-
Which of the intermolecular forces is the weakest?
London dispersion forces
-
What force exists between all molecules?
London dispersion forces
-
London dispersion forces increase as molar mass _______
increases
-
Dipole-dipole forces increase with _____________ polarity
increasing
-
Hydrogen bonding is a type of ________ force
dipole-dipole
-
Hydrogen bonding bonds hydrogen to _________
fluorine, oxygen, or nitrogen
-
Viscosity is a measure of a fluid's ____________________
resistance to flow
-
Viscosity increases as the strength of intermolecular force __________
increases
-
Surface tension is __________
the amount of energy required to increase the surface area of a liquid
-
Cohesive forces __________
bind molecules of the same kind to each other
-
Adhesive forces __________
bind molecules of different kinds to each other
-
Liquid boils when __________
the vapor pressure equals the external pressure
-
Temperature of boiling point increases as pressure __________
increases
-
__________ are well ordered, definite arrangement of molecules, atoms, or ions
Crystalline solids
-
Crystals have a(n) __________ structure
ordered, repeated
-
A unit cell is __________
the smallest repeating unit in a crystal
-
A crystal lattice is __________
three dimensional stacking of unit cells
-
Molecular solids are__________
soft with low melting points and poor conductivity
-
Weak intermolecular forces means __________ melting point
Low
-
Room temperature gases and liquids usually form __________ solids at low temperature
molecular
-
Covalent solids are __________
very hard with high melting points and poor conductivity
-
Covalent solids are __________ ordered
well
-
Ionic solids are __________
hard, brittle, have a high melting point, and poor conductivity
-
Metallic solids are
both soft and hard, have high melting points, have good conductivity, and are malleable and ductile
-
A solution is __________
a homogeneous mixture of two or more substances
-
The more carbon atoms in a chain the __________ soluble in water a solvent is
less
-
Solubility __________ as pressure increases
increases
-
Henry's law says __________
the concentration of a gas is directly proportional to partial pressure of the gas
-
Solubility of a gas __________ as temperature increases
decreases
-
Solubility of a solid __________ as temperature increases
increases
-
Molarity is
the number of moles of solute over number of liters of solution
-
__________ is temperature dependent
Molarity
-
Mass percent of a component is __________
the mass of the component over the total mass of the solution multiplied by 100
-
Parts per million is __________
the mass of the component over total mass of the solution multiplied by 1 million
-
Mole fraction is __________
moles of the component in solution over total moles of the solution
-
Molality is __________
moles of solute over mass of solvent in kilograms
-
Osmotic pressure is __________
the pressure required to stop osmosis from occurring
-
Vapor pressure of a solvent is __________ when a non-volatile solute is dissolved in it.
lowered
-
Boiling point of a solvent __________ when a non-volatile solute is added to it
increases
-
Freezing point of a solvent __________ when a non-volatile solute is added to it
decreases
-
The integrated rate equation for a first order reaction is
ln [A]f = -kt +ln [A]i
-
In first order reactions, plotting __________ will produce a straight line with slope of __________
ln [A]f versus time, -k
-
The half-life equation for first order reactions is __________
0.693/k
-
In first order reactions, k has units of __________
inverse time
-
The integrated rate equation for a second order reaction is __________
1/[A]f = kt + 1/[A]i
-
In second order reactions, plotting __________ will produce a straight line with slope of __________
1/[A]f versus time, k
-
The half-life equation for second order reactions is __________
1/(k*[A]i)
-
In second order reactions, k has units of __________
inverse concentration inverse time
-
Half-life depends on initial concentration in __________ reactions
second order
-
Reactions __________ as temperature increases
speed up
-
An intermediate is __________
something that appears in an elementary step but is not a reactant or product
-
Catalysts __________ the activation energy and __________
lower, change the path for a reaction
-
Heterogeneous catalysts __________
are in a different phase than the reactants and products
-
Homogeneous catalysts __________
are in the same phase as the reactants and products
-
Equilibrium is established when __________
the rate of forward reaction is comparable to the rate of reverse reaction
-
Equilibrium constant is __________
the ratio of products to reactants
-
The larger K is, __________
the more products there are at equilibrium
-
A large K means equilibrium lies __________
to the right
-
The smaller K is, __________
the more reactants there are at equilibrium
-
A small K means equilibrium lies __________
to the left
-
Q is known as __________
the ion product constant
-
If Q is greater than K
the reaction proceeds to the left
-
If Q is less than K
the reaction proceeds to the right
-
Adding a reactant or product shifts the equilibrium __________
away from the increase
-
Removing a reactant or product shifts the equilibrium __________
towards the decrease
-
Heat is a reactant in __________
an endothermic reaction
-
Heat is a product in __________
an exothermic reaction
-
A catalyst will decrease __________
the time taken to reach equilibirium
-
A catalyst has no effect on __________
the position of equilibrium
-
Arrhenius acids _________ in aqueous solutions.
