## single vs double vs triple bonds

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

Chris Tai 1B
Posts: 102
Joined: Sat Aug 24, 2019 12:16 am

### single vs double vs triple bonds

Why doesn't the number of bonds affect which hybrid orbital is formed? For instance, in ethylene c2h4, why is the double bond in between the carbons just two sp^2 hybrid orbitals instead of two individual sp^3 orbitals (since there are four bonds formed by carbon in total)?

Selena Yu 1H
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Joined: Fri Aug 09, 2019 12:16 am
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### Re: single vs double vs triple bonds

The number of bonds don't affect the hybridization because we see double and triple bonds as one region of electron density just like how we did when we determining shape using VSEPR.

Veronica_Lubera_2A
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### Re: single vs double vs triple bonds

Single, double, and triple bonds all represent one region of electron density. Therefore, sp hybridization has 2 regions of electron density, sp2 has 3 regions of electron density, sp3 has 4 regions, sp3d has 5 regions, and so on.

Joelle 3L
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Joined: Sat Jul 20, 2019 12:16 am

### Re: single vs double vs triple bonds

Single, double, and triple bonds each represent only one region of electron density. Other regions of electron density would include lone pairs. In C2H4 the hybridization of the carbon would be sp2 since there are three regions of electron density.

Rebecca Remple 1C
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### Re: single vs double vs triple bonds

Chris Tai 1L wrote:Why doesn't the number of bonds affect which hybrid orbital is formed? For instance, in ethylene c2h4, why is the double bond in between the carbons just two sp^2 hybrid orbitals instead of two individual sp^3 orbitals (since there are four bonds formed by carbon in total)?

Hi Chris,

I agree with the previous posters that any bond (single, double, or triple) is a single area of electron density and has no effect on hybridization. For hybridization, I find it helpful to draw an Aufbau diagram to visualize where areas of high electron density are. I hope this helps! Have a great day :)

-Rebecca