
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
163.5k+ views
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.
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.
Recently Updated Pages
JEE Main 2021 July 25 Shift 1 Question Paper with Answer Key

JEE Main 2021 July 22 Shift 2 Question Paper with Answer Key

JEE Main 2025 Session 2: Exam Date, Admit Card, Syllabus, & More

JEE Atomic Structure and Chemical Bonding important Concepts and Tips

JEE Amino Acids and Peptides Important Concepts and Tips for Exam Preparation

JEE Electricity and Magnetism Important Concepts and Tips for Exam Preparation

Trending doubts
Types of Solutions

Degree of Dissociation and Its Formula With Solved Example for JEE

Instantaneous Velocity - Formula based Examples for JEE

JEE Main Chemistry Question Paper with Answer Keys and Solutions

JEE Main Reservation Criteria 2025: SC, ST, EWS, and PwD Candidates

What is Normality in Chemistry?

Other Pages
Thermodynamics Class 11 Notes: CBSE Chapter 5

Total MBBS Seats in India 2025: Government College Seat Matrix

NEET Total Marks 2025: Important Information and Key Updates

Neet Cut Off 2025 for MBBS in Tamilnadu: AIQ & State Quota Analysis

Karnataka NEET Cut off 2025 - Category Wise Cut Off Marks

NEET Marks vs Rank 2024|How to Calculate?
