The incorrect order of boiling point is :

Options

A. `H_(2)O gt CH_(3)OH`
B. `N(CH_(3))_(3) gt NH(CH_(3))_(2)`
C. `H_(3)PO_(4) gt Me_(3)PO_(4)`
D. `CH_(3)N_(3) gt HN_(3)`

Explanation

To determine the incorrect order of boiling points among the given compounds, we need to analyze the boiling points based on their molecular structures and the types of intermolecular forces they exhibit. Here’s a step-by-step breakdown of the solution:

### Step 1: Analyze the first option (H2O vs. CH3OH)
- **H2O (water)** has a higher boiling point than **CH3OH (methanol)**. This is because both molecules can form hydrogen bonds, but water has a greater capacity for hydrogen bonding due to its smaller size and higher electronegativity of oxygen. Therefore, this order is **correct**.

### Step 2: Analyze the second option (N(CH3)2 vs. NH(CH3)2)
- **N(CH3)2 (dimethylamine)** has a higher molecular mass and surface area compared to **NH(CH3)2 (methylamine)**. The presence of two methyl groups in dimethylamine increases its boiling point due to increased van der Waals forces. Thus, this order is also **correct**.

### Step 3: Analyze the third option (H3PO4 vs. Me3PO4)
- **H3PO4 (phosphoric acid)** has a higher boiling point than **Me3PO4 (trimethyl phosphate)** because H3PO4 can form strong intermolecular hydrogen bonds, while Me3PO4 cannot. Therefore, this order is **correct**.

### Step 4: Analyze the fourth option (CH3N3 vs. HN3)
- **HN3 (hydrazoic acid)** can form hydrogen bonds due to the presence of hydrogen attached to nitrogen, while **CH3N3 (methyl azide)** primarily exhibits dipole-dipole interactions. Since hydrogen bonding is a stronger intermolecular force than dipole-dipole interactions, HN3 will have a higher boiling point than CH3N3. Thus, the order CH3N3 < HN3 is **incorrect**.

### Conclusion
The incorrect order of boiling points is given in option D: **CH3N3 < HN3**. Therefore, the correct answer is option D.

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