VSEPR Theory Practice Problems - Chemistry Steps - Free Printable
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Step-by-step solution for: VSEPR Theory Practice Problems - Chemistry Steps
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Step-by-step solution for: VSEPR Theory Practice Problems - Chemistry Steps
It looks like you've uploaded a list of chemical compounds, labeled from (a) to (z), but no specific task was mentioned in your message. However, based on the format and typical chemistry problems involving such lists, it's likely that the task is to determine the molecular geometry, hybridization, or bond angles for each molecule.
Since no explicit instruction was given, I’ll assume the most common type of problem: Predict the molecular geometry and hybridization of the central atom for each molecule.
Let’s go through each compound one by one:
---
- Central atom: B
- Valence electrons: 3
- Bonded to 3 F atoms → 3 bonding pairs
- No lone pairs
- Electron geometry: Trigonal planar
- Molecular geometry: Trigonal planar
- Hybridization: sp²
---
- Central atom: C
- C bonded to 2 H and 1 O (double bond)
- 3 electron domains (2 single bonds + 1 double bond)
- No lone pairs on C
- Electron geometry: Trigonal planar
- Molecular geometry: Trigonal planar
- Hybridization: sp²
---
- Central atom: C
- C triple-bonded to N, single bond to H
- Linear arrangement
- 2 electron domains (triple bond counts as one domain)
- No lone pairs on C
- Electron geometry: Linear
- Molecular geometry: Linear
- Hybridization: sp
---
- Central atom: Be
- Be has 2 valence electrons, bonded to 2 Cl atoms
- 2 bonding pairs, no lone pairs
- Electron geometry: Linear
- Molecular geometry: Linear
- Hybridization: sp
---
- Central atom: C
- C bonded to 2 H and 2 Cl → 4 single bonds
- 4 bonding pairs, no lone pairs
- Electron geometry: Tetrahedral
- Molecular geometry: Tetrahedral
- Hybridization: sp³
---
- Central atom: S
- S bonded to 1 O (double bond), 2 Cl (single bonds)
- Sulfur has 6 valence electrons
- Double bond to O = 1 domain, two single bonds to Cl = 2 domains → 3 bonding domains
- One lone pair on S (total electrons: 6 - 4 used in bonds = 2 electrons = 1 lone pair)
- Electron geometry: Trigonal pyramidal? Wait — let's count:
- 3 bonding domains + 1 lone pair → Tetrahedral electron geometry
- Molecular geometry: Trigonal pyramidal
- Hybridization: sp³
Wait — actually, sulfur in SOCl₂ has:
- Double bond to O (counts as 1 domain)
- Two single bonds to Cl
- One lone pair
→ 4 electron domains → sp³ hybridization
But SOCl₂ has a trigonal pyramidal shape due to the lone pair.
✔ Molecular geometry: Trigonal pyramidal, Hybridization: sp³
---
- Central atom: S
- S double-bonded to two O atoms
- Sulfur has 6 valence electrons
- Two double bonds → 2 bonding domains
- But S also has 1 lone pair (since total electrons: 6 - 4 = 2 electrons = 1 lone pair)
- Electron domains: 3 (2 double bonds + 1 lone pair)
- Electron geometry: Trigonal planar
- Molecular geometry: Bent
- Hybridization: sp²
---
- Central atom: P
- P bonded to 5 Cl atoms
- 5 bonding pairs, no lone pairs
- Electron geometry: Trigonal bipyramidal
- Molecular geometry: Trigonal bipyramidal
- Hybridization: sp³d
---
- Central atom: Xe
- Xe bonded to 4 O atoms (double bonds)
- Xe has 8 valence electrons → all used in bonding (4×2 = 8)
- 4 bonding domains, no lone pairs
- Electron geometry: Tetrahedral
- Molecular geometry: Tetrahedral
