Write the Lewis structure for CO[latex]_{2}[/latex].

Because carbon is the less electronegative atom, put it in the central position. O C O Total number of electrons for Lewis structure = [latex] \left( \begin{matrix} \text{number of} \\ \text{valence} \\ e^- \text{for }C \end{matrix} \right) [/latex] +2 [latex] \left( \begin{matrix} \text{number of } \\ \text{valence }\\ e^- \text{for } O \end{matrix}\right) [/latex] = 4 + 2(6) = 16 Bonding electrons are first. O:C:O (4 of 16 electrons used) Lone pairs on terminal atoms are next. [latex]:\overset{..}{\underset{..}{O}}:C:\overset{..}{\underset{..}{O}}:[/latex] (16 of 16 electrons used) Carbon lacks an octet in this case. Move lone pairs from the oxygen atoms to bonding regions to form double bonds.

Question 9.4: Write the Lewis structure for CO2.

Principles of Chemistry: A Molecular Approach

Write the Lewis structure for CO $_{2}$ .

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Because carbon is the less electronegative atom, put it in the central position.
O C O

Total number of electrons for Lewis structure =

$\left( \begin{matrix} \text{number of} \\ \text{valence} \\ e^- \text{for }C \end{matrix} \right)$ +2 $\left( \begin{matrix} \text{number of } \\ \text{valence }\\ e^- \text{for } O \end{matrix}\right)$

= 4 + 2(6) = 16

Bonding electrons are first.
O:C:O
(4 of 16 electrons used) Lone pairs on terminal atoms are next.