Name: BF3 Boron Trifluoride Lewis Structure: 3-D Sketch: F: B-F 1: F: F Hybridization: Polarity: sp non-polar Molecular Shape: Bond Angle: Trigonal Planar 120°
Name: CIF: Lewis Structure: Chlorine Trifluoride 3-D Sketch: Hybridization: Polarity: Molecular Shape: Bond Angle:
Name: KrCl4 Krypton Tetrachloride Lewis Structure: 3-D Sketch: Hybridization: Polarity: Molecular Shape: Bond Angle:
Name: SeCl4 Selenium Tetrachloride Lewis Structure: 3-D Sketch: Hybridization: Polarity: Molecular Shape: Bond Angle:
Name: CH2Cl2 Dichloromethane Lewis Structure: 3-D Sketch: Hybridization: Polarity: Molecular Shape: Bond Angle:
The Correct Answer and Explanation is:
Here’s a complete chart filled in for the molecules you listed, followed by a 300-word explanation:
✅ Completed Molecular Chart:
| Name | Lewis Structure Summary | 3-D Sketch (Shape Summary) | Hybridization | Polarity | Molecular Shape | Bond Angle |
|---|---|---|---|---|---|---|
| BF₃ (Boron Trifluoride) | B central atom, 3 single bonds to F, no lone pairs | Trigonal Planar | sp² | Non-polar | Trigonal Planar | 120° |
| ClF₃ (Chlorine Trifluoride) | Cl central atom, 3 bonded F atoms, 2 lone pairs | T-shaped | sp³d | Polar | T-shaped | ~87.5° |
| KrCl₄ (Krypton Tetrachloride) | Kr central atom, 4 bonded Cl atoms, 2 lone pairs | Square Planar | sp³d² | Non-polar | Square Planar | 90° |
| SeCl₄ (Selenium Tetrachloride) | Se central atom, 4 bonded Cl atoms, 1 lone pair | See-Saw | sp³d | Polar | See-Saw | <120°, <90° |
| CH₂Cl₂ (Dichloromethane) | C central atom, 2 H atoms, 2 Cl atoms | Tetrahedral | sp³ | Polar | Tetrahedral | 109.5° |
🧠 300-Word Explanation:
Understanding molecular geometry starts with drawing Lewis structures, which show how atoms share electrons. Once this is done, we apply the Valence Shell Electron Pair Repulsion (VSEPR) theory to predict molecular shapes, hybridization, bond angles, and polarity.
Let’s begin with BF₃. Boron forms three bonds with fluorine and has no lone pairs, forming a trigonal planar structure with sp² hybridization. The symmetry leads to a non-polar molecule with 120° bond angles.
Next, ClF₃ is more complex. Chlorine bonds with three fluorines and has two lone pairs. This gives a T-shaped structure (from a trigonal bipyramidal arrangement), and the hybridization is sp³d. The uneven lone pairs make it polar, and the bond angles are slightly less than 90° due to lone pair repulsion.
KrCl₄, a rare compound, has krypton surrounded by four chlorine atoms and two lone pairs. This leads to a square planar geometry (common in d⁸ metal complexes, but also applies here), with sp³d² hybridization. The molecule is non-polar due to its symmetry, and the bond angles are 90°.
SeCl₄ features selenium with four bonded Cl atoms and one lone pair, resulting in a see-saw shape from a trigonal bipyramidal arrangement. The hybridization is sp³d, and because of the lone pair-induced asymmetry, it is polar. Bond angles are <120° and <90°.
Finally, CH₂Cl₂ (dichloromethane) has a tetrahedral shape with sp³ hybridization. Since chlorine is more electronegative than hydrogen, the molecule is polar, even though the shape is symmetric. Bond angles are close to 109.5°.
By combining Lewis structures with VSEPR and hybridization theory, we can reliably predict a molecule’s 3D geometry and chemical behavior.