ground-state configuration that results is the configuration with the
minimum possible energy
88
(ch 4) electromagnetic radiation: form of energy that exhibits
wavelike behavior as it travels through space
89
(ch 4) electromagnetic spectrum formed by
all forms of electromagnetic radiation
90
(ch 4) wavelength: the distance between corresponding points on
adjacent waves
91
(ch 4) frequency: defined as the number of waves that pass a given point in a
specific time, usually one second
92
(ch 4) photoelectric effect: emission of electrons from a metal when
light shines on the metal
93
(ch 4) quantum of energy is the minimum quantity of energy that can be
lost or gained by an atom
94
(ch 4) photon: particle of electromagnetic radiation having
zero mass and carrying a quantum of energy
95
(ch 4) ground state: lowest ... of an atom
energy state
96
(ch 4) excited state: a state in which an atom has a higher ... than it has in its ....
potential energy; ground state
97
(ch 4) continuous spectrum: emission of a continuous range of
frequencies of electromagnetic radiation
98
(ch 4) principal quantum number: n, indicates the main
energy level occupied by electron
99
(ch 4) angular momentum quantum number, l, indicates the
shape of the orbital
100
(ch 4) magnetic quantum number, m, indicates the orientation of an
orbital around the nucleus
101
(ch 4) spin quantum number has only two possible values (+1/2, -1/2) which indicate the two fundamental
spin states of an eelctron in an orbital
102
(ch 4) aufbau principle: an electron ocupies the lowest-energy
orbital that can receive it
103
(ch 4) pauli exclusion principle: no two electrons in the same atom can have the same
set of four quantum numbers
104
(ch 4) hund's rule: orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singlyu occupied orbitals must have
the same spin state
105
(ch 5) the periodic law states that the physical and chemical properties of the elements are
periodic functionso ftheir atomic numbers
106
the periodic table is an arrangement of the elements in order of their atomic numbers so that elements with simialr properties
fall in the same column
107
(ch 5) the columns in the periodic table are referred to as
groups
108
(ch 5) the rows in the periodic table are called
periods
109
(ch 5) many chemical properties of the elements can be explained by the configurations of the
elements' outermost electrons
110
(ch 5) the nobel gases exhibit unique chemical stability because their highest occupied levels have an
octet of electrons, ns^2np^6
111
(ch 5) based on the electron configurations of the elements, the periodic table can be divided into four blocks:
s, p, d, and f
112
(ch 5) the groups and periods of the periodic table display general trends in following proterties:
electron affinity; electronegativity; ionization energy; atomoic radius; ionic radius
113
(ch 5) the electrons in an atom that are available to lost, gained, or shared in the formation of chemical compounds are
valence electrons
114
(ch 5) in determining the electron configuration of an ion, the order in which electrons are removed from the atom is the reverse of the order given by the
atom's electron-configuration notation
115
(ch 5) lanthanides are 14 elements with atomic numbers from
58 to 71
116
(ch 5) actinides are 14 elements with atomic numbers from
90 to 103
117
(ch 5) alkali metals:
group 1
118
(ch 5) alkaline-earth metals:
group 2
119
(ch 5) transition elements: d-block elements with typical
metallic properties
120
(ch 5) main-group elements:
p-block and s-block elements
121
(ch 5) halogens:
group 17
122
(ch 5) atomic radius: 1/2 distance between
nucei of identical atoms that are bonded
123
(ch 5) ion: an atom or group of bonded atoms that has a
postive/ negative charge
124
(ch 5) ionization: any process that results int he formation of
an ion
125
(ch 5) ionization energy: energy required to remove
one electron from a neutral atom of an element
126
(ch 5) electron affinity: energy change that occurs when an electron is
acquired by a neutral atom
127
(ch 5) cation:
positive ion
128
(ch 5) anion:
negative ion
129
(ch 5) electronegativity: measure of the ability of an atom in a chemical compound to attract
electrons from another atom in the compound
130
(ch 6) most atoms are ... to other atoms
chemically bonded
131
(ch 6) the three major types oc hemical bonding are
ionic, covalent, and metallic
132
(ch 6) in general, atoms of metals bond ionically with atoms of
nonmetals
133
(ch 6) atoms of metals bond metallically with
each other
134
(ch 6) and atoms of nonmetals bond
covalently with each other
135
(ch 6) atoms in molecules are joined by
covalent bonds
136
(ch 6) in a covalent bond, two atoms share
one or more pairs of electrons
137
(ch 6) the octet rule states that many chemical compounds tend to form bonds so that each atom shares or has
eight electrons in its highest occupied energy level
138
(ch 6) bonding within many molecules and ions can be indicated by a
lewis structure
139
(ch 6) molecules or ions that cannot be correctly represented by a single Lewis structure are represented by
resonance structures
140
(ch 6) an ionic compound is a 3d network of
cations and anions mutually attracted to each other
141
(ch 6) ionic compounds tend to be harder and more brittle and to have higher ... than materials containing only ....
