(Polar molecules, Non-polar molecules, etc.)
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O3 and NO2- both have the same VSEPR formula. Why then, are the bond angles for 03 116.8 degrees and the bond angles for NO2- 116 degrees? Does this have to with central/surrounding atom size or electronegativities?
The bond angle decreases as the central atom's size increases. Thus, since Nitrogen is slightly larger than Oxygen, the NO2- should have a slightly smaller bond angle. Also, if the electronegativity of the central atom decreases, then the bond angle decreases.
Exactly^! Dr. Lavelle has mentioned, though, that we will not be expected to know these exact angles--we just need to know which normal bond angle (90, 109.5, 120, etc.) the angle will be slightly less than due to repulsion from lone pairs.
I believe if the electronegativity of the central atom decreases, so will the bond angle.
The bond angle varies with multiple factors. For this specific example, you can look at electronegativity. The bond angle will decrease as electronegativity decreases. You can also look at the size, since those with more electrons will have more repulsion and create a smaller bond angle. We don't need to know specific numbers; just knowing an approximation or knowing it's less than some number should be enough.
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