Organic Chemistry
6th Edition
ISBN: 9781936221349
Author: Marc Loudon, Jim Parise
Publisher: W. H. Freeman
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Question
Chapter 1, Problem 1.5P
Interpretation Introduction
(a)
Interpretation:
The formal charges on each atom of the given structure are to be computed. Also, the charge on the entire structure is to be stated.
Concept introduction:
A charge that is assigned to an atom, on the assumption that all the electrons in the
The formal charge on an atom is calculated by the formula,
Interpretation Introduction
(b)
Interpretation:
The formal charges on each atom of the given structure are to be computed. Also, the charge on the entire structure is to be stated.
Concept introduction:
A charge that is assigned to an atom, on the assumption that all the electrons in the chemical bonds are equally shared, is known as the formal charge. The sum of the formal charges on the independent atoms should equal the total charge present on the ion.
The formal charge on an atom is calculated by the formula,
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Draw Lewis structures for each of the following compounds. In each case, specify the number of valence electrons surrounding the central atom. (Assign lone pairs and radical electrons where appropriate.)
(Assume the central atom does not contain an expanded octet.)
(a) bromine dioxide (BrO2)
(b) beryllium bromide (BeBr2)
(c) phosphorus pentafluoride (PF5)
The molecular ion S3N, has the cyclic structure
'N
All S-N 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 consis-
tent with the overall +1 charge on the molecular ion.
Z-S
Draw a Lewis Structure for each of the following species and assign formal charge where appropriate. Using electronegative values from the period table that was provided identify polar covalent bonds and label the atoms δ+ and δ−. For each of the molecules indicate whether or not it has a dipole moment. (a)CH5N (b) HCN (c) H2CO (d) CH3NC(e) CH3SOCH3 (f) H6BN
Chapter 1 Solutions
Organic Chemistry
Ch. 1 - Prob. 1.1PCh. 1 - Prob. 1.2PCh. 1 - Prob. 1.3PCh. 1 - Prob. 1.4PCh. 1 - Prob. 1.5PCh. 1 - Prob. 1.6PCh. 1 - Prob. 1.7PCh. 1 - Prob. 1.8PCh. 1 - Prob. 1.9PCh. 1 - Prob. 1.10P
Ch. 1 - Prob. 1.11PCh. 1 - Prob. 1.12PCh. 1 - Prob. 1.13PCh. 1 - Prob. 1.14PCh. 1 - Prob. 1.15PCh. 1 - Prob. 1.16PCh. 1 - Prob. 1.17PCh. 1 - Prob. 1.18PCh. 1 - Prob. 1.19PCh. 1 - Prob. 1.20PCh. 1 - Prob. 1.21APCh. 1 - Prob. 1.22APCh. 1 - Prob. 1.23APCh. 1 - Prob. 1.24APCh. 1 - Prob. 1.25APCh. 1 - Prob. 1.26APCh. 1 - Prob. 1.27APCh. 1 - Prob. 1.28APCh. 1 - Prob. 1.29APCh. 1 - Prob. 1.30APCh. 1 - Prob. 1.31APCh. 1 - Prob. 1.32APCh. 1 - Prob. 1.33APCh. 1 - Prob. 1.34APCh. 1 - Prob. 1.35APCh. 1 - Prob. 1.36APCh. 1 - Prob. 1.37APCh. 1 - Prob. 1.38APCh. 1 - Prob. 1.39APCh. 1 - Prob. 1.40APCh. 1 - Prob. 1.41APCh. 1 - Prob. 1.42APCh. 1 - Prob. 1.43APCh. 1 - Prob. 1.44APCh. 1 - Prob. 1.45APCh. 1 - Prob. 1.46APCh. 1 - Prob. 1.47APCh. 1 - Prob. 1.48APCh. 1 - Prob. 1.49AP
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