Question

intermolecular forces (imfs)
thinking steps:

1. all molecules have london dispersion forces (ldfs)
2. if the molecule is polar, it will have dipole - dipole forces
3. if the molecule contains an h - f, h - n, or h - o bond, it will have hydrogen bonds.

evaluate the following molecules below. determine the intermolecular forces present

1. h₂o

polar or nonpolar?
forces present:

1. ccl₄

polar or nonpolar?
forces present:
3.
(chemical structure image)
polar or nonpolar?
forces present:

Explanation:

For Molecule 1: $\boldsymbol{H_2O}$

Step1: Determine Polarity

$H_2O$ has a bent molecular geometry. The electronegativity difference between O and H creates a dipole moment, so it is polar.

Step2: Identify IMFs

All molecules have LDFs. Since it's polar, it has Dipole - Dipole Forces. Also, it has H - O bonds, so it has Hydrogen Bonds.

Step1: Determine Polarity

$CCl_4$ has a tetrahedral geometry. The individual C - Cl dipoles cancel out due to symmetry, so it is nonpolar.

Step2: Identify IMFs

All molecules have LDFs. Since it's nonpolar, only London Dispersion Forces are present (no dipole - dipole as it's nonpolar, and no H - F, H - N, or H - O bonds).

Step1: Determine Polarity

The molecular geometry around the O atom is bent (with two $CH_3$ groups). The electronegativity difference between O and C creates a net dipole moment, so it is polar.

Step2: Identify IMFs

All molecules have LDFs. Since it's polar, it has Dipole - Dipole Forces. It does not have H - F, H - N, or H - O bonds (the H atoms are bonded to C, not O in a way to form H - bonds here), so no Hydrogen Bonds.

Answer:

Polar or nonpolar? Polar
Forces present: London Dispersion Forces, Dipole - Dipole Forces, Hydrogen Bonds

For Molecule 2: $\boldsymbol{CCl_4}$