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57. draw the correct lewis structure, determine shape and polarity of t…

Question

  1. draw the correct lewis structure, determine shape and polarity of the following molecules (ions): ocl₂, so₂, nh₄⁺ pcl₃, no₂⁻, ch₂cl₂

Explanation:

Response
1. $\boldsymbol{\ce{OCl2}}$
Step 1: Calculate Valence Electrons

O: 6, Cl: 7 (2 Cl atoms: $2 \times 7 = 14$). Total: $6 + 14 = 20$.

Step 2: Draw Lewis Structure

O is central. Single bonds to 2 Cl atoms. O has 2 lone pairs (4 electrons), each Cl has 3 lone pairs (6 electrons each).
Lewis structure: $\ce{Cl - O - Cl}$ (with 2 lone pairs on O, 3 on each Cl).

Step 3: Determine Electron and Molecular Geometry
  • Electron geometry: Tetrahedral (4 electron groups: 2 bonds, 2 lone pairs).
  • Molecular geometry: Bent (angular).
Step 4: Determine Polarity

Bond dipoles: $\ce{O - Cl}$ bonds are polar (O is more electronegative). Lone pairs on O create a net dipole. Polar.

2. $\boldsymbol{\ce{SO2}}$
Step 1: Valence Electrons

S: 6, O: 6 (2 O atoms: $2 \times 6 = 12$). Total: $6 + 12 = 18$.

Step 2: Lewis Structure

S is central. Double bond to one O, single bond to the other (resonance). S has 1 lone pair.
Lewis structure: $\ce{O=S - O}$ (with 1 lone pair on S, and resonance forms).

Step 3: Geometry
  • Electron geometry: Trigonal planar (3 electron groups: 2 bonds, 1 lone pair).
  • Molecular geometry: Bent (angular).
Step 4: Polarity

Bond dipoles: $\ce{S - O}$ bonds are polar. Lone pair on S and bond dipoles create a net dipole. Polar.

3. $\boldsymbol{\ce{NH4+}}$
Step 1: Valence Electrons

N: 5, H: 1 (4 H atoms: $4 \times 1 = 4$). Charge: +1 (lose 1 electron). Total: $5 + 4 - 1 = 8$.

Step 2: Lewis Structure

N is central. Single bonds to 4 H atoms. No lone pairs on N.
Lewis structure: $\ce{[H - N - H]+}$ (tetrahedral, 4 single bonds).

Step 3: Geometry
  • Electron and molecular geometry: Tetrahedral (4 bond pairs, no lone pairs).
Step 4: Polarity

Bond dipoles: $\ce{N - H}$ bonds are polar, but symmetry (tetrahedral) cancels dipoles. Nonpolar.

4. $\boldsymbol{\ce{PCl3}}$
Step 1: Valence Electrons

P: 5, Cl: 7 (3 Cl atoms: $3 \times 7 = 21$). Total: $5 + 21 = 26$.

Step 2: Lewis Structure

P is central. Single bonds to 3 Cl atoms. P has 1 lone pair.
Lewis structure: $\ce{Cl - P - Cl}$ (with 1 lone pair on P, 3 on each Cl).

Step 3: Geometry
  • Electron geometry: Tetrahedral (4 electron groups: 3 bonds, 1 lone pair).
  • Molecular geometry: Trigonal pyramidal.
Step 4: Polarity

Bond dipoles: $\ce{P - Cl}$ bonds are polar. Lone pair on P creates a net dipole. Polar.

5. $\boldsymbol{\ce{NO2-}}$
Step 1: Valence Electrons

N: 5, O: 6 (2 O atoms: $2 \times 6 = 12$). Charge: -1 (gain 1 electron). Total: $5 + 12 + 1 = 18$.

Step 2: Lewis Structure

N is central. Double bond to one O, single bond to the other (resonance). N has 1 lone pair.
Lewis structure: $\ce{[O=N - O]-}$ (with 1 lone pair on N, resonance forms).

Step 3: Geometry
  • Electron geometry: Trigonal planar (3 electron groups: 2 bonds, 1 lone pair).
  • Molecular geometry: Bent (angular).
Step 4: Polarity

Bond dipoles: $\ce{N - O}$ bonds are polar. Lone pair and bond dipoles create a net dipole. Polar.

6. $\boldsymbol{\ce{CH2Cl2}}$
Step 1: Valence Electrons

C: 4, H: 1 (2 H atoms: $2 \times 1 = 2$), Cl: 7 (2 Cl atoms: $2 \times 7 = 14$). Total: $4 + 2 + 14 = 20$.

Step 2: Lewis Structure

C is central. Single bonds to 2 H and 2 Cl atoms. No lone pairs on C.
Lewis structure: $\ce{H - C - H}$ (with 2 Cl atoms: $\ce{Cl - C - Cl}$).

Step 3: Geometry
  • Electron and molecular geometry: Tetrahedral (4 bond pairs).
Step 4: Polarity

Bond dipoles: $\ce{C - Cl}$ bonds are polar, $\ce{C - H}$ bonds are nonpolar. Asymmetry (2 Cl, 2 H) creates a net dip…

Answer:

See the detailed breakdown above for Lewis structures, geometries, and polarities of $\ce{OCl2}$, $\ce{SO2}$, $\ce{NH4+}$, $\ce{PCl3}$, $\ce{NO2-}$, and $\ce{CH2Cl2}$.