boiling points; covalently bonded atoms
142
(ch 6) the "electron sea" formed in metallic bonding gives metals their properties of .... and ... conductivity, ..., ..., and ...
high electrical; thermal; malleability; ductility; luster
143
(ch 6) vsepr theory is used to predic tthe ... of molecules based on the fact that electron pairs strognly
shape; strongly repel each other
144
(ch 6) hybridization theory is used to predict the shapes of molecules based on the fact that orbitals within an atom can
mix to form orbitals of equal energy
145
(ch 6) intermolecular forces include ... and ...
dipole-dipole forces; london dispersion forces
146
(ch 6) hydrogen bonding is a special case of
dipole-dipole forces
147
(ch 6) chemical bond: mutual electrical attraction between nuclei and valence electrons of
different atoms that binds the atoms together
148
(ch 6) ionic bonding: chemical bonding that results from electrical attraction between
cations and anions
149
(ch 6) covalent bonding: sharing of electron pairs between
two atoms
150
(ch 6) nonpolar-covalent bond: covalent bond in which bonding electrons are shared equally by the bonded atoms, resulitng in a balanced
distribution of electrical charge
151
(ch 6) a polar-covalent bond is a covalent bond in whicht he bonded atoms have an
unequal attraction for the shared electrons
152
(ch 6) molecule: neuttral group of atoms that are held together by
covalent bonds
153
(ch 6) molecular compound: chemical compound whose simplest units are
molecules
154
(ch 6) chemical formula: indicates relative numbers of atoms of each kind in a chemical compound by using
atomic symbols and numerical subscripts
155
(ch 6) molecular formula: shows types and numbers of atoms combined in a single molecule of a
molecular ompound
156
(ch 6) bond energy: energy required to ... a chemical bond and form...
break; neutral isolated atoms
157
(ch 6) structural formula: indicates..., ..., ..., and /... but not the unshared pairs of the atoms in a molecule
kind; number; arrangement; bonds
158
(ch 6) single bond: covalent bond in which one pair of electrons is shared between
two atoms
159
(ch 6) multiple bonds:
deouble and triple bonds
160
(ch 6) formula unit: simplest collection of atoms from which an ionic compound's formula can be
established
161
(ch 6) lattice enrgy: energy released when one mole of an ionci crystalline compound is
formed from gaseous ions
162
(ch 6) polyatomic ion: charged group fo
covalently bonded atoms
163
(ch 6) metallic bonding: chemical bonding that results from the attraction betweern ... and the surrounding...
metal atoms; sea of electrons
164
(ch 6) malleability: ability of a substance to be ... or ...
