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Chapter 22: Problem 53

Write the Lewis structure for each of the following species, describe its geometry, and indicate the oxidation state of the nitrogen: (a) \(\mathrm{HNO}_{2},(\mathbf{b}) \mathrm{N}_{3}^{-},(\mathrm{c}) \mathrm{N}_{2} \mathrm{H}_{5}{ }^{+},(\mathrm{d}) \mathrm{NO}_{3}^{-}\).

Short Answer

Expert verified
(a) HNO2: Lewis structure - H-O-N=O; Electronic and Molecular geometry - Tetrahedral, Bent; Oxidation state of Nitrogen - +3. (b) N3-: Lewis structure - N=N-N; Electronic and Molecular geometry - Linear; Oxidation state of Nitrogen - Central Nitrogen +1 and Terminal Nitrogens -1. (c) H5N2+: Lewis structure - (NH2)-N+(NH3); Electronic and Molecular geometry - Tetrahedral; Oxidation state of Nitrogen - Central Nitrogen +3, in NH2 -1, and in NH3 -2. (d) NO3-: Lewis structure - N(=O)(O^-)(O^-); Electronic and Molecular geometry - Trigonal planar; Oxidation state of Nitrogen - +5.

Step by step solution

01

Lewis Structure

To draw the Lewis structure, we begin by writing the formula showing connectivity: H-O-N=O. The nitrogen has two single bonds (to the hydrogen and oxygen atoms) and one double bond (to the other oxygen). It also has one lone pair of electrons.
02

Electronic Geometry

In this case, the central atom nitrogen connected to three atoms and has one lone pair, which is a total of 4 electron domains. The electronic geometry of HNO2 is tetrahedral.
03

Molecular Geometry

Since two of the electron domains are bonding (H-O and N=O) and one is a nonbonding electron pair, the molecular geometry is bent.
04

Oxidation State of Nitrogen

To find the oxidation state, assign all bonding electrons to the more electronegative atom in each bond. Here, we treat the single bond H-O as nitrogen's bonded atom, and nitrogen gets one electron from it. In the N=O bond, both electrons go to oxygen. Therefore, the oxidation number of nitrogen in HNO2 is +3. (b) N3-
05

Lewis Structure

To draw the Lewis structure, the azide anion, N3-, has one N=N double bond and another nitrogen with a single bond, N=N-N. The terminal nitrogen atoms have two lone pairs, while the central nitrogen has one.
06

Electronic Geometry

Since the central nitrogen of N3- has two electron domains (one double bond and one single bond), its electronic geometry is linear.
07

Molecular Geometry

As both electron domains are bonding, the molecular geometry is also linear.
08

Oxidation State of Nitrogen

In this case, the oxidation states for the three nitrogen atoms are different: the central nitrogen is +1, while both terminal nitrogen atoms are -1. (c) H5N2+
09

Lewis Structure

In the structure, we have a nitrogen atom with one side bonded to an ammonia molecule, NH3, and the other side bonded to an NH2 group: (NH2)-N+(NH3)
10

Electronic Geometry

The central nitrogen is connected to four atoms (two hydrogens and two nitrogens). Therefore, the electronic geometry is tetrahedral.
11

Molecular Geometry

All four electron domains are bonding. Hence, the molecular geometry is also tetrahedral.
12

Oxidation State of Nitrogen

In this case, the oxidation state of the central nitrogen is +3, the nitrogen in NH2 is -1, and in NH3 is -2. (d) NO3-
13

Lewis Structure

In this Lewis structure, the central nitrogen atom is bonded to three oxygens, with one oxygen having a double bond: N(=O)(O^-)(O^-)
14

Electronic Geometry

The central nitrogen is attached to three oxygen atoms giving three electron domains and a trigonal planar electronic geometry.
15

Molecular Geometry

All three electron domains are bonding, therefore, the molecular geometry is also trigonal planar.
16

Oxidation State of Nitrogen

In the N=O double bond, both electrons go to the oxygen. The other two single-bonded oxygens give one electron each to the nitrogen. Therefore, the oxidation number of nitrogen in NO3- is +5.

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