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Concept explainers
(a)
Interpretation:
Lewis structure with the lowest formal charges of
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:
(a)
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Answer to Problem 10.5BFP
Lewis structure with lowest formal charges for
The formal charge on
The formal charge on each
Explanation of Solution
The total number of valence electrons of
Substitute 3 for the total number of
The Lewis structure of
Substitute 2 for the number of valence electrons, 0 for the number of nonbonded electrons and 4 for the number of bonding electrons in equation (1) to calculate the formal charge on
Substitute 1 for the number of valence electrons, 0 for the number of nonbonded electrons and 2 for the number of bonding electrons in equation (1) to calculate the formal charge on each hydrogen atom.
(b)
Interpretation:
Lewis structure with the lowest formal charges of
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:
(b)
![Check Mark](/static/check-mark.png)
Answer to Problem 10.5BFP
The Lewis structure of
The formal charge on central
The formal charge on the terminal
Explanation of Solution
The total number of valence electrons of
Substitute 3 for the total number of
The Lewis structure of
Substitute 7 for the number of valence electrons, 6 for the number of nonbonded electrons and 4 for the number of bonding electrons in equation (1) to calculate the formal charge on the central
Substitute 7 for the number of valence electrons, 6 for the number of nonbonded electrons and 2 for the number of bonding electrons in equation (1) to calculate the formal charge on each terminal
Only one Lewis structure is possible for
(c)
Interpretation:
Lewis structure with the lowest formal charges of
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:
(c)
![Check Mark](/static/check-mark.png)
Answer to Problem 10.5BFP
Lewis structure of
The formal charge on
The formal charge on each
Explanation of Solution
The Lewis structures of
For structure I:
Substitute 8 for the number of 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
Substitute 6 for the number of valence electrons, 6 for the number of nonbonded electrons and 2 for the number of bonding electrons in equation (1) to calculate the formal charge on each single bonded oxygen atom.
For structure II:
Substitute 8 for the number of 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
Substitute 6 for the number of valence electrons, 6 for the number of nonbonded electrons and 2 for the number of bonding electrons in equation (1) to calculate the formal charge on each single bonded oxygen atom.
Substitute 6 for the number 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.
For structure III:
Substitute 8 for the number of 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
Substitute 6 for the number of valence electrons, 6 for the number of nonbonded electrons and 2 for the number of bonding electrons in equation (1) to calculate the formal charge on the single bonded oxygen atom.
Substitute 6 for the number 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.
For structure IV:
Substitute 8 for the number of valence electrons, 2 for the number of nonbonded electrons and 12 for the number of bonding electrons in equation (1) to calculate the formal charge on
Substitute 6 for the number 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.
Four Lewis structures are possible for
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Connect 2-Year Access Card for Chemistry: The Molecular Nature of Matter and Change
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