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The bond angles in the nitrite ion, nitrogen dioxide, and
Chapter 13, Problem 88P(choose chapter or problem)
Problem 88P
The bond angles in the nitrite ion, nitrogen dioxide, and the nitronium ion (NO2+) are 115º, 134º, and 180º, respectively. Explain these values using Lewis structures and VSEPR theory.
Questions & Answers
QUESTION:
Problem 88P
The bond angles in the nitrite ion, nitrogen dioxide, and the nitronium ion (NO2+) are 115º, 134º, and 180º, respectively. Explain these values using Lewis structures and VSEPR theory.
ANSWER:
Solution 88P
Here we have to explain the given values of bond angles by using Lewis structure and VSEPR theory.
Step 1
The bond angles in the nitrite ion is 115º
In nitrite ion (NO2-)the central atom is N-atm, surrounded by two O-atoms.
The electronic configuration of N and O-atoms are given below,
7N 1s2 2s2 2p3 8O 1s2 2s2 2p4
Total number of valence electron = 5 + 2(6) + 1= 18
The Lewis structure of nitrite ion (NO2)- is given below,
Here the central N-atom is surrounded by two bond pairs and one lone pair. Thus according to VSEPR theory it can form AX2E structure, where A is the central atom, X is the number of bonded atoms and E is the lone pair electron.
According to VSEPR model the class of the molecule is AX2E has trigonal electron arrangement.
The bond angle of trigonal planar structure must be 120o but due to the presence of one lone pair electron, the bond angle reduces to 115o.