Intermolecular Forces Quiz

Four hybrid sp3 orbitals are formed from

• two s orbitals and two p orbitals.

• an s orbital and a p orbital.

• three s orbitals and one p orbital.

• one s orbital and three p orbitals.

Dipole-dipole forces are considered the most important forces in polar substances because the London dispersion forces present in polar substances

• are no longer present.

• are usually much weaker than the dipole-dipole forces.

• are too unpredictable.

• act only in solids.

The strength of London dispersion forces between molecules depends on

• only the number of electrons in the molecule.

• only the number of protons in the molecule.

• both the number of electrons in the molecule and the mass of the molecule.

• both the number of electrons and the number of neutrons in the molecule

The strong forces of attraction between the positive and negative regions of molecules are called

• dipole-dipole forces.

• London forces.

• lattice forces.

• orbital forces.

Compared with molecular bonds, the strength of intermolecular forces is

• weaker.

• stronger.

• about the same.

• too variable to compare.

The equal but opposite charges present in the two regions of a polar molecule create a(n)

• electron sea.

• dipole.

• crystal lattice.

• ionic bond.

The reason the boiling point of water (H2O) is higher than the boiling point of hydrogen sulfide (H2S) is partially explained by

• London forces.

• covalent bonding.

• ionic bonding.

• hydrogen bonding.

The following molecules contain polar bonds. The only polar molecule is

• CCl4.

• CO2.

• NH3.

• CH4.

A polar molecule contains

• ions.

• a region of positive charge and a region of negative charge.

• only London forces.

• no bonds.

When a polar molecule attracts the electron in a nonpolar molecule,

• a dipole is induced.

• a crystal lattice forms.

• an ionic bond forms.

• a Lewis structure forms.