What is the molecular geometry of chloramine (NH2Cl)?

• A. Bent
• B. Tetrahedral
• C. Trigonal pyramidal
• D. Linear

Answer: (C)

Verified step by step guidance

1. Step 1: Draw the Lewis structure of chloramine (NH2Cl). Nitrogen (N) is the central atom bonded to two hydrogen (H) atoms and one chlorine (Cl) atom. Count the total valence electrons: N has 5, each H has 1, and Cl has 7, for a total of 5 + 2(1) + 7 = 15 electrons.
2. Step 2: Arrange the atoms with nitrogen in the center, bonded to two hydrogens and one chlorine. Distribute the remaining electrons to satisfy the octet rule for the outer atoms and then place any leftover electrons as lone pairs on the central nitrogen atom.
3. Step 3: Determine the number of electron groups around the nitrogen atom. There are three bonding pairs (N-H, N-H, N-Cl) and one lone pair on nitrogen, making a total of four electron groups.
4. Step 4: Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to predict the molecular geometry. Four electron groups with one lone pair correspond to a trigonal pyramidal shape because the lone pair repels the bonding pairs, causing the molecule to adopt this geometry.
5. Step 5: Confirm that the molecular geometry is trigonal pyramidal, not tetrahedral (which would require four bonding pairs) or bent/linear (which have fewer electron groups or different arrangements).