Multiple Choice
Which of the following best describes the electron domain geometry and molecular geometry of the ion ICl4−?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Ions
Multiple Choice
Which of the following statements correctly describes the Lewis dot structure of the CH(NH2)2^+ ion?
A
The central carbon atom forms three single bonds and has no lone pairs.
B
Each nitrogen atom in the ion has two lone pairs and forms a double bond with carbon.
C
The ion contains a carbon-nitrogen triple bond.
D
The central carbon atom forms two double bonds and has one lone pair.
Verified step by step guidance1
Identify the central atom in the ion CH(NH2)2^+. Typically, carbon is the central atom because it can form four bonds and is less electronegative than nitrogen.
Determine the total number of valence electrons available. Carbon has 4 valence electrons, each nitrogen has 5, each hydrogen has 1, and account for the positive charge by subtracting one electron.
Distribute electrons to form bonds between the central carbon and the two nitrogen atoms, and between each nitrogen and its attached hydrogens. Remember that each bond represents two shared electrons.
Assign lone pairs to the nitrogen atoms after bonding. Nitrogen typically has one lone pair when forming three bonds (as in NH2 groups), so check if this fits the electron count and formal charges.
Analyze the bonding around the carbon atom. Since carbon usually forms four bonds and prefers no lone pairs, verify if it forms three single bonds (to two nitrogens and one hydrogen) and has no lone pairs, consistent with the positive charge on the ion.
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