- Hybridization: sp³
---
- Central atom: N
- N bonded to 3 Cl atoms
- Nitrogen has 5 valence electrons → 3 used in bonds → 2 left → 1 lone pair
- 3 bonding pairs, 1 lone pair
- Electron geometry: Tetrahedral
- Molecular geometry: Trigonal pyramidal
- Hybridization: sp³
---
- Central atom: Si
- Si bonded to 4 Cl atoms
- 4 bonding pairs, no lone pairs
- Electron geometry: Tetrahedral
- Molecular geometry: Tetrahedral
- Hybridization: sp³
---
- Central atom: S
- S bonded to 2 F atoms
- S has 6 valence electrons → 2 used in bonds → 4 left → 2 lone pairs
- 2 bonding pairs, 2 lone pairs
- Electron geometry: Tetrahedral
- Molecular geometry: Bent
- Hybridization: sp³
---
- Central atom: S
- S bonded to 2 H atoms
- S has 6 valence electrons → 2 used in bonds → 4 left → 2 lone pairs
- Same as SF₂
- Electron geometry: Tetrahedral
- Molecular geometry: Bent
- Hybridization: sp³
---
- Central atom: S
- S bonded to 3 O atoms (double bonds)
- S has 6 valence electrons → all used in bonding (3×2 = 6)
- 3 bonding domains, no lone pairs
- Electron geometry: Trigonal planar
- Molecular geometry: Trigonal planar
- Hybridization: sp²
---
- Central atom: C
- C double-bonded to O, single-bonded to two Cl atoms
- 3 bonding domains (one double bond, two single bonds)
- No lone pairs on C
- Electron geometry: Trigonal planar
- Molecular geometry: Trigonal planar
- Hybridization: sp²
---
- Central atom: P
- P bonded to 3 Cl atoms
- P has 5 valence electrons → 3 used in bonds → 2 left → 1 lone pair
- 3 bonding pairs, 1 lone pair
- Electron geometry: Tetrahedral
- Molecular geometry: Trigonal pyramidal
- Hybridization: sp³
---
- Central atom: O
- O bonded to 2 F atoms
- O has 6 valence electrons → 2 used in bonds → 4 left → 2 lone pairs
- 2 bonding pairs, 2 lone pairs
- Electron geometry: Tetrahedral
- Molecular geometry: Bent
- Hybridization: sp³
---
- Central atom: Br
- Br bonded to 5 F atoms
- Br has 7 valence electrons → 5 used in bonds → 2 left → 1 lone pair
- 5 bonding pairs, 1 lone pair
- Electron geometry: Octahedral
- Molecular geometry: Square pyramidal
- Hybridization: sp³d²
---
- Structure: N≡N–O or N=N=O
- Common structure: N≡N⁺–O⁻ or ⁻N=N⁺=O
- Central atom: Middle N
- In linear form: N–N≡O or N≡N–O with resonance
- Best representation: Linear molecule
- Bonding: Central N has two double bonds (or triple + single with resonance)
- Electron domains: 2 (linear)
- No lone pairs on central atom
- Molecular geometry: Linear
- Hybridization: sp
---
- Central atom: S
- S bonded to 6 Cl atoms
- Sulfur expands octet (has d-orbitals)
- 6 bonding pairs, no lone pairs
- Electron geometry: Octahedral
- Molecular geometry: Octahedral
- Hybridization: sp³d²
---
- Central atom: P
- P bonded to 3 Cl and 1 O (double bond)
- P has 5 valence electrons → 4 bonds (3 single + 1 double) → 8 electrons
- No lone pairs on P
- 4 bonding domains
- Electron geometry: Tetrahedral
- Molecular geometry: Tetrahedral
- Hybridization: sp³
---
- Central atom: Xe
- Xe bonded to 2 F atoms
- Xe has 8 valence electrons → 2 used in bonds → 6 left → 3 lone pairs
- 2 bonding pairs, 3 lone pairs
- Electron geometry: Trigonal bipyramidal (5 domains)
- Molecular geometry: Linear
- Hybridization: sp³d
---
- Central atom: Xe
- Xe bonded to 4 F atoms
- Xe has 8 valence electrons → 4 used in bonds → 4 left → 2 lone pairs
- 4 bonding pairs, 2 lone pairs
- Electron geometry: Octahedral
- Molecular geometry: Square planar
