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The correct order of increasing bond angles in the following triatomic species is:

1. NO2− < NO2 < NO2+
2. NO2 < NO2− < NO2+
3. NO2+ < NO2 < NO2−
4. NO2+ < NO2− < NO

Correct answer: NO2− < NO2 < NO2+

Solution

The bond angle depends on the number of lone pairs and bond pairs around the central atom. NO2− has the most lone pair repulsion, leading to the smallest bond angle, while NO2+ has no lone pairs, resulting in the largest bond angle.

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