The correct order for bond angles is :

Options

A. `NO_(2)^(+) lt NO_(2) lt NO_(2)^(-)`
B. `NO_(2)^(+) lt NO_(2)^(-) lt NO_(2)`
C. `NO_(2)^(-) lt NO_(2)^(+) lt NO_(2)`
D. `NO_(2)^(-) lt NO_(2) lt NO_(2)^(+)`

Explanation

To determine the correct order of bond angles for the species NO2+, NO2, and NO2-, we will analyze the bond angles based on their molecular geometries and the effects of lone pairs of electrons.

### Step 1: Identify the molecular geometries
- **NO2+ (Nitronium ion)**: This species has a linear geometry due to the absence of lone pairs on the nitrogen atom. The bond angle is 180 degrees.
- **NO2 (Nitrogen dioxide)**: This molecule has a bent geometry due to one lone pair of electrons on the nitrogen atom. The bond angle is approximately 134 degrees.
- **NO2- (Nitrite ion)**: This species also has a bent geometry, but it has two lone pairs of electrons on the nitrogen atom. The bond angle is reduced to about 115 degrees.

### Step 2: Compare the bond angles
Now, we can summarize the bond angles:
- NO2+ has a bond angle of 180 degrees.
- NO2 has a bond angle of 134 degrees.
- NO2- has a bond angle of 115 degrees.

### Step 3: Establish the order of bond angles
From the values obtained:
- NO2+ (180°) > NO2 (134°) > NO2- (115°)

### Conclusion
The correct order for the bond angles is:
**NO2+ > NO2 > NO2-**