Question

What is the bond order of CO2

Answer 1

 The bond order refers to the number of bonds between a pair of atoms. The bond order can be determined by adding up all of the electrons in the bond, and subtracting the antibonding electrons (the lone pairs), and dividing the answer by 2: 
Bonding Order = number of bonding electrons – number of antibonding electrons/2. 

So for CO2, there is a total of 16 electrons, 8 of which are antibonding electrons. 
So 16 – 8 = 8; divided by 2 = 4. So, 4 is the bonding order of CO2. The molecular structure of CO2 looks like this: 
..~-~~.. 
O=C=O 
..~-~~.. 

There are two electrons on both the top and bottom of the O atoms, with a double bond between the C and O atoms. *Note: The electrons on top of the O atoms add up to 8 (4 for each O atom), and the other 8 electrons come from the double bonds between the O and C atoms - each line counts for 2 electrons. This is where you get a total of 16 electrons. 

Hope that helps you! Good luck! :) 

P.S here is a link to a tutorial on the bonding of CO2: http://treefrog.fullerton.edu/chem/LS/CO...

Answer 2

Please mark it as brainliest..

Answer:

Bond Order of CO2 is 2.

Explanation:

When we draw the canonical structure of CO2 we find out that three structure will formed.

By using the formula of bond order for resonating structure

Bond Order = Total number of bonds/

Total number of sigma bonds

In resonating structure of CO2 ;

Total bonds = 4

Total sigma bond =2

By using formula

Bond Order = 4/2

Bond Order =2

Hope it helps ..