What should you never change when balancing a chemical equation?

product subscripts and reactant subscripts

What must be equal for an atom to have no net or a neutral charge?

number of protons and electrons

What does VSEPR stand for?

valence shell electron pair repulsion

which of the following is true about an orbital?

hold at most 2 electrons and they must be of opposite spins

which of these processes can be used to accomplish desalination?

reverse osmosis and distillation

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Chemistry Multiple Choice Flashcards | StudBud

Chemistry Multiple Choice

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Questions 370

Answers

1
What are the units for molarity?
moles/kg
liters/mole
milliliters/mol
moles/liter
2
a neutral alkaline metal loses an electron, what type of electron configuration does it have?
alkaline metal
halogen metal
alkaline earth metal
noble gas
3
among fundamental atomic properties what is best indicator element behaves as metal or nonmetal
electron configuration
first ionization energy
atomic radius
electron affinity
4
Name of the phenomena by DeBroglie that proposed that electrons exhibit wave like properties
photoelectric effect
radial electron density
electromagnetic waves
matter waves
5
Which of these molecules do not have an sp³ hybrid orbital?
BF3
NH3
H2O
CH4
6
What should you never change when balancing a chemical equation?
product coefficients and reactant coefficients
product subscripts and reactant coefficients
product subscripts and reactant subscripts
product coefficients and reactant subscripts
7
what is the plot of pH of an acid (base) as a function of the volume of added base (or acid)?
pOH titration curve
Kb titrat
pH titration curve
Ka titration curve
8
which of the following is not a primitive lattice structure?
rhombic
octagonal
hexagonal
square
9
What is the name of the symbols used to represent valence electrons in a dot notation called?
Lewis dot notation
Bon-Haber notation
electron valence shell notation
electron force notation
10
at what pressure does the normal boiling point of water occur?
0oC
1 atm
the triple point
the critical pressure
11
What is used to measure the strength of a covalent bond?
bond momentum
bond enthalpy
bond structure
bond polarity
12
What is the name of the SO₄ ion?
sulfite
sulfurous
sulfate
sulfonic
13
which layer is the lowest in the atmosphere?
thermosphere
mesosphere
stratosphere
troposphere
14
How does effective nuclear charge change across the periodic table?
it generally increases
it remains constant
it increases then decreases
it generally decreases
15
what products form because of the reaction of a strong acid and strong base?
salt and water
weak acid and a weak base
water and carbon dioxide
salt and hydrogen gas
16
What must be equal for an atom to have no net or a neutral charge?
number of neutrons and electrons
number of protons and electrons
number of protons and neutrons
number of electrons in eachorbital
17
Which of the following is not a state function?
heat
pressure
internal energy
temperature
18
If the formula weight being calculated is for a molecule, this is called a . . .
molecular weight
tare weight
gross weight
atomic weight
19
Which of the following is the unit used for measuring atomic dimensions?
kg
coulomb
angstrom
amu
20
what is produced in one elementary step, and is consumed in a later elementary step?
a solvent
a spectator ion
an intermediate
a colute
21
what is the general expression relating Kp and Kc?
Kp = λ Kc
Kp = Kc RT (n(products)-n(reactants))
Kp = Kc (RT)^Δn
Kp = Kc nRT
22
Which of the following terms can be used to describe a system?
isolated
open
closed
all of the above
23
particular combination of motions & locations of atoms & molecules of system at particular inst
a macrostate
a state of equilibrium
a microstate
a kinetic state
24
what type of element is silicon?
metalloid
metal
non-metal
free metal
25
which of the following is not a primitive lattice structure?
rhombic
hexagonal
square
octagonal
26
In the isotope nitrogen-14, how many nucleons are present?
6 protons and 8 neutrons
14 protons and 14 neutrons
8 protons and 6 neutrons
7 protons and 7 neutrons
27
What are ions that appear in identical forms on both sides of a complete ionic equation called?
reaction ions
complete ions
incomplete ions
spectator ions
28
what term describes a substance that can function as either a Bronsted-Lowry acid or base?
amphibionic
diacidobasic
bipolar
amphiprotic
29
what are the small molecules that make up polymers called?
dimers
hexamers
trimers
monomers
30
what are layers of porous rock which hold water called?
sponge ponds
water layers
aquifers
lakes
31
The magnitude of interactions with ionic bonding is measured by what type of energy?
lattice energy
covalent energy
potential energy
kinetic energy
32
which type of semi-conductor is doped so there is an excess of electrons in the conduction band
p-type
n-type
s-type
a-type
33
which of the following is not a spectator ion in acid-base chemistry?
I-
Cl-
F-
Br-
34
What is the name given for a series of ions that have the same electric charge called?
isoelectronic series
isodynamic series
isotonic series
isotopic series
35
To which orbital block to the actinide elements belong?
p block
s block
d block
f block
36
what uses a spontaneous oxidation-reduction reaction to generate electricity?
a corrosion cell
an osmotic cell
a galvanic cell
an electrodynamic hybrid cell
37
What does VSEPR stand for?
voltage seconds electron proton repair
valence shell electron pair repulsion
valence suborbital electron proton resonance
valence suborbital electron pair reduction
38
What are rapid reactions which produce a flame called?
Combination reactions
Decomposition reactions
Double replacement reactions
Combustion reactions
39
point in titration where stoichiometrically equivalent quantities are brought together known as
the neutralization point
the equivalence point
the end point
the titration point
40
what is the measure of tendency of a liquid to maintain minimum surface area?
surface volume
surface tension
surface area
surface elasticity
41
what is a substance that donates a proton to another substance called?
a Brondted-Lowry acid
an Arrhenius acid
an ion
a Lewis acid
42
what type of colloids are common in living organisms?
random
hydrophilic
atomic
hydrophobic
43
Rule state lowest energy is attained by maximizing the number of electrons with the same spin
Heisenberg's rule
Hund's rule
Schrodinger's rule
Hess's rule
44
which of the following is true about an orbital?
hold at most 14 electrons and they must be of opposite spins
hold at most 14 electrons and they must be of neutral spins
hold at most 2 electrons and they must be of the same spin
hold at most 2 electrons and they must be of opposite spins
45
which of these processes can be used to accomplish desalination?
mechanical filtering and distillation
mechanical filtering and reverse osmosis
reverse osmosis and distillation
fracking and reverse osmosis
46
Which of the following is an empirical formula for C₁₂H₂₄O₁₈?