hhammered; beaten into sheets
165
(ch 6) ductility: ability of substance to be ..,..., or .... through a small opening to produce a wire
drawn; pulled; extruded
166
(ch 6) hybrid orbitals: orbitals of equal energy produced by the combination of two or more
orbitals on the same atom
167
(ch 6) dipole is created by equal but opposite charges that are
separated by a short distance
168
(ch 6) hydrogen bonding: intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an ubnshared pair of electrons of an
electronegative atom in a nearby molecule
169
(ch 6) london dispersion forces: intermolecular attractions resulting fromt he cosntant motion of electrosn and the creation fo
instantaneous dipoles
170
(ch 7) positive monatomic ion is identified simply by the name of the
appropriate element
171
(ch 7) a negative monatomic ion is named by dropping parts of the ending of the element's name and adding
-ide to the root
172
(ch 7) the charge of each ion in an ionic comjpound may be used to determine the simplest
chemical formula for the compound
173
(ch 7) binary compounds are composed of
two elemetns
174
(ch 7) binary ionic compounds are named by combining the names of the
positive and negative ions
175
(ch 7) the old system of naming binary molecular compounds uses
prefixes
176
(ch 7) the new system, known ans the Stock system, uses
oxidation numbers
177
(ch 7) oxidation numbers are useful in ..., writing..., and in ....
naming compounds; formulas; balancing chemical equations
178
(ch 7) compounds containing elements that have more than one oxidation state are named by using the
stock system
179
(ch 7) stock-system names and prefix-system names are used... for many molecular compounds
interchangeably
180
(ch 7) oxidation numbers of each element in a compound may be used to determine the compound's simplest
chemical formula
181
(ch 7) by knowing oxidation numbers, we can name compounds without knowing whether theya re
ionic or molecular
182
(ch 7) ...,..., and ... cnan be calculated form the chemical formula for a compound
formula mass, molar mass, percentage composition
183
(ch 7) percentage composition of a compound si the percentage by mass of each
element in the compound
184
(ch 7) molar mass is used as conversion factor between amojunt in moles and mass in grams of a given
compound/ element
185
(ch 7) an empirical formula shows the simplest whole number ratio of
atoms in a given compound
186
(ch 7) empirical formulas indicate how many atoms of each elemnt are combined in the simplest
unit of a chemical compound
187
(ch 7) a molecular formula can be found from the empirical formula if the
molar mass is measured
188
(ch 7) oxyanion: polyatomic ions that
contian oxygen
189
(ch 7) salt: an ionic compound composed of a ... and the ... from an acid
cation; anion
190
(ch 7) oxidation state: assiged to the atoms composing the
compound or ion
191
(ch 7) formula mass: sum of the average atomic masses of
all atoms represented in the formula
192
(Ch 8) four observations that suggest a chemical reaction is taking place are the
evolution of energy as heat and light
production of gas
change in color
formation of a precipitate
193
(Ch 8) a balanced chemical equation represents, with symbols and formulas, the identities and relative amoutns of
products in a chemical reactio
194
(Ch 8) synthesis rections equation:
A+X→AX
195
(Ch 8) decomposition reaction equation
AX→A + X
196
(Ch 8) single-displacement reactions represented by two equation:
A + BX→AX + B
| Y + BX→BY + X
197
(Ch 8) double diosplacement reaction equatio
AX + BY→AY + BX
198
(Ch 8) in a combustion reaction, a substance combines with..., realsing energy in the form of ... and ...
oxygen; heat; light
199
(Ch 8) activity series list the elements in order of their chemical reactivity and are useful in predicting wither a
chemical reaction will occur
200
(Ch 8) chemists determine activity series through
experiments
201
(Ch 8) precipitate: a solid that is produced as a result of a chemical reaction in solution and that
separates from the solutio
202
(Ch 8) coefficient: small whole number that ppears in front of a
formula in a chemical equation
203
(Ch 8) word equation: an equation in which the reactants and products in a chemical reactiona represented by
words
204
(Ch 8) formula equation: represents reactants and products of a chemical reaction by their
symbols or formulas
205
(Ch 8) electrolysis: decomposition of a substance by an
electric current
206
(ch 9) reaction stoichiometry involves the mass relationships between
reactants and products in a chemical reaction
207
(ch 9) relating one substance to another requires expressing the amount of each
substance in moles
208
(ch 9) a mole ratio is the conversion factor that relates the amount in ... of any two substances in a ...
moles; chemical reaction
209
(ch 9) the mole ratio is derived from the
balanced equation
210
(ch 9) amount of a substance is expressed in...., and mass of a substance is expressed by using mass units such ass..., ..., or ...
moles; grams; kilograms; milligrams
211
(ch 9) mass and amount of substance are.., wherars moles and grams are ...