increase the concentration of H+ ions
-
Arrhenius bases _________ in aqueous solutions.
increase the concentration of OH- ions
-
Bronsted-Lowry acids _________
donate an H+ ion
-
Bronsted-Lowry bases_________
accept an H+ ion
-
The conjugate base is _________
whatever is left of the acid after the proton is donated
-
The conjugate acid is _________
whatever is left of the base after the proton is accepted
-
To find conjugate base, _________
remove an H+ ion from the reactant acid
-
To find conjugate acid _________
add an H+ ion to the reactant base
-
A strong acid means a _________ conjugate base
weak
-
The formula for pH is _________
-log [H+]
-
The formula for pOH is _________
-log [OH-]
-
All strong acids _________ in solution
ionize completely
-
A large Ka means _________
a strong acid
-
The pOH of a weak base solution is _________
the square root of Kb multiplied by the initial concentration of the base
-
Percent hydrolysis in a weak base solution is _________
the pOH over initial concentration multiplied by 100
-
Lewis bases _________
donate an electron pair
-
Lewis acids _________
accept an electron pair
-
A common ion is _________
an ion that is the same as an ion that is preset at equilibrium
-
A buffer is _________
a substance that resists change in pH when a small amount of acid or base is added
-
The buffer system that controls blood is _________
carbonic acid and bicarbonate
-
A buffer consists of _________
a weak acid and its conjugate base or a weak base and its conjugate acid
-
The Henderson-Hasselbalch equation is used to _________
calculate the pH of a buffer solution
-
The Henderson-Hasselbalch equation is _________
pH equals pKa + log [Base]/[Acid]
-
For a strong acid-strong base titration, pH_________
increases dramatically near the equivalence point
-
For a weak acid-strong base titration, pH _________
initially rises steeply
-
Solubility is _________
grams of substance that dissolves to form a saturated solution
-
Molar solubility is _________
the number of moles of solute dissolving to form a liter of saturated solution
-
When a common ion is added, solubility _________
decreases
-
As pH decreases, solubility _________
increases
-
If Q is greater than Ksp, the reaction _________
shifts to the left
-
The first law of thermodynamics says _________
the change in energy is equal to heat plus work
-
Exothermic reactions tend to occur _________
spontaneously
-
Endothermic reactions tend to occur _________
non-spontaneously
-
The reverse reaction of a spontaneous reaction is _________
non-spontaneous
-
The total amount of energy in the universe _________
is constant
-
All chemical systems in equilibrium are _________
reversible
-
In a spontaneous process, the path between reactants and products is _________
irreversible
-
The second law of thermodynamics says _________
in any spontaneous process, the entropy of the universe increases
-
The third law of thermodynamics says _________
the entropy of a perfect crystal at 0K is zero
-
As volume increases, entropy _________
increases
-
As temperature increases, entropy _________
increases
-
Gibbs free energy is _________
used to predict maximum work
-
The Gibbs free energy equation is _________
dG equals dH -TdS
-
If dG is negative then the forward reaction is _________
spontaneous
-
If dG is positive then the forward reaction is _________
nonspontaneous
-
dG is equal to _________
-RT multiplied by ln K
-
Oxidation reduction reactions are where _________
electrons are transferred from one atom to another
-
Atoms that gain electrons are _________
being reduced
-
Atoms that lose electrons are _________
being oxidized
-
The oxidation number of an element increases in _________
oxidation
-
A compound adds oxygen in _________
oxidation
-
A compound loses hydrogen in _________
oxidation
-
A half-reaction has electrons as the product in _________
oxidation
-
The oxidation number of an element decreases in _________
reduction
-
A compound loses oxygen in _________
reduction
-
A compound gains hydrogen in _________
reduction
-
A half-reaction has electrons as the reactants in _________
reduction
-
Spontaneous redox reactions take place in _________
voltaic cells
-
Voltaic cells are also known as _________
galvanic cells
-
Nonspontaneous redox reactions can occur in electrolytic cells by _________
the addition of electrical energy
-
Oxidation occurs at the _________
anode
-
Anions are attracted to the _________
anode
-
The _________ is connected to the positive end of a battery in an electrolytic cell
anode
-
The _________ loses weight in an electrolytic cell
anode
-
Reduction occurs at the _________
cathode
-
Cations are attracted to the _________
cathode
-
The _________ is connected to the negative end of a battery in an electrolytic cell
cathode
-
The _________ loses weight in an electrolytic cell
cathode
-
In cell notation, the oxidation half-cell is _________
on the left
-
In cell notation, the reduction half-cell is _________
on the right
-
The _________ is the source of the electrons and has a negative charge in voltaic cells
anode
-
The _________ draws electrons and has a positive charge in voltaic cells
cathode
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