Semester Exam Review Flashcards
(296 cards)
1
Q
which SI prefix means “one million” or 10^6?
A
mega-
2
Q
which SI prefix means “one billionth” ore 10^-9
A
nano-
3
Q
which SI prefix means “one millionth” or 10^-6?
A
micro-
4
Q
meters in a kilometer
A
1000
5
Q
a millimeter is what fraction of a meter?
A
1/1000
6
Q
centimeters in a meter
A
100
7
Q
a lowercase letter m is the symbol of which SI prefix
A
milli-
8
Q
symbol for the prefix centi-
A
c
9
Q
carbon
A
C
10
Q
chlorine
A
Cl
11
Q
aluminum
A
Al
12
Q
hydrogen
A
H
13
Q
oxygen
A
O
14
Q
iron
A
Fe
15
Q
potassium
A
K
16
Q
sodium
A
Na
17
Q
calcium
A
Ca
18
Q
neon
A
Ne
19
Q
Cu
A
copper
20
Q
Ag
A
silver
21
Q
Si
A
silicon
22
Q
He
A
helium
23
Q
Zn
A
zinc
24
Q
Co
A
cobalt
25
U
uranium
26
Pb
lead
27
Hg
mercury
28
F
fluorine
29
subatomic particle of the atom that has no electric charge
neutron
30
phenomenon that consists of electrons flowing between electrodes in a vacuum tube
cathode rays
31
type of particle that nucleons are believed to be made of
quarks
32
if there is a + after an element, than there will one ______________ electron than proton
LESS
33
equation to determine number of neutrons in an element
N= A (top number) - Z (lower number)
34
proposed the planetary model of the atom
Rutherford
35
experiment used to determine the electron's charge
oil-drop experiment
36
this value is the number of nucleons in an atom
mass number
37
atoms of the same element that have different numbers of nucleons
isotopes
38
the prefix deca- in a molecular formula indicates that ___________ atoms of that element are present in each molecule
10
39
hepta-
7
40
nona-
9
41
octa
8
42
compound consisting of two nitrogen atoms and four oxygen atoms is named
dinitrogen tetroxide
43
compound consisting of two nitrogen atoms and five oxygen atoms
dinitrogen pentoxide
44
compound consisting of a carbon atom and four fluorine atoms is named
carbon tetrafluoride
45
compound consisting of a sulfur atom and six fluorine atoms is
sulfur hexafluoride
46
diphosphorus tetraiodide
P2 I4
47
diiron hexachloride
Fe2 Cl6
48
hydroxide
OH-
49
nitrate
NO3-
50
chlorate
ClO3-
51
ammonium
NH4+
52
bicarbonate
HCO3-
53
sulfate
SO4 2-
54
carbonate
CO3 2-
55
iron (III)
Fe 3+
56
silicate
SiO3 2-
57
phosphate
PO4 3-
58
the principle requiring that chemical reactions be balanced is the law of conservation of
mass
59
a symbolic representation of a chemical reactions is a
chemical equation
60
when writing a chemical reaction, the _________ are on the left and the _____________ are on the right
reactants- left
products- right
61
A + B -----> AB
combination reaction
62
AB -------------> A + B
decomposition reaction
63
AB + CD ----------------> AD + CB
double-displacement reaction
64
AB + C --------------> A + BC
single-displacement reaction
65
According to Boyle's law, if the pressure upon a gas INCREASES, the volume will
decrease (indirect proportioned)
66
According to Charle's law, if the temperature of a gas is INCREASES, the volume will
increase (direct proportioned)
67
if the temperature of a gas is increases while its volume remains constant, its pressure will
increase
68
in the ideal gas law, the constant R is the ___________
universal gas constant
69
According to _________________ law, equal volumes of gases at the same temperature and pressure have the same number of molecules
Avogadro's law
70
the acronym STP stands for
standard temperature and pressure
71
the molar volume of an ideal gas under STP conditions is about
22.4 L/mol
72
law that says that when gases react the volumes of reactants and products are in small, whole-number ratios
Gay-Lussac's Law
73
the number of this type of particle identifies an atom as a given element
protons
74
type of chemist that would most likely study alcohols, which consist of carbon, hydrogen, and oxygen
organic chemist
75
indicates a chemical change
1. change in color
2. formation of gas
3. formation of precipitate
76
group of two or more atoms linked together by chemical bonds
molecule
77
relative charge of an electron
-1
78
developed the atomic theory of matter
John Dalton
79
a homogenous part of a system that is in contact with but physically distinct from other parts of the system
phase
80
a measure of the force of gravity upon an object is
weight
81
as the internal kinetic energy of a substance increases, the substance's temperature
INCREASES
82
the discovery of the nucleus and the development of the planetary model of the atom were results of the
gold-foil experiment
83
the smallest particles into which a compound may be broken down without changing it into another substance are
molecules
84
the general term for techniques of separating liquids based on their boiling points is