- Hybridization: sp³d²
---
- Structure: H–C≡C–H
- Each carbon is bonded to 1 H and triple-bonded to other C
- Each C has 2 electron domains (1 single + 1 triple bond)
- Linear geometry around each C
- Molecular geometry: Linear
- Hybridization: sp
---
| Molecule | Geometry | Hybridization |
|---------|----------------------|---------------|
| (a) BF₃ | Trigonal planar | sp² |
| (b) CH₂O | Trigonal planar | sp² |
| (c) HCN | Linear | sp |
| (d) BeCl₂ | Linear | sp |
| (e) CH₂Cl₂ | Tetrahedral | sp³ |
| (f) SOCl₂ | Trigonal pyramidal | sp³ |
| (g) SO₂ | Bent | sp² |
| (h) PCl₅ | Trigonal bipyramidal | sp³d |
| (i) XeO₄ | Tetrahedral | sp³ |
| (j) NCl₃ | Trigonal pyramidal | sp³ |
| (k) SiCl₄ | Tetrahedral | sp³ |
| (l) SF₂ | Bent | sp³ |
| (m) H₂S | Bent | sp³ |
| (n) SO₃ | Trigonal planar | sp² |
| (o) COCl₂ | Trigonal planar | sp² |
| (p) PCl₃ | Trigonal pyramidal | sp³ |
| (q) OF₂ | Bent | sp³ |
| (r) BrF₅ | Square pyramidal | sp³d² |
| (s) N₂O | Linear | sp |
| (t) SCl₆ | Octahedral | sp³d² |
| (u) POCl₃ | Tetrahedral | sp³ |
| (x) XeF₂ | Linear | sp³d |
| (y) XeF₄ | Square planar | sp³d² |
| (z) C₂H₂ | Linear | sp |
---
If your original task was something different (like predicting polarity, dipole moment, or Lewis structures), please clarify, and I can adjust accordingly. But this is the standard interpretation of such a list.
Since no explicit instruction was given, I’ll assume the most common type of problem: Predict the molecular geometry and hybridization of the central atom for each molecule.
Let’s go through each compound one by one:
---
(a) BF₃
- Central atom: B
- Valence electrons: 3
- Bonded to 3 F atoms → 3 bonding pairs
- No lone pairs
- Electron geometry: Trigonal planar
- Molecular geometry: Trigonal planar
- Hybridization: sp²
---
(b) CH₂O (Formaldehyde)
- Central atom: C
- C bonded to 2 H and 1 O (double bond)
- 3 electron domains (2 single bonds + 1 double bond)
- No lone pairs on C
- Electron geometry: Trigonal planar
- Molecular geometry: Trigonal planar
- Hybridization: sp²
---
(c) HCN
- Central atom: C
- C triple-bonded to N, single bond to H
- Linear arrangement
- 2 electron domains (triple bond counts as one domain)
- No lone pairs on C
- Electron geometry: Linear
- Molecular geometry: Linear
- Hybridization: sp
---
(d) BeCl₂
- Central atom: Be
- Be has 2 valence electrons, bonded to 2 Cl atoms
- 2 bonding pairs, no lone pairs
- Electron geometry: Linear
- Molecular geometry: Linear
- Hybridization: sp
---
(e) CH₂Cl₂ (Dichloromethane)
- Central atom: C
- C bonded to 2 H and 2 Cl → 4 single bonds
- 4 bonding pairs, no lone pairs
- Electron geometry: Tetrahedral
- Molecular geometry: Tetrahedral
- Hybridization: sp³
---
(f) SOCl₂ (Thionyl chloride)
- Central atom: S
- S bonded to 1 O (double bond), 2 Cl (single bonds)
- Sulfur has 6 valence electrons
- Double bond to O = 1 domain, two single bonds to Cl = 2 domains → 3 bonding domains
- One lone pair on S (total electrons: 6 - 4 used in bonds = 2 electrons = 1 lone pair)
- Electron geometry: Trigonal pyramidal? Wait — let's count:
- 3 bonding domains + 1 lone pair → Tetrahedral electron geometry
- Molecular geometry: Trigonal pyramidal
- Hybridization: sp³
Wait — actually, sulfur in SOCl₂ has:
- Double bond to O (counts as 1 domain)
- Two single bonds to Cl
- One lone pair
→ 4 electron domains → sp³ hybridization
But SOCl₂ has a trigonal pyramidal shape due to the lone pair.
