IMF UNIT 10 questions well answered
graded A+ 2025/2026
1) Intramolecular force
2) What are condensed states
3) Intermolecular forces
4) What causes states - correct answers 1) Bonds formed within molecules
2) liquids and solids
3) Forces between molecules
4) Covalent, ionic, and intermolecular forces
1) What causes states
2) What happens in a state change
3) Do forces inside molecules break - correct answers 1) What causes states
2) The bonds between molecules are broken or formed. In ice, the particles are locked in place, and gain
more disorder as they move to liquid stage. They eventually are able to virbate lots in the gas stage
3) Not easily. Much more energy is required to break the intramolecular bonds than the intermolecular
bonds
1) How do polar bonds cause dipoles
2) Compare dipole-diople to ionic and covalent bonds - correct answers 1) The polar molecules have a
positive and negaitive charge, and line up opposite charges. This works best in liquid, where molecules
are close but able to move. They do it to maximize attraction and decrease repulsion.
2) dipole-dipole are about 0.99% as strong, and severly decrease with distance. Insignifican it low
pressure gas
1) Hydrogen bonds
2) Why do top 5,6,7,and 8A groups have much higher initial boiling points?
, 3) Why is high boiling point important for molar mass - correct answers 1) Hydrogen bonded with N, O,
of F are most strong, and called hydrogen bonds. Due to great polatitity difference and small hydrogen
atom
2) Because the first atom in the group is smallest and most polar.
3) very polar OH bonds
1) London Dispersion Forces evidence and most effective for
2) What are they
3) Freezing point periodicity
4) How does LDF force create dipole - correct answers 1) All elements can exist as liquid, so must have
waek IMFs. Most effective in large atoms wth lots of electrons
2) Because atoms do ot have electrons always evenly distributed, they sometimes move around. This
leads to a flickering dipole that induces a dipole attraction to another atom
3) atoms freeze at higher temperature down a colomn because of more electrons, so more likelyhood of
london dispersion force and stronger IMF, as described below
4) When one atom has partial charge, the electrons of another atom will pollarize to have electrons
furthest away from most concentrated part of atom, resulting in both atoms having distorted clound of
electorns and london dispesion force.
Properties of liquids
1) Surface tension
2) Capilary action
3) Viscosity - correct answers 1) Comes from liquids having molecules that more to the surface to increas
surface area. THis takes energy, so common iwth polar liquids. Tenson comes form attraction of liquids
on surface for molecules below, but none above.
2) Results from polar molecules with high cohesion and adhesion forces. Polar molecules in polar
container are attracted up the tibe, but stick to liquid molecules and pull them up too. REsults in polar-
concave mimicus and nonpolar-convex meniscus
3) Measurement of how difficult it is for liquid to move. Large molecules get tangled up easily, so have
high viscosity (high resistance to flow) . Molecules with large IMFs have high vescosity also.
1) Classifying solids
2) Lattice
graded A+ 2025/2026
1) Intramolecular force
2) What are condensed states
3) Intermolecular forces
4) What causes states - correct answers 1) Bonds formed within molecules
2) liquids and solids
3) Forces between molecules
4) Covalent, ionic, and intermolecular forces
1) What causes states
2) What happens in a state change
3) Do forces inside molecules break - correct answers 1) What causes states
2) The bonds between molecules are broken or formed. In ice, the particles are locked in place, and gain
more disorder as they move to liquid stage. They eventually are able to virbate lots in the gas stage
3) Not easily. Much more energy is required to break the intramolecular bonds than the intermolecular
bonds
1) How do polar bonds cause dipoles
2) Compare dipole-diople to ionic and covalent bonds - correct answers 1) The polar molecules have a
positive and negaitive charge, and line up opposite charges. This works best in liquid, where molecules
are close but able to move. They do it to maximize attraction and decrease repulsion.
2) dipole-dipole are about 0.99% as strong, and severly decrease with distance. Insignifican it low
pressure gas
1) Hydrogen bonds
2) Why do top 5,6,7,and 8A groups have much higher initial boiling points?
, 3) Why is high boiling point important for molar mass - correct answers 1) Hydrogen bonded with N, O,
of F are most strong, and called hydrogen bonds. Due to great polatitity difference and small hydrogen
atom
2) Because the first atom in the group is smallest and most polar.
3) very polar OH bonds
1) London Dispersion Forces evidence and most effective for
2) What are they
3) Freezing point periodicity
4) How does LDF force create dipole - correct answers 1) All elements can exist as liquid, so must have
waek IMFs. Most effective in large atoms wth lots of electrons
2) Because atoms do ot have electrons always evenly distributed, they sometimes move around. This
leads to a flickering dipole that induces a dipole attraction to another atom
3) atoms freeze at higher temperature down a colomn because of more electrons, so more likelyhood of
london dispersion force and stronger IMF, as described below
4) When one atom has partial charge, the electrons of another atom will pollarize to have electrons
furthest away from most concentrated part of atom, resulting in both atoms having distorted clound of
electorns and london dispesion force.
Properties of liquids
1) Surface tension
2) Capilary action
3) Viscosity - correct answers 1) Comes from liquids having molecules that more to the surface to increas
surface area. THis takes energy, so common iwth polar liquids. Tenson comes form attraction of liquids
on surface for molecules below, but none above.
2) Results from polar molecules with high cohesion and adhesion forces. Polar molecules in polar
container are attracted up the tibe, but stick to liquid molecules and pull them up too. REsults in polar-
concave mimicus and nonpolar-convex meniscus
3) Measurement of how difficult it is for liquid to move. Large molecules get tangled up easily, so have
high viscosity (high resistance to flow) . Molecules with large IMFs have high vescosity also.
1) Classifying solids
2) Lattice
