Concept explainers
(a)
Interpretation:
The formal charge on each atom has to be determined and structure of lower energy has to be identified.
Concept Introduction:
The formal charge on each atom in the Lewis structure can be calculated from the equation written as follows:
Here,
Lowest energy structure is the one that has zero or nearly zero formal charge.
(a)
Explanation of Solution
The formal charge on each atom in the Lewis structure can be calculated from the equation as follows:
For structure 1:
Substitute 5 for
Substitute 4 for
Similarly for other Lewis structure, substitute 5 for
Substitute 5 for
Substitute 4 for
Hence formal charge on each structure is illustrated below:
Since the former has less formal charges on maximum number of atoms so I is lower in energy than II therefore I represents structure of lowest energy.
(b)
Interpretation:
The formal charge on each atom has to be determined and structure of lower energy has to be identified.
Concept Introduction:
Refer to part (a).
(b)
Explanation of Solution
The formal charge on each atom in the Lewis structure can be calculated from the equation as follows:
For structure I:
Substitute 6 for
Substitute 6 for
Substitute 5 for
For structure II:
Similarly for second Lewis structure, substitute 6 for
Substitute 6 for
Substitute 5 for
For structure III:
Similarly for third Lewis structure, substitute 6 for
Substitute 5 for
Hence formal charge in the two structures is illustrated below.
Since the II has a
(b)
Interpretation:
The formal charge on each atom has to be determined and structure of lower energy has to be identified.
Concept Introduction:
Refer to part (a).
(b)
Explanation of Solution
The formal charge on each atom in the Lewis structure can be calculated from the equation as follows:
For Lewis structureI, substitute 6 for
Substitute 6 for
Substitute 7 for
For Lewis structure II,
Substitute 6 for
Substitute 6 for
Substitute 7 for
For Lewis structure III, substitute 6 for
Substitute 6 for
Substitute 7 for
Hence formal charge in the three structures is illustrated below:
Since I has zero formal charges on central electronegative iodine atom compared to other cases with
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Chapter 2 Solutions
Chemical Principles: The Quest for Insight
- Assign formal charges to all atoms in the following Lewis diagrams. (a) SO42 (b) S2O32 (c) SbF3 (d) SCNarrow_forwardA complete Lewis structure must show all nonzero formal charges. Complete each of thefollowing Lewis structures by adding any missing formal charges.arrow_forwardWrite the correct Lewis structure and assign a formal charge to each atom in fulminate ion, CNO.arrow_forward
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- Chloromethane has the Lewis structure _______________________________ The carbon atom is sharing 4 electron pairs. In each shared pair the carbon atom “owns” 1 electron. The number of electrons that “belong” to carbon is ___. Carbon, being a Group ___ element would have 4 , outer shell electrons in the unbonded, neutral state. Therefore, the carbon atom in chloromethane has a formal charge of zero.arrow_forwardThe Lewis structure of acetone is Circling the carbonyl carbon, i.e., the carbon atom attached to oxygen, and its octet gives Circling the oxygen atom and its octet gives Thus, atoms share electrons in making bonds, and a pair of electrons may be included in the octet of two different atoms. When computing the formal charge on an atom, the number of electrons that belong to that atom is compared with the number of electrons the atom would have in the unbonded and neutral state. If the two numbers are the same, the formal charge on the atom is zero. In a Lewis structure both electrons in an unshared pair belong to the atom, and one of every pair of shared (bonding) electrons belongs to the atom.arrow_forward
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