Covalent Bonding Examples Worksheet

Let's solve this step by step. The task is to complete the table for covalent bonding examples, providing:

1. Lewis Dot Diagram of the final compound.
2. "Stick" Diagram (also known as a structural diagram, where lines represent bonds).

We’ll go through each compound one by one.

---

1. H₂ (Hydrogen gas)

- Atoms: 2 Hydrogen atoms
- Each hydrogen has 1 valence electron.
- To satisfy the octet rule (duet rule for H), they share their electrons to form a single covalent bond.

#### ✔ Lewis Dot Diagram:
```
H : H → H—H
```
But in Lewis notation:
```
H· + ·H → H:H
```
Or more clearly:
H—H with two electrons shared (a single bond).

> Lewis Structure: `H:H` or `H—H` with a line representing the shared pair.

#### ✔ "Stick" Diagram:
Just a single line between two H atoms:
```
H—H
```

---

2. Cl₂ (Chlorine gas)

- Atoms: 2 Chlorine atoms
- Each chlorine has 7 valence electrons.
- They share one electron each to form a single bond and achieve an octet.

#### ✔ Lewis Dot Diagram:
Each Cl has 3 lone pairs (6 electrons) and shares 1 electron with the other.

```
:Cl : :Cl: → :Cl — Cl:
|
(each Cl has 3 lone pairs)
```

More accurately:
```
.. ..
:Cl — Cl:
.. ..
```

So:
- Single bond between Cl atoms.
- Each Cl has three lone pairs (6 electrons) plus 2 shared electrons.

#### ✔ "Stick" Diagram:
```
Cl—Cl
```

---

3. HCl (Hydrogen chloride)

- Atoms: 1 H + 1 Cl
- H has 1 valence electron; Cl has 7.
- They share one electron each → single covalent bond.

#### ✔ Lewis Dot Diagram:
```
H — Cl:
..
..
```

With three lone pairs on Cl:
```
H — Cl:
..
..
```

Or:
```
H—Cl:
..
..
```

Full Lewis structure:
```
H—Cl: with three lone pairs on Cl
```

#### ✔ "Stick" Diagram:
```
H—Cl
```

---

4. NH₃ (Ammonia)

- Atoms: 1 Nitrogen + 3 Hydrogens
- Nitrogen has 5 valence electrons.
- Each hydrogen has 1.
- Nitrogen forms three single bonds with three H atoms.
- After bonding, nitrogen has one lone pair left.

#### ✔ Lewis Dot Diagram:
Nitrogen in center, bonded to three H atoms, and one lone pair on N.

```
H
|
H—N:
|
H
```

With two dots (lone pair) on N:
```
H
|
H—N:
|
H
```

Or written as:
```
H
|
H—N: (with two dots above N)
|
H
```

#### ✔ "Stick" Diagram:
```
H
|
H—N—H
```

This shows the three single bonds from N to H.

---

✔ Final Table Filled In:

| Atoms in the compound | Lewis Dot Diagram of the Final Compound | "Stick" Diagram |
|------------------------|------------------------------------------|------------------|
| H₂<br>2 Hydrogen Atoms | `H:H` or `H—H` (with shared pair) | `H—H` |
| Cl₂<br>2 Chlorine Atoms | `:Cl—Cl:` (each Cl has 3 lone pairs) | `Cl—Cl` |
| HCl<br>1 Hydrogen + 1 Chlorine | `H—Cl:` (Cl has 3 lone pairs) | `H—Cl` |
| NH₃<br>1 Nitrogen + 3 Hydrogen | ```
H
|
H—N:
|
H
``` (N has one lone pair) | ```
H
|
H—N—H
``` |

---

🔍 Explanation Summary:

- Covalent bonds occur when atoms share electrons to achieve stable electron configurations.
- Lewis structures show valence electrons as dots and bonds as lines.
- "Stick" diagrams simplify this by showing only bonds (lines) and atoms.
- Hydrogen needs 2 electrons (duet rule); others need 8 (octet rule).
- Lone pairs are shown in Lewis diagrams but not in stick diagrams.

Let me know if you'd like these drawn visually!