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QuestionChemistry
Question: no one two three The Lewis structure of NO^2 shows that nitrogen has bonding group(2$) and nonbonding group(2$). Therefore, it has a electron...
| Bond angles in NO^2NO^2 and associate ions | |
| --- | --- |
| Species | Bond angle |
| NO^2NO^2 | 134∘ |
| NO^2 +NO^2 + | 180∘ |
| NO^2 -NO^2 - | 115∘ |
| no | |
| --- | --- |
| one | |
| two | |
| three | |
| four | |
| linear | |
| bent | |
| trigonal planar | |
| trigonal pyramidal | |
| tetrahedral | |
| 90° | |
| 109.5° | |
| 120° | |
The Lewis structure of NO^2 shows that nitrogen has bonding group(2$) and nonbonding group(2$). Therefore, it has a electron geometry and a molecular geometry. For this molecular geometry, the idealized bond angles are , and the bond angle is predicted to be than that because bonding groups are repelled by a lone electron than by a pair of bonding electrons.
The Lewis structure of NO^2 + shows that nitrogen has bonding group(2$) and nonbonding group(2$). Therefore, it has a electron geometry and a molecular geometry. For this molecular geometry, the idealized bond angles are .
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Step 1:: Identify the molecular geometry of NO^2 and NO^2 +.
The molecular geometry of NO^2 is bent, and the molecular geometry of NO^2 + is linear.
Step 2:: Identify the ideal bond angles for each molecular geometry.
For a bent molecular geometry, the ideal bond angle is 120°. For a linear molecular geometry, the ideal bond angle is 180°.
Step 3:: Compare the ideal bond angles to the measured bond angles and explain the difference.
The measured bond angle for NO^2 is 134°, which is smaller than the ideal bond angle of 120°. This decrease in bond angle is due to the repulsion between the bonding groups and the lone electron pair on the nitrogen atom. The repulsion between bonding groups and lone electron pairs is greater than the repulsion between two bonding groups, causing the bond angle to be smaller than the ideal angle. The measured bond angle for NO^2 + is 180°, which is the same as the ideal bond angle for a linear molecular geometry. This is because there are no lone electron pairs on the nitrogen atom, and the bonding groups are not repelled by any lone electron pairs.
Final Answer
The molecular geometry of NO^2 is bent, with an ideal bond angle of 120° and a measured bond angle of 134°. The molecular geometry of NO^2 + is linear, with an ideal bond angle of 180° and a measured bond angle of 180°. The difference in bond angles is due to the repulsion between bonding groups and lone electron pairs.
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