## 2F.7

$sp, sp^{2}, sp^{3}, dsp^{3}, d^{2}sp^{3}$

Annie Ye
Posts: 106
Joined: Wed Sep 18, 2019 12:22 am

### 2F.7

Identify the hybrid orbitals used by the atom in boldface red type in each of the following species: (a) BF3; (b) AsF3; (c) BrF3; (d) SeF31.

AArmellini_1I
Posts: 107
Joined: Fri Aug 09, 2019 12:15 am

### Re: 2F.7

What I do first is draw the lewis structures. The number of electron dense regions corresponds with the hybridization orbital. For hybridization orbitals it go s, p1, p2, p3, d1, d2, d3, d4, d5 and so on (I believe)

Julie Park 1G
Posts: 100
Joined: Thu Jul 25, 2019 12:15 am

### Re: 2F.7

You'll first want to find the # of electron densities surrounding the atom in question. In (a), BF3, B is bonded to three F atoms in single bonds. According to the chart, the three bonds (electron densities) would give the B in BF3 to a s1p2 (sp2) hybrid orbital.

1 --> s1
2 --> s1p1
3 --> s1p2
4 --> s1p3
5 --> d1s1p3

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