C3H8O6
C2H3O4
C2H4O3
C6H12O9
47
what model is used to explain the melting points of transition metals?
conduction valence model
molecular orbital model
electron sea model
lattice amorphous model
48
Which of the following equations denotes a metathesis reaction?
AX + BY + AY → BX
AX → BY + AY + BX
AX + BY → AB + XY
AX + BY → AY + BX
49
A compound is 37.3% by weight carbon. in a 100 g sample what mass is attributed to carbon?
0.627 grams
37.3 grams
0.373 grams
62.7 grams
50
What does the symbol Δ above the arrow mean in a chemical equation?
change in reaction products
change in reaction reactants
addition of heat
the equation can go either direction
51
what elements are used in a standard hydrogen electrode?
zinc and water
hydrogen and platinum
hydrogen and zinc
hydrogen and copper
52
Which for these molecules are non-polar?
HCl
NH3
CCl4
CH3Cl
53
What quantity is denoted by the symbol (delta Hf)?
enthalpy of fusion
enthalpy of formation
enthalpy of fission
enthalpy of friction
54
What is the name given to the process which occurs when a system absorbs heat?
endothermic
exothermic
endocaloric
isothermic
55
Which of the following is a non-metal?
Ag
Al
Fe
Br
56
In an isoelectric series, as charge increases what happens to atomic radius?
it decreases
it increases
it increases then decreases
it remains the same
57
what is a self-contained electrochemical power source that contains one or more voltaic cells?
a geothermal generator
a wind mill
a battery
a photocell
58
How many sigma bonds and how many pi bonds are present in a CO₂ molecule?
1 sigma and 2 pi
2 sigma and 2 pi
2 sigma and 1 pi
1 sigma and 1 pi
59
Which law states that energy is conserved?
the zeroth law of thermodynamics
the second law of thermodynamics
the third law of thermodynamics
the first law of thermodynamics
60
increases when fuel burns and chemical e converts to thermal e increases speed of the particles
potential energy
heat of composition
work of enthalpy
kinetic energy
61
which equation is used to predict the behavior of real gases?
the van der Waals equation
the Kinetic Molecular equation
the ideal gas equation
Graham's Law of Effusion
62
which of the following is not a strong acid?
HF
HI
HBr
HCl
63
What is the energy change that occurs when an electron is added to a gaseous atom called?
electron equillibrium
electron affinity
ionization energy
metallic character
64
what are liquids or solids that can also exist at a gaseous state called?
fumes
steam
ozone
vapors
65
Plants use what reaction to convert sunlight, water and carbon dieoxide into glucose and oxygen
photosynthesis
fermentation
cellular respiration
chemosynthesis
66
What are the units for molarity?
milliliters/mol
moles/liter
moles/kg
liters/mole
67
what type of catalysts typically reacts with molecules by adsorption?
homogeneous
intermediate
liquefaction
heterogeneous
68
What is the atomic number of tungsten?
52
22
74
43
69
what is the name of the property which is characterized by the scattering of light in a colloid
Tyndall effect
Raoult's effect
osmotic effect
hydration effect
70
what is the electrode where oxidation takes place called?
cathode
the neutral electrode
anode
salt bridge
71
What is the most abundant element in the known universe?
Oxygen
Carbon
Helium
Hydrogen
72
which of the following is the correct metric unit for density?
kg/m2
kg-m/sec2
kg/m3
kg/sec
73
What is the term that is used to denote the prefix for a metric unit of 10^-6?
Mega
Kilo
Giga
Micro
74
Which element on the periodic chart has the following electron configuration [At]4s¹?
K
Na
Li
Rb
75
Which group of elements tends to have the highest ionization energy?
alkali metals
alkali earth metals
noble gases
halogens
76
which of the following indicate a spontaneous reaction?
a positive value of E and a positive value of ΔG
a negative value of E and a positive value of ΔG
a positive value of E and a negative value of ΔG
a negative value of E and a negative value of ΔG
77
Which of the following is a sulfate (-2) ion?
SO3
SO2
SO
SO4
78
Which of the following is the correct metric unit for density?
kg/m3
kg/m2
kg/m-sec2
kg/sec
79
which of the following is not soluble in water?
magnesium chloride
silver nitrate
lead chloride
sodium sulfate
80
What is the magnitude of the separation of charge produced called?
a dipole force
a dipole moment
a charge force
a formula charge
81
Which of the following is soluble in water?
FeS
Sr(OH)2
MgCO3
AlPO3
82
what is the energy needed to remove the first electron from a neutral atom called?
first ionization energy
primeionization energy
absorbtion energy
excitation energy
83
What are the centers of charge density for a pi bond?
between the d and f suborbitals
inside the last electron shell
at perpendicular angles to the sigma bonds
above and below the internuclear axis
84
In a thought experiment on uncertainty, Schrodinger used which animal to illustrate his point?
dog
mouse
elephant
cat
85
The molar mass in grams per mole of any substance is numerically equal to what quantity?
The number of protons and neutrons in the nucleus of an atom
Whole number multiplier of the substances empirical formula
The formula weight in atomic mass units
Avogadro's number of molecules
86
Which of the following molecule's Lewis structure is best represented by a resonance structure?
NH4
H2O
NaCl
O3
87
which of the following is not a unit of pressure?
torr
bar
atmosphere
Joule
88
which is the equivalence point for pH titration of a strong acid and strong base?
1
7
5
3
89
the molar mass in grams per mole of any substance is numerically equal to what quantity?
