Concept explainers
Each of the following species will be encountered at some point in this text. They all have the same number of electrons binding the same number of atoms and the same arrangement of bonds; they are isoelectronic. Specify which atoms, if any, bear a formal charge in the Lewis formula given and the net charge for each species.
Interpretation:
For the given isoelectronic species, the formal charge on the atoms and the net charge on each species is to be determined.
Concept introduction:
Formula to calculate the formal charge on an atom:
In a molecule, the charge that is assigned to an atom is called the formal charge.
Answer to Problem 46P
Solution:
The formal charge is
The net charge on the species is
The formal charge on
The net charge on the species is
The formal charge on
The net charge on the species is
The formal charge on
The net charge on the species is
The formal charge on
Explanation of Solution
(a)
Nitrogen belongs to Group
Since, both the nitrogen atoms have zero formal charge on them, the net charge of the species is also zero.
(b)
Carbon belongs to Group
For carbon atom,
Hence, the formal charge on the carbon atom is
For nitrogen atom,
Hence, the formal charge on nitrogen is
Therefore, the net charge on the species is
(c)
Carbon belongs to Group
Hence, the formal charge on each carbon atom is
Therefore, the net charge on the species is
(d)
Nitrogen belongs to Group
For nitrogen atom,
Hence, the formal charge on nitrogen is
For oxygen atom,
Hence, the formal charge on oxygen is
Therefore, the net charge on the species is
(d)
Carbon belongs to Group
For carbon atom,
Hence, the formal charge on the carbon atom is
For oxygen atom,
Hence, the formal charge on oxygen is
Therefore, the net charge on the species is
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Chapter 1 Solutions
Organic Chemistry - Standalone book
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