Question

part b:
the diagram below shows an incorrect model of co, identify one error in the diagram and explain why it does not correctly show covalent bonding.
o - c - o

part c:
draw a correct lewis structure for co,

Explanation:

Carbon has 4 valence electrons and each oxygen has 6 valence electrons. In \(CO_2\), carbon forms double bonds with each oxygen to complete the octet (8 - electron) rule. The given diagram \(O - C - O\) shows single bonds. With single bonds, carbon would only have 6 electrons around it (\(2\) from each single bond), which violates the octet rule.

Answer:

One error is that the diagram shows single bonds (\(O - C - O\)) instead of double bonds (\(O = C = O\)). Carbon needs to share 4 electrons (in \(CO_2\), two double bonds) to complete its octet. With single bonds, carbon has only 6 electrons (violates octet rule). For the Lewis structure of \(CO_2\):

• Place carbon in the center.
• Each oxygen forms a double bond with carbon (\(O = C = O\)).
• Add the remaining non - bonding electrons on the oxygen atoms (each oxygen has 4 non - bonding electrons: \(O::C::O\) with two pairs of dots on each oxygen).