✔ Molecular geometry: Trigonal pyramidal, Hybridization: sp³
---
(g) SO₂
- Central atom: S
- S double-bonded to two O atoms
- Sulfur has 6 valence electrons
- Two double bonds → 2 bonding domains
- But S also has 1 lone pair (since total electrons: 6 - 4 = 2 electrons = 1 lone pair)
- Electron domains: 3 (2 double bonds + 1 lone pair)
- Electron geometry: Trigonal planar
- Molecular geometry: Bent
- Hybridization: sp²
---
(h) PCl₅
- Central atom: P
- P bonded to 5 Cl atoms
- 5 bonding pairs, no lone pairs
- Electron geometry: Trigonal bipyramidal
- Molecular geometry: Trigonal bipyramidal
- Hybridization: sp³d
---
(i) XeO₄
- Central atom: Xe
- Xe bonded to 4 O atoms (double bonds)
- Xe has 8 valence electrons → all used in bonding (4×2 = 8)
- 4 bonding domains, no lone pairs
- Electron geometry: Tetrahedral
- Molecular geometry: Tetrahedral
- Hybridization: sp³
---
(j) NCl₃
- Central atom: N
- N bonded to 3 Cl atoms
- Nitrogen has 5 valence electrons → 3 used in bonds → 2 left → 1 lone pair
- 3 bonding pairs, 1 lone pair
- Electron geometry: Tetrahedral
- Molecular geometry: Trigonal pyramidal
- Hybridization: sp³
---
(k) SiCl₄
- Central atom: Si
- Si bonded to 4 Cl atoms
- 4 bonding pairs, no lone pairs
- Electron geometry: Tetrahedral
- Molecular geometry: Tetrahedral
- Hybridization: sp³
---
(l) SF₂
- Central atom: S
- S bonded to 2 F atoms
- S has 6 valence electrons → 2 used in bonds → 4 left → 2 lone pairs
- 2 bonding pairs, 2 lone pairs
- Electron geometry: Tetrahedral
- Molecular geometry: Bent
- Hybridization: sp³
---
(m) H₂S
- Central atom: S
- S bonded to 2 H atoms
- S has 6 valence electrons → 2 used in bonds → 4 left → 2 lone pairs
- Same as SF₂
- Electron geometry: Tetrahedral
- Molecular geometry: Bent
- Hybridization: sp³
---
(n) SO₃
- Central atom: S
- S bonded to 3 O atoms (double bonds)
- S has 6 valence electrons → all used in bonding (3×2 = 6)
- 3 bonding domains, no lone pairs
- Electron geometry: Trigonal planar
- Molecular geometry: Trigonal planar
- Hybridization: sp²
---
(o) COCl₂ (Phosgene)
- Central atom: C
- C double-bonded to O, single-bonded to two Cl atoms
- 3 bonding domains (one double bond, two single bonds)
- No lone pairs on C
- Electron geometry: Trigonal planar
- Molecular geometry: Trigonal planar
- Hybridization: sp²
---
(p) PCl₃
- Central atom: P
- P bonded to 3 Cl atoms
- P has 5 valence electrons → 3 used in bonds → 2 left → 1 lone pair
- 3 bonding pairs, 1 lone pair
- Electron geometry: Tetrahedral
- Molecular geometry: Trigonal pyramidal
- Hybridization: sp³
---
(q) OF₂
- Central atom: O
- O bonded to 2 F atoms
- O has 6 valence electrons → 2 used in bonds → 4 left → 2 lone pairs
- 2 bonding pairs, 2 lone pairs
- Electron geometry: Tetrahedral
- Molecular geometry: Bent
- Hybridization: sp³
---
(r) BrF₅
- Central atom: Br
- Br bonded to 5 F atoms
- Br has 7 valence electrons → 5 used in bonds → 2 left → 1 lone pair
- 5 bonding pairs, 1 lone pair
- Electron geometry: Octahedral
