Multiple choice: Which subatomic particle defines the atomic number of an element?
A) Neutron
B) Proton
C) Electron
D) Positron

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Short answer: State the law of conservation of mass in a chemical reaction.

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Fill in: Avogadro’s number is approximately ____ × 10^23 particles per mole.

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Multiple choice: Which orbital can hold a maximum of six electrons?
A) s orbital
B) p orbital
C) d orbital
D) f orbital

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True or False: An endothermic process absorbs heat from the surroundings.

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Short answer: Define electronegativity.

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Multiple choice: Which bond is generally the most polar?
A) Carbon–hydrogen
B) Carbon–oxygen
C) Hydrogen–hydrogen
D) Sodium–chlorine

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Fill in: The sum of all oxidation numbers in a neutral compound is ____ .

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Multiple choice: Which statement best describes a catalyst?
A) A substance that increases reaction rate and is consumed
B) A substance that decreases reaction rate and is not consumed
C) A substance that increases reaction rate and is regenerated
D) A substance that increases equilibrium constant

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Short answer: State Le Châtelier’s principle.
 

Multiple choice: Which gas law states that volume is directly proportional to absolute temperature at constant pressure and amount?
A) Boyle’s law
B) Charles’s law
C) Avogadro’s law
D) Dalton’s law
 

Fill in: Standard temperature and pressure commonly mean a temperature of ____ kelvin and a pressure of ____ atmosphere.
 

True or False: The rate constant of a reaction always increases when temperature increases.
 

Multiple choice: Which factor does not change the equilibrium constant for a given reaction?
A) Temperature
B) Adding a catalyst
C) Changing reaction stoichiometry representation
D) Choice of standard states
 

Short answer: Define molarity.
 

Multiple choice: Which quantum number describes the shape of an orbital?
A) Principal quantum number (n)
B) Angular momentum quantum number (l)
C) Magnetic quantum number (m_l)
D) Spin quantum number (m_s)
 

Fill in: A solution that resists significant change in pH upon addition of small amounts of acid or base is called a ____ .
 

True or False: Ionic solids typically have high melting points due to strong electrostatic attractions.
 

Multiple choice: Which intermolecular force is strongest among these for neutral molecules?
A) London dispersion force
B) Dipole–dipole interaction
C) Hydrogen bonding
D) Instantaneous dipole–induced dipole
 

Short answer: Define standard enthalpy of formation.
 

Multiple choice: Which pair of elements is most likely to form a covalent bond?
A) Sodium and chlorine
B) Calcium and oxygen
C) Carbon and oxygen
D) Magnesium and bromine
 

Fill in: The number of significant figures in 0.00340 is ____ .
 

True or False: In a first-order reaction, the half-life is independent of initial concentration.
 

Short answer: Define the term “limiting reactant.”
 

Multiple choice: Which statement about an ideal gas is correct?
A) Gas particles strongly attract each other
B) Gas particles have significant volume compared with the container
C) Gas particles move randomly and do not attract significantly
D) Gas particles lose energy during elastic collisions
 

Fill in: The mass percent of an element in a compound equals (mass of element in 1 mole of compound ÷ molar mass of compound) × ____ .
 

Multiple choice: Which substance is a strong electrolyte in water?
A) Sucrose
B) Acetic acid
C) Sodium chloride
D) Ammonia
 

Short answer: State Hess’s law.
 

True or False: The entropy of a perfectly crystalline substance at absolute zero kelvin is zero.
 

Multiple choice: Which molecule is nonpolar overall?
A) Water
B) Carbon dioxide
C) Ammonia
D) Hydrogen fluoride
 

Fill in: The conjugate acid of ammonia is ____ .
 

Short answer: Define activation energy.
 

Multiple choice: Which statement about the equilibrium constant is correct?
A) It depends on initial amounts of reactants and products
B) It depends only on temperature for a given reaction
C) It always increases when a catalyst is used
D) It equals one at equilibrium
 

True or False: A saturated solution contains more solute than can dissolve at a given temperature.
 

Fill in: In a redox reaction, oxidation is the ____ of electrons and reduction is the ____ of electrons.
 

