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Concept explainers
(a)
Interpretation:
Lewis structure for a resonance form of each ion of BrO−3 with the lowest possible formal charges is to be drawn. Also, the oxidation number of the atom is to be determined.
Concept introduction:
The steps to draw the Lewis structure of the molecule are as follows:
Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.
Step 2: Calculate the total number of valence electrons.
Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.
Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.
Formula to calculate the formal charge of the atom is as follows:
Formal charge=(number ofvalenceelectrons)−((number of non-bonding electrons )+(12) (number of bonding electrons)) (1)
The formula to calculate the oxidation number of an atom is as follows:
Oxidation number=(number ofvalenceelectrons)−((number of non-bonding electrons )+ (number of bonding electrons)) (2)
(a)
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Answer to Problem 10.17P
The possible Lewis structures for a resonance form of each ion of BrO−3 with the lowest possible formal charges are,
The oxidation numbers of Br is +5 and the oxidation number of oxygen is –2.
Explanation of Solution
Lewis structures for a resonance form of BrO−3 is,
For structure I:
Substitute 7 for valence electrons, 2 for the number of nonbonded electrons and 6 for the number of bonding electrons in equation (1) to calculate the formal charge on Br atom.
Formal charge=(7)−((2)+(12) (6))=+2
Substitute 6 for valence electrons, 6 for nonbonded electrons and 2 for the number of bonding electrons in equation (1) to calculate the formal charge on each oxygen atom.
Formal charge=(6)−((6)+(12) (2))=−1
For structure II:
Substitute 7 for valence electrons, 2 for the number of nonbonded electrons and 8 for the number of bonding electrons in equation (1) to calculate the formal charge on Br atom.
Formal charge=(7)−((2)+(12) (8))=+1
Substitute 6 for valence electrons, 6 for nonbonded electrons and 2 for the number of bonding electrons in equation (1) to calculate the formal charge on each single bonded oxygen atom.
Formal charge=(6)−((6)+(12) (2))=−1
Substitute 6 for the value of valence electrons, 4 for the number of nonbonded electrons and 4 for the number of bonding electrons in equation (1) to calculate the formal charge on the double bonded oxygen atom.
Formal charge=(6)−((4)+(12) (4))=0
For structure III:
Substitute 7 for valence electrons, 2 for the number of nonbonded electrons and 10 for the number of bonding electrons in equation (1) to calculate the formal charge on Br atom.
Formal charge=(7)−((2)+(12) (10))=0
Substitute 6 for valence electrons, 6 for nonbonded electrons and 2 for number of bonding electrons in equation (1) to calculate the formal charge on the single bonded oxygen atom.
Formal charge=(6)−((6)+(12) (2))=−1
Substitute 6 for the value of valence electrons, 4 for the number of nonbonded electrons and 4 for the number of bonding electrons in equation (1) to calculate the formal charge on each double bonded oxygen atom.
Formal charge=(6)−((4)+(12) (4))=0.
Therefore, structure II has the more acceptable and reasonable distribution of formal charges.
The oxidation numbers of Br is +5 and the oxidation number of oxygen is –2.
BrO−3 has three possible resonating structures. Structure II is more acceptable and has a more distributed formal charge.
(b)
Interpretation:
Lewis structure for a resonance form of each ion of SO2−3 with the lowest possible formal charges is to be drawn. Also, the oxidation number of the atom is to be determined.
Concept introduction:
The steps to draw the Lewis structure of the molecule are as follows:
Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.
Step 2: Calculate the total number of valence electrons.
Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.
Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.
Formula to calculate the formal charge of the atom is as follows:
Formal charge=(number ofvalenceelectrons)−((number of non-bonding electrons )+(12) (number of bonding electrons)) (1)
The formula to calculate the oxidation number of an atom is as follows:
Oxidation number=(number ofvalenceelectrons)−((number of non-bonding electrons )+ (number of bonding electrons)) (2)
(b)
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Answer to Problem 10.17P
The possible Lewis structures for a resonance form of each ion of SO2−3 with the lowest possible formal charges are,
The oxidation numbers of. S is +4 and the oxidation number of oxygen is –2.
Explanation of Solution
Lewis structure for a resonance form of SO2−3 is,
For structure I:
Substitute 6 for valence electrons, 2 for the number of nonbonded electrons and 6 for the number of bonding electrons in equation (1) to calculate the formal charge on S atom.
Formal charge=(6)−((2)+(12) (6))=+1
Substitute 6 for valence electrons, 6 for nonbonded electrons and 2 for the number of bonding electrons in equation (1) to calculate the formal charge on each oxygen atom.
Formal charge=(6)−((6)+(12) (2))=−1
For structure II:
Substitute 6 for valence electrons, 2 for the number of nonbonded electrons and 8 for the number of bonding electrons in equation (1) to calculate the formal charge on S atom.
Formal charge=(6)−((2)+(12) (8))=0
Substitute 6 for valence electrons, 6 for nonbonded electrons and 2 for the number of bonding electrons in equation (1) to calculate the formal charge on each single bonded oxygen atom.
Formal charge=(6)−((6)+(12) (2))=−1
Substitute 6 for the value of valence electrons, 4 for the number of nonbonded electrons and 4 for the number of bonding electrons in equation (1) to calculate the formal charge on the double bonded oxygen atom.
Formal charge=(6)−((4)+(12) (4))=0.
Therefore, structure II has the more acceptable and reasonable distribution of formal charges.
The oxidation numbers of. S is +4 and the oxidation number of oxygen is –2.
SO2−3 has two possible resonating structures.
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Chapter 10 Solutions
Chemistry: The Molecular Nature of Matter and Change
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