Molecular Geometry and Polarity Worksheet for chemistry students.

To solve the problem, we need to analyze each molecule or ion step by step using the following guidelines:

1. Draw the Lewis Dot Structure: Ensure that all atoms follow the Octet Rule.
2. Predict Molecular Geometry: Use VSEPR (Valence Shell Electron Pair Repulsion) theory to determine the geometry.
3. Determine Molecular Polarity: Assess whether the molecule is polar or nonpolar based on its geometry and bond dipoles.
4. Identify Intermolecular Forces: Determine the types of intermolecular forces present.

Let's go through each molecule or ion:

---

1. CH₃Br

- Lewis Dot Structure: Carbon (C) is the central atom with three H atoms and one Br atom bonded to it. All atoms have a complete octet.
```
H
|
H-C-Br
|
H
```
- Molecular Geometry: Tetrahedral (all four groups around C are bonding pairs).
- Molecular Polarity: Polar (due to the difference in electronegativity between C and Br, creating a dipole moment).
- Intermolecular Forces: Dipole-dipole interactions and London dispersion forces.

---

2. Nl₃

- Lewis Dot Structure: Nitrogen (N) is the central atom with three I atoms bonded to it. All atoms have a complete octet.
```
I
|
I-N-I
|
I
```
- Molecular Geometry: Trigonal pyramidal (three bonding pairs and one lone pair on N).
- Molecular Polarity: Polar (due to the lone pair and the asymmetry of the molecule).
- Intermolecular Forces: Dipole-dipole interactions and London dispersion forces.

---

3. H₂S

- Lewis Dot Structure: Sulfur (S) is the central atom with two H atoms bonded to it. S has two lone pairs.
```
H
|
H-S
|
H
```
- Molecular Geometry: Bent (two bonding pairs and two lone pairs on S).
- Molecular Polarity: Polar (due to the lone pairs and the asymmetry of the molecule).
- Intermolecular Forces: Dipole-dipole interactions and London dispersion forces.

---

4. CS₂

- Lewis Dot Structure: Carbon (C) is the central atom with one S atom on each side. Both S atoms have two lone pairs.
```
S
|
C=S
|
S
```
- Molecular Geometry: Linear (two double bonds and no lone pairs on C).
- Molecular Polarity: Nonpolar (symmetrical structure with equal bond dipoles canceling out).
- Intermolecular Forces: London dispersion forces.

---

5. SO₂

- Lewis Dot Structure: Sulfur (S) is the central atom with two O atoms bonded to it. S has one lone pair.
```
O
|
S=O
|
O
```
- Molecular Geometry: Bent (two double bonds and one lone pair on S).
- Molecular Polarity: Polar (due to the lone pair and the asymmetry of the molecule).
- Intermolecular Forces: Dipole-dipole interactions and London dispersion forces.

---

6. CO₃²⁻

- Lewis Dot Structure: Carbon (C) is the central atom with three O atoms bonded to it. Each O has a negative charge and one lone pair.
```
O⁻
|
O⁻-C-O⁻
|
O⁻
```
- Molecular Geometry: Trigonal planar (three double bonds and no lone pairs on C).
- Molecular Polarity: Nonpolar (symmetrical structure with equal bond dipoles canceling out).
- Intermolecular Forces: Dipole-dipole interactions and London dispersion forces.

---

7. CCl₂O

- Lewis Dot Structure: Carbon (C) is the central atom with two Cl atoms and one O atom bonded to it. O has two lone pairs.
```
Cl
|
Cl-C-O
|
Cl
```
- Molecular Geometry: Trigonal planar (three bonding pairs and no lone pairs on C).
- Molecular Polarity: Polar (due to the difference in electronegativity between C and Cl/O, creating a dipole moment).
- Intermolecular Forces: Dipole-dipole interactions and London dispersion forces.

---

8. OF₂

- Lewis Dot Structure: Oxygen (O) is the central atom with two F atoms bonded to it. O has two lone pairs.
```
F
|
O-F
|
F
```
- Molecular Geometry: Bent (two bonding pairs and two lone pairs on O).
- Molecular Polarity: Polar (due to the lone pairs and the asymmetry of the molecule).
- Intermolecular Forces: Dipole-dipole interactions and London dispersion forces.

---

9. AsCl₃

- Lewis Dot Structure: Arsenic (As) is the central atom with three Cl atoms bonded to it. As has one lone pair.
```
Cl
|
Cl-As-Cl
|
Cl
```
- Molecular Geometry: Trigonal pyramidal (three bonding pairs and one lone pair on As).
- Molecular Polarity: Polar (due to the lone pair and the asymmetry of the molecule).
- Intermolecular Forces: Dipole-dipole interactions and London dispersion forces.

---

10. NH₄⁺

- Lewis Dot Structure: Nitrogen (N) is the central atom with four H atoms bonded to it. There are no lone pairs on N.
```
H
|
H-N-H
|
H
```
- Molecular Geometry: Tetrahedral (four bonding pairs and no lone pairs on N).
- Molecular Polarity: Nonpolar (symmetrical structure with equal bond dipoles canceling out).
- Intermolecular Forces: Ion-dipole interactions (if interacting with other ions) and London dispersion forces.

---

Final Answer:

\[
\boxed{
\begin{array}{|c|c|c|c|c|}
\hline
\text{Molecule or ion} & \text{Lewis Dot Structure} & \text{Molecular Geometry} & \text{Molecular Polarity} & \text{Intermolecular Forces} \\
\hline
\text{CH}_3\text{Br} & \text{Tetrahedral} & \text{Polar} & \text{Dipole-dipole, London dispersion} \\
\hline
\text{Nl}_3 & \text{Trigonal pyramidal} & \text{Polar} & \text{Dipole-dipole, London dispersion} \\
\hline
\text{H}_2\text{S} & \text{Bent} & \text{Polar} & \text{Dipole-dipole, London dispersion} \\
\hline
\text{CS}_2 & \text{Linear} & \text{Nonpolar} & \text{London dispersion} \\
\hline
\text{SO}_2 & \text{Bent} & \text{Polar} & \text{Dipole-dipole, London dispersion} \\
\hline
\text{CO}_3^{2-} & \text{Trigonal planar} & \text{Nonpolar} & \text{Dipole-dipole, London dispersion} \\
\hline
\text{CCl}_2\text{O} & \text{Trigonal planar} & \text{Polar} & \text{Dipole-dipole, London dispersion} \\
\hline
\text{OF}_2 & \text{Bent} & \text{Polar} & \text{Dipole-dipole, London dispersion} \\
\hline
\text{AsCl}_3 & \text{Trigonal pyramidal} & \text{Polar} & \text{Dipole-dipole, London dispersion} \\
\hline
\text{NH}_4^+ & \text{Tetrahedral} & \text{Nonpolar} & \text{Ion-dipole, London dispersion} \\
\hline
\end{array}
}
\]