## hybridization

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

Guzman_1J
Posts: 72
Joined: Wed Sep 18, 2019 12:16 am

### hybridization

Is hybridization just a blend of all resonance structures or is it atoms making certain bonds? I'm still a little confused on the topic.

zachary_nhem_4I
Posts: 57
Joined: Sat Aug 17, 2019 12:18 am

### Re: hybridization

Hybridization is the idea that atomic orbitals fuse to form newly hybridized orbitals, which in turn, influences molecular geometry and bonding properties.

ThomasNguyen_Dis1H
Posts: 102
Joined: Fri Aug 30, 2019 12:17 am

### Re: hybridization

Hybridization is the concept of combing orbitals so that an atom has space in their orbitals to hold bonding electrons.

Kevin Liu 1J
Posts: 53
Joined: Thu Jul 25, 2019 12:16 am

### Re: hybridization

Hybridization does represent the blend of the resonance structures and refers to their molecular shapes (i.e. sp, sp2, sp3, etc.)

alex_4l
Posts: 109
Joined: Thu Sep 26, 2019 12:18 am

### Re: hybridization

Hybridization is basically the concept of mixing atomic orbitals into new hybrid orbitals (these can have new energies, shapes different from the component atomic orbitals) which then make it suitable for the pairing of electrons to form chemical bonds. The regions of electron density = the number of hybrid orbitals. I'm sure he'll go more in depth with the process of what this is but the example from class is a good introduction to it:
C: [He] 2s^2, 2px^1, 2pz^1 would be the atomic orbitals and the hybridization orbital would be sp^3 since you combine the 1 s orbital and the 3 p orbitals to get 4, therefore each spot has one upward arrow in the hybrid orbital. This is pretty much combining the atomic orbitals into one hybrid version of the orbitals.
I hope that makes more sense! It's a new tricky topic

alex_4l
Posts: 109
Joined: Thu Sep 26, 2019 12:18 am

### Re: hybridization

Also an easy trick is just to count the number of electron density areas around an atom. 4 areas is sp^3, 3 areas is sp2, 2 is sp