Avogadro's number
the formula weight in atomic mass units
whole number multiplier of the substances empirical formula
the number of protons and neutrons in the nucleus of an atom
90
the slope of a line drawn tangent to the concentration-versus-time curve at a specific time?
instantaneous rate
differential rate
integral rate
average rate
91
which compound can undergo photodissociation in the stratosphere, introducing atomic chlorine?
chlorofleuorocarbons
methane
acid rain
greenhouse gases
92
what is the state of the substance which exists on a phase diagram beyond the critical point?
a subcooled fluid
a plasma
a saturated fluid
a supercritical fluid
93
how does the value of the acid-dissociation constant, Ka related to acid strength?
the larger the value the smaller the pOH
the larger the value the higher the pH
the larger the value the weaker the acid
the larger the value the stronger the acid
94
Planck coined a term for radiation emitted from hot objects, this radiation is called?
ultraviolet radiation
infrared radiation
gamma radiation
blackbody radiation
95
what is the random three dimensional motion of liquid molecules called?
hydrophyllic effect
Brownian motion
tydall motion
henry's law
96
What is the name of the intermediate elements between metals and non-metals?
non-metals
noble metals
semi metals
metalloids
97
which of the following is a chemical change?
adding air to a closed volume
using a Bunsen burner
freezing water at a reduced pressure
pouring nitric acid from a graduated cylinder to a beaker
98
the metal that is oxidized while preventing the cathode in a cathodic protection system is?
the sacrificial cathode
the noble metal
the sacrificial anode
the catalyst
99
what is the equilibria for which substances are in different phases called?
thermal equilibria
heterogeneous equilibria
homogeneous equilibria
isochemical equilibria
100
what is an electron pair receptor called?
a Lewis acid
an ion
a Bronsted-Lowry acid
an Arrhenius acid
101
how does solubility of a compound containing a basic anion (the anion of a weak acid) behave?
increases as the solution becomes more acidic
decreases as the solution becomes more basic
increases as the solution becomes more basic
increases as the solution temperature decreases
102
what are liquids that mix together in all proportions?
immiscible
solvent
miscible
unmiscible
103
which affects speed at which equilibrium is reached &doesnt affect magnitude of equil. constant
reaction reactant concentration
reaction product concentration
a catalyst
reaction temperature
104
Who used an experiment which shot alpha particle into gold foil to determine structure of atom?
Rutherford
Curie
Fermi
Thompson
105
in what reaction do molecules form new linkages by opening existing pi bonds?
vulcanization
substitutional bonding
intermetallic bonding
additon polymerization
106
what units are typically used to express solubility?
kg/mol
g/L
g/mol
g/kg
107
Which two state functions does Gibbs free energy combine?
enthalpy and entropy
pressure and temperature
enthalpy and energy
work and energy
108
Heated BaCO₃ forms BaO and CO₂ gas, which type of reaction does this represent?
Combustion reaction
Decomposition reaction
Combination reaction
Double replacement reaction
109
what should you expect to see on the titration curve of a polyprotic acid?
multiple points where Ka = Kb
pH slowly increase to equivalence point and then decrease
inverese relationship between Ka and pH
multiple equivalence points
110
why do CO₂ bubbles come out of solution when a carbonated beverage is opened?
kinetic energy of the bubbles increase and escape container
the partial pressure above the solution is increased
the partial pressure above the solution is reduced
there is a decrease in osmotic pressure
111
What is the name of a positively charged ion?
anion
neutron
cation
proton
112
How is energy transferred into and out of a system?
heat and work
enthalpy and entropy
kinetic energy and potential energy
composition and decomposition
113
What products form because of the reaction of a strong acid and strong base?
salt and hydrogen gas
salt and water
water and carbon dioxide
weak acid and a weak base
114
A process which occurs at a constant temperature is called
athermal
isothermal
bithermal
equathermal
115
the troposphere and which other layer account for 99.9% of the mass of the atmosphere?
troposphere
thermosphere
stratosphere
mesosphere
116
which group has this electron suborbital configuration ns²p⁶?
the alkali metals
the oxygen group
the halogens
the noble gases
117
which indicator is more suitable for a titration of acetic acid and sodium hydroxide?
methyl blue
bromol blue
phenolphthalein
methyl red
118
which of the following is true regarding the equilibrium-constant expression?
depends only on stoichiometry of reaction not on mechanism
depends only on kinetic energy of reaction not on potential
depends only on potential energy of reaction not on kinetic
depends only on mechanism of reaction not on stoichiometry
119
Heisenberg's uncertainty principle involves what two quantities?
position and momentum
time and space
matter and energy
position and time
120
what consists of atoms held together in large networks by covalent bonds?
molecular solids
covalent network solids
organic solids
intermolecular solids
121
What rule do valence shell electrons tend to follow when gaining or losing electrons?
the hexagonal rule
the triple rule
the octet rule
the quadrilateral rule
122
what is the breaking of bonds in molecules because of the absorption of light called?
photoabsorption
photoionization
photodissociation
photodisintegration
123
What does the first law of thermodynamics state?
matter is conserved
heat is conserved
energy is conserved
work is conserved
124
which of the following is not an intermolecular interaction involved in solution formation?
solute-hydrate
solute-solvent
solute-solute
solvent-solute
125
what are the units of measure for osmotic pressure?
joules/square meter
kilograms-meters/sec
atmospheres
meters
126
oxides that are only slightly soluble in water but dissolve on addition of either acid or base
compound oxides
strong oxides
weak oxides
amphoteric oxides
127
What is the chemical formula for ozone?
O3
O4
O1
O2
128
a substance which is reduced is called?
a catalytic converter
a catalyst
a reducing agent
an oxidizing agent
129
The [Xe]6s² electron configuration is for which element?
Beryllium
Calcium
Magnesium
Barium
130
What is the actual amount of a product actually obtained in a reaction called?
percent yield
actual product
actual yield
theoretical yield
131
according to LeChatelier's principle how does a system react to adding substance at equilibrium
the system increases temperature to consume son of substance
the system reacts to remove some of the substance
the system reacts to consume some of the substance
the system does not react
132
which equation defines the autoionisation constant for water?
Kw = [H3O+]/[OH-]
Kw = [H3O+][OH-]
Kw = -Log[H3O+][OH-]
Kw = [H3O+]+[OH-]
133
Which of the following are motions a molecule can undergo?
vibrational
rotational
translational
all of the above
134
Which of the following diatomic molecules has a triple bond?
H2
F2
O2
N2
135
Which of the following is a chemical change?
