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Chapter 22: Problem 26

Draw a Lewis structure for the \(\mathrm{C}_{2}^{2-}\) ion.

Short Answer

Expert verified
The Lewis structure for the \(\mathrm{C}_{2}^{2-}\) ion has a triple bond between the two carbon atoms, and each carbon atom has one lone pair of electrons.

Step by step solution

01

Determine total number of valence electrons

For carbon, there are 4 valence electrons. The ion has two carbons and 2 extra electrons (associated with the charge), so \(4*2 + 2 = 10\) electrons in total.
02

Draw skeleton structure of the ion

Carbon atoms typically make multiple bonds, so the carbon atoms will be bonded together. Draw a line to represent the bond between the two carbon atoms, which uses up 2 electrons, leaving \(10 - 2 = 8\) electrons.
03

Distribute remaining electrons

Next, distribute the remaining 8 electrons to the outer atoms. In this case, they're both carbons. Each atom will get 4 electrons, which are represented as dots. Now, each carbon atom has a total of 6 electrons (2 from the bond and 4 around it).
04

Check the octet rule

Looking at the structure, it can be observed that each carbon atom only has 6 electrons, violating the octet rule. To fulfill this rule, shift one pair of non-bonding electrons from each carbon atom to form a bond between them.
05

Draw final Lewis structure

The Lewis structure will now show a triple bond between the carbon atoms. Each carbon atom will now be surrounded by 8 electrons (6 from the triple bond and 2 lone electrons), hence fulfilling the octet rule.

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