Complete the following table by filling in the type of hybridisation, type of bonds, geometry and bond angle for each molecule (some cells are already printed in the book and are shown here; the rest, marked '-', are blank):
CH4: hybridisation - , bonds 4 C-H (4σ bonds), geometry

Question

Complete the following table by filling in the type of hybridisation, type of bonds, geometry and bond angle for each molecule (some cells are already printed in the book and are shown here; the rest, marked '-', are blank):
CH4: hybridisation - , bonds 4 C-H (4σ bonds), geometry Tetrahedral, bond angle -
NH3: hybridisation sp3, bonds 3 N-H (3σ bonds) + 1 lone pair, geometry - , bond angle -
H2O: hybridisation - , bonds - , geometry angular, bond angle 104.5°
BF3: hybridisation sp2, bonds - , geometry - , bond angle 120°
C2H4: hybridisation - , bonds - , geometry - , bond angle 120°
BeF2: hybridisation - , bonds 2 Be-F, geometry Linear, bond angle -
C2H2: hybridisation sp, bonds (3σ+2π): 1 C-C σ, 2 C-H σ, 2 C-C π, geometry - , bond angle -

Accepted Answer

**Step 1. CH4** (given: 4 C-H, 4σ bonds, Tetrahedral). Hybridization: sp3 (one s + three p, section 5.4.5). Bond angle: 109.5° (109°28'), the regular, uncompressed tetrahedral angle since carbon carries no lone pair.

**Step 2. NH3** (given: sp3, 3 N-H/3σ bonds + 1 lone pair). Geometry: trigonal pyramidal (VSEPR AB3E, Table 5.4). Bond angle: ~107° (107°18'), compressed from 109.5° by the one lone pair's repulsion (section 5.3).

**Step 3. H2O** (given: angular, 104.5°). Hybridization: sp3 (four electron-pair positions on O). Type of bonds: 2 O-H sigma bonds + 2 lone pairs on O (section 5.3's worked water example).

**Step 4. BF3** (given: sp2, 120°). Type of bonds: 3 B-F sigma bonds (sp2-p overlap), no lone pair on B. Geometry: trigonal planar (matching the given 120° angle and Table 5.3).

**Step 5. C2H4** (given: 120°). Hybridization: sp2 (each carbon). Type of bonds: 4 C-H sigma bonds + 1 C-C sigma bond + 1 C-C pi bond (section 5.4.5's ethene example). Geometry: trigonal planar around each carbon (matching the given 120°).

**Step 6. BeF2** (given: 2 Be-F, Linear). Hybridization: sp (two orbitals, 180° apart). Bond angle: 180°, matching its linear shape and no lone pair on Be. …

🎓Unlock everything free for 14 days

Unlock everything free for 14 days