# What is the hybridization for C2H6? my teacher wrote sp-s sigma bond [C-H] and sp-sp sigma bond[C-C]

##### 1 Answer

Either your teacher is incorrect or your molecular formula is incorrect.

**IF YOUR FORMULA IS CORRECT**

**four** electron groups surrounding each carbon. It made *four* ** identical** bonds in a perfect

**tetrahedral**geometry, which means it needed

*four*

**orbitals to make those bonds.**

*identical*Each carbon has to hybridize **one** **three** **four** identical

Therefore, each **(b)**), and each **(b)**).

**IF YOUR TEACHER WAS CORRECT ON THE HYBRIDIZATIONS**

On the other hand,

With **two** electron groups on a **POLYatomic** molecule, each carbon requires only **two** ** lobes** and hence only

**one**

*other*carbon AND a

*single*hydrogen.

In this case we can see that:

- The
#sp# of carbon 1 (YELLOW dumbbell) overlaps with one hydrogen's#1s# (BLUE sphere) to make a#\mathbf(sigma)# **bond**. - The
#sp# of carbon 1 (YELLOW dumbbell) overlaps with the#sp# of carbon 2 (YELLOW dumbbell) and vice versa to make a#\mathbf(sigma)# **bond**. - The
#sp# of carbon 2 (YELLOW dumbbell) overlaps with the second hydrogen's#1s# (BLUE sphere) to make a#\mathbf(sigma)# **bond**.

Each **triple bond** incorporates an *additional* **two**

Hence, when including those two *the* ** triple bond** between carbons 1 and 2.

(One triple bond = 1