![Organic Chemistry](https://www.bartleby.com/isbn_cover_images/9780321803221/9780321803221_largeCoverImage.gif)
Organic Chemistry
7th Edition
ISBN: 9780321803221
Author: Paula Y. Bruice
Publisher: Prentice Hall
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 1, Problem 65P
Interpretation Introduction
Interpretation:
The formal charge of carbon should be indicated from given set of species.
Concept Introduction:
- Lone-pair electrons are valence electrons that are not used in bonding.
- A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.
- Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).
- Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.
Expert Solution & Answer
![Check Mark](/static/check-mark.png)
Want to see the full answer?
Check out a sample textbook solution![Blurred answer](/static/blurred-answer.jpg)
Students have asked these similar questions
In the following Lewis structure of [(CH3)2OH]*, every atom, bond and lone pair is positioned. To complete the
structure, drag the formal charge tags to the appropriate atom(s). Each marker may be used more than once,
or not at all. If an atom has a formal charge of zero, do not drag a tag to it.
When you drag the marker in, place the little crosshairs in the upper left corner of the marker directly
over the atom(s) in question (not above them).
H.
H-C
Н-С-О-С-Н
C-H
H HH
2-
II
2-
In the following Lewis structure of [(CH3)2OH]+, every atom, bond and lone pair is positioned. To
complete the structure, drag the formal charge tags to the appropriate atom(s). Each marker may be
used more than once, or not at all. If an atom has a formal charge of zero, do not drag a tag to it.
When you drag the marker in, place the little crosshairs in the upper left corner of the marker
directly over the atom(s) in question (not above them).
H
H-C-O-C-H
HHH
-
H
I
Η Η Η
0 0
+
2+
2-
[Review Topics]
[References]
Unshared, or lone, electron pairs play an important role in determining the chemical and physical
properties of organic compounds. Thus, it is important to know which atoms carry unshared pairs.
Use the structural formulas below to determine the number of unshared pairs at each designated
atom.
Be sure your answers are consistent with the formal charges on the formulas.
H3C -C=N=O
a
H₂C-C=N
a b
C
Submit Answer
C
The number of unshared pairs at atom a is
The number of unshared pairs at atom b is
The number of unshared pairs at atom c is
The number of unshared pairs at atom a is
The number of unshared pairs at atom b is
The number of unshared pairs at atom c is
Retry Entire Group 1 more group attempt remaining
V
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
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Determine (draw) the total number of resonance structures for the following molecule.arrow_forwardIn the following Lewis structure of [BrO3]", every atom, bond and lone pair is positioned. To complete the structure, drag the formal charge tags to the appropriate atom(s). Each marker may be used more than once, or not at all. If an atom has a formal charge of zero, do not drag a tag to it. When you drag the marker in, place the little crosshairs in the upper left corner of the marker directly over the atom(s) in question (not above them). Ö: Br: 2+ 2-arrow_forward1) Don't forget to show formal charges where necessary Draw the resonance hybrid for the following ion based upon the given resonance structures. C=CH₂ CH₂ Os. -CH₂arrow_forward
- what is the formal charge to the O atom in the following molecule. All lone pairs have been drawn in.arrow_forwardPlease provide the formal charge of the above question. c)arrow_forwardPick the one reaction whose products don't match the given arrows. Assume lone pairs and formal charges are correct. A B C D H 07:0 H : OCH 3 :F: H-CI: 61: HO. :OCH 3 :ךד: + F: 어 HOTarrow_forward
- Which of the following species is a valid resonance structure of A? Usecurved arrows to show how A is converted to any valid resonancestructure. When a compound is not a valid resonance structure of A,explain why not.arrow_forwardDraw two additional resonance structures of the following. Remember to include all formal charges needed. Clearly show the arrows to go from one structure to the next.arrow_forwardDtermine the formal charge of N and the number of lone pairs present.arrow_forward
- Draw all applicable Lewis Structures complete with formal charges for HN3.arrow_forwardPlease answer very soonarrow_forwardUnshared, or lone, electron pairs play an important role in determining the chermical and physical properties of organic compounds. Thus, it is important to know which atoms carry unshared pairs. Use the structural formulas below to determine the number of unshared pairs at each designated atom. Be sure your answers are consistent with the formal charges on the formulas. The number of unshared pairs at atom a is The number of unshared pairs at atom b is HyC CH The number of unshared pairs at atom e is The number of unshared pairs at atom a is The number of unshared pairs at atom b is HC CH The number of unshared pairs at atom e isarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningOrganic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
![Text book image](https://www.bartleby.com/isbn_cover_images/9781133951889/9781133951889_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781133109655/9781133109655_smallCoverImage.jpg)
World of Chemistry, 3rd edition
Chemistry
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Brooks / Cole / Cengage Learning
![Text book image](https://www.bartleby.com/isbn_cover_images/9780618974122/9780618974122_smallCoverImage.gif)
Organic Chemistry: A Guided Inquiry
Chemistry
ISBN:9780618974122
Author:Andrei Straumanis
Publisher:Cengage Learning
![Text book image](https://www.bartleby.com/isbn_cover_images/9781285199047/9781285199047_smallCoverImage.gif)
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning