Organic Chemistry: Principles and Mechanisms (Second Edition)
2nd Edition
ISBN: 9780393663556
Author: Joel Karty
Publisher: W. W. Norton & Company
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Question
Chapter 6, Problem 6.6P
Interpretation Introduction
Interpretation:
Among the two given bases, the stronger base is to be determined. It is to be explained by what numerical factor it is stronger.
Concept introduction:
To determine the strength of base, pKa values of the corresponding conjugate acids are to be compared. The conjugate acid for a given base is generated when the proton gets attached to the negatively charged conjugate base. Weaker the conjugate acid, stronger is the base. When comparing two conjugate acids, the acid whose pKa is more is weaker than the one whose pKa is less.
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Look at the table in Figure 5-8. (There is only one correct answer for each blank)
In Row 1 [a or b] is the stronger acid because [ a) O is more electronegative than S or b) S is bigger than O] .
In Row 2 [a or b] is the stronger acid because [a) because O is more electronegative than C or H, b)because the conjugate base is resonance stablalized or c) because of indction from the Cl] .
In Row 3 [a or b] is the stronger acid because [a)because F is more elecronegative than Cl or b) because Cl is bigger than F].
In Row 4 [a or b] is the stronger acid because [a) because the two chlorines are further apart delocalizing the indicative effect in the conjugate base or because the two chlorines are closer to the negative charge in the conjugate base] .
2. Arrange the following in order of decreasing acidity (strongest 1").
COH
CH,SO,H
O,N-
-он
HCI
он
C
D
E
strongest
weakest
3. Arrange the following in order of decreasing basicity (strongest 1")
-ONa
O,N-
Nal
Na
Cl,CCO,Na
A
B
D
>_>_>_:
strongest
weakest
Explain the following questions using 3-5 sentences
1. What is Dipole Moment and why do some compounds like Ethane or Benzene
have no Dipole moment while water and Ammonia has large Dipole moment?
2. How does the Formal Charge contribute to the proper formation of Lewis'
Structural formation of compound and/ or ions?
3. How does the Bronsted-Lowry's acids and bases differ from Lewis' acids and
bases?
Chapter 6 Solutions
Organic Chemistry: Principles and Mechanisms (Second Edition)
Ch. 6 - Prob. 6.1PCh. 6 - Prob. 6.2PCh. 6 - Prob. 6.3PCh. 6 - Prob. 6.4PCh. 6 - Prob. 6.5PCh. 6 - Prob. 6.6PCh. 6 - Prob. 6.7PCh. 6 - Prob. 6.8PCh. 6 - Prob. 6.9PCh. 6 - Prob. 6.10P
