Textbook Question
a. Draw a Lewis structure for each of the following:
b. Draw a structure for each of the species that shows approximate bond angles.
c. Which species have no dipole moment?
1. CH3N2+
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1. A Review of General Chemistry
Formal Charges
Multiple Choice
Given the Lewis structure of , determine the formal charge on each atom.
A
The carbon atom has a formal charge of , and each oxygen atom has a formal charge of .
B
The carbon atom has a formal charge of , and each oxygen atom has a formal charge of .
C
The carbon atom has a formal charge of , and each oxygen atom has a formal charge of .
D
The carbon atom has a formal charge of , and each oxygen atom has a formal charge of .
Verified step by step guidance1
Draw the Lewis structure of CO\_2, showing the carbon atom in the center double bonded to each oxygen atom, with lone pairs on the oxygens to complete their octets.
Recall the formula for formal charge: \(\text{Formal Charge} = \text{Valence Electrons} - \text{Nonbonding Electrons} - \frac{1}{2} \times \text{Bonding Electrons}\).
Calculate the formal charge on the carbon atom by counting its valence electrons (4 for carbon), the number of nonbonding electrons on carbon (usually zero in CO\_2), and the bonding electrons (4 bonds total, so 8 bonding electrons).
Calculate the formal charge on each oxygen atom by counting their valence electrons (6 for oxygen), the number of nonbonding electrons (usually 4 lone pair electrons per oxygen), and the bonding electrons (4 bonding electrons per oxygen from the double bond).
Verify that the sum of all formal charges equals the overall charge of the molecule (which is zero for CO\_2), confirming the correctness of your formal charge assignments.
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