Bent/Angular Bond Angles
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Bent/Angular Bond Angles
Please confirm: The approximate bond angles for a bent/angular molecule will be <120 or <109.5 depending on the number of lone pairs. (AX2E2 is <109.5 and AX2E is <120)
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Re: Bent/Angular Bond Angles
Yes, this is because the existence of lone pairs causes the bond angles to repel resulting in a decreased angle.
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Re: Bent/Angular Bond Angles
Yes you are correct.
If there is one lone pair (and 2 atoms) the electron geometry will be trigonal planar, however the molecular geometry is bent. Since it has 3 regions of e- density, the bond angles would be a little less than that of a trigonal planar with no lone pairs, so <120*
If there are 2 lone pairs (and 2 atoms) the electron geometry will be tetrahedral, however the molecular geometry is bent. Since there are 4 regions of e- density the bond angles would be less than that of a tetrahedral with no lone pairs, so <109.5*
If there is one lone pair (and 2 atoms) the electron geometry will be trigonal planar, however the molecular geometry is bent. Since it has 3 regions of e- density, the bond angles would be a little less than that of a trigonal planar with no lone pairs, so <120*
If there are 2 lone pairs (and 2 atoms) the electron geometry will be tetrahedral, however the molecular geometry is bent. Since there are 4 regions of e- density the bond angles would be less than that of a tetrahedral with no lone pairs, so <109.5*
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