Organic Chemistry
7th Edition
ISBN: 9780321803221
Author: Paula Y. Bruice
Publisher: Prentice Hall
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Textbook Question
Chapter 1.4, Problem 14P
An atom with a formal charge does not necessarily have more or less electron density than the atoms in the molecule without formal charges. We can see this by examining the potential maps for H2O, H3O+, and HO–.
- a. Which atom bears the formal negative charge in the hydroxide ion?
- b. Which atom has the greater electron density in the hydroxide ion?
- c. Which atom bears the formal positive charge in the hydronium ion?
- d. Which atom has the least electron density in the hydronium ion?
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One resonance structure for O2Cl– ion is drawn below. What is the formal charge on each atom?
a. Cl atom = 0 and each O atom = 0
b. Cl atom = 0 and each O atom = –1
c. Cl atom = –1 and each O atom = 0
d. Cl atom = +1 and each O atom = –1
e. Cl atom = 0, one O atom = 0, one O atom = –1
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A. Calculate the formal charge on each atom in CO.
B. Draw the dipole for CO.
C. Calculate the oxidation numbers for the carbon and oxygen atoms in CO.
D. Formal charges, dipoles, and oxidation numbers are different ways of understanding the charges on covalently-bonded atoms. They tend to agree or be similar. At least in some ways, they disagree for CO. Formal charge guidelines assume that all bonding electrons are shared evenly between the two bonded atoms. Oxidation number guidelines assume that the more electronegative atom in the bond gets all of the electrons. Dipole theory assumes that the bonded electrons are associated more with the more electronegative atom. Now that you understand the basis for the oxidation number guidelines, determine the oxidation number for each carbon in propane assuming that the more electronegative atom gets all of the bonded electrons. You will need to draw the Lewis structure of propane for your answer.
Draw Lewis structures for tye following molecules.
a.) Atom "X" has 4 valence electrons and Atom "Y" has 6 valence electrons. Draw the Lewis structure for the molecule XY2, showing all lone pairs and formal charges when necessary
b.) Atom "M" has 5 valence electrons and Atom "L" has 7 valence electrons. Draw the Lewis structure for the molecule M2L4, showing all lone pairs and formal charges when necessary
Chapter 1 Solutions
Organic Chemistry
Ch. 1.1 - Oxygen has three isotopes, 16O, 17O, and 18O. The...Ch. 1.1 - Chlorine has two isotopes, 35Cl and 37Cl; 75.77%...Ch. 1.2 - Prob. 3PCh. 1.2 - a. Write the ground-state electronic configuration...Ch. 1.2 - Look at the relative positions of each pair of...Ch. 1.3 - a. Find potassium (K) in the periodic table and...Ch. 1.3 - Which bond is more polar? a. b. c. d.Ch. 1.3 - Which of the following has a. the most polar bond?...Ch. 1.3 - Use the symbols + and to show the direction of...Ch. 1.3 - Explain why HCL has a smaller dipole moment than...
Ch. 1.3 - After examining the potential maps for LiH, HF,...Ch. 1.4 - An atom with a formal charge does not necessarily...Ch. 1.4 - Prob. 15PCh. 1.4 - a. Draw two Lewis structure for C2H6O. b. Draw...Ch. 1.4 - Draw the lone-pair electrons that are not shown in...Ch. 1.4 - Prob. 19PCh. 1.4 - Which of the atoms in the molecular models in...Ch. 1.4 - Prob. 21PCh. 1.5 - Draw the following orbitals: a. 3s orbital b. 4s...Ch. 1.6 - Prob. 23PCh. 1.6 - Indicate the kind of molecular orbital (, , , or )...Ch. 1.7 - What orbitals are used to form the 10 sigma bonds...Ch. 1.7 - Explain why a bond formed by overlap of s orbital...Ch. 1.9 - Put n number in each of the blanks: a. __ s...Ch. 1.11 - Predict the approximate bond angles in a. the...Ch. 1.11 - According to the potential map for the ammonium...Ch. 1.12 - Prob. 32PCh. 1.13 - a. What are the relative lengths and strengths of...Ch. 1.13 - Prob. 35PCh. 1.14 - Prob. 36PCh. 1.15 - Which of the bond in a carbon-oxygen double bond...Ch. 1.15 - Would you expect a CC bond formed by sp2sp2...Ch. 1.15 - Caffeine is a natural insecticide found in the...Ch. 1.15 - Prob. 41PCh. 1.15 - Predict the approximate bond angles for a. the CNC...Ch. 1.16 - If the dipole moment of CH3F is 1.847 D and the...Ch. 1.16 - Account for the difference in the shape and color...Ch. 1.16 - What of the following molecules would you expect...Ch. 1 - Prob. 46PCh. 1 - Prob. 47PCh. 1 - What is the hybridization of all the atoms (other...Ch. 1 - Draw the condensed structure of a compound that...Ch. 1 - Predict the approximate bond angles: a. the CNH...Ch. 1 - Prob. 51PCh. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - 53. What is the hybridization of each of the...Ch. 1 - Rank the bonds from most polar. a. CO, CF, CN b....Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - What is the hybridization of the indicated atom in...Ch. 1 - Prob. 57PCh. 1 - Prob. 58PCh. 1 - Draw the missing lone-pair electrons and assigns...Ch. 1 - a. Which of the indicated bonds in each molecule...Ch. 1 - For each of the following molecules, indicate the...Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - Rank the following compounds from highest dipole...Ch. 1 - In which orbitals are the lone pairs in nicotine?Ch. 1 - Prob. 65PCh. 1 - Prob. 66PCh. 1 - a. Which of the species have bond angles of 109.5?...Ch. 1 - Prob. 68PCh. 1 - Which compound has a larger dipole moment: CH3Cl...Ch. 1 - Prob. 70PCh. 1 - Prob. 71PCh. 1 - Explain why CH3Cl has a greater dipole moment than...Ch. 1 - Prob. 73P
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