NO2-? NH,SCI4NO,SO2CH2SubstanceLewis structuresNumber of bondinggroupsNumber of lone pairsNumber of electrongroups about the centralatomElectron geometryMolecular geometryApproximate bondanglesPolarity of moleculeor ionNumber of resonancestructuresHybridization stateabout the central atom

Answered: NO2-? | bartleby

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

NO2-?

NH,
SCI4
NO,
SO2
CH2
Substance
Lewis structures
Number of bonding
groups
Number of lone pairs
Number of electron
groups about the central
atom
Electron geometry
Molecular geometry
Approximate bond
angles
Polarity of molecule
or ion
Number of resonance
structures
Hybridization state
about the central atom

Expert Solution

Step 1

Lewis structure represents the systematic arrangement of atoms around the central atom. Electrons in this structure are indicated by dots. The central atom is the least electronegative element in a molecule.

Step 2

The given molecule is ${NO}_{2}^{-}$ . Oxygen (O) is more electronegative than nitrogen (N). Therefore, N is the central atom in the molecule.

The N atom has 5 valence electrons and O has 6 valence electrons. Calculate the total number of valence electrons in ${NO}_{2}^{-}$ .

$\begin{array}{rcl} Total number of valence electrons in {NO}_{2}^{-} & = & 5 + 2 \times 6 + 1 \\ = & 18 \end{array}$

The total number of valence electrons in ${NO}_{2}^{-}$ are 18. The number of valence electron pairs is half of the total number of valence electrons. Therefore, the number of valence electron pairs in ${NO}_{2}^{-}$ are 9, which is 18/2.

Step 3

Draw the skeletal structure of ${NO}_{2}^{-}$ by assigning 2 valence electron pairs between N and O atoms (two on each side of N).

The remaining valence electron pairs are assigned as the lone pairs to the surrounding two O atoms. In this way, 4 electron pairs are used. With the distribution of electron pairs the octet of one O is completed.

The central N atom does not have a complete octet of electrons. Therefore, one pair of electrons remain as lone pair on the nitrogen atom. Another pair forms a double bond with the oxygen atom.

Draw the complete Lewis dot structure of ${NO}_{2}^{-}$ .

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