Using a Bunsen burner
Adding air to a closed volume
Freezing water at a reduced pressure
Heating a solid until it melts
136
type of force binds molecules together when an ionic compound is dissolved in a polar solvent
dipole-dipole force
hydrogen bond
dispersion force
ion-dipole force
137
What do the letters k and W stand for in Boltzmann's equation: ΔS=k ln W?
k = kinetic energy, W = work
k = temperature in K, W = microstates
k = temperature in K, W = work
k = Boltzmann's constant, W = microstates
138
What is the inherent directionality of most reactions and chemical processes:
lose entropy n 1 direction gain enthalpy n reverse direction
spontaneous one temperature nonspontaneous lower temperature
spontaneous in 1 direction nonspontaneous in other direction
spontaneous in forming products nonspontaneous in reactants
139
What is the piece of laboratory equipment used to perform a titration called?
a burette
a flask
a beaker
a dropper
140
What is the standard Gibbs free energy for an element in its standard state?
-1
6.022E23
+1
0
141
Which phrases best describe potential and kinetic energy?
potential energy is stored energy kinetic energy of motion
potential energy is heat; kinetic energy is work
potential energy is heat out; kinetic energy is heat in
potential energy is endothermic kinetic energy is exothermic
142
In the isotope nitrogen-14, how many nucleons are present?
14 protons and 14 neutrons
6 protons and 8 neutrons
8 protons and 6 neutrons
7 protons and 7 neutrons
143
What is the predicted bond angle in a tetrahedral electron domain geometry?
120o
60o
90o
109.5o
144
Which of the following does not equal a mole?
6.02E23 eggs
44 grams of carbon dioxide
16 grams of oxygen gas
6.02E23 atoms of carbon
145
Which two electron subshells do noble gases have completely filled?
p and d
p and d
f and d
s and p
146
what is adhesion and cohesion of liquids in a narrow tube called?
adhesion
surface tension
capillary action
cohesion
147
which theory accounts for the properties of an ideal gas?
Avogadro's theory
van der Waals theory
kinetic-molecular theory of gas
Avogadro's hypothesis
148
to which orbital block to the actinide elements belong?
p block
f block
d block
s block
149
What is the term that is used to denote the metric unit of mass?
Kelvin
Kilogram
Meter
Mole
150
in which region can only the simplest chemical compounds survive radiation bombardment?
mesosphere
troposhpere
thermosphere
stratosphere
151
What oxidation number does the element form of an atom have?
0
-1
1
-2
152
Which of the following is a chemical change?
freezing water at a reduced pressure
pouring nitric acid from a graduated cylinder
using a Bunsen burner
adding air to a closed system
153
In the solid components of cells which element is the most prevalent by mass?
Carbon
Hydrogen
Silicon
Oxygen
154
This is a measure of the distances separating atoms in their chemical compounds.
valence orbitals
ionization energy
effective nuclear charge
bonding atomic radius
155
on a phase diagram, the point where all three phases of matter occur is called
the end point
the triple point
the saturation point
the critical point
156
What is the rule for multiplication and division of significant digits?
result has atleast same number of sig figs as fewest measure
result has same number of sig figs as measure with fewest
result has same number of sig figs as measure with most
result has atleast same number of sig figs as most measure
157
Every AB₂ molecule has the same molecular geometry shape, what is it?
square planar
bent
trigonal planar
linear
158
What is a molecule whose centers of positive and negative charge do not coincide called?
polar molecule
atomic molecule
non-polar molecule
resonance molecule
159
in which of the following solids are particles arranged in a regularly repeating pattern?
amorphous solid
ionic solid
metallic solid
crystalline solid
160
What determines the optimal distance between nuclei in a covalent bond?
all bond angles are perpendicular
decreasing nuclear orbital overlap
a balance between attractive and repulsive forces
nucleus to nucleus repulsion >0 kJ/mol
161
Which group has this electron suborbital configuration ns2p6?
the halogens
the noble gases
the oxygen group
the alkali metals
162
Which of the following can never be true?
actual yield equals theoretical yield
actual yield greater than the theoretical yield
actual yield minus theoretical yield equal zero
actual yield less than the theoretical yield
163
What is the best indicator of whether an element behaves as a metal or a non-metal?
electron configuration
first ionization energy
atomic radius
electron affinity
164
which model helps explain why magnitudes of rate constants increase with increasing temperature
the rate equilibrium model
the collision model
the Arrhenius model
the ideal model
165
What is the amount of material completely consumed in a reaction called?
the least common product
the limiting product
the limiting reactant
the least common reactant
166
What is the name of the group which has elements that are harder and denser than alkali metals
noble gases
halogens
halides
alkali earth metals
167
which of the following is not an intermolecular force?
hydrogen bond
dipole-dipole force
ionic bond
dispersion force
168
which of the following is not a colligative property?
vapor pressure elevation
freezing point depression
vapor pressure lowering
boiling point elevation
169
Which of the following is a definition of a pure substance?
It can only exist as a solid, liquid or gas
It is composed of two or more elements
It can be decomposed into a simpler substance
distinct properties and a composition that does not vary
170
Which group in the periodic table are the alkali metals?
group 2A
group 1A
group 7A
group 4A
171
a solution when there is less solute present than needed to saturate the solution is called
asaturated solution
unsaturated solution
supersatureated solution
subcooled solution
172
what is the value of the standard enthalpy of formation of the most stable form of any element
-2
0
-1
1
173
Which phrases best describe potential and kinetic energy?
potential energy is released; kinetic energy is stored
potential energy is heat out; kinetic energy is heat in
potential energy stored; kinetic energy = energy of motion
potential energy endothermic; kinetic energy exothermic
174
What are the SI units for frequency and wavelength?
inverse seconds and meters
seconds and meters
hertz and joules
hertz and feet
175
What is the name of the non-reactive gases that appear in column 8A of the periodic table?
Alkali gases
Halogens
Noble gases
Rare earth gases
176
in what reaction do molecules form new linkages by opening existing pi bonds?
substitutional bonding
intermetallic bonding
vulcanization
addition polymerization
177
what doe the equation N₂ + 3H₂ ↔ 2NH₃ represent?
the catalytic conversion process
the Haber process
the photosynthesis process
the Le Chatelier process
178
Properties of matter which dont rely on amount of matter present called what kind of property?
Intrinsic
Exothermic
Extensive
Intensive
179
What is the list of metals in order of decreasing ease of oxidation called?
the activity series
the lanthanide series
the metalloids
the noble metals
180
what is the name of an acid such as H₂SO₃ that have more than one ionizable proton?
oxyacid
multiprotic acid
polyprotic acid
conjugation acid
181
What law states that the total mass present before and after a chemical reaction is the same?