distillation
85
an ion that 3 protons, 4 neutrons, and 2 electrons is a
cation
86
best explanation as to why liquid becomes a gas at the boiling point
the kinetic energy of the particles is great enough to overcome their attraction of each other
87
term refers to the ration of an object's mass to its volume
density
88
refers to energy that is possessed by matter due to its motion
kinetic
89
which of the three main particles composing that atom has the smallest mass
electron
90
value of Avogadro's number
6.022 x 10^23
91
if the empirical formula of a substance is known, what additional information is needed to calculate the molecular formula
molar mass
92
unit that is equivalent to Avogadro's number of objects
molle
93
set of symbols that tells how many of each type of atom are found in a molecule
formula
94
sum of the atomic masses of all the atoms in a molecule
mass
95
the smallest particles into which an element may be broken down without changing the identity of the element
atoms
96
1 millimeter of mercury is equal to
1 torr
97
number of protons in an atom
atomic number
98
standard atmosphere equals
760 torr
99
the isotope that the atomic mass unit is relative to
carbon-12
100
standard pressure and temperature
273.15 K and 760 torr
101
number of atoms in exactly one mole of atoms
6.022 x 10^23
102
the instrument used to measure atmospheric pressure
barometer
103
amount of force exerted upon a surface per unit area is
pressure
104
in the ___________ state of matter, particles have enough energy to move freely but not enough energy to overcome their attraction for each other
liquid
105
how closely a measured value matches the actual value is
accuracy
106
the dense central portion of an atom is called the
nucleus
107
the link between the microscopic and the macroscopic levels of chemistry is
Avogadro's number
108
which law implies that at constant temperature and pressure, the molar volume of an ideal gas is constant
Avogadro's law
109
negatively charged subatomic particles in an atom
electrons
110
the type of energy associated with motion is called
kinetic energy
111
the type of energy associated with the position of an object relative to the forces upon it is known as
potential energy
112
in thermodynamics, the portion of the universe of the sample of matter being studied is referred to as the
system
113
according to the first law of thermodynamics, the change in internal energy is the sum of
heat and work
114
the SI unit of work and energy
joule
115
the thermodynamic function denoted by the symbol H, which takes into account internal energy (E), volume (V), and pressure (P), is
enthalpy
116
a chemical reaction that can be summarized by the formula
reactants + heat ----------------------> products is an
endothermic equation
117
reactants--------------------> products + heat
exothermic reaction
118
heat required to raise the temperature of a unit mass of a substance by a unit temperature is the
specific heat
119
device in which energy changes during a chemical reaction may be measured is the
calorimeter
120
the highest or peak point on a wave is the wave's
crest
121
the distance between any two corresponding points on successive waves is the
wavelength
122
the number of complete waves that pass by a point in a given time is the wave's
frequency
123
individual "bundles" or quanta of light energy are called
photons
124
an arrangement of all forms of electromagnetic radiation in order of frequency and wavelength
electromagnetic spectrum
125
SI unit of frequency
Hertz
126
height of the wave
amplitude
127
the particle theory of light was first propsed by
Isaac Newton
128
the amount of energy an individual quantum of light contains depends on its
frequency
129
the speed of light in a vacuum is approximately
3.00 x 10^8 m/s
130
quantum number that describes the orientation of an orbital in space
magnetic quantum number (ml)
131
quantum number describes the shell in which an electron is located
principal quantum number (n)
132
states that no two electrons in the same atom have the same four quantum numbers
Pauli exclusion principle
133
states that a single electron occupies each orbital within a subshell before electrons begin pairing
Hund's rule
134
specifies the order in which subshells fill with electrons
aufbau principle
135
type of orbital that has a spherical shape
s
136
the second shell from the center of an atom can hold up to ______________ electrons
8
137
the complete arrangement of electrons in an atom is the atom's
electron configuration
138
the outermost electrons which are involved in chemical reactions
valence electrons
139
how many electrons are in the 2p subshell of a nitrogen atom?
