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Chapter 15: Problem 4

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

Short Answer

Expert verified
The number of electrons in the Lewis structure of CO2 is determined by adding the valence electrons of individual atoms. Carbon contributes 4, each Oxygen contributes 6, giving a total of 16 valence electrons. These are divided into bonding and non-bonding electrons in accordance with the structure, including double or triple bonds.

Step by step solution

01

Understanding Electron Count

To count the electrons in Lewis structure, sum the valence electrons from each atom. The valence electrons are the electrons in the outermost shell of an atom that participate in bond formation. Carbon has 4 valence electrons and Oxygen has 6. So for CO2, the total number of valence electrons would be \((1\times 4)+(2\times 6) =16 \) electrons.
02

Drawing the Lewis Structures

In Lewis structure, a line represents a pair of bonded electrons, and the other electrons are distributed around the atoms. The first Lewis structure of CO2 is linear with carbon in the middle and a double bond to each oxygen atom - each pair of dots or line represents 2 electrons. So, there are 4 lines which means 8 electrons are used in bonding. The remaining 8 are non-bonding electrons, located on the oxygen atoms.\n The alternative Lewis structure of CO2 involves a single bond, a coordinate bond and a triple bond. The total is still 16 valence electrons.
03

Confirming the Electron Count

By counting the total number of electrons in each structure, we can confirm they sum up to 16 in both cases. Thus, this shows how the number of electrons in the Lewis structure for CO2 was determined.

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Most popular questions from this chapter

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

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?
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