ORGANIC CHEMISTRY-STUD.SOLNS.MAN+SG(LL)
4th Edition
ISBN: 9781119659587
Author: Klein
Publisher: WILEY
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Chapter 1, Problem 66ASP
Interpretation Introduction
Interpretation: The correct statement that described the missing formal charge(s) in the following structure should be identified:
Concept Introduction: Any atom with a formal charge lacks the necessary number of valence electrons. Formal charge is assigned when an atom is present in Lewis structure.
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Students have asked these similar questions
Write a Lewis structure for each of the following molecules/ions. Be sure to show all non-zero
formal charges. Start by counting the valence electrons.
Choose the INCORRECT statement.
In a Lewis structure, the number of valence electrons shown is one more for each negative charge.
The central atom is typically the atom with the highest electronegativity.
Formal charges are apparent charges associated with atoms in a Lewis structure.
Resonance is when more than one plausible structure can be written but the "correct" structure cannot be
written.
Determine if the structural
formula below are acceptable
Lewis structures for organic
compounds. Point out the
problems in cases where
structure is invalid.
CH3
CH;-N-CH-CH3
ČH3
A. This structure is correct because
the valance of Nitrogen is complete.
B. This is not a correct Lewis structure
because Nitrogen can accommodate
more atoms.
C. This is not a correct Lewis structure
because Nitrogen has a charge if it does
not have three bonds.
D. This is a correct Lewis structure.
Chapter 1 Solutions
ORGANIC CHEMISTRY-STUD.SOLNS.MAN+SG(LL)
Ch. 1.2 - Prob. 1LTSCh. 1.2 - Prob. 2ATSCh. 1.2 - Prob. 2LTSCh. 1.3 - Prob. 3LTSCh. 1.3 - Prob. 4PTSCh. 1.3 - Prob. 5PTSCh. 1.4 - Prob. 4LTSCh. 1.4 - Prob. 7PTSCh. 1.4 - Prob. 8PTSCh. 1.4 - Prob. 9ATS
Ch. 1.5 - Prob. 5LTSCh. 1.5 - Prob. 10PTSCh. 1.5 - Prob. 11ATSCh. 1.5 - Prob. 12ATSCh. 1.6 - Prob. 6LTSCh. 1.6 - Prob. 14ATSCh. 1.7 - Prob. 7LTSCh. 1.7 - Prob. 17ATSCh. 1.10 - Prob. 18CCCh. 1.10 - Prob. 20CCCh. 1.10 - Prob. 8LTSCh. 1.10 - Prob. 21PTSCh. 1.10 - Nemotin is a compound that was first isolated from...Ch. 1.10 - Prob. 23CCCh. 1.11 - Prob. 9LTSCh. 1.11 - Prob. 24PTSCh. 1.11 - Prob. 25PTSCh. 1.11 - Prob. 26PTSCh. 1.11 - Prob. 27ATSCh. 1.12 - Prob. 10LTSCh. 1.12 - Prob. 29ATSCh. 1.13 - Prob. 11LTSCh. 1.13 - Prob. 31ATSCh. 1 - Prob. 32PPCh. 1 - Prob. 33PPCh. 1 - Prob. 34PPCh. 1 - Prob. 35PPCh. 1 - Prob. 36PPCh. 1 - Prob. 37PPCh. 1 - Prob. 38PPCh. 1 - Prob. 39PPCh. 1 - Prob. 40PPCh. 1 - Prob. 41PPCh. 1 - Prob. 42PPCh. 1 - Prob. 44PPCh. 1 - Prob. 45PPCh. 1 - Prob. 46PPCh. 1 - Prob. 47PPCh. 1 - Prob. 48PPCh. 1 - Prob. 49PPCh. 1 - Prob. 50PPCh. 1 - Prob. 51PPCh. 1 - Prob. 52PPCh. 1 - Prob. 53PPCh. 1 - Prob. 54PPCh. 1 - Nicotine is an addictive substance found in...Ch. 1 - Prob. 56PPCh. 1 - Prob. 57PPCh. 1 - Prob. 59PPCh. 1 - Prob. 63ASPCh. 1 - Prob. 64ASPCh. 1 - Prob. 66ASPCh. 1 - Prob. 69ASPCh. 1 - Prob. 71ASPCh. 1 - Prob. 72ASPCh. 1 - Prob. 75IP
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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
- Draw Lewis structure(s) for the acetate ion (CH2CO0). If there are equivalent resonance structures, draw all of them. • Draw one structure per sketcher box, and separate added sketcher boxes with the Do not include overall ion charges or formal charges in your drawing. • Do not draw double bonds to oxygen unless they are needed in order for the central atom to obey the octet rule. symbol. CH3COO":arrow_forwardSteps for Lewis Structures: 1. Determine the total number of valence electrons. Add electrons for negative charges, subtract electrons for positive charges. 2. Place least electronegative atom (except H) as central atom in structure. 3. Connect atoms by singles bonds. Each single bond = 2 electrons. 4. “Sprinkle” remaining electrons around outside atoms first to complete octets. Don’t use more electrons than the total found in step 1. Then complete the central atom’s octet last if you have enough electrons. 5. Make double or triple bonds as needed to complete octets. 6. Place brackets and charge for ions. For the central atom in each formula, draw the Lewis Structure with all valence electrons shown. 1. PH3 2. H2O 3. CO2 4. CHCl3 5. O2 6. N2 7. CF4 8. C3H8 9. CH3COOH 10. N2O 11. OCN-arrow_forwardAnswer all of the question above and dont left even one question behind.arrow_forward
