Match the molecule to the correct molecular shape. CH2Cl2  [1]SO2   [2]NF3   [3]SO3   [4]Group of answer choicesCH2Cl2SO2NF3SO3

To match the molecules with their respective molecular shapes, we first need to identify the shapes based on VSEPR theory.

1. Breakdown the Problem

We have four molecules (CH2Cl2, SO2, NF3, and SO3) and need to determine their molecular shapes.

2. Relevant Concepts

• VSEPR Theory: This theory helps predict the geometry of individual molecules based on the repulsions between electron pairs around a central atom.
• Molecular shapes:
  • CH2Cl2: Tetrahedral
  • SO2: Bent
  • NF3: Trigonal pyramidal
  • SO3: Trigonal planar

3. Analysis and Detail

• CH2Cl2 (Dichloromethane):

  • Valence Electrons: C has 4, each H has 1 (2), each Cl has 7 (2) → Total = 20
  • It has a tetrahedral arrangement with four substituents (H, H, Cl, Cl).

• SO2 (Sulfur Dioxide):

  • Valence Electrons: S has 6, each O has 6 (2) → Total = 18
  • There are two bonding pairs and one lone pair, causing a bent shape.

• NF3 (Nitrogen Trifluoride):

  • Valence Electrons: N has 5, each F has 7 (3) → Total = 26
  • It has three bonding pairs and one lone pair, resulting in a trigonal pyramidal shape.

• SO3 (Sulfur Trioxide):

  • Valence Electrons: S has 6, each O has 6 (3) → Total = 24
  • It has three bonding pairs with no lone pairs, providing a trigonal planar shape.

4. Verify and Summarize

• CH2Cl2: Tetrahedral
• SO2: Bent
• NF3: Trigonal pyramidal
• SO3: Trigonal planar

Final Answer

• CH2Cl2: Tetrahedral
• SO2: Bent
• NF3: Trigonal pyramidal
• SO3: Trigonal planar

Match the molecules with their shapes accordingly:

• CH2Cl2 → Tetrahedral
• SO2 → Bent
• NF3 → Trigonal pyramidal
• SO3 → Trigonal planar