The second law of thermodynamics
The law of the conservation of energy
The law of the conservation of mass
The law of multiple proportions
182
what is the attractive interaction between solvent molecules with a solute called?
weak interaction
van't Hoff interaction
solvation
osmotic interaction
183
What is atmospheric pressure at STP?
0.0821 atm
1 atm
273 atm
760 atm
184
what is the correct electron configuration for a ground-state atom with 7 electrons?
1s22s5
1s22s32p2
1s22s22p23s1
1s22s22p3
185
which of the following denote elementary reactions?
all of the above
unimolecular
bimolecular
termolecular
186
If a collection of matter is not uniform throughout, what is the classification of the mixture?
Heterogeneous
Pure
Uniform
Homogeneous
187
Which noble gas would be used to write a condensed notation for 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁵?
Br
Ne
He
Ar
188
Whose model of the atom employed a "planetary" system used to explain electron orbits?
Schrodinger
Bohr
Einstein
de Broglie
189
What is the term that is used to describe how closely measurements agree with one another?
accuracy
uncertainty
precision
significant figure
190
Most metal oxides tend to dissolve in water to form what kind of compound?
metal acids
metal hydroxides
metal salts
semiconductors
191
oil and water are immiscible. which is the most likely reason?
oil molecules are denser than water
oil molecules are composed mostly of carbon and hydrogen
oil molecules have higher molar masses than water
oil molecules have higher vapor pressures than water
192
In a solution, a solute is dissolved in a?
electrolyte
solvent
non-electrolyte
mixture
193
What type of electrolytes are water soluble ionic compounds?
strong electrolytes
weak electrolytes
covalent electrolytes
neutral electrolytes
194
when is the vapor pressure of a liquid the partial pressure of that liquid?
when it is in dynamic equilibrium with the liquid
when the liquid temperature is at STP
when it is the thermal equilibrium with the liquid
when it is in secular equilibrium with the liquid
195
what is the branch of chemistry that relates electricity and chemical reactions?
chemical kinetic theory
chemoelectricity
chemical bond theory
electrochemistry
196
Which of the following molecules would have delocalized pi bonds?
NH3
SF6
H2O
C6H6
197
Which of the following is not a basic force?
strong
weak
gravity
quantum
198
What type of element is silicon?
free metal
metalloid
metal
non-metal
199
how is energy transferred into and out of a system?
heat and work
composition and decomposition
enthalpy and entropy
kinetic energy and potential energy
200
which of the following crystal lattices is used to describe the NaCl structure?
primitive cubic lattice
face centered cubic lattice
body centered cubic lattice
hexagonal close packing
201
What kind of compounds tend to be made up by the combination of metals and non-metals?
molecular compounds
covalent compounds
neutral compounds
ionic compounds
202
what rule do valence shell electrons tend to follow when gaining r losing electrons?
the quadrilateral rule
the hexagonal rule
the pentonix rule
the octet rule
203
time required for concentration of reactant to drop to one-half of its original value is called
the half life
the half time
the shelf life
the mean time
204
which principle describes how a system responds to counteract the effect of a disturbance?
kinetic energy principle
mass action principle
equilibrium principle
Le Chatelier principle
205
in the equation Zeff = Z - S, what does the S represent?
silicon
sulfur
ionization constant
screening constant
206
What is the law which is used to help balance equations?
the law of entropy
the law of the conservation of momentum
the law of the conservation of mass
the law of the conservation pf energy
207
why do real gases depart from ideal gases?
real gases lose energy due to inelastic collisions
ideal gases only exist at or near absolute zero K
molecules tend to repel each other b/c van der Waals forces
molecules possess finite volume
208
which of the following is a hydronium ion?
H2O+
H2O-
H3O-
H3O+
209
What type of molecular geometry does SF₆ have?
square planar
octahedral
pentagonal planar
t-shaped
210
as molecular weight increases what also increases which results in stronger dispersion forces?
polarizability
viscosity
surface tension
volatility
211
what analysis determines only the presence of particular metal ion relative to some threshold?
quantitative analysis
titration analysis
stoichiometry analysis
qualitative analysis
212
Entropy is generally expressed in which metric units?
J/K
J-K
K-J
K/J
213
how does chemical equilibrium shift when the volume of a system is reduced?
to the right
in the direction that decreases the number of gas molecules
in the direction that increases the number of gas molecules
to the left
214
Which of the following are not soluble in water?
sodium sulfate
silver nitrate
lead chloride
magnesium chloride
215
What generally composes an ionic compound?
a metal and a non-metal
two metals
two non-metals
a metalloid and a metal
216
which of the following is the correct abbreviation for parts per million?
ppb
ppm
pmp
mpp
217
the measure of energy needed to change a substance from a solid to liquid is called
heat of liquefaction
heat of solidification
heat of fusion
heat of vaporization
218
what model accounts for the properties of metals in a qualitative way?
the electron-sea model
the weak interaction model
the molecular bond model
the molecular dispersion model
219
what are the units of the equilibrium constant?
M-1/s-1
M/s
there are no units for this constant
M/s2
220
which of the following is a possible relationship between Q and K?
they are all possible relationships
Q < K
Q > K
Q = K
221
what are two important characteristics of a buffered solution?
Ksp and pH
pH range and pOH rang
buffer capacity and pH range
buffer capacity and common ions
222
which of the following describes Henri's law?
Sg=kPg
F =ma
ΔT=-iKbm
H = KbNT
223
in the Gibbs free energy equation, ΔG = -nFE, what does the letter F represent?
the number of moles of free electrons
the standard electric cell potential
the free energy constant
Faraday's constant
224
which of the following is not a category of an alloy?
substitutional
homogeneous
interstitial
heterogeneous
225
What conclusion can you draw for a reaction where ΔS is positive and ΔH is negative?
