Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN: 9780618974122
Author: Andrei Straumanis
Publisher: Cengage Learning
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Question
Chapter 2, Problem 17E
(a)
Interpretation Introduction
Interpretation: A molecule containing a carbon with a -1 formal charge should be drawn.
Concept introduction: Having an extra electron around an atom gives a -1 formal charge to that atom.
(b)
Interpretation Introduction
Interpretation: A molecule containing a carbon with a +1 formal charge should be drawn.
Concept introduction: Losing 1 electron around an atom from its ground state gives a +1 formal charge to that atom.
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1) what is the formal charge of G? a. -1 b. 0 c. +1
2) what is the formal charge of the labelled atom (refer to the blue arrow)? a. -1 b. 0 c. +1
What is the formal charge on each atom in dichloromethane, CH2Cl2?
a. C atom = 0, each H atom = 0, and each Cl atom = 0
b. C atom = –2, each H atom = +1, and two Cl atoms = 0
c. C atom = +4, each H = –1, and each Cl atom = –1
d. C atom = +4, each H = +1, and each Cl atom = –1
e. C atom = –4, each H = +1, and each Cl atom = +1
Draw a single best Lewis structure for each molecule below. Assign non-zero formal charges to each atom.
(a.) H2O2 (hydrogen peroxide)
b) N2H4 (hydrazine)
c) CH3SCN (methyl thiocyanate)
d) CH2Cl2 (dichloromethane)
e) SF6 (sulfur hexafluoride)
f) PCl5 (phosphorus pentachloride)
g) HClO4 (perchloric acid)
h) BH3 (boron trihydride)
Chapter 2 Solutions
Organic Chemistry: A Guided Inquiry
Ch. 2 - Prob. 1CTQCh. 2 - The valence shell of an atom in a legitimate Lewis...Ch. 2 - Prob. 3CTQCh. 2 - Prob. 4CTQCh. 2 - Prob. 5CTQCh. 2 - It is impossible to draw a legitimate Lewis...Ch. 2 - Describe how to calculate the total number of...Ch. 2 - Prob. 8CTQCh. 2 - Prob. 9CTQCh. 2 - Prob. 10CTQ
Ch. 2 - Prob. 11CTQCh. 2 - Prob. 12CTQCh. 2 - A complete Lewis structure must show all nonzero...Ch. 2 - Prob. 14CTQCh. 2 - Prob. 15CTQCh. 2 - Prob. 16CTQCh. 2 - Prob. 17CTQCh. 2 - Prob. 18CTQCh. 2 - Complete the rest of the table for N, O or X by...Ch. 2 - Prob. 20CTQCh. 2 - Prob. 21CTQCh. 2 - Make a checklist that can be used to determine if...Ch. 2 - Prob. 2ECh. 2 - Prob. 3ECh. 2 - Draw the Lewis structure of a neutral molecule...Ch. 2 - Prob. 5ECh. 2 - For each element, predict (and draw a Lewis...Ch. 2 - Predict which of the following species is least...Ch. 2 - The molecules BH3 and SF6 and the ion SO42 exist...Ch. 2 - These are NOTlegitimate Lewisstructures (and...Ch. 2 - Fill in missing formal charges where needed (all...Ch. 2 - Below each structure in the previous question is a...Ch. 2 - Prob. 12ECh. 2 - Carbon monoxide (CO) is an example of an overall...Ch. 2 - Explain why this Lewis structure for CO is not as...Ch. 2 - Prob. 15ECh. 2 - Prob. 16ECh. 2 - Prob. 17ECh. 2 - Prob. 18ECh. 2 - Prob. 19E
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- Why is this structure wrong and how can it be corrected? It should be neutral and the formal charge for each atom should be 0.arrow_forward1. Conjugated radicals, ions, or molecules are more stable than non-conjugated ones, why? 2. Charge separation decreases stability, why? 3. Structures in which all of the atoms have a complete valence shell of electrons are especially stable and make large contributions to the hybrid, why?arrow_forwardWhy is it less clear to see the electrons on HBrO2 molecular electron geometry than it is on something like H2O? I know there should be 20 electrons on HBrO2, but this leads me to an incorrect drawing. And with the correct drawing, I don't see where all the electrons are. It seems like there's only 10 total. What am I missing here?arrow_forward
