Question

The single, double, and triple bond lengths of carbon in carbon dioxides are respectively.
(a) \[1.15,1.15,\]and \[1.10\] Angstrom
(b) \[1.22,1.15,\]and \[1.10\] Angstrom
(c) \[1.10,1.15,\]and \[1.22\] Angstrom
(d) \[1.15,1.10,\]and \[1.22\] Angstrom

Answer 1

Hint: Based on sharing of elections during the chemical bond formation. The chemical bond can be classified into three types (a) single bond, (b) double bond, and (c) triple bond, respectively.

Complete step by step solution:We all know atoms involved in chemical bond formation. On the other hand, we can say that atoms combined to complete their octet.
On the basis of the requirement of the electron by the atoms to complete their octet, they can form single, double and triple bonds respectively.
Carbon dioxide is a linear molecule which has a \[C{O_2}\]formula.
The structure of carbon dioxide is composed of one carbon atom and two oxygen atoms.
At room temperature, the carbon dioxide molecule exists in gaseous form.
The structure of carbon dioxide exists in three resonating forms and in its resonating structure it has single, double and triple bonds respectively.

Image: Resonating structure of carbon dioxide.
Because of the three resonating structures, the carbon dioxide has single, double and triple bonds.
The bond length for single, double, and triple bonds will be \[1.22,1.15\] and \[1.10\] Angstrom respectively.

Therefore from the above explanation we can say option (b) will be the correct option:

Note: The carbon di-oxide is a nonpolar molecule due to linear and symmetrical structure.
Carbon dioxide is known as an electrophile in organic chemistry.
The carbon dioxide molecule has \[s{p^2}\]hybridization with linear geometry and shape.