It is spontaneous at high temperatures
It is not spontaneous at all temperatures
It is spontaneous at low temperatures
It is spontaneous at all temperatures
226
Which law states that in an irreversible (spontaneous) process ΔS_univ>0
the second law of thermodynamics
the zeroth law of thermodynamics
the third law of thermodynamics
the first law of thermodynamics
227
what does the term A in the Arrhenius equation represent?
the absorbtion factor
the activation factor
the frequency factor
the molarity of the solution
228
which two gases are critical in maintaining the Earth's surface temperature?
water and carbon dioxide
carbon dioxide and methane
oxygen and water
oxygen and carbon dioxide
229
how is catalysis in living organisms achieved?
by enzymes
by fats
by vitamins
by DNA and RNA
230
batteries which can be recharged are constructed from what types of cells?
tertiary cells
standard electron cells
primary cells
secondary cells
231
which equation is used to predict the behavior of real gases?
the ideal gas equation
the van der Waals equation
the Kinetic Molecular equation
Graham's Law of Effusion
232
Numerical measure of ability of an atom to compete with other atoms for e^- shared between them?
bond enthalpy
electronegativity
dipole moment
affinity
233
Which of the following is not a radioactive decay type?
beta ray
gamma ray
omega ray
alpha ray
234
which gases play a an important role in photochemical smog?
carbon monoxide and water
ozone and sulfur compounds
sulfur oxides and carbon monoxide
nitrogen oxides and ozone
235
what is the name of the property which is characterized by the scattering of light in a colloid
Raouls't's effect
Tyndall effect
osmotic effect
hydratoin effect
236
which of the following is not a basic force?
gravity
quantum
weak
strong
237
rule states the lowest energy is attained by maximizing number of electrons with the same spin
Hess's rule
Heisenberg's rule
Schrodinger's rule
Hund's rule
238
Reactions that result in the formation of an insoluble product are called?
decomposition reactions
combustion reactions
combination reactions
precipitate reactions
239
A molecule which is made up of two atoms is called?
a duo molecule
a diatomic molecule
a heterogeneous molecule
a bipolar
240
How many carbon atoms are representd in the formula for acetic acid (CH₃COOH)?
none
two
three
one
241
Which of the following is not a hybrid orbital configuration?
sp0
sp3
sp2
sp
242
The [Xe]6s² electron configuration is for which element?
Calcium
Barium
Strontium
Magnesium
243
Which of the following is not true regarding standard molar entropies?
they generally increase with increased molar mass
entropies for gases are greater than for liquids or solids
they are equal to zero at the reference temperature
they increase with the number of atoms in a formula
244
What is the relationship between a bonding atomic radius?
non-bonding atomic radius > bonding atomic radius
bonding radius = non-bonding atomic radius
bonding radius > non-bonding radius except for halogens
bonding atomic radius > non-bonding atomic radius
245
What is the law which is used to help balance equations?
the law of conservation of momentum
the law of enthalpy
the law of the conservation of mass
the law of the conservation of energy
246
what is the arrangement of electron domains around a central atom called?
electron domain trigonometry
electron domain geometry
molecular geometry
electron domain algebra
247
The bond polarity increases as what between two atoms increases
the difference in electronegativity
the difference in electric charge
the difference in valence shell repulsion
the difference in electron affinity
248
how do you determine the solvent and solute in a solid alloy?
the higher metling point element is the solute
the majority element is the solvent
the majority element is the solute
the higher melting point element is the solvent
249
Where does the human body store most excess energy?
carbohydrates
sugars
proteins
fats
250
which type of semi-conductor is doped so there is an excess of electrons in the conduction band
s-type
a-type
p-type
n-type
251
What is the molecular formula of the following compound, dinitrogen tetroxide?
2(NO2)
N2O4
2N4O
N2O4
252
which theory accounts for the properties of an ideal gas?
Avogadro's hypothesis
vandal Waals theory
Avogadro's theory
kinetic-molecular theory of gas
253
what is the name given to substances that can be decomposed by bacteria?
antibacterial
bioenzymes
biodegradable
antibiotics
254
When calculating enthalpies reaction using bond enthalpies, ΔHrxn which is negative indicates:
the reaction is isothermic
the reaction is ionic
the reaction is exothermic
the reaction is endothermic
255
which of the following is true regarding acids and bases?
acids turn litmus red, bases turrn litmus blue
acids turn litmus green, bases turn litmus blue
acids turn litmus blue, bases turn litmus red
acids turn litmus red, bases turn litmus green
256
Which of the following is an alkane?
Methane
Butyl Methyl Ether
Methene
Methanol
257
what is the equilibriua for which all substances are in the same phase called?
thermal equilibria
heterogeneous equilibria
iso chemical equilibria
homogeneous equilibria
258
Which of the following is not a strong acid?
HF
HCl
HI
H2SO4
259
what is the minimum energy for a reaction to occur called?
minimum potential energy
minimum energy
activation energy
minimum kinetic energy
260
law governs relationship between the concentrations of reactants and products at equilibrium
the law of conservation of mass
the law of conservation of energy
the law of potential energy
the law of mass action
261
what are organic acids containing the COOH group called?
carboxylic acid
conjugate acid
oxyacid
Lewis acid
262
which of these elements typically exhibits exceptions to octet rule in it's Lewis strctures?
oxygen
calcium
argon
sulfur
263
what is theoverall rate in an elementary reaction limited by the slowest elementary step called
the activation energy step
the rate determining step
the limiting reaction step
the instantaneous rate
264
what materials posses characteristic metal properties and are composed of more than one element
elastomers
LEDs
semi-conductors
alloys
265
properties of matter which dont rely on aount of matter present are what kind of property
intensive
extensive
exothermic
instrinsic
266
What is the process called when water surrounds ions to prevent them from recombining?
electrolysis
solvation
ionization
encapsulation
267
How is atomic weight determined?
sum of isotope mass times that fractional isotope abundance
sum of naturally occurring isotopes/number of isotopes
product of isotope mass times fractional isotope abundance
sum of the masses of protons and electrons of an element
268
what equation is used to express relationship between strength of acid and its conjugate base
Kw = Ka + Kb
Kw = Ka - Kb
Kw = Ka x Kb
Kw = Ka / Kb
269
which of the following is not a characteristic of green chemistry?
safer chemical design
renewable energy
atom economy
use of renewable feedstocks
270
What is the atomic of tungsten?
22
43
74
52
271
Boyle's law, what is the relationship between the P and V of a gas maintained at a constant T
inversely proportional
the sum of pressure and volume equal a constant
the inverse square of each other
directly proportional
272
What trend does ionic radius tend to follow in a group going down?
increases then decreases
increases
remains constant
decreases
273
if an electron transitions from one energy level to another, ΔE>0 and n_f>n_i, what has occurred?
an electron has been ejected
a matter wave was created
a photon was emitted
a photon was absorbed
274
when increasing the temperature of an endothermic reaction, how does the value of Kc change?
