Educational worksheet on covalent bonding between non-metals, illustrating shared electrons with examples and a water molecule diagram.

It looks like you've uploaded a worksheet about covalent bonding, and the task is to draw the electron dot structures (Lewis structures) for various molecules, showing how electrons are shared between atoms. The goal is to illustrate covalent bonds using dots to represent valence electrons.

Let’s go through each molecule one by one and explain how to draw its Lewis structure.

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🔹 Covalent Bonding Basics:

- Covalent bonds form between non-metal atoms.
- Atoms share electrons to achieve a stable electron configuration (usually an octet, or 2 electrons for hydrogen).
- Each bond consists of two shared electrons (a single bond = 2 electrons).

---

✔ Step-by-step Solutions:

#### 1. O₂ (Oxygen molecule)
- Oxygen has 6 valence electrons.
- Two oxygen atoms share 2 electrons each to form a double bond.
- Each oxygen also has two lone pairs (4 non-bonding electrons).

```
.. ..
:O = O:
.. ..
```

Or in text form:
```
.. ..
:O=O:
.. ..
```

✔ Explanation: Double bond between two O atoms; each has two lone pairs.

---

#### 2. Br₂ (Bromine molecule)
- Bromine has 7 valence electrons.
- Two bromine atoms share one pair of electrons → single bond.
- Each Br has three lone pairs (6 non-bonding electrons).

```
.. ..
:Br - Br:
.. ..
```

Or:
```
.. ..
:Br—Br:
.. ..
```

✔ Explanation: Single bond between two Br atoms; each has three lone pairs.

---

#### 3. F₂ (Fluorine molecule)
- Fluorine has 7 valence electrons.
- Two F atoms share one pair → single bond.
- Each F has three lone pairs.

```
.. ..
:F - F:
.. ..
```

Or:
```
.. ..
:F—F:
.. ..
```

✔ Same as Br₂ — single bond, three lone pairs on each atom.

---

#### 4. I₂ (Iodine molecule)
- Iodine has 7 valence electrons.
- Similar to F₂ and Br₂ → single bond, three lone pairs per atom.

```
.. ..
:I - I:
.. ..
```

Or:
```
.. ..
:I—I:
.. ..
```

✔ Identical pattern: single bond, three lone pairs each.

---

#### 5. HCl (Hydrogen chloride)
- Hydrogen has 1 valence electron.
- Chlorine has 7 valence electrons.
- They share one pair → single bond.
- Chlorine has three lone pairs.

```
H - Cl:
..
..
```

Or more clearly:
```
H — Cl:
..
..
```

With dots around Cl:
```
H — :Cl:
..
```

✔ Hydrogen shares one electron with Cl; Cl completes octet.

---

#### 6. CH₄ (Methane)
- Carbon has 4 valence electrons.
- Each hydrogen has 1 valence electron.
- Carbon forms four single bonds with four H atoms.
- No lone pairs on carbon; each H has no lone pairs.

```
H
|
H - C - H
|
H
```

In electron dot form:
```
H
|
H - C - H
|
H
```

But with dots:
```
H
|
H - C - H
|
H
```

Each bond represents 2 shared electrons.

✔ Carbon shares one electron with each H; all atoms have full valence shells.

---

✔ Final Answer Summary:

| Molecule | Lewis Structure (Text Representation) |
|---------|----------------------------------------|
| 1. O₂ | `:O=O:` with two lone pairs on each O |
| 2. Br₂ | `:Br—Br:` with three lone pairs on each Br |
| 3. F₂ | `:F—F:` with three lone pairs on each F |
| 4. I₂ | `:I—I:` with three lone pairs on each I |
| 5. HCl | `H—:Cl:` with three lone pairs on Cl |
| 6. CH₄ | Central C bonded to four H atoms (no lone pairs) |

---

📌 Tips for Drawing Lewis Structures:

1. Count total valence electrons.
2. Place atoms (least electronegative in center, except H always on outside).
3. Connect atoms with single bonds (each bond = 2 electrons).
4. Distribute remaining electrons as lone pairs.
5. Check that atoms satisfy octet rule (H only needs 2 electrons).

Let me know if you'd like these drawn visually or need help with a specific molecule!