Respuesta :
Explanation:
When carbon atom tends to form single bonds then its hybridization is [tex]sp^{3}[/tex], when carbon atom tends to form double bond then its hybridization is [tex]sp^{2}[/tex] and when a carbon atom is attached to a triple bond or with two double bonds then its hydridization is sp.
For example, in HCN molecule there is a triple existing between the carbon and nitrogen atom.
So, hybridization of carbon in this molecules is sp. Moreover, nitrogen atom is also attached via triple bond and it also has a lone pair of electrons. Hence, the hybridization of nitrogen atom is also sp.
Thus, we can conclude that s and p type of orbitals overlap to form the sigma bond between C and N in H−C≡N:
They conclude that s and also p-type of orbitals over-lap to form the sig-ma bond between C and then N in H−C≡N
What is the Sigma bond?
When carbon a-tom tends to form single bonds then its hybridization is sp³ when carbon a-tom tends to form a dual bond then its hybridization is sp² and also when a carbon a-tom is connected to a tripartite bond or with two dual bonds then its hybridization is sp.
For illustration, in the H-C-N molecule, there is a tripartite existing between the carbon and nitrogen atom.
Although, hybridization of carbon in these molecules is sp. Moreover, when the nitrogen a-tom is also attached via a tripartite bond and it also has a lone pair of electrons. Therefore, the hybridization of nitrogen a-toms is also sp.
Therefore, we can conclude that s and also p-type of orbitals over-lap to form the sig-ma bond between C and then N in H−C≡N
Find more information about Sigma bond here:
https://brainly.com/question/10123266