quantities; units
212
(ch 9) a balanced chemical equation is necessary to solve any
stoichiometric problem
213
(ch 9) in an ideal stoichiometric calculation, the mass or the amount of any reactnat or product can be calculated if the .... and the ... or ... of any other reactant or product is known
balanced chemical equation; mass; amount
214
(ch 9) in actual reactions, the reactants may be present in proportions that differ from the stoichiometric proportions required for a complete reaction in which all of
each reactant is converted to product
215
(ch 9) the limiting reactant controls the .... of product formed
maximum possible amount
216
(ch 9) for many reactions, the quantity of a product is less than the
theoretical maximum for that product
217
(ch 9) percentage yield shows the relationship between the ... and ... for the product of a reaction
theoretical yield; actual yield
218
(ch 9) composition stochiometry: deals with the mass relationships of
elements in compounds
219
(ch 9) excess reactant: substance that is not
used up completely in a reaction
220
(ch 9) theoretical yield: maximum amount of product that can be produced from a
giv en amount of reactant
221
(ch 9) actual yield: measured amount of a product obtained from a
reaction
222
(ch 10) the kinetic-molecular theory of matter can be used to explain the properties of
gases, liquids, and solids
223
(ch 10) the kinetic-molecular theory of gases describes a model of an
ideal gas
224
(ch 10) gases consist of large numbers of tiny, fast-moving ... that are ... relative to their sized
particles; far apart
225
(ch 10) particles of a liquid are ... and more ... than those of a gas and are less ... than those of a solid
closer together; ordered; ordered
226
(ch 10) liquids have a definite ... and a fairly high ..., and they are relatively ....
volume; density; incompressible
227
l(ch 10) like gases, liquids can .. and are thus considered to be ...
flow; fluids
228
(ch 10) the particles of a solid ar enot nearly as free to ... as those of a liquid or gas
move about
229
(ch 10) solids have a definite .. and may be ... or ...
shape; crystalline; amorphous
230
(ch 10) solids have a definite ... and are generally non...
volume; nonfluid
231
(ch 10) a crystal structure is the total 3d array of ... that describes teh arrangement of the ..
.points; particles of a crystal
232
(ch 10) unlike crystalline solids, amorphous solids do not have a highly.... or a regular...
ordered structure; shape
233
(ch 10) a liquid in a closed system will gradually reach a... as the rate at which molecules ... equals the rate at which they...
liquid-vapor equilibrium; condense; evaporate
234
(ch 10) when two opposing changes occur at equal rates in the same closed system, nthe system is said to be in
dynamic equilibrium
235
(ch 10) water is a
polar covalent compound
236
(ch 10) the structure and the hydrogen bonding in water are responsible for its relatively high...., molar ....., ....., and molar....
melting point; enthalpy of fusion; boiling point; enthalpy of vaporization
237
(ch 10) ideal gas: hypothetical gas that perfectly fits all the assumptions of the
kinetic-molecular theory
238
(ch 10) elastic collision: one in which there is no net loss of
total kinetic energy
239
(ch 10) diffusion: result of the spontaneous ... of the particles of two substances caused by their....