- Draw the lewis structure of SO2 ( best resonance) and 2nd best resonance showing the shape and bond angles of each one, the 3D structure with polar bonds or bonds dipole of each one and the molecular polarity. Here is an example of what I want the answer to be like:arrow_forwardA resonance hybrid is a structure that can be depicted by more than one valid Lewis structure. part1: Draw the major resonance form of fulminic acid, HCNO, with the atoms connected as indicated in the formula. Your structure should have nonzero formal charges minimized, and it should include all nonzero formal charges and all nonbonding electrons. part2: Draw the second most important resonance form of fulminic acid, HCNO, with the atoms connected as indicated in the formula. Your structure should have nonzero formal charges minimized, and it should include all nonzero formal charges and all nonbonding electrons. part3: Draw the least important resonance contributor for fulminic acid, HCNO, with the atoms connected as indicated in the formula. Your structure should have nonzero formal charges minimized and should include all nonzero formal charges and all nonbonding electrons.arrow_forwardA resonance hybrid is a structure that can be depicted by more than one valid Lewis structure. part1: Draw the major resonance form of fulminic acid, HCNO, with the atoms connected as indicated in the formula. Your structure should have nonzero formal charges minimized, and it should include all nonzero formal charges and all nonbonding electrons. part2: Draw the second most important resonance form of fulminic acid, HCNO, with the atoms connected as indicated in the formula. Your structure should have nonzero formal charges minimized, and it should include all nonzero formal charges and all nonbonding electrons.arrow_forward
- What is the formal charge of each atom (from left to right), neglecting the hydrogens, in the following resonance structure of CH2N2? Select one: a. 0, +1, −1 b. 0, −1, +1 c. −1, −1, +1 d. −1, +1, 0 e. 0, 0, 0arrow_forwardIn Structure 1, the formal charge on O is _____ and the formal charge on N is _____ In Structure 2, the formal charge on O is _____ and the formal charge on N is ______ On the basis of formal charge, the 'better' structure is _______ fill in the blanks pleasearrow_forwardWhy don't we draw double bonds between the Be atom and the Cl atoms in BeCl2? That would give positive formal charges to the chlorine atoms and a negative formal charge to the beryllium atom. There aren't enough electrons. That would result in more than eight electrons around beryllium. That would result in more than eight electrons around each chlorine atom. That would result in the formal charges not adding up to zero.arrow_forward
- Consider this “Dr. Yan’s imaginary” molecule below in line-angle formula. Note that you MAY NOT add or remove lone pairs. How many CH groups are there in the molecule? ____________ b) The formal charge of O is:__________; and the formal charge of N is: ____________________ c) The overall charge of the molecule: ___________arrow_forward8. Compute for the formal charge (FC) on each atom in the following compounds. a. H3N - BH3 b. [H2CNH2]+ c. H3O+ d. HCO3- 9. Draw Lewis structures for the following compounds, showing an appropriate formal charges. a. [CH3OH2]+ b. [HONH3]+ c. NaBH3CN d. CH3NH3+ 10. For each of the following compounds, draw the important resonance forms. Indicate which structures are major and minor contributors or whether they would have the same energy. a. [CH3OCH2]+ b. H2SO4 c. CO3-2 d. H2C=CH-+CH2 e. [CH3C(OCH3)2 ]+ 11. Draw the complete Lewis structures for the following condensed structural formulas. a. CH3(CH2)3CH(CH3)2arrow_forward8. Compute for the formal charge (FC) on each atom in the following compounds. a. H3N - BH3 b. [H2CNH2]+ c. H3O+ d. HCO3- 9. Draw Lewis structures for the following compounds, showing an appropriate formal charges. a. [CH3OH2]+ b. [HONH3]+ c. NaBH3CN d. CH3NH3+ 10. For each of the following compounds, draw the important resonance forms. Indicate which structures are major and minor contributors or whether they would have the same energy. a. [CH3OCH2]+ b. H2SO4 c. CO3-2 d. H2C=CH-+CH2 e. [CH3C(OCH3)2 ]+ 11. Draw the complete Lewis structures for the following condensed structural formulas. a. CH3(CH2)3CH(CH3)2 b. CH3CH2COCN c. (CH3)3CCOCHCH2 d. (CH3CH2)2CO e. (CH3)2CHCH2Cl 12. Draw the line-angle formula for the following condensed structural formulas. a. CH3(CH2)3CH(CH3)2 b. CH3CH2COCN c. (CH3)3CCOCHCH2 d. (CH3CH2)2CO e. (CH3)2CHCH2Clarrow_forward
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