1s^2 2s^2 2p^3
3
140
the energy required to remove an electron from an atom
ionization energy
141
describes how strongly a chemically combined atom draws electrons to itself
electronegativity
142
which are larger, simple cations or the neutral atoms from which they were formed?
neutral atoms
143
periodic trend: decreases down, increases across
ionization energy, electron affinity, electronegativity
144
periodic trend: increases down, decreases across
atomic radii, metallic character
145
refers to the randomness of a substance or system
entropy
146
internal energy of a system plus the product of its pressure and volume
enthalpy
147
energy is commonly defined as
the ability to do work
148
device used to measure heat flow during physical processes or chemical reactions
calorimeter
149
the change in a system's internal energy is the sum of the heat added to the system and the work done on the system is the ____________ law of thermodynamics
1st
150
chemical and physical changes that release heat are known as
exothermic processes
151
the field of chemistry that deals with the energy changes in chemical reactions is chemical
thermodynamics
152
chemical reactions and physical changes that absorb heat are known as
endothermic processes
153
type of energy associated with position relative to a force is
potential energy
154
an endothermic reaction is characterized by ______________ change in enthalpy
positive
155
the enthalpy of formation for any element in its standard state is
0
156
when a cup of water evaporates into water vapor, the entropy change in the system is
positive
157
at constant pressure, enthalpy change equals
heat
158
the heat per unit mass required to vaporize a substance at its normal boiling point is
heat of vaporization
159
the total amount of heat liberated or absorbed because of a chemical reaction
heat of reaction
160
the heat per unit mass required to melt a substance at its normal melting point
heat of fusion
161
the amount of heat required to cause a unit rise in temperature of a unit mass of a substance
specific heat
162
individual packets of light energy
photons
163
amplitude of wave is the measure of its
strength
164
if the wavelength of a light wave decreases, how must its frequency change
increase
165
light consists of
electromagnetic waves
photons
166
developed the periodic table of the elements
Mendeleev
167
unit wave frequency is measured in
hertz
168
the lines in the hydrogen spectrum represent
photons emitted as electrons drop from higher to lower energy levels
169
consists of elements that usually exist as 2+ ions
alkaline earth metals
170
the lowest energy state of an atom
ground state
171
the elements in column 1 are the
alkali metals
172
the elements in column 2 are the
alkaline earth metals
173
the elements in column 17 are the
halogens
174
the elements in column 18
noble gases
175
elements in columns 1, 2, and 13-18 are all classified as
main-group elements
176
probable formula for the bromide of beryllium
1234321 (Br= 1; Be= 2) therefore BeBr2
177
not an alkali metal
calcium
178
when an element is vaporized and heated in a flame or an electric arc, the light emitted forms a
line spectrum
179
characterized by the transfer of electrons from one atom to another
ionic bond
180
characterized by the sharing of a "sea" of delocalized electrons among many atoms
metallic bond
181
produces substances that are characteristically malleable and ductile
metallic bond
182
bond in which cations are attracted to anions
ionic bond
183
states that atoms tend to react to achieve a noble-gas electron configuration
octet rule
184
unequal sharing of electrons produces a
polar bond
185
a bond that involves sharing of four electrons
double covalent bond
186
a bonding situation in which electrons are shared by more than two atoms is known as
delocalization
187
electrons that circulate freely through a molecule instead of being bound to a single atom or pair of atoms are said to be
delocalized (resonant)
188
a molecule that has a symmetrical distribution of polar covalent bonds will be ______________ as a whole
nonpolar
189
a formula in which nonbonding electrons are shown as dots around atoms and bonds are shown as lines or dots between atoms is a
Lewis structure
190
tetrahedral
4 bonds
0 nonbonds
polar or nonpolar
191
trigonal pyramidal
3 bonding
1 nonbonding
always polar
192
trigonal planar
3 bonding
0 nonbonding
polar or nonpolar
193
angular
2 bonding
2 nonbonding
always polar
194
linear
1 or 2 bonding
0 nonbonding
polar or nonpolar
195
why one group would be polar and the other not
arranged symmetrically vs. asymmetrically
196
superior system of measurement because of its divisibility
metric system
197
metric unit of mass
kilogram
198
metric unit of length
meter
199
10^-3
milli-
200
temperature scale for scientific measurement
Kelvin
201
makes numbers more manageable
scientific notation
202
numbers that are always significant
1-9
203
most abundant state of matter in the universe
plasma
204
smallest whole/complete particle
atoms
205
subatomic particles
proton (+)
electron (-)
neutron
206
chemical grouping of different types of atoms
compounds
207
mixture that is the same throughout
homogenous
208
mixture that is different throughout
heterogenous
209
change in state of matter
physical change
210
burn wood
chemical change
211
boil water into gas
physical change
212
processes used to separate mixture
distillation, chromatography
213
discovered the electrons
Thompson
214
discovered proton
Rutherford
215
discovered the neutron
Chadwick
216
shows number of protons
