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WorksheetsUnit 4 Chemistry Review: IMFs, Polarity, Lewis Structures
Total questions: 20
Worksheet time: 19mins
Which of the following can result in a London dispersion force?
When a non-polar molecule becomes slightly polar for an instant
When the oppositely charged ends of a polar molecule attract each other.
When there is very strong dipole-dipole attraction between a hydrogen atom and a polar molecule
When an ion comes close enough to a non-polar molecule to change its electron density.
In liquid sulfur dioxide, which of the following types of intermolecular force(s) would be present?
London dispersion forces
London dispersion forces, dipole-dipole forces
London dispersion forces, dipole-dipole forces, hydrogen bonding
London dispersion forces, dipole-dipole forces, hydrogen bonding, covalent bonds
Which one of the following substances will have hydrogen bonding as one of its intermolecular forces?
IV only
II and V
I and III
IV and II
Which phrase best completes the following statement: “The electrons in a bond between two iodine atoms (I2) are shared…”?
Equally, and the resulting bond is polar.
Equally, and the resulting bond is nonpolar.
Unequally, and the resulting bond is polar.
Unequally, and the resulting bond is nonpolar
Which number represents the hydrogen that is capable of hydrogen bonding in acetic acid?
(i)
(ii)
(iii)
(iv)
Consider the following structures. If the A-B bonds are polar, which of the following molecules are polar?
I and III
II and V
I, II, and IV
II and IV
Water (H2O) and dihydrogen monosulfide (H2S) have similar chemical formulas and structures. At room temperature, H2O is a liquid and H2S is a gas. Which of the following best explains this difference?
H2S molecules are larger and exhibit stronger London dispersion forces and require a greater amount of energy to break.
H2S molecules are larger and thus the electrons are not attracted as strongly, which makes the covalent bonds in H2S molecules easier to break.
H2O molecules exhibit hydrogen bonding, and thus the attractive forces between water molecules are stronger than the attractive forces between H2S molecules.
H2O molecules are smaller and thus exhibit weaker London dispersion forces and require a lesser amount of energy to break
Which of the following lists all intermolecular forces experienced between this molecule and an identical molecule?
Covalent bonding, dipole-dipole, and London dispersion forces would be present.
Only dipole-dipole and London dispersion forces would be present
Only covalent bonding and London dispersion forces would be present.
Only London dispersions forces would be present.
Which of the following describes changes in forces of attraction that occur as H2O changes phase from liquid to gas?
H – O bonds break as H – H and O – O bonds form.
Hydrogen bonds between H2O molecules are broken
Covalent bonds between H2O molecules are broken
Ionic bonds between H+ and OH- ions are broken
The boiling points of three halide compounds are shown above. Which of the following identifies the substance that has the strongest intermolecular forces and provides reasoning?
CH2Cl2, because it has the lowest boiling point.
CH2Cl2, because it exhibits hydrogen bonding
CH2Br2, because it has the highest boiling point
CH2I2, because it has the highest boiling point
According to VSEPR theory, what is the three-dimensional shape of the NH3 molecule?
Linear
Bent
Trigonal planar
Trigonal pyramidal
A diagram of methanol molecules is shown here. Which letter labels a line that represents hydrogen bonding between the molecules?
A
B
C
D
For a container of liquid trimethylamine, what intermolecular forces would be present?
London Dispersion Forces
London Dispersion Forces, Dipole-Dipole
London Dispersion Forces, Dipole-Dipole, Hydrogen Bonding
London Dispersion Forces, Dipole-Dipole, Covalent bonds
For a container of liquid propylamine, what intermolecular forces would be present?
London dispersion forces
London dispersion forces, dipole-dipole forces
London dispersion forces, dipole-dipole forces, hydrogen bonding
London dispersion forces, dipole-dipole forces, covalent bonding
What is the VSPER Shape of the pictured molecule?
Trigonal planar
Bent
Linear
Tetrahydral
What is the VSPER Shape of the pictured molecule?
Trigonal Planar
Tetrahydral
Trigonal Pyramidal
Octahydral
What is the VSPER Shape of the pictured molecule?
Trigonal Pyramidal
Trigonal Planar
Linear
Tetrahydral
Which compound is represented in the picture?
H2O
SO2
H2S
CCl2
Which of the following compounds will be the hardest to break up with heat?
H-Cl
NH3
F2
O2
Which compound contains only London Dispersion Forces and Dipole-Dipole IMFs?
H2O
F2
SO2
HF
