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 105CP
Carbon monoxide (CO) forms bonds to a variety of metals and metal ions. liS ability to bond to iron in hemoglobin is the reason that CO is so toxic. The bond carbon monoxide forms to metals is through the carbon atom:
a. On the basis of electronegativities, would you expect the carbon atom or the oxgen atom to form bonds to metals?
b. Assign formal charges to the atoms in CO. Which atom would you expect to bond to a metal on this basis?
c. In the MO model, bonding MOs place more electron density near the more electronegative atom. (See the HF molecule in Figs. 4-54 and 4-55.) Antibonding MOs place more electron density near the less electronegative atom in the diatomic molecule. Use the MO model to predict which atom of carbon monoxide should form bonds to metals.
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2. The amide linkage is the connection between amino acids in the
primary structure of proteins; a representation of the linkage is
shown to the right:
R2
(note: R1 and R2 represent the carbon centers of the respective
amino acids)
R1
H
The expected bond angle around the Nitrogen is ~109°; the
experimentally determined angle is 123°. What does this suggest about the C- N bond?
(hint: consider possible resonance structures)
Both carbon and oxygen are nonmetals, having 4 and 6 valence electrons, respectively. In this type of bond, a
central atom must be identified.
Carbon and Oxygen- Carbon Dioxide
Bonds must be formed depending on the number of bonding and non-bonding electrons.
Non-bonding electrons are called lone pairs, they are the ones left at the end of bonding. The illustration of
its bonding is shown below:
CO,
Centras Atom ?
To tal vE, 4 +(2x b)- 뇨
:4 VE
6 VE
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If you investigate the illustration, you will notice that carbon atom is double bonded to two oxygen atoms. The
reason for that is because carbon atom must also have complete eight electrons, therefore octet rule must also be
followed at the same time.
Using the sample figure, let us answer the following problems.
DIRECTION: Show the bond fomation of the following compounds. SHOW YOUR SOLUTION.
1. CH,O.
2. . HCN
3. NH3
PROCESSING QUESTION
What basic Science Process Skills have you openly demonstrated in forming…
There are several possible Lewis structures for the molecule N2O as shown below.
See attachment
For Structure A what are the formal charges on atoms:1 , 2 , and 3 ?For Structure B what are the formal charges on atoms:1 , 2 , and 3 ?For Structure C what are the formal charges on atoms:1 , 2 , and 3 ?Compare the formal charges that you calculated for each structure.What is the letter of the BEST Lewis structure for N2O?
Chapter 9 Solutions
Chemistry
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- a Carbonyl fluoride, COF2, is an extremely poisonous gas used in organofluorine synthesis. Give the valence bond description of the carbonyl fluoride molecule. (Both fluorine atoms are attached to the carbon atom.) b Nitrogen, N2, makes up about 80% of the earths atmosphere. Give the valence bond description of this molecule.arrow_forwardWhich of the species with octets in Question 33 are dipoles?arrow_forwardThe molecular ion S3N3 has the cyclic structure All SN bonds are equivalent. (a) Give six equivalent resonance hybrid Lewis diagrams for this molecular ion. (b) Compute the formal charges on all atoms in the molecular ion in each of the six Lewis diagrams. (c) Determine the charge on each atom in the polyatomic ion, assuming that the true distribution of electrons is the average of the six Lewis diagrams arrived at in parts (a) and (b). (d) An advanced calculation suggests that the actual charge resident on each N atom is 0.375 and on each S atom is +0.041 . Show that this result is consistent with the overall +1 charge on the molecular ion.arrow_forward
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