This chemistry worksheet guides students through the process of drawing covalent bond diagrams using Lewis structures.

It looks like you've uploaded a worksheet titled "Drawing Covalent Bonds", which is designed to teach students how to draw covalent bonding diagrams (also known as Lewis structures) for simple molecules. The worksheet includes instructions, examples, and an activity section.

Since you mentioned solving the problem but didn't specify a particular question or task beyond what's shown, I will:

1. Explain the concepts in the worksheet.
2. Walk through the examples provided (A and B).
3. Provide guidance on how to complete similar problems, assuming you need help with the next steps.

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🔍 Understanding the Worksheet

#### ✔ What is a Covalent Bond?
- A covalent bond forms between nonmetals.
- It involves sharing pairs of electrons so that each atom achieves a stable octet (8 valence electrons), except hydrogen, which only needs 2 (duet rule).

Types of bonds:
- Single bond: 1 shared pair (2 electrons)
- Double bond: 2 shared pairs (4 electrons)
- Triple bond: 3 shared pairs (6 electrons)

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📝 Step-by-Step Guide from the Worksheet

Let’s go through the four steps:

#### 1. Draw electron dot diagrams (Lewis symbols) for each element
- Show the element symbol with dots around it representing valence electrons.

Example:
- Hydrogen (H): `H·` (1 valence e⁻)
- Chlorine (Cl): `:Cl:` with 7 dots (7 valence e⁻)
- Oxygen (O): `:Ö:` with 6 dots (6 valence e⁻)

#### 2. Count total valence electrons
- Add up all valence electrons from all atoms in the molecule.
- For HCl: 1 (H) + 7 (Cl) = 8 electrons
- For H₂O: 1×2 (H) + 6 (O) = 8 electrons

💡 Goal: Total should be 8 (or 2 for H), unless it's a special case.

#### 3. Determine the central atom
- Usually the atom with largest valence number or the one present only once.
- In HCl: Only two atoms → no central atom.
- In H₂O: Oxygen is central because there are two H atoms and one O.

#### 4. Pair electrons to form bonds
- Use single/double/triple bonds to share electrons.
- Each bond is a pair of electrons.
- After bonding, check if all atoms have full outer shells:
- H: 2 electrons (duet)
- Others: 8 electrons (octet)

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✔ Example A: HCl (Hydrogen Chloride)

| Element | Valence Electrons |
|--------|-------------------|
| H | 1 |
| Cl | 7 |
| Total: | 8 electrons |

Steps:
1. Draw Lewis symbols:
- H·
- :Cl: (with 7 dots)
2. Share one electron from H and one from Cl → forms a single bond.
3. Remaining electrons go around Cl to complete its octet.

Final Diagram:
```
H — Cl:
..
```

But properly drawn as:
```
H — Cl:
..
..
```
(With 3 lone pairs on Cl)

✔ Check: H has 2 electrons (bonded), Cl has 8 (1 bond + 3 lone pairs). ✔️

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✔ Example B: H₂O (Water)

| Element | Valence Electrons |
|--------|-------------------|
| H | 1 × 2 = 2 |
| O | 6 |
| Total: | 8 electrons |

Steps:
1. Oxygen is central (only one O, two H atoms).
2. Connect each H to O via a single bond (each bond uses 2 electrons).
- Two bonds = 4 electrons used.
3. Remaining 4 electrons go as two lone pairs on oxygen.

Final Diagram:
```
H
\
O:
/ ..
H
```

Or more clearly:
```
H
\
O:
/ ..
H
```

Each H shares 2 electrons → duet satisfied.
Oxygen has 2 bonds (4 electrons) + 2 lone pairs (4 electrons) = 8 electrons → octet satisfied. ✔️

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❓ How to Complete the Rest?

Assuming the table continues (C, D, etc.), here’s how to approach any new compound:

#### Example: NH₃ (Ammonia)

| Nonmetal | Nonmetal | Formula | Bonding Diagram |
|---------|----------|--------|------------------|
| Nitrogen | Hydrogen | NH₃ | ? |

Steps:
1. Electron dots:
- N: `:N:` (5 valence e⁻)
- H: `H·` (1 e⁻)
2. Total valence e⁻: 5 + 1×3 = 8
3. Central atom: Nitrogen (only one N)
4. Attach three H atoms to N via single bonds.
- Uses 3×2 = 6 electrons
- Remaining 2 electrons → one lone pair on N

Diagram:
```
H
\
N:
/ ..
H
\
H
```

Or better:
```
H
\
N:
/ ..
H
\
H
```

Each H has 2 e⁻, N has 3 bonds (6 e⁻) + 1 lone pair (2 e⁻) = 8 e⁻ → octet ✔️

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✔ Summary: Tips for Drawing Covalent Bonds

| Tip | Explanation |
|-----|-------------|
| 💡 Count valence electrons first | Helps ensure correct total |
| ⚠️ Hydrogen only needs 2 electrons | Never forms double/triple bonds |
| 🧩 Central atom usually has most valence e⁻ | Or appears once |
| 🔁 Try different arrangements | If not working, try double bonds |
| 🔄 Practice makes perfect | Trial and error is normal! |

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📌 Final Answer (if this was a request to "solve" the worksheet):

The worksheet is already partially solved with two examples (HCl and H₂O). To continue:

You would apply the same steps to other compounds like:
- CH₄ (Methane) – Carbon central, 4 H atoms, 4 single bonds
- CO₂ (Carbon dioxide) – Double bonds needed
- N₂ (Nitrogen gas) – Triple bond between two N atoms

Would you like me to complete the rest of the worksheet? Just let me know the remaining compounds listed in the table!

Let me know if you'd like:
- A downloadable version of the completed worksheet
- More examples
- Help with a specific molecule

I'm happy to assist further!