Question

Which of the following statement is correct?

• A. $CO_2$ molecule contains one C-O and one C=O bonds and one lone pair on each oxygen atom.
• B. $CO_2$ molecule contains two C-O bonds and one lone pair on each oxygen atom
• C. $CO_2$ molecule contains one C-O bond and one C=O bond with two lone pairs on each oxygen atom.
• D. $CO_2$ molecule contains one C-O bond and one C$\equiv$O and one lone pair on each oxygen atom.
• E. $CO_2$ contains two $C=O$ bonds and two lone pairs on each oxygen atom

Hint:

Remember the formula $VSEPR$: Carbon is $sp$ hybridized in $CO_2$, leading to a linear shape and double bonds to satisfy the valency of 4 for Carbon.

Answer 1

Answer: (E)

Step 1: Understanding the Concept:
To determine the bonding in CO\textsubscript{2}, we must draw the Lewis structure based on valence electrons. Carbon has 4 valence electrons and Oxygen has 6.
Step 2: Key Formula or Approach:
1. Total valence electrons = 4 + (2 \(\times\) 6) = 16.
2. Carbon is the central atom. Form double bonds with oxygen to complete the octet for Carbon.
Step 3: Detailed Explanation:
In the stable Lewis structure of CO\textsubscript{2}, Carbon forms two double bonds (C=O) with the two Oxygen atoms.
Structure: O=C=O
Carbon octet is complete (4 electrons from double bonds).
Each Oxygen atom has used 2 electrons for the double bond, leaving 4 valence electrons (2 lone pairs) on each Oxygen atom to complete its octet.
Total electrons: (2 bonds \(\times\) 4) + (2 oxygens \(\times\) 4) = 16.
Step 4: Final Answer:
Statement E is correct: CO\textsubscript{2} has two C=O bonds and two lone pairs on each oxygen.