Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question

Transcribed Image Text:**Question 3:** What are the formal charges on the atoms in:
**Diagram:**
The diagram depicts a molecule with a central carbon atom (C) which is bonded to three hydrogen atoms (H) and has a lone pair of electrons represented as dots next to the carbon atom.
**Explanation:**
To determine the formal charge on each atom:
1. **Carbon (C):**
- Valence electrons in a free carbon atom = 4
- Electrons in bonds + lone pair electrons:
- 3 bonds to hydrogen = 3 electrons
- 1 lone pair = 2 electrons
- Total assigned electrons = 3 + 2 = 5
- Formal charge = Valence electrons - Total assigned electrons
- Formal charge of carbon = 4 - 5 = -1
2. **Hydrogen (H):**
- Valence electrons in a free hydrogen atom = 1
- Each hydrogen is in a single bond with carbon, using 1 electron
- Formal charge = Valence electrons - Assigned electrons
- Formal charge of each hydrogen = 1 - 1 = 0
In conclusion, the carbon atom has a formal charge of -1, while each hydrogen atom has a formal charge of 0.
Expert Solution

Step 1
Formal charge is the charge assigned in atoms of a molecule.
It is calculated by :
FC = V - N - B/2
Where
- FC = formal charge
- V = total valence electrons
- N = number of non-boning electrons
- B = total number of electrons shared in bonds
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