Organic Chemistry
7th Edition
ISBN: 9780321803221
Author: Paula Y. Bruice
Publisher: Prentice Hall
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Textbook Question
Chapter 1.2, Problem 5P
Look at the relative positions of each pair of atoms listed here in the periodic table. How many core electrons does each have? How many valence electrons does each have?
- a. carbon and silicon
- b. oxygen and sulphur
- c. nitrogen and phosphorus
- d. magnesium and calcium
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Identifying the major species in weak acid or weak base equilibria
The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at
equilibrium. You can leave out water itself.
Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the
formulas of the species that will act as neither acids nor bases in the 'other' row.
You will find it useful to keep in mind that NH3 is a weak base.
acids: ☐
1.8 mol of HCl is added to
1.0 L of a 1.0M NH3
bases: ☐
solution.
other: ☐
0.18 mol of HNO3 is added
to 1.0 L of a solution that is
1.4M in both NH3 and
NH₁Br.
acids:
bases: ☐
other: ☐
0,0,...
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000
18
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1
Using reaction free energy to predict equilibrium composition
Consider the following equilibrium:
2NH3 (g) = N2 (g) +3H₂
—N2 (g) AGº = 34. kJ
Now suppose a reaction vessel is filled with 4.19 atm of ammonia (NH3) and 9.94 atm of nitrogen (N2) at 378. °C. Answer the following questions about this
system:
rise
Under these conditions, will the pressure of NH 3 tend to rise or fall?
☐ x10
fall
Х
Is it possible to reverse this tendency by adding H₂?
In other words, if you said the pressure of NH 3 will tend to rise, can that
be changed to a tendency to fall by adding H₂? Similarly, if you said the
pressure of NH3 will tend to fall, can that be changed to a tendency to
rise by adding H₂?
If you said the tendency can be reversed in the second question, calculate
the minimum pressure of H₂ needed to reverse it.
Round your answer to 2 significant digits.
yes
no
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18
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Identifying the major species in weak acid or weak base equilibria
The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at
equilibrium. You can leave out water itself.
Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the
formulas of the species that will act as neither acids nor bases in the 'other' row.
You will find it useful to keep in mind that HF is a weak acid.
2.2 mol of NaOH is added to
1.0 L of a 1.4M HF
solution.
acids:
П
bases:
Х
other: ☐
ப
acids:
0.51 mol of KOH is added to
1.0 L of a solution that is
bases:
1.3M in both HF and NaF.
other: ☐
00.
18
Ar
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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