Q30E - Chemistry (OpenStax)

Question

For each of the following structures, determine the hybridization requested and whether the electrons will be delocalized:

(a)Hybridization of each carbon

(b)Hybridization of sulphur

(c)

All atoms

 

Step-by-Step Solution

Answer

(a) From left to right, the hybridization of each carbon atom is  sp², \({\rm{s}}{{\rm{p}}^{\rm{3}}}\), and sp² .  Delocalized electrons do not exist.

(b) Electrons are delocalized after  sp² hybridization of sulphur.

(c) All carbons and nitrogen have been  sp² hybridised, while hydrogen has been s hybridised

Step 1: Define hybridization

Hybridization is a concept in organic chemistry that is used to explain chemical bonding when the valence bond theory fails to provide adequate explanation. This hypothesis is particularly useful for explaining organic molecules' covalent bonding

Step 2: Explanation

(a) There will be no delocalization of electrons.

Acetone

The hybridisation of saturated carbon is \(s{p^3}\) and double bonded carbon it is  sp².

Step 3: Explanation

(b) Delocalization of electrons will occur.

Sulfur dioxide

The hybridisation of sulfur is sp² . 

Step 4: Explanation

a. Delocalization of electrons will occur.

 

 

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