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Chapter 13: Problem 11

For \(\mathrm{N}_{2}\), is the sum of the bonding electrons and nonbonding electrons around each nitrogen atom consistent with the Lewis model?

Short Answer

Expert verified
Yes, the sum of the bonding and nonbonding electrons around each nitrogen atom in \(\mathrm{N}_{2}\) is consistent with the Lewis model as each nitrogen atom has 8 electrons (bonding + nonbonding), fulfilling the octet rule.

Step by step solution

01

Draw the Lewis Dot Structure

The Lewis dot structure for \(\mathrm{N}_{2}\) shows each nitrogen atom sharing three electrons with the other, forming a triple bond. Each nitrogen atom also has one pair of nonbonding electrons.
02

Calculating Bonding and Nonbonding Electrons

The bonding electrons in each nitrogen atom are 6 (3 pairs shared) and the nonbonding electrons are 2 (1 pair not shared). Thus, for each nitrogen atom, the sum of bonding and nonbonding electrons is 8.
03

Compare with the Lewis Model

According to the Lewis model, each element wants to complete its octet and since each nitrogen atom has 8 electrons around it (bonding + nonbonding), this is consistent with the Lewis model.

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Most popular questions from this chapter

What is the total number of electrons in the Lewis structure in Model 3 for each molecule: a) \(\mathrm{H}_{2} \mathrm{CO}\) b) \(\mathrm{N}_{2}\) c) \(\mathrm{Cl}_{2}\)

For \(\mathrm{H}_{2} \mathrm{CO}\) : a) Is the sum of the bonding electrons and lone pair electrons around the carbon atom consistent with the Lewis model? b) Is the sum of the bonding electrons and lone pair electrons (nonbonding electrons) around the oxygen atom consistent with the Lewis model?

Answer the following for the nitrogen atom: a) What is the Lewis representation for \(\mathrm{N}\) ? b) How many additional electrons does one \(\mathrm{N}\) atom require when it forms a molecule? c) What is the likely formula for a molecule composed of hydrogen atoms and one nitrogen atom? Draw the Lewis structure for this molecule.

Given the shell model of the atom, suggest a possible reason that Lewis proposed a maximum of two electrons for hydrogen and a maximum of eight for carbon, nitrogen, oxygen, and fluorine atoms?

Without attempting to draw a Lewis structure, calculate the total number of valence electrons in each of these molecules: a) \(\mathrm{H}_{2} \mathrm{CO}\) b) \(\mathrm{N}_{2}\) c) \(\mathrm{Cl}_{2}\)
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