Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Textbook Question
Chapter 9, Problem 20Q
The three NO bonds in NO3− are all equivalent in length and strength. How is this explained even though any valid Lewis structure for NO3− has one double bond and two single bonds to nitrogen?
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Answer the questions in the table below about the shape of the phosphorus trifluoride (PF3) molecule.
How many electron groups are around the central phosphorus
atom?
Note: one "electron group" means one lone pair, one single bond,
one double bond, or one triple bond.
What phrase best describes the arrangement of these electron
groups around the central phosphorus atom?
(You may need to use the scrollbar to see all the choices.)
(choose one)
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Consider peroxynitrite (chemical formula: ONOO−), a structural isomer of the nitrate anion. It is generated in the cell when nitric oxide (NO) reacts with the superoxide radical anion (O2-.). Peroxynitrite is a potent oxidant and nitrating agent and can lead to DNA and protein damage (this is the complete question)
Draw the correct Lewis structure for peroxynitrite and indicate approximate bond angles.
Tell how many molecular degrees of freedom of motion are present in peroxynitrite and what motions they correspond to.
The bonds N=N, N=N and N-N have known measured values of bond energies and bond lengths
that can be found in various tables. What is the expected sequence of nitrogen-nitrogen bond
lengths and bond enthalpies?
O Bond lengths: N=N N=N > N-N.
Bond lengths: N=N N=N> N-N; Bond enthalpies: N=N N=N > N=N; Bond enthalpies: N=N N=N> N-N; Bond enthalpies: N=N > N=N > N-N.
Chapter 9 Solutions
Chemistry
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