UNE CHEM 1011 General Chemistry II
Midterm Fall 2026
1. If the temperature of a gas is increased, what effect does this have on the
kinetic energy of its particles and their intermolecular interactions?
The kinetic energy remains constant, with no effect on intermolecular
interactions.
The kinetic energy decreases, leading to no change in intermolecular
interactions.
The kinetic energy increases, leading to weaker intermolecular
interactions.
The kinetic energy decreases, leading to stronger intermolecular
interactions.
2. The solubility of a substance in a solvent depends on
Temperature
Pressure
Nature of solute and solvent
All of the above
3. Which type of intermolecular force is primarily affected by the size and mass
of atoms and molecules?
Dispersion forces
Dipole-dipole interactions
Hydrogen bonding
Ionic bonds
,4. The presence of an instantaneous dipole can distort the electrons of a
neighboring atom or molecule, producing
An induced dipole
A hydrogen bond
A permanent dipole
An ion
5. Describe the characteristics that differentiate colloids from suspensions and
solutions.
Colloids can be separated by simple filtration, unlike solutions.
Colloids are completely uniform mixtures with no visible particles.
Colloids have particle sizes that are larger than those in solutions
but smaller than those in suspensions, leading to unique properties.
Colloids consist of particles that settle quickly, similar to suspensions.
6. What is the nature of the energy change during vaporization?
Endothermic
Exothermic
Isothermal
Adiabatic
7. What is the main factor that collision theory states affects the rate of a
chemical reaction?
Presence of catalysts
Frequency of reactant collisions
, Temperature of the reactants
Concentration of products
8. What is kinetic energy?
The energy stored in the bonds of compounds and molecules
The energy stored by matter due to its position
The energy associated with matter in motion
The energy released by exergonic reactions
9. If a solution has a higher boiling point than pure solvent, what can be inferred
about the solute present?
The solute causes boiling point elevation.
The solute has a lower molecular weight than the solvent.
The solute is a non-volatile substance.
The solute is a gas.
10. What is the definition of colloids in chemistry?
Colloids or colloidal dispersions have properties intermediate
between those of suspensions and solutions.
Colloids are solutions that do not settle upon standing.
Colloids are mixtures that can be separated by filtration.
Colloids are homogeneous mixtures of two or more substances.
11. What is defined as the temperature at which a liquid's vapor pressure equals
the surrounding pressure?
Boiling point
, Freezing point
Sublimation point
Melting point
12. If you were to mix oil and water in a beaker, what would you expect to
observe and why?
You would observe two separate layers because oil and water are
immiscible liquids.
You would observe a reaction producing bubbles.
You would observe a solid precipitate forming at the bottom.
You would observe a single homogeneous mixture due to their
similar densities.
13. Which states that the vapor pressure lowering of a solution is equal to its
vapor pressure in its pure state multiplied by the mole fraction of the solute?
Amagat's law
Raoult's law
Boyle's law
Henry's law
14. Describe the process by which an instantaneous dipole is created in a
molecule.
An instantaneous dipole is a permanent feature of polar molecules.
An instantaneous dipole forms when a molecule is ionized.
An instantaneous dipole is created when the electrons are
unevenly distributed, leading to a temporary dipole.
Midterm Fall 2026
1. If the temperature of a gas is increased, what effect does this have on the
kinetic energy of its particles and their intermolecular interactions?
The kinetic energy remains constant, with no effect on intermolecular
interactions.
The kinetic energy decreases, leading to no change in intermolecular
interactions.
The kinetic energy increases, leading to weaker intermolecular
interactions.
The kinetic energy decreases, leading to stronger intermolecular
interactions.
2. The solubility of a substance in a solvent depends on
Temperature
Pressure
Nature of solute and solvent
All of the above
3. Which type of intermolecular force is primarily affected by the size and mass
of atoms and molecules?
Dispersion forces
Dipole-dipole interactions
Hydrogen bonding
Ionic bonds
,4. The presence of an instantaneous dipole can distort the electrons of a
neighboring atom or molecule, producing
An induced dipole
A hydrogen bond
A permanent dipole
An ion
5. Describe the characteristics that differentiate colloids from suspensions and
solutions.
Colloids can be separated by simple filtration, unlike solutions.
Colloids are completely uniform mixtures with no visible particles.
Colloids have particle sizes that are larger than those in solutions
but smaller than those in suspensions, leading to unique properties.
Colloids consist of particles that settle quickly, similar to suspensions.
6. What is the nature of the energy change during vaporization?
Endothermic
Exothermic
Isothermal
Adiabatic
7. What is the main factor that collision theory states affects the rate of a
chemical reaction?
Presence of catalysts
Frequency of reactant collisions
, Temperature of the reactants
Concentration of products
8. What is kinetic energy?
The energy stored in the bonds of compounds and molecules
The energy stored by matter due to its position
The energy associated with matter in motion
The energy released by exergonic reactions
9. If a solution has a higher boiling point than pure solvent, what can be inferred
about the solute present?
The solute causes boiling point elevation.
The solute has a lower molecular weight than the solvent.
The solute is a non-volatile substance.
The solute is a gas.
10. What is the definition of colloids in chemistry?
Colloids or colloidal dispersions have properties intermediate
between those of suspensions and solutions.
Colloids are solutions that do not settle upon standing.
Colloids are mixtures that can be separated by filtration.
Colloids are homogeneous mixtures of two or more substances.
11. What is defined as the temperature at which a liquid's vapor pressure equals
the surrounding pressure?
Boiling point
, Freezing point
Sublimation point
Melting point
12. If you were to mix oil and water in a beaker, what would you expect to
observe and why?
You would observe two separate layers because oil and water are
immiscible liquids.
You would observe a reaction producing bubbles.
You would observe a solid precipitate forming at the bottom.
You would observe a single homogeneous mixture due to their
similar densities.
13. Which states that the vapor pressure lowering of a solution is equal to its
vapor pressure in its pure state multiplied by the mole fraction of the solute?
Amagat's law
Raoult's law
Boyle's law
Henry's law
14. Describe the process by which an instantaneous dipole is created in a
molecule.
An instantaneous dipole is a permanent feature of polar molecules.
An instantaneous dipole forms when a molecule is ionized.
An instantaneous dipole is created when the electrons are
unevenly distributed, leading to a temporary dipole.