atomic number (Z)
217
the sum of neutrons and protons
mass number (A)
218
average mass of all isotopes
atomic mass
219
two types of chemical formulas
molecular, empirical
220
1 mole of substance =
Avogadro's number
221
chemical changes caused by collisions between atoms/ molecules
chemical reaction
222
reactants on the ______________
products on the ______________
left
right
223
the reactant giving the smallest amount of production is the
limiting reactant
224
solid to liquid
heat of fusion
225
absorbs heat; cold to touch
endo-
226
product; releases energy
exo-
227
increases entropy
exothermic
228
reverse processes that don't seem natural
spontaneity
229
states you can't simultaneously know position and momentum of an electron
uncertainty principle
230
3D regions of probability
orbitals
231
2D pathway
orbit
232
tells chem properties and where the electrons are located
electron configuration
233
V and T are _______________ related
directly
234
units of pressure
pascal, torr atmosphere
235
measures pressure but does not require fluid
aneroid barometer
236
standard pressure
1 atm, 760 torr
237
measure pressure of gas sample
monometer
238
P and V are inversely related at constant T
Boyle's Law
239
T and V are directly related at constant P
Charle's law
240
temperature scale needed for the gas laws
Kelvin
241
constant T, P, V
Avogadro's law
241
small whole number ratios
Gay-Lusac's law
242
1 mole of gas at STP =
22.4 L
243
combines Boyle, Charles, and Avogadro's law
ideal gas law
244
PVnRT
n= number of moles
R= universal gas constant (o.0821 L x atm/K x mol
245
mixing of gas by random molecular motion
diffusion
246
states that the heavier the gas the slower the rate of diffusion
Graham's law of diffusion
247
states that the total pressure of gas = sum of all individual parts of pressure
Dalton's law of partial pressure
248
1 calorie =
4.184 J
249
states that energy of the unierse is conserve
1st law of thermodynamics
250
total heat energy content of the system
enthalpy
251
exothermic has _ enthalpy
negative
252
a negative change in enthalpy is in ________________ in entropy
increase
253
specific heat of water
4.18 J/g x C
254
when the word heat is added
thermochemical equation
255
in fusion and vaporization, the _____________ does not change; the _________________ changes the ______________
temperature not change
energy changes state
256
Gibbs free energy helps determine
spontaneity
257
delta G is 0
equilibrium
258
-delta G
spontaneous
259
+ delta G
nonspontaneous
260
at a constant speed, wavelength and frequency are
inverse
261
max displacement
amplitude
262
particle theory of light
Newton
263
wave theory of light
Huygens
264
wave-particle duality
Einstein
265
electromagnetic waves
Maxwell
266
causes light to be emitted in LINE spectrum
excited and dropped to ground state
267
Bohr's model proposed
energy levels
268
Schrodinger model
wave-mechanical model
269
Born's Model
electron-cloud model
270
subshel shapes
s, p, d, f
271
determines the number of valence electrons
group
272
filling up from lowest to highest
aufbau
273
high EN
high ability to pull electrons to self
274
hydrogen bonded to _______ _____________ or __________ makes it a hydrogen bond
N, O, F
275
strongest intermolecular force
hydrogen bond
276
weakest intermolecular force; occurs in all atoms, molecules etc
London forces
277
present when molecules are polar; EN
dipole-dipole force
278
bonding present when greater than 1.7
ionic
279
bonding present when less than 1.7
covalent
280
determines type of bonding
electronegativity difference
281
only elements that do not require 8 valence electrons
hydrogen H
helium HE
282
states that nonbonding pairs have more force than bonding
VSEPR (valence-shell electron-pair repulsion)
283
Atoms will tend to react chemically so as to achieve a noble-gas electron configuration, either by losing or gaining electrons with other atoms
Octet rule
284
How do ionic and covalent bonds differ in the electron rearrangements involved?
Ionic bonding- electrons transferred
Covalent bonding- electrons shares
285
Why do covalent networks such as diamond and silicon carbide tend to be very hard?
Billions and trillions of atoms are joined into one unit by strong covalent bonds.
286
Primary difference between covalent and metallic bonding—
Covalent bonding involves the sharing of electrons
Metallic bonding involves the sharing of delocalized electrons among large number of atoms
287
Type of covalent bond that forms a dipole
Polar bond
288
How is resonance indicated when drawing Lewis structures?
Double-headed arrows between Lewis structures
289
How does an intermolecular force differ from a chemical bond?
Intermolecular forces physically attract molecules to each other without transfer or sharing of electrons
Chemical bonds chemical bond atoms into compounds through the transfer or sharing of electrons
290
What is the difference between crystalline and amorphous solids at the molecular level? How does this affect the properties of the substances?
Crystalline solid has particles arranged in a regular and repeated 3D pattern; definite melting point
Amorphous solids have no ordered arrangement or pattern for the particles that compose it; has not definite melting point.
291
Three main types of cubic unit cells
Body-centered cubic
Face-centered cubic
Simple unit cell
292
Cubic close packing
Face-centered cubic
293
The bcc’s atoms has ________ identical neighbors
8
294
The fcc’s and hcp’s atoms have _____________ identical neighbors
12
295
The simplest repeating unit in a crystal is called the
Unit cell
