Polar and non polar

Question

N-H POLAR

C-O POLAR

B-F POLAR

C-H NONPOLAR

1) Determine whether the following substances are: ionic, polar covalent molecules, or non-polar

1. For which of the compounds above (if any) would you expect to see hydrogen bonding between molecules of that type? Justify your answer.

NaH NH3 CH2O BF3

1. What characteristics must a compound have in order for hydrogen bonding to be possible?
2. For each pair of molecules below, list all of the intermolecular forces you would expect to be present between them. Many will have more than one force as part of a complete answer.
3. NaH and NaH
4. NHs and NHs
5. CH2O and CH2O
6. BF3 and BF;
7. NH, and CH2O

Answer 1

1) Determine whether the following substances are: ionic, polar covalent molecules, or non-polar

NaH - ionic (this is a metal hydride and is considered ionic)

NH₃ - polar covalent.

CH₂O - polar covalent.

BF₃ - non polar.

For which of the compounds above (if any) would you expect to see hydrogen bonding between molecules of that type? Justify your answer.

The only one that will exhibit hydrogen bonding is NH₃ because it is the only compound that has a hydrogen atom (H) attached to either an O, N or F atom. Obviously, the H is bonded to N.

The characteristics that a compound must have in order to exhibit hydrogen bonding is that the hydrogen atom (H) of the molecule must be bonded to either N, O or F.

NaH and NaH will exhibit ionic bonding

NH₃ and NH₃ will exhibit hydrogen bonding as well as dipole-dipole and London dispersion

CH₂O and CH₂O will exhibit dipole-dipole and London dispersion

BF₃ and BF₃ will exhibit London dispersion

NH₃ and CH₂O will exhibit dipole-dipole and London dispersion