Concept explainers
(a)
Interpretation:
The appropriate formal charge for each of the given atom has to be given.
Concept Introduction:
Formal charge: The formal charge is defined as the charge carried by an atom in a molecule assuming that, irrespective of the relative electronegativity of the shared atoms, all the
Formal Charge: The formal charge on atoms in the Lewis structure is calculated by the equation below.
Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dot.
(b)
Interpretation:
The appropriate formal charge for each of the given atom has to be given.
Concept Introduction:
Formal charge: The formal charge is defined as the charge carried by an atom in a molecule assuming that, irrespective of the relative electronegativity of the shared atoms, all the chemical bonds are shared equally between the two atoms.
Formal Charge: The formal charge on atoms in the Lewis structure is calculated by the equation below.
Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dot.
(c)
Interpretation:
The appropriate formal charge for each of the given atom has to be given.
Concept Introduction:
Formal charge: The formal charge is defined as the charge carried by an atom in a molecule assuming that, irrespective of the relative electronegativity of the shared atoms, all the chemical bonds are shared equally between the two atoms.
Formal Charge: The formal charge on atoms in the Lewis structure is calculated by the equation below.
Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dot.
(d)
Interpretation:
The appropriate formal charge for each of the given atom has to be given.
Concept Introduction:
Formal charge: The formal charge is defined as the charge carried by an atom in a molecule assuming that, irrespective of the relative electronegativity of the shared atoms, all the chemical bonds are shared equally between the two atoms.
Formal Charge: The formal charge on atoms in the Lewis structure is calculated by the equation below.
Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dot.
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Check out a sample textbook solutionChapter 1 Solutions
Essential Organic Chemistry, Global Edition
- Pick 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_forwardWhich ones have an oxygen with a formal charge of -1?arrow_forwardUsing correct arrow formalism, write the contributors to the resonance hybrid structure of the acetate ion, CH3CO2, and Indicate any formal charges.arrow_forward
- Write structural formulas for at least three constitutional isomers with the molecular formula ch3no2. (In answering this problem you should assign a formal charge to any atom that bears one.)arrow_forwardDraw the indicated number of resonance structures for each species:arrow_forwardIndicate whether each of the following bonds is polar or non polar. If polar, indicate the factor affecting polarity. O non-polar O polar, due to electronegativity polar, due to varied nature of adjacent atoms polar, due to symmetry of the molecule Indicate whether each of the following bonds is polar or non-polar. If polar, indicate the factor affecting polarity. * H Br C non-polar O polar, due to electronegativity polar, due to varied nature of adjacent atoms polar, due to symmetry of the moleculearrow_forward
- what is the complete lewis structure of acetic anhydride such that all atoms have zero formal charge?arrow_forwardDraw the missing lone-pair electrons and assign the missing formal charge on N or O for the following H-C-O-Harrow_forwardSpecify the formal charges on the atoms labeled a-c in each structure. b a:0: CH3CH2, CH2CH3 b H3CN-CH3 CH;CH2 CH2CH3 ČH3 a a b barrow_forward
- Assign formal charges to each carbon atom in the given species. All lone pairs have been drawn in. H H | нН — Са— Съ H Harrow_forward19.) The thiocyanate ion (SCN-) has thee resonance structures. Each follows the octet rule (#1) has a sulfur to carbon single bond and a carbon to nitrogen triple bond. (#2) has a sulfur to carbon triple bond and a carbon to nitrogen single bond. (#3) has a sulfur to carbon double bond and a carbon to nitrogen double bond. Which structure is the "best" one using formal charge arguments? Group of answer choices 2 all three are equal 1 3 1 and 2 are equalarrow_forwardIn which structure(s) below does the oxygen have a formal charge of -1? H-0-H H-ö: H-C=ö-H H3C-0-CH3 ČH3 I II III IV I only O Il only I and II I and IV O , II, and IV :0-Iarrow_forward
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