Question

Identify the major intermolecular forces between each of the

following atoms or molecules:

a. $P{H}_3$

b. $N{O}_2$

c. localid="1652945006972" $C{H}_{3_{}}N{H}_2$

d.localid="1652945003975" $Ar$

Short answer

a. The major intermolecular forces between given molecule in$P{H}_3$ is dipole-dipole interaction .

b. The major intermolecular forces between given molecule in$N{O}_2$ is dipole-dipole interaction.

c. The major intermolecular forces between given molecule in$C{H}_{3}N{H}_2$ is Hydrogen bonding.

d, The major intermolecular forces between given molecule in$Ar$ is Van Der Waals forces.

Step-by-step solution

Part(a) Step 1: Given information

We need to find the intermolecular force between $P{H}_3$.

Part(a) Step 2: Explanation

It is a polar molecule, it creates dipole-dipole. Since $P{H}_3$ isn't symmetrical, it must be polar. It is not symmetrical since it has a lone pair and lacks a trigonal planar shape.

Part(b) Step 1: Given information

We need to find the intermolecular force between $N{O}_2$.

Part(b) Step 2: Explanation

Because $N{O}_2$is a polar molecule with a bent structure, dipole-dipole forces are the most important intermolecular interactions.

Part(c) Step 1: Given information

We need to find the intermolecular force between$C{H}_{3}N{H}_2$

Part(c) Step 2: Explanation

Hydrogen Bonding: A dipole-dipole force that requires one of the three most electronegative elements, $F$, $O$, or $N$, to be covalently bound to a hydrogen atom (such as $C{H}_{3}N{H}_2$).

Part(d) Step 1: Given information

We need to find the intermolecular force between$Ar$

Part(d) Step 2: Explanation

Argon ionises at a temperature of $15.76$degrees Kelvin, which is greater than hydrogen but lower than helium, neon, or fluorine. Van der Waals molecules containing argon can be kept together by London dispersion forces only very weakly.