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Chapter 13: Problem 4

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.

Short Answer

Expert verified
a) The Lewis representation for Nitrogen is N surrounded by 5 dots (representing 5 valence electrons). b) A Nitrogen atom requires 3 additional electrons to form a molecule. c) The likely formula for a molecule composed of Hydrogen atoms and a Nitrogen atom is \(\mathrm{NH_3}\), and the Lewis structure for this molecule is drawn with the Nitrogen atom connected to 3 Hydrogen atoms by single bonds, with a lone pair of electrons present on the Nitrogen atom.

Step by step solution

01

Drawing the Lewis Structure for Nitrogen

The Lewis structure for a Nitrogen atom will be represented with 5 dots surrounding the symbol \(\mathrm{N}\). This is because Nitrogen is located in the 5th column of the periodic table, meaning it has 5 valence electrons - 2 in the s orbital and 3 in the p orbital.
02

Calculating Additional Electrons Required

To form a stable molecule, an element tries to achieve a configuration in which its outer shell is full. This is usually 8 electrons (known as the octet rule). Nitrogen already has 5 valence electrons, so it could accept 3 more electrons to complete its octet.
03

Finding the Likely Formula and Drawing Lewis Structure for Nitrogen and Hydrogen Molecule

A single Hydrogen atom contributes 1 electron to form a molecule. Since Nitrogen needs 3 more electrons to complete its octet, the likely formula for a molecule composed of Hydrogen atoms and one Nitrogen atom would be \(\mathrm{NH_3}\). The Lewis structure for this molecule can be drawn with a Nitrogen atom at the center, connected to 3 Hydrogen atoms by single bonds (represented by a line for each bond), with a lone pair of electrons present on Nitrogen atom.

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Most popular questions from this chapter

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

For each of the following neutral atoms give the core charge. a) Li. b) \(\quad \ddot{C l}\) c) He:

Revise (as necessary) your checklist that can be used to determine if a Lewis structure for a molecule is correct.

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?

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) \(\mathrm{Cl}_{2}\)
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