Question

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

c₂br₄

number of single bonds

number of double bonds

number of sigma bonds

number of pi bonds

number of unshared electrons

Explanation:

Step1: Determine the central atom

Carbon is the central atom. Each carbon has 4 valence electrons, and each bromine has 7 valence electrons. The total number of valence electrons is \(2\times4 + 4\times7= 8 + 28=36\).

Step2: Draw the Lewis structure

The structure is \(Br - C - C - Br\) with each carbon having two more bromine atoms attached. Each single bond is a sigma bond. There are no double bonds (so no pi bonds from double bonds).

• Number of single bonds: Each \(C - Br\) and \(C - C\) is a single bond. There are \(6\) single bonds (\(4\) \(C - Br\) and \(2\) \(C - C\)).
• Number of double bonds: \(0\)
• Number of sigma bonds: All single bonds are sigma bonds. So, \(6\) (same as single - bond count since single bonds are sigma bonds)
• Number of pi bonds: \(0\) (no double or triple bonds)
• Number of unshared electrons: Each bromine has \(6\) unshared electrons (since each \(Br\) has \(7\) valence electrons and uses \(1\) in bonding). There are \(4\) \(Br\) atoms. So, \(4\times6 = 24\)

Answer:

Number of single bonds: \(6\)
Number of double bonds: \(0\)
Number of sigma bonds: \(6\)
Number of pi bonds: \(0\)
Number of unshared electrons: \(24\)