Multiple choice: Which of the following has the highest boiling point under similar conditions?
A) Methane
B) Ethane
C) Propane
D) Butane
 

Short answer: Define solubility.
 

True or False: Bond enthalpy is always negative.
 

Multiple choice: What is the shape around a central atom with four bonding pairs and no lone pairs?
A) Tetrahedral
B) Trigonal planar
C) Trigonal pyramidal
D) Bent
 

Fill in: The process by which a liquid changes to a gas below its boiling point is called ____ .
 

Multiple choice: Which solution has the highest osmotic pressure at the same temperature?
A) 0.10 molar glucose (nonelectrolyte)
B) 0.10 molar sodium chloride (assume complete dissociation)
C) 0.10 molar magnesium chloride (assume complete dissociation)
D) 0.05 molar magnesium chloride (assume complete dissociation)
 

Short answer: Define standard enthalpy change of reaction.
 

True or False: A spontaneous process always occurs rapidly.
 

Fill in: The pH of a solution is defined as the negative base-ten logarithm of the ____ ion concentration.
 

Multiple choice: Which statement about hydrogen bonding is correct?
A) It occurs only between hydrogen and carbon
B) It requires hydrogen bonded to nitrogen, oxygen, or fluorine
C) It is weaker than all other intermolecular forces
D) It requires an ionic bond
 

Short answer: Define lattice energy.
 

Multiple choice: Which change increases the solubility of most solid solutes in water?
A) Lowering temperature
B) Increasing temperature
C) Decreasing pressure
D) Adding a seed crystal
 

True or False: The vapor pressure of a liquid increases as temperature increases.
 

Fill in: The substance that is oxidized is the ____ agent, and the substance that is reduced is the ____ agent.
 

Multiple choice: Which pair represents an acid–base conjugate pair in the Brønsted–Lowry sense?
A) Sodium and chlorine
B) Hydrochloric acid and chloride ion
C) Water and hydrogen gas
D) Oxygen and oxide ion
 

Short answer: Define the term “enthalpy.”
 

True or False: A negative free energy change indicates that a process is spontaneous under the given conditions.
 

Multiple choice: Which factor generally increases the rate of a reaction?
A) Lower temperature
B) Larger particle size for solids
C) Higher concentration of reactants
D) Removal of catalyst
 

Fill in: According to the collision model, molecules must collide with sufficient energy and proper ____ to react.
 

Short answer: Define partial pressure.
 

Multiple choice: Which statement about a buffer is correct?
A) It is made from a strong acid and its salt only
B) It is made from a strong base and its salt only
C) It is made from a weak acid and its conjugate base or a weak base and its conjugate acid
D) It must have equal volumes of acid and base
 

True or False: The energy of a photon is directly proportional to its wavelength.

 

Fill in: The principal quantum number n indicates the ____ of an electron in an atom.

 

Multiple choice: Which aqueous solution has the lowest freezing point, assuming ideal behavior?
A) 0.20 molar glucose
B) 0.10 molar sodium chloride
C) 0.10 molar calcium chloride (assume complete dissociation)
D) 0.20 molar urea

 

Short answer: Define enthalpy of vaporization.
Correct answer: The heat required to convert one mole of a liquid to vapor at constant pressure and at its boiling temperature.
Explanation: It measures the strength of intermolecular forces in the liquid.

 

Multiple choice: Which statement about molecular orbital theory is correct?
A) Bonding orbitals are higher in energy than antibonding orbitals
B) Antibonding orbitals stabilize a bond
C) Bond order is proportional to the difference between electrons in bonding and antibonding orbitals divided by two
D) Bond order is always an integer

 

Fill in: The empirical formula represents the ____ whole-number ratio of atoms in a compound.

 

True or False: In a galvanic cell, oxidation occurs at the anode and reduction occurs at the cathode.

 

Short answer: Define standard reduction potential.

 

Multiple choice: Which of the following increases the solubility of a gas in a liquid?
A) Increasing temperature
B) Decreasing pressure of the gas above the liquid
C) Increasing pressure of the gas above the liquid
D) Decreasing the polarity of the solvent

 

Fill in: The constant of proportionality in the ideal gas equation, often called the gas constant, has a value of approximately ____ liter·atmosphere per mole·kelvin.

