Question

draw the lewis structure of the following molecule. use it to give the information

c₂i₂

number of single bonds

number of triple bonds

number of sigma bonds

number of pi bonds

number of unshared electrons

Explanation:

Step1: Determine valence electrons

Carbon has 4 valence electrons, iodine has 7 valence electrons. For \(C_2I_2\), total valence electrons \(= 2\times4 + 2\times7=8 + 14 = 22\).

Step2: Draw Lewis structure

The Lewis structure of \(C_2I_2\) is \(I - C\equiv C - I\).

Step3: Analyze bond types

• Single bonds: Each \(C - I\) bond is a single bond. So, number of single bonds \(= 2\).
• Triple bonds: The \(C\equiv C\) bond is a triple bond. So, number of triple bonds \(= 1\).
• Sigma bonds: A single bond has 1 sigma bond, a triple bond has 1 sigma bond. Total sigma bonds \(=2 + 1=3\).
• Pi bonds: A triple bond has 2 pi bonds. So, number of pi bonds \(= 2\).
• Unshared electrons: Each iodine has 3 lone pairs (6 unshared electrons). Total unshared electrons \(=2\times6 = 12\).

Answer:

Number of single bonds: \(2\)
Number of triple bonds: \(1\)
Number of sigma bonds: \(3\)
Number of pi bonds: \(2\)
Number of unshared electrons: \(12\)