Rank N2, 02, LiBr, and SCl, in order of increasing boiling point, based on polarity and intermolecular forces.

Answer 1

To rank N₂, O₂, LiBr, and SCl in order of increasing boiling point, we need to consider the types and strengths of intermolecular forces that each compound experiences. Here's a brief summary of the relevant intermolecular forces and polarity for each compound:

1. **N₂ (Nitrogen gas)**:
- **Polarity**: Nonpolar
- **Intermolecular Forces**: Dispersion forces (also called London dispersion forces)

2. **O₂ (Oxygen gas)**:
- **Polarity**: Nonpolar
- **Intermolecular Forces**: Dispersion forces (London dispersion forces)

3. **LiBr (Lithium bromide)**:
- **Polarity**: Ionic compound
- **Intermolecular Forces**: Ionic bonds, which are very strong compared to dispersion forces

4. **SCl (Sulfur monochloride)**:
- **Polarity**: Polar (has a dipole moment due to differences in electronegativity between sulfur and chlorine)
- **Intermolecular Forces**: Dipole-dipole interactions, possibly some dispersion forces

Based on the strength of intermolecular forces:

- Dispersion forces are generally weak.
- Dipole-dipole interactions are stronger than dispersion forces but weaker than ionic bonds.
- Ionic bonds are much stronger than both dispersion forces and dipole-dipole interactions.

Given this information, we can rank the compounds in order of increasing boiling point:

1. **N₂ (Nitrogen gas)**: Nonpolar with weak dispersion forces, so it has the lowest boiling point.
2. **O₂ (Oxygen gas)**: Nonpolar with weak dispersion forces, slightly higher than N₂ but still very low.
3. **SCl (Sulfur monochloride)**: Polar with dipole-dipole interactions, so higher boiling point than nonpolar molecules.
4. **LiBr (Lithium bromide)**: Ionic compound with very strong ionic bonds, so it has the highest boiling point.

Therefore, the order of increasing boiling point is:

\[ \text{N}_2 < \text{O}_2 < \text{SCl} < \text{LiBr} \]