mixing; random motion
240
(ch 10) effusion: process by which gas particles pass through a
tiny opening
241
(ch 10) real gas: a gas that does not behave completely according to the assumptions of the
kinetic-molecular theory
242
(ch 10) fluid: substance that can ... and therefore take the ... of of its container
flow; shape
243
(ch 10) surface tension: force that tends to pull adjacent parts of aliquid's surface ..., thereby decreasign
together; surface area to the smallest possible size
244
(ch 10) capillary action: attraction of the surface of a liquid to the s
surface of a solid
245
(ch 10) vaporization: process by which a liquid or solid
changes to a gas
246
(ch 10) evaporation: process by which particles escape from the surface of a nonboiling liquid and
enter the gas state
247
(ch 10) freezing/ solidification: physical change of a liquid to a solid by
removal of energy as heat
248
(ch 10) crystalline solids: consist of
crystals
249
(ch 10) amorphous solid: one in which the particles are
arranged randomly
250
(ch 10) meltin: physical change of a solid to a liquid by the addition of
nergy as heat
251
(ch 10) melting point: temperature at which a solid
becomes a liquid
252
(ch 10) supercooled liquids: substances that retain certain liquid properties even at
temperatures at which they appear to be solid
253
(ch 10) crystal: a substance in which the particles are arranged in an
orderly, geometric, repeating pattern
254
(ch 10) unit cell: the smallest portionof a crystal lattice that shows the
3d pattern of the entire lattice
255
(ch 10) phase; any part of a system that has
uniform composition and properties
256
(ch 10) condensation: process by which a gas changes to a
liquid
257
(ch 10) equilibrium: dynamic condition in which two opposing changes occur at
equal rates in a closed system
258
(ch 10) equilibrium vapor presssure: pressure exerted by a vapor in equilibrium with its
corresponding liquid at a given temeprature
259
(ch 10) volatile liquids: liquids that
evaporate readily
260
(ch 10) boiling: conversion of a liquid to a vapor within the liquid as well as
at its surface
261
(ch 10) boiling point: temeprature at which the equilibrium vapor pressure of the liquid equals
the atmospheric pressure
262
(ch 10) molar enthalpy of vaporization: amount of energy as heat that is needed to vaporize on mole of liquid at the liquid's
boiling point at constant pressure
263
(ch 10) freezing point: temperature at whicht eh solid and liquid are in
equilibrium at 1 atm
264
(ch 10) molar enthalpy of fusion: amount of energy as heat required to melt one mole of
solid at the soldi's melting pint
265
(ch 10) sublimation: change of state from a solid directly to a
gas
266
(ch 10) deposition: change of state from a gas directly to a
solid
267
(ch 10) phase diagram: graph of pressure versus temperature that shows the conditions under whicht he
phases of a substance exist
268
(ch 10) triple point: indicates the temeprature and pressure conditions at which the solid, liquid, and vapor of the substance can
coexist at equilibrium
269
(ch 10) critical point: indicates the critical
temperature and critical pressure
270
(ch 10) critical temperature: temperature above which the substance cannot exist in the
liquid state
271
(ch 10) critical pressure: lowest pressure at which the substance can exist as a liquid at the
critical temperature
272
(ch 11) kinetic moleculr teory of gases describes an
ideal gas
273
(ch 11) the behvior of most gases is nearly ideal except at very
high pressures and low temperatures
274
(ch 11) a barometer measures
atmospheric pressure
275
(ch 11) dalton's law of partial pressure states that in a mixture of unreacting gases, the total pressure equals the sum of the
partial pressures of each gas
276
(ch 11) boyle's law states the inverse relationship between the volume and pressure of a gas:
PV=k
277
(ch 11) charles law illustrates the direct relationship between a gas's ... and its ... in kelvins:
volume; temperature
| V=kT
278
(ch 11) gay-lussac's law represents the direct relationshjip betrween a gas's ... and its ... in kelvins:
pressure; temperature
| P=kT
279
(ch 11) the combined gas law combines boyle's, charles's, and gay-lussac's law into this epression:
PV/ T=k
280
(ch 11) gay-lussac's law of combining volumes states that the volumes of recting gases and their products at the same temperature and pressure can be expressed as
ratios of whole numbers
281
(ch 11) avogadro's law states that equal volumes of gases at the same temperature and pressure contain
equal numbers of molecules
282
(ch 11) the volume occupied by one mole of an ideal gas at STP is called the ..., which ...