 

True or False: The heat capacity of a substance is the amount of heat required to raise the temperature of one gram by one degree Celsius.

 

Short answer: Define enthalpy of solution.

 

Multiple choice: Which is the best description of resonance in Lewis structures?
A) Atoms move rapidly among positions
B) Electrons are localized in one unique structure
C) The true structure is a hybrid of multiple valid structures differing only in electron arrangement
D) The molecule alternates between two shapes over time

 

Fill in: A process with negative enthalpy change and positive entropy change is ____ under all temperatures.

 

Multiple choice: Which aqueous salt solution is expected to be acidic?
A) Sodium chloride
B) Potassium nitrate
C) Ammonium chloride
D) Sodium acetate

 

Short answer: Define the term “common ion effect.”

 

True or False: Increasing ionic strength of a solution can affect activities of ions and therefore equilibrium calculations.

 

Fill in: The heat required to raise the temperature of one mole of a substance by one degree Celsius is called the ____ heat capacity.
 

 

Multiple choice: Which trend is correct across a period from left to right in the periodic table?
A) Atomic radius increases
B) Ionization energy decreases
C) Electronegativity increases
D) Metallic character increases

 

Short answer: Define solubility product constant.

 

True or False: For a spontaneous endothermic dissolution, the entropy increase of the system must be significant.

 

Fill in: When titrating a strong acid with a strong base, the pH at the equivalence point is approximately ____ .

 

Multiple choice: Which statement about colligative properties is correct?
A) They depend on the identity of solute particles
B) They depend on the number of solute particles present
C) They are unaffected by electrolyte dissociation
D) They include color and viscosity.

 

Short answer: Define enthalpy of fusion.
 

Multiple choice: Which pair correctly matches hybridization with ideal geometry?
A) sp — trigonal planar
B) sp^2 — tetrahedral
C) sp^3 — tetrahedral
D) sp^3d — linear
 

Fill in: The tendency of a liquid to rise in a thin tube due to adhesive and cohesive forces is called ____ action.
 

True or False: The half-reaction method is used to balance oxidation–reduction equations.
 

Short answer: Define heat of neutralization.

 

Multiple choice: Which state function is path independent?
A) Heat
B) Work
C) Enthalpy
D) Heat plus work

 

Fill in: The minimum amount of solute that must be added to a solvent to produce a saturated solution at a given temperature is the ____ at that temperature.

 

True or False: In a voltaic cell, electrons flow through the salt bridge.

Short answer: Define standard state for a gas and for a solute in solution.
 

Multiple choice: Which compound will show geometric (cis–trans) isomerism?
A) Methane
B) Ethane
C) 2-butene
D) Propane

 

Fill in: A solution with a hydrogen ion concentration of 1.0 × 10^−9 moles per liter has a pH of ____ .

 

Multiple choice: Which factor most directly determines whether a reaction is product-favored at equilibrium?
A) Initial concentrations only
B) The magnitude of the equilibrium constant
C) The size of the activation energy
D) The presence of a catalyst

 

Short answer: Define the term “enthalpy of atomization.”

 

True or False: An amphiprotic substance can act as both an acid and a base by donating or accepting a proton.

 

Fill in: The process by which a solid changes directly to a gas is called ____ .

 

Multiple choice: Which factor does not appear in the expression for the equilibrium constant for the reaction of pure solids and pure liquids?
A) Concentration of dissolved species
B) Partial pressure of gases
C) Activities of pure solids and pure liquids
D) Temperature

Short answer: Define the heat of combustion.
 

True or False: A reaction with positive enthalpy change and negative entropy change can be spontaneous at high temperature.

Fill in: The slope of a plot of the natural logarithm of the rate constant versus the inverse of temperature is proportional to the negative of the ____ energy divided by the gas constant.

Multiple choice: Which aqueous solution is expected to be basic?
A) Ammonium nitrate
B) Sodium carbonate
C) Sodium chloride
D) Potassium bromide
 

Short answer: Define polarizability.