Kc does not change
Kc increases to equilibrium then decreases
Kc increases
Kc decreases
275
The term that is used to describe how closely measurements agree with the correct value?
precision
significant figure
uncertainty
accuracy
276
What is the instrument used to measure atmospheric pressure?
barometer
altimeter
hygrometer
thermometer
277
Which of the following is an empirical formula for C₁₂H₂₄O₁₈?
C2H4O3
C3H8O6
C6H12O9
C2H4O4
278
What do double arrows in a chemical equation signify?
a redox reaction
chemical equilibrium
dissociation of an ionic compound
a strong electrolyte
279
What is the term that describes two or more atoms joined in a specific shape?
Element
Molecule
Atom
Isotope
280
What is the term that is used to describe elements that separate metals from non-metals?
Transition metals
Actinides
Metalloids
Lanthanides
281
What are the outer shells electrons involved in chemical bonding called?
valence electrons
free electrons
hybrid electrons
degenerate electrons
282
What is the atomic number of tungsten?
22
52
43
74
283
process of removing dissolved salts from seawater/brackish water to make fit for human intake
solvation
desalination
fracking
hydrolysis
284
Which of the following is not a renewable energy source?
solar
biomass
natural gas
wind
285
what is the number of molecules of the step in an elementary reaction called?
the ion constant
the molecularity
the rate limiting step
the half life
286
which force holding particles together is the strongest?
hydrogen bonds
ionic bonds
dispersion force
metallic bonds
287
Which of the following equations denotes a metathesis reaction?
AX + BY → XY + BA
AX → BY + AY + BX
AX + BY → AY + BX
AX + BY + AY → BX
288
Which of the following is not an angular momentum quantum number designation?
s
e
d
f
289
an undesirable redox reaction in which a metal is attacked by some substance in its environment
disintegration
dissolution
corrosion
corruption
290
Which of the following is the unit used for measuring atomic weight?
picometers
coulombs per unit area
angstroms
atomic mass units
291
when a substance changes from a gas to a solid phase, this process is called
fission
fusion
sublimation
deposition
292
what is the equation for the ideal gas law?
PnT = RV
PT = nRV
PV = nRT
PRT = nV
293
What does a temperature increase ΔT>0 in the water surroundings mean when a calorimeter is used
reaction is exothermic qrxn<0
reaction is endothermic qrxn>0
reaction is endothermic qrxn<0
reaction is exothermic qrxn>0
294
which of the following is the unit used for measuring atomic weight?
atomic mass units
coulombs per unit area
Avogadro's number
angstroms
295
What happens to the internal energy of a system when heat is added or work is done on a system
the internal energy increases
the internal energy becomes negative
the internal energy decreases
there is no change in the internal energy
296
which of the following is not a chemical bond?
Lewis bond
ionic bond
covalent bond
metallic bond
297
law states that the entropy of a pure, perfect crystalline substance at absolute zero is zero
the first law of thermodynamics
the third law of thermodynamics
the zeroth law of thermodynamics
the second law of theermodynamics
298
what are the major contributors to acid rain?
oxides of fluorine
oxides of sulfur
oxides of carbon
oxides of nitrogen
299
properties of matter which do not rely on the amount of matter present are what property?
intensive
intrinsic
exothermic
extensive
300
which of the following is not a diatomic gas?
nitrogen
hydrogen
helium
oxygen
301
What is the reactant called in a chemical equation that is not the limiting reactant?
the over reactant
the empirical reactant
the excess reactant
the molecular reactant
302
What are balanced chemical equations that show enthalpy change called?
molar heat balance reactions
thermochemical reactions
energy balance reactions
full ionic reactions
303
on a phase diagram the point where all three phases of matter occur is called
the critical point
the end point
the saturation point
the triple point
304
Which of the following techniques would be most useful in separating a solid-liquid mixture?
Filtration
Distillation
Solidification
Agitation
305
which values in electromagnetic radiation have an inverse relationship?
frequaency and energy
momentum and energy
wavelength and energy
frequency and wavelength
306
when will a precipitate form in a solution?
when Ksp = Q
when Ksp > Q
when Ksp > Keq and Ksp < Q
when Q > Ksp
307
What is the term that is used to denote the metric unit of electric current?
Meter
Kilogram
Mole
Ampere
308
Possible values of an angular momentum quantum number for a principal quantum number of 3
0
1
3
2
309
which of the following is not a factor affecting reaction rates?
concentration
physical state of the reactants
temperature
pressure
310
which of the following is not a characteristic of a liquid
flows readily
assumes shape of portion of container it occupies
is compressible
does not expand to fill its container
311
what is the reaction of ions with water with a resultant change in pH called?
neutralization
equilibrium
hydrolysis
disassociation
312
When two or more products form a single product, what is this reaction called?
Decomposition reaction
Double replacement reaction
Combustion reaction
Combination reaction
313
Which of the following is not true regarding significant digits?
zeros at the beginning of a number are never significant
zeros between nonzero digits are always significant
something properly reported all nonzero digits significant
zeros in scientific notation are never significant
314
How many moles of Na+ ions are in a 0.025 M NaCl solution?
1.0 M
-0.025 M
0.025 M
0.050 M
315
What type of reaction is a bomb calorimeter used to study?
decomposition reactions
reduction reactions
double replacement reactions
combustion reactions
316
not possible as molecular geometry for a trigonal bipyrimiydal electron domain geometry?
square planar
linear
seesaw
t-shaped
317
What type of quantities are bond dipoles and dipole moments?
vector quantities
trabslational quantities
scalar quantities
transitional quantities
318
what is the reverse of the solution process called?
hydration
crystallization
solvation
dynamic equilibrium
319
what are liquids or solids that can also exist at a gaseous state called?
ozone
vapors
steam
plasma
320
What can you determine about a reaction where ΔG=0?