- Molecular geometry: Square pyramidal
- Hybridization: sp³d²
---
(s) N₂O (Nitrous oxide)
- Structure: N≡N–O or N=N=O
- Common structure: N≡N⁺–O⁻ or ⁻N=N⁺=O
- Central atom: Middle N
- In linear form: N–N≡O or N≡N–O with resonance
- Best representation: Linear molecule
- Bonding: Central N has two double bonds (or triple + single with resonance)
- Electron domains: 2 (linear)
- No lone pairs on central atom
- Molecular geometry: Linear
- Hybridization: sp
---
(t) SCl₆
- Central atom: S
- S bonded to 6 Cl atoms
- Sulfur expands octet (has d-orbitals)
- 6 bonding pairs, no lone pairs
- Electron geometry: Octahedral
- Molecular geometry: Octahedral
- Hybridization: sp³d²
---
(u) POCl₃ (Phosphoryl chloride)
- Central atom: P
- P bonded to 3 Cl and 1 O (double bond)
- P has 5 valence electrons → 4 bonds (3 single + 1 double) → 8 electrons
- No lone pairs on P
- 4 bonding domains
- Electron geometry: Tetrahedral
- Molecular geometry: Tetrahedral
- Hybridization: sp³
---
(x) XeF₂
- Central atom: Xe
- Xe bonded to 2 F atoms
- Xe has 8 valence electrons → 2 used in bonds → 6 left → 3 lone pairs
- 2 bonding pairs, 3 lone pairs
- Electron geometry: Trigonal bipyramidal (5 domains)
- Molecular geometry: Linear
- Hybridization: sp³d
---
(y) XeF₄
- Central atom: Xe
- Xe bonded to 4 F atoms
- Xe has 8 valence electrons → 4 used in bonds → 4 left → 2 lone pairs
- 4 bonding pairs, 2 lone pairs
- Electron geometry: Octahedral
- Molecular geometry: Square planar
- Hybridization: sp³d²
---
(z) C₂H₂ (Acetylene)
- Structure: H–C≡C–H
- Each carbon is bonded to 1 H and triple-bonded to other C
- Each C has 2 electron domains (1 single + 1 triple bond)
- Linear geometry around each C
- Molecular geometry: Linear
- Hybridization: sp
---
✔ Summary Table
| Molecule | Geometry | Hybridization |
|---------|----------------------|---------------|
| (a) BF₃ | Trigonal planar | sp² |
| (b) CH₂O | Trigonal planar | sp² |
| (c) HCN | Linear | sp |
| (d) BeCl₂ | Linear | sp |
| (e) CH₂Cl₂ | Tetrahedral | sp³ |
| (f) SOCl₂ | Trigonal pyramidal | sp³ |
| (g) SO₂ | Bent | sp² |
| (h) PCl₅ | Trigonal bipyramidal | sp³d |
| (i) XeO₄ | Tetrahedral | sp³ |
| (j) NCl₃ | Trigonal pyramidal | sp³ |
| (k) SiCl₄ | Tetrahedral | sp³ |
| (l) SF₂ | Bent | sp³ |
| (m) H₂S | Bent | sp³ |
| (n) SO₃ | Trigonal planar | sp² |
| (o) COCl₂ | Trigonal planar | sp² |
| (p) PCl₃ | Trigonal pyramidal | sp³ |
| (q) OF₂ | Bent | sp³ |
| (r) BrF₅ | Square pyramidal | sp³d² |
| (s) N₂O | Linear | sp |
| (t) SCl₆ | Octahedral | sp³d² |
| (u) POCl₃ | Tetrahedral | sp³ |
| (x) XeF₂ | Linear | sp³d |
| (y) XeF₄ | Square planar | sp³d² |
| (z) C₂H₂ | Linear | sp |
---
If your original task was something different (like predicting polarity, dipole moment, or Lewis structures), please clarify, and I can adjust accordingly. But this is the standard interpretation of such a list.
Parent Tip: Review the logic above to help your child master the concept of vsepr worksheet with answers.