- Determine if the structural formula below is an acceptable Lewis structures for organic compounds. Point out the problems in cases where structure is invalid. •. :OH CH- .CH3 A. Non of the options here are correct. B. This is not a correct Lewis structural formula because carbon cannot have five bonds. C. This structure is a correct Lewis structural formula. D. This is not a correct Lewis structure because the methyl group does not have an octet of electrons.arrow_forwardThe formal charge of an atom in a Lewis structure is defined as ________ Select one: a. the difference between the number of bonding electrons and nonbonding electrons assigned to an atom. b. the difference between the number of valence electrons in a free atom and the number of nonbonding electrons assigned to it. c. the difference between the number of valence electrons in a free atom and the number of electrons assigned to it in a Lewis structure. d. the difference between the number of valence electrons in a free atom and the number of bonding electrons assigned to it. e. the difference between the number of valence electrons in a free atom and the total number of valence electrons in the molecule.arrow_forward6. Write the singly bonded Lewis dot structure for BF3. Which of the following statements best describes this structure? A. It obeys the octet rule on all atoms. B. It has less than an octet on at least one atom. C. It has a lone pair of electrons on the boron atom. D. It has less than an octet of electrons on all atoms.arrow_forward
- Which statement is NOT correct regarding the lattice energy of an ionic solid? a.Lattice energy of MgO is higher than NaCl, due to MgO's higher ionic charge and smaller ionic sizes b.As the lattice energy increases melting point increases c.It is the energy change when one mole of an ionic compound is created under standard conditions from its pure elements d.It is the energy change on formation of one mole of an ionic compound from its constituent ions in the gaseous state e.As the lattice energy increases solubility decreasesarrow_forwardTwo major resonance structures are possible for the anion shown. One resonance form is given, but it is incomplete. Complete the given structure by adding nonbonding electrons and formal charges. Draw the remaining structure, including nonbonding electrons and formal charges. Omit curved arrows. Structure A: complete the structure by adding nonbonding electrons and formal charges. H H H I Structure B: draw the remaining resonance structure, including nonbonding electrons and formal charges. H- : z: H Harrow_forward2. In biologically relevant molecules, carbon and the halogens don't have a charge. In contrast, nitrogen (neutral or positively charged) and oxygen (neutral or negatively charged) don't always appear in their uncharged form. Consider the following questions. a. Add any unshared pairs of electrons necessary to complete the Lewis structure shown for formaldehyde (note: there are no formal charges in this molecule). b. Assign any formal charges necessary to complete the structure shown for the acetylide anion. c. Recalling that atoms want a complete octet, add unshared pairs of electrons, and assign formal charges as appropriate to the Lewis structure of the amino acid aspartic acid as it would exist at a physiological pH of ~7.4 (aspartic acid has an overall -1 charge at this pH). A. H O H formaldehyde B. H C C: C. H H \/ acetylide anion H-N O=C H он O H aspartic acidarrow_forward
- Counting available electrons and drawing a Lewis structuresarrow_forwardWrite all the possible resonance structure(s). Show the movement of electrons by drawing arrow(s). Indicate the formal charges and identify the most stable structure for the compound. ö: а. b. a.arrow_forwardAdding electrons to the skeleton by making single bonds between all bonded atoms gives Each hydrogen atom now has a pair of electrons, but each carbon has only 6 electrons. Adding a pair of electrons to each carbon gives the trial structure The number of electrons in the trial structure is ____. Since this number exceeds the number of available valence electrons, the structure is incorrect.arrow_forward
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