The reaction is spontaneous at all temperatures
The reaction is in equilibrium
The reaction has an entropy of zero
The reaction is exothermic
321
What is the name of the substances on the left side of a chemical equation called?
reactants
excess products
limiting components
products
322
The term that is used to describe how closely measurements agree with the correct or true value
significant figure
uncertainty
precision
accuracy
323
what mechanism helps blood and seawater maintain their pH levels?
buffers
weak acids
storng bases
enzymes
324
What is the name given to the orbitals of the same energy?
similar
grounded
degenerate
isoelectronic
325
property of semi-conductors modified by electrical engineers to manufacture electrical devices
band gap
electronegativity
polar constants
cross linking
326
in a half-cell which way do anions and cations migrate?
cations migrate toward anode and anions toward cathode
anions migrate to anode and caations to cathode only at >1 V
anions migrate toward anode and cations toward cathode
anions and cations migrate toward anode and reverse at equil
327
in the ideal gas equation, what does the letter R represent?
the pressure constant
the mole constant
the gas constant
the volume constant
328
Which values in electromagnetic radiation have an inverse relationship?
wavelength and energy
momentum and energy
frequency and energy
frequency and wavelength
329
What is the molar mass of Antimony?
27 g/mol
121.8 g/mol
74.9 g/mol
227 g/mol
330
which of the following is the form for the rate law equation?
rate = [product 1]m[product 2]n...
rate = [product 1]m[product 2]n...
rate = [reactant 1]m[reactant 2]n...
rate = [reactant 1]m[reactant 2]n...
331
what value is used to calculate standard cell potentials?
standard half-cell free energies
standard reduction potentials
standard anion potentials
standard cell molar enthalpies
332
What is the energy needed to remove the first electron from a neutral atom called?
absorption energy
excitation energy
first ionization energy
prime ionization energy
333
which order rate equation has a graph of ln[A] versus time that yields straight line slope=-k
zeroth order equation
third order equation
first order equation
second order equation
334
1 mol gas A and 2 mole gas B are constant T and fixed V container. what is true about the gases
same urms
same ump
same kinetic energy
same potential energy
335
Which of the following compounds are soluble in water?
sodium sulfate and silver nitrate
sodium chloride
magnesium chloride
they are all soluble
336
rule states lowest energy is attained by maximizing the number of electrons with the same spin
Hess's rule
Heisenberg's rule
Schrodinger's rule
Hund's rule
337
What is the name given to the process which occurs when a system absorbs heat?
endocaloric
endothermic
isothermic
exothermic
338
what characteristic defines a strong acid?
poor conductor
reacts with metals to form oxygen gas
ionize completely in aqueous solution
bitter taste
339
Which of the following is the SI unit for energy?
kilogram
joule
meter
newton
340
which of the following does not equal a mole of He gas?
6.022E23 molecules of He
They all equal one mole of He gas
22.4 L of He
4 grams of He
341
What is the definition of the amount of heat required to raise an object's temperature by 1 K
specific enthalpy
heat capacity
specific energy
temperature capacity
342
what is the overall reaction order of a second order reaction?
1
2
-2
-1
343
which value is neutral on the pH scale?
7
0
11
1
344
which of the following techniques would be most useful in separating a solid-liquid mixture?
Filtration
Distillation
Solidification
Agitation
345
When looking at a phase diagram when does the largest increase per K change in entropy occur?
heating a liquid
heating a solid
phase change from solid to liquid
phase change from liquid to gas
346
What element is the greatest composition by percentage in the human body and the earth's crust?
Silicon
Carbon
Oxygen
Iron
347
Which of the following scales have the same increments in temperature change?
Celsius and Fahrenheit
Kelvin and Meters
Celsius and Kelvin
Fahrenheit and Kelvin
348
Which of the following elements exhibits exceptions to the octet rule in it's Lewis structures?
oxygen
argon
sulfur
calcium
349
law states fixed quantity of gas at constant P the V is directly proportional to absolute T
Dalton's Law
Boyle's Law
Charles's Law
Graham's Law
350
which is a noteworthy characteristic of a weak acid, strong base titration?
the pOH at the equivalence point is above 7.0
moles of acid and base not equal at the equivalence point
after equivalnce point adding more base wont increase pH
the pH at the equivalence point is above 7.0
351
which gas comprises the largest mole fraction gas content of dry air at sea level?
oxygen
argon
carbon dioxide
nitrogen
352
What is the most abundant element in the known universe?
Helium
Oxygen
Carbon
Hydrogen
353
what are the units for electromotive force (emf)?
volts
joules
kilojoules/mol
amps
354
what is a polymer formed from two different monomers called?
a dipolymer
a copolymer
a polar polymer
a bipolymer
355
What is the term that is used to denote the prefix for a metric unit of 10⁶?
Micro
Mega
Kilo
Giga
356
what are the SI units for frequency and wavelength?
seconds and feet
inverse seconds and meters
seconds and meters
hertz and joules
357
When two atoms of the same element have different numbers of neutrons they are called?
isotones
isoelexes
isotopes
isomers
358
which of the following is liquid at 30 ^oC?
iodine
bromine
chlorine
fluorine
359
Which of these is not a state of a reactant?
liquid
solid
ion
gas
360
What is the rule for addition and subtraction of significant digits?
result has same number of decimals as measurement withfewest
result has at least same number of decimals as most measure
result has same number of decimals as measurement with most
result had at least same number of decimals as fewestmeasure
361
what is a motif?
a weakly bound molecular solid
atom or group of atoms associated with every lattice point
one of the seven primitive structures
a structure with close cubic packing
362
What is the term for a rainbow of colors containing light of all wavelengths?
continuous spectrum
dark light
white light
line spectrum
363
Which of the following bonds will have the shortest bond length?
double bond
they are all the same length but different energies
triple bond
single bond
364
which of the following is not a factor affecting reaction rates?
concentration
pressure
physical state of the reactants
temperature
365
Which of the following is not a state of matter?
Liquid
Gas
Ion
Solid
366
hydrogen bonds form between hydrogen and which other element
chlorine
fluorine
carbon
helium
367
net movement of solvent toward solution with lower solvent (higher solute) concentration called
solvation
hydration
colloid
osmosis
368
the absorption of photons which leads to the formation of ions is called?
photodissociation
photoabsorption
photoionization
photodisintegration
369
Which element has the highest first ionization energy?
P
Cl
Al
Si
370
What is the name of the symbols used to represent valence electrons in a dot notation called?
electron valence shell notation
electron force notation
Lewis dot notation
Bon-Haber notation