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Chapter 15: Problem 2

a) Explain explicitly why there is a total of 10 electrons in the Lewis structure for CO. b) Explain why a Lewis structure of \(\mathrm{CO}\) with a single bond between \(\mathrm{C}\) and \(\mathrm{O}\) and two lone pairs of electrons on each atom is not a valid Lewis structure. (Hint: consider drawing the Lewis structure that is described.) c) Show explicitly why the formal charge on \(\mathrm{C}\) is \(-1\) and the formal charge on \(\mathrm{O}\) is \(+1\) for the Lewis structure of \(\mathrm{CO}\) shown in Model 2

Short Answer

Expert verified
In the Lewis structure of CO, there are 10 valence electrons. However, a structure with a single bond between Carbon and Oxygen and two lone pairs on each atom is invalid as it contradicts real world Lewis structures. From Model 2, the formal charge on Carbon is -1 and the charge on Oxygen is +1.

Step by step solution

01

Identify the Total Number of Electrons

To construct a Lewis structure, it is first important to count the total number of valence electrons in the atom. Carbon has 4 valence electrons and Oxygen has 6 valence electrons. Thus, a total of 10 valence electrons (4 from Carbon + 6 from Oxygen) are present in a CO molecule.
02

Determine the Validity of Lewis Structure of CO

A Lewis structure of CO with a single bond between C and O and two lone pairs of electrons on each atom is not valid. This is because such a structure leads to a formal charge of +2 on Carbon and -2 on Oxygen, which does not match with real-world observations. In real world, Carbon usually forms 4 bonds while Oxygen forms 2 bonds and retains two lone pairs.
03

Determine the formal charges

In Model 2, the Lewis structure of CO shows a triple bond between Carbon and Oxygen with one lone pair on each of the atoms. The calculation of the formal charge on C and O is done with the formula Formal Charge = (Valence electrons) – (Lone pair electrons + 1/2 Bonding electrons). For Carbon, Formal charge = 4 - (0 + (1/2 * 6)) = -1. For Oxygen, Formal charge = 6 - (2 + (1/2 * 8)) = +1

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Most popular questions from this chapter

a) Explain explicitly why there are eight electrons in the Lewis structure for \(\mathrm{H}_{2} \mathrm{O}\). b) Complete the following table based on the Lewis structure of \(\mathrm{H}_{2} \mathrm{O}\). $$ \begin{array}{|l|c|c|c|} \hline & \begin{array}{c} \text { Left H } \\ \text { atom } \end{array} & \text { O atom } & \begin{array}{c} \text { Right H } \\ \text { atom } \end{array} \\ \hline \text { Core charge } & & & \\ \hline \text { Total assigned electrons } & & & \\ \hline \text { Formal charge } & & & \\ \hline \end{array} $$

If the net charge on a molecule is zero, must the formal charge on every atom in the molecule equal zero? Why or why not?

Show explicitly how the number of electrons in each of the two Lewis structures for \(\mathrm{CO}_{2}\) was determined.
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