standard molar volume; 22.414 L
283
(ch 11) charles's law, Boyle's law, and Avogadro's law can be bombined to create the ideal gas law:
PV=nRT
284
(ch 11) gases diffuse, or become morespread out, due to their
constant random molecular motion
285
(ch 11) graham's law of effusion states that the relative rates of effusion of gases at the same temperature and pressurea re inversely proportional to the
square roots of their molar masses
286
(ch 11) pressure is defined as the force per
unit area on a surface
287
(ch 11) newton: force that will increase the speed of a 1 kilogram mass by one meter per second each second that the
force is applied
288
(ch 11) millimeters of mercury: common unit of
pressure
289
(ch 11) atmosphere of pressure: exactly equivalent to
760 mm Hg
290
(ch 11) pascal: the pressure exerted by a force of one ... acting on an area of one
newton; square meter
291
(ch 11) partial pressure: pressure of each
gas in a mixture
292
(ch 11) absolute zero: teh temperature ..., given a value of ... in the kelvin scale
-273.15 C; zero
293
(ch 11) ideal gas constant: the constant ..., with balues of ... atm and .... kPa
R; .082 atm; 8.314 kPa
294
( ch 12) solutions are
homogenous mixtures
295
( ch 12) mixtures are classified as:
solutions
suspensions
colloids
296
( ch 12) the way mixtures are classified depends on the ... of the solute particles in the mixture
size
297
( ch 12) the dissolved substance is the
solute
298
( ch 12) solutions that have water as a solvent are
aqueous solutions
299
( ch 12) solutions can consist of solutes and solvents that are
solids, liquids, or gases
300
( ch 12) suspensions settle out upon
standing
301
( ch 12) colloids do not settle out, and they scatter
light that's shined through them
302
( ch 12) most ionic solutes and some molecular solutes form aqueous solutions that conduct an electric current:
electrolytes
303
( ch 12) nonelectrolytes are solutes that dissolve in water to form
solutions that do not conduct
304
( ch 12) a solute dissolves at a rate that depends on the ... of the solute, how vigorously the solution is.., and the ... of the solvent
surface area; mixed; temperature
305
( ch 12) the solubility of a substance indicates how much of that substance will dissolve in a specified amount of solvent under
certain conditions
306
( ch 12) the solubility of a substance depends on the
temeprature
307
( ch 12) the solubilityof gases in liquids increases with icreases in
pressure
308
( ch 12) the solubility of gases in liquids decreases wtih
increases in temperature
309
( ch 12) the overall energy absorbed as heat by the system when a specified amount osf solute dissolved during solution formation is caleld the
enthalpy of solution
310
( ch 12) two useful expressions of concentration are
molarity and molality
311
( ch 12) the molar concentration of a solution represents the ratio fo moles of solute to
liters of solutio
312
n( ch 12) the molal concentration of a solution represents the ratio fo moles of solute to
kilograms of solvent
313
( ch 12) soluble: capable of being
dissolved
314
( ch 12) solvent: dissolving
medium
315
( ch 12) solution equilibrium: physical state in which the opposing processes of ... and ... of a solute occur at equal rates
dissolution; crystallization
316
( ch 12) saturated solution: a solution that contains the maximum amount of
dissolved solute
317
( ch 12) unsaturated solution: solution that contains less solute than a
saturated solution under same conditions
318
( ch 12) supersaturated solution: contains more dissolved solute that a saturated solution contains under the
same conditions
319
( ch 12) hydration: solution process with water as the
solvent
320
( ch 12) immiscible: liquids that are nto
soluble in each other
321
( ch 12) miscible: liquids that dissolve freely in one another in any
proportion
322
( ch 12) henry's law: solubilityof a gas in al iquid is directly proportional to the partial pressure of that gas on the
surface of the liquid
323
( ch 12) effervescence: rapid escape of a gas from a liquid in which it is
dissovled
324
( ch 12) solvated: solute particle that is surrounded by
solvent molecules
325
( ch 12) enthalpy of solution: the net amount of energy absorbed as heat by the solution when a specific amount of
solute dissolves in a solvent
326
( ch 12) concentration: measure fo the amount of solute in a given amount of
solvent or solution
327
In general, the atomic radii of the main-group elements... down a group
increase
328
In general, ionization energies of the main-group elements ... across each period.
increase
329
Among the main-group elements, ionization energies generally... down the groups;
decrease
330
Ionic radii: cationic radii ...across a period
decrease
331
anionic radii ....across each period
decrease
332
there is a gradual ...of ionic radii down a group
increase
333
electronegativities tend to ...across each period, although there are exceptions;
increase
334
electronegativities tend to either ...down a group or remain about the same
decrease
