Covalent Bonding Worksheet - Colina Middle School - Free Printable

Problem: Covalent Bonding Worksheet

The task is to draw Lewis dot diagrams for various molecules and determine how electrons are shared between atoms to form covalent bonds. Below is a step-by-step solution for each part of the worksheet.

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#### 1. H₂ (Hydrogen)
- Atoms involved: 2 Hydrogen atoms (H)
- Electron configuration: Each H atom has 1 valence electron.
- Goal: Both H atoms need 2 electrons to complete their outer shell (duet rule).
- Solution:
- Each H atom shares its 1 electron with the other H atom.
- Result: A single covalent bond is formed.
- Lewis Dot Diagram:
```
H : H
```

---

#### 2. F₂ (Fluorine)
- Atoms involved: 2 Fluorine atoms (F)
- Electron configuration: Each F atom has 7 valence electrons.
- Goal: Each F atom needs 1 more electron to complete its octet.
- Solution:
- Each F atom shares 1 electron with the other F atom.
- Result: A single covalent bond is formed.
- Lewis Dot Diagram:
```
F : F
```

---

#### 3. O₂ (Oxygen)
- Atoms involved: 2 Oxygen atoms (O)
- Electron configuration: Each O atom has 6 valence electrons.
- Goal: Each O atom needs 2 more electrons to complete its octet.
- Solution:
- Each O atom shares 2 electrons with the other O atom.
- Result: A double covalent bond is formed.
- Lewis Dot Diagram:
```
O = O
```

---

#### 4. N₂ (Nitrogen)
- Atoms involved: 2 Nitrogen atoms (N)
- Electron configuration: Each N atom has 5 valence electrons.
- Goal: Each N atom needs 3 more electrons to complete its octet.
- Solution:
- Each N atom shares 3 electrons with the other N atom.
- Result: A triple covalent bond is formed.
- Lewis Dot Diagram:
```
N ≡ N
```

---

#### 5. BF₃ (Boron Trifluoride)
- Atoms involved: 1 Boron (B) and 3 Fluorine (F) atoms.
- Electron configuration:
- B: 3 valence electrons
- F: 7 valence electrons each
- Goal:
- B needs 3 more electrons to complete its octet.
- Each F atom needs 1 more electron to complete its octet.
- Solution:
- B shares its 3 electrons with 3 F atoms, forming 3 single bonds.
- Lewis Dot Diagram:
```
F
|
F - B - F
|
F
```

---

#### 6. NH₃ (Ammonia)
- Atoms involved: 1 Nitrogen (N) and 3 Hydrogen (H) atoms.
- Electron configuration:
- N: 5 valence electrons
- H: 1 valence electron each
- Goal:
- N needs 3 more electrons to complete its octet.
- Each H atom needs 1 more electron to complete its duet.
- Solution:
- N shares its 3 electrons with 3 H atoms, forming 3 single bonds.
- Lewis Dot Diagram:
```
H
|
H - N - H
```

---

#### 7. CO₂ (Carbon Dioxide)
- Atoms involved: 1 Carbon (C) and 2 Oxygen (O) atoms.
- Electron configuration:
- C: 4 valence electrons
- O: 6 valence electrons each
- Goal:
- C needs 4 more electrons to complete its octet.
- Each O atom needs 2 more electrons to complete its octet.
- Solution:
- C shares 2 electrons with each O atom, forming 2 double bonds.
- Lewis Dot Diagram:
```
O = C = O
```

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#### 8. CH₄ (Methane)
- Atoms involved: 1 Carbon (C) and 4 Hydrogen (H) atoms.
- Electron configuration:
- C: 4 valence electrons
- H: 1 valence electron each
- Goal:
- C needs 4 more electrons to complete its octet.
- Each H atom needs 1 more electron to complete its duet.
- Solution:
- C shares its 4 electrons with 4 H atoms, forming 4 single bonds.
- Lewis Dot Diagram:
```
H
/ \
H - C - H
\ /
H
```

---

#### 9. H₂O (Water)
- Atoms involved: 1 Oxygen (O) and 2 Hydrogen (H) atoms.
- Electron configuration:
- O: 6 valence electrons
- H: 1 valence electron each
- Goal:
- O needs 2 more electrons to complete its octet.
- Each H atom needs 1 more electron to complete its duet.
- Solution:
- O shares 2 electrons with each H atom, forming 2 single bonds.
- Lewis Dot Diagram:
```
H
/ \
H - O
\ /
```

---

#### 10. SO₂ (Sulfur Dioxide)
- Atoms involved: 1 Sulfur (S) and 2 Oxygen (O) atoms.
- Electron configuration:
- S: 6 valence electrons
- O: 6 valence electrons each
- Goal:
- S needs 2 more electrons to complete its octet.
- Each O atom needs 2 more electrons to complete its octet.
- Solution:
- S forms a double bond with one O atom and a single bond with the other O atom. The extra electron pair on S acts as a lone pair.
- Lewis Dot Diagram:
```
O
||
O - S
```

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Final Answer:

Each molecule's Lewis dot diagram is provided above. The key is to ensure that all atoms achieve a stable electron configuration (octet or duet rule) through sharing electrons.

Boxed Final Answer:
\boxed{\text{See detailed solutions above for each molecule's Lewis dot diagram.}}