Ch. 6 - Prob. 6.11PCh. 6 - Prob. 6.12PCh. 6 - Prob. 6.13PCh. 6 - Prob. 6.14PCh. 6 - Prob. 6.15PCh. 6 - Prob. 6.16PCh. 6 - Prob. 6.17PCh. 6 - Prob. 6.18PCh. 6 - Prob. 6.19PCh. 6 - Prob. 6.20PCh. 6 - Prob. 6.21PCh. 6 - Prob. 6.22PCh. 6 - Prob. 6.23PCh. 6 - Prob. 6.24PCh. 6 - Prob. 6.25PCh. 6 - Prob. 6.26PCh. 6 - Prob. 6.27PCh. 6 - Prob. 6.28PCh. 6 - Prob. 6.29PCh. 6 - Prob. 6.30PCh. 6 - Prob. 6.31PCh. 6 - Prob. 6.32PCh. 6 - Prob. 6.33PCh. 6 - Prob. 6.34PCh. 6 - Prob. 6.35PCh. 6 - Prob. 6.36PCh. 6 - Prob. 6.37PCh. 6 - Prob. 6.38PCh. 6 - Prob. 6.39PCh. 6 - Prob. 6.40PCh. 6 - Prob. 6.41PCh. 6 - Prob. 6.42PCh. 6 - Prob. 6.43PCh. 6 - Prob. 6.44PCh. 6 - Prob. 6.45PCh. 6 - Prob. 6.46PCh. 6 - Prob. 6.47PCh. 6 - Prob. 6.48PCh. 6 - Prob. 6.49PCh. 6 - Prob. 6.50PCh. 6 - Prob. 6.51PCh. 6 - Prob. 6.52PCh. 6 - Prob. 6.53PCh. 6 - Prob. 6.54PCh. 6 - Prob. 6.55PCh. 6 - Prob. 6.56PCh. 6 - Prob. 6.57PCh. 6 - Prob. 6.58PCh. 6 - Prob. 6.59PCh. 6 - Prob. 6.60PCh. 6 - Prob. 6.61PCh. 6 - Prob. 6.62PCh. 6 - Prob. 6.63PCh. 6 - Prob. 6.64PCh. 6 - Prob. 6.65PCh. 6 - Prob. 6.66PCh. 6 - Prob. 6.67PCh. 6 - Prob. 6.68PCh. 6 - Prob. 6.69PCh. 6 - Prob. 6.70PCh. 6 - Prob. 6.71PCh. 6 - Prob. 6.72PCh. 6 - Prob. 6.73PCh. 6 - Prob. 6.74PCh. 6 - Prob. 6.75PCh. 6 - Prob. 6.76PCh. 6 - Prob. 6.77PCh. 6 - Prob. 6.78PCh. 6 - Prob. 6.79PCh. 6 - Prob. 6.80PCh. 6 - Prob. 6.81PCh. 6 - Prob. 6.82PCh. 6 - Prob. 6.83PCh. 6 - Prob. 6.84PCh. 6 - Prob. 6.85PCh. 6 - Prob. 6.86PCh. 6 - Prob. 6.87PCh. 6 - Prob. 6.88PCh. 6 - Prob. 6.1YTCh. 6 - Prob. 6.2YTCh. 6 - Prob. 6.3YTCh. 6 - Prob. 6.4YTCh. 6 - Prob. 6.5YTCh. 6 - Prob. 6.6YTCh. 6 - Prob. 6.7YTCh. 6 - Prob. 6.8YTCh. 6 - Prob. 6.9YTCh. 6 - Prob. 6.10YTCh. 6 - Prob. 6.11YTCh. 6 - Prob. 6.12YTCh. 6 - Prob. 6.13YTCh. 6 - Prob. 6.14YTCh. 6 - Prob. 6.15YTCh. 6 - Prob. 6.16YTCh. 6 - Prob. 6.17YTCh. 6 - Prob. 6.18YTCh. 6 - Prob. 6.19YTCh. 6 - Prob. 6.20YT
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- 3 of 19 <. Part D I Review | Constants | Periodic Table Among three bases, X, Y, and Z¯, the strongest one is Y, and the weakest one is Z. Rank their conjugate acids, HX, HY, and HZ, in order of decreasing strength. Rank the acids from strongest to weakest. To rank items as equivalent, overlap them. • View Available Hint(s) Reset Help HX HZ HY Strongest acid Weakest acidarrow_forwardGiven the K, for bases below, which K, will be the strongest base? 5.7 x 10-16 O 2.8 x 104 O 7.2 x 106 O 6.2 x 1012arrow_forwardQ2-3:(a) Given that Kb for ammonia is 1.8 X 10 -5 and that for methylamine is 4.4 X 10 -4, which is the stronger base? (b) which is the stronger acid ,the ammonium ion or the methylammonium ion ? (c) calculate the Ka for NH,* and CH;NH;* + Q2-4: A particular sample of vinegar has a pH of 2.90, assuming that the vinegar contains only acetic acid (Ka acetic acid in vinegar . 1.8 X 10 -5), calculate the concentration of Q2-5: Calculate the molar concentration of OH-ions in an 0.85M solution of hypobromite ion , BrO- (Kp 4.0X10-6) .what the pH value of this solution?arrow_forward
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