UNE CHEM 1011 General Chemistry II Midterm Fall 2025
with Answers Graded A
Intermolecular Forces - -Attractions atomic radius, melting point, and boiling point
between molecules impacting physical properties increase from top to bottom in the halogen group
of a substance
Reason for Trends in Properties - -Valence
Kinetic Energies - -Energy needed to electrons farther from nucleus contribute to molar
overcome attractive forces and increase distance mass, atomic radius, melting point, and boiling
between particles point trends
Intramolecular Forces - -Forces within a Polarizability - -Measure of how easily a
molecule that hold it together molecule's charge distribution can be distorted by
an external charge
Van der Waals Forces - -Attractive forces
between neutral atoms and molecules Hydrogen Bonding - -Occurs in molecules
with F-H, O-H, or N-H bonds
London Dispersion Force - -Type of van
der Waals force present in all condensed phases Viscosity - -Resistance of a liquid to flow
due to electron motion
Factors Affecting Viscosity - -IMFs,
Instantaneous Dipole - -Occurs when molecule size/shape, and temperature influence
electrons are distributed asymmetrically viscosity
Induced Dipole - -Caused by distortion of Effect of Temperature on Viscosity - -
electrons in a neighboring atom or molecule Increasing temperature decreases viscosity as
molecules move more rapidly
Dispersion Forces Trend - -Larger and
heavier atoms/molecules have stronger Cohesive Forces - -IMFs between identical
dispersion forces than smaller and lighter ones molecules within a substance
Halogen Properties Trend - -Molar mass, Surface Tension - -Energy required to
, UNE CHEM 1011 General Chemistry II Midterm Fall 2025
with Answers Graded A
increase surface area of a liquid Freezing Point of the Liquid - -Temperature
at which solid and liquid phases are in equilibrium
Adhesive Forces - -IMFs between different
molecules Sublimation - -Solids transition directly into
the gaseous state, bypassing the liquid state
Capillary Action - -Liquid flow in porous
material due to molecular attraction Deposition - -Reverse of sublimation
Boiling Point - -Solutions boil at higher Supercritical Fluid - -Physical properties
temperatures than the pure solvent intermediate between gaseous and liquid states
Normal Boiling Point - -Boiling point when Critical Point - -Temperature and pressure
surrounding pressure is equal to 1 atm above which supercritical fluid exists.
Vaporization - -Process that is Crystalline Solids - -Atoms, ions, or
endothermic molecules are arranged in a definite repeating
pattern.
Endothermic - -Associated with a positive
number Amorphous Solids - -Atoms, ions, or
molecules are arranged in a definite NON-
repeating pattern.
Exothermic - -Associated with a negative
number
Alloy - -Solid solutions of one metal
dissolved in another.
Melting Point of the Solid - -Temperature
at which solid and liquid phases are in
equilibrium Spontaneous Process - -A process that
occurs without the requirement of energy, with
requirements: (1) decrease in internal energy
(exothermic change), (2) increased dispersal of
with Answers Graded A
Intermolecular Forces - -Attractions atomic radius, melting point, and boiling point
between molecules impacting physical properties increase from top to bottom in the halogen group
of a substance
Reason for Trends in Properties - -Valence
Kinetic Energies - -Energy needed to electrons farther from nucleus contribute to molar
overcome attractive forces and increase distance mass, atomic radius, melting point, and boiling
between particles point trends
Intramolecular Forces - -Forces within a Polarizability - -Measure of how easily a
molecule that hold it together molecule's charge distribution can be distorted by
an external charge
Van der Waals Forces - -Attractive forces
between neutral atoms and molecules Hydrogen Bonding - -Occurs in molecules
with F-H, O-H, or N-H bonds
London Dispersion Force - -Type of van
der Waals force present in all condensed phases Viscosity - -Resistance of a liquid to flow
due to electron motion
Factors Affecting Viscosity - -IMFs,
Instantaneous Dipole - -Occurs when molecule size/shape, and temperature influence
electrons are distributed asymmetrically viscosity
Induced Dipole - -Caused by distortion of Effect of Temperature on Viscosity - -
electrons in a neighboring atom or molecule Increasing temperature decreases viscosity as
molecules move more rapidly
Dispersion Forces Trend - -Larger and
heavier atoms/molecules have stronger Cohesive Forces - -IMFs between identical
dispersion forces than smaller and lighter ones molecules within a substance
Halogen Properties Trend - -Molar mass, Surface Tension - -Energy required to
, UNE CHEM 1011 General Chemistry II Midterm Fall 2025
with Answers Graded A
increase surface area of a liquid Freezing Point of the Liquid - -Temperature
at which solid and liquid phases are in equilibrium
Adhesive Forces - -IMFs between different
molecules Sublimation - -Solids transition directly into
the gaseous state, bypassing the liquid state
Capillary Action - -Liquid flow in porous
material due to molecular attraction Deposition - -Reverse of sublimation
Boiling Point - -Solutions boil at higher Supercritical Fluid - -Physical properties
temperatures than the pure solvent intermediate between gaseous and liquid states
Normal Boiling Point - -Boiling point when Critical Point - -Temperature and pressure
surrounding pressure is equal to 1 atm above which supercritical fluid exists.
Vaporization - -Process that is Crystalline Solids - -Atoms, ions, or
endothermic molecules are arranged in a definite repeating
pattern.
Endothermic - -Associated with a positive
number Amorphous Solids - -Atoms, ions, or
molecules are arranged in a definite NON-
repeating pattern.
Exothermic - -Associated with a negative
number
Alloy - -Solid solutions of one metal
dissolved in another.
Melting Point of the Solid - -Temperature
at which solid and liquid phases are in
equilibrium Spontaneous Process - -A process that
occurs without the requirement of energy, with
requirements: (1) decrease in internal energy
(exothermic change), (2) increased dispersal of
