Atomic Structure worksheet with Bohr diagram instructions and element examples.

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Part 1: Understanding the Periodic Table Symbols

You are given three elements:

1. Oxygen (O)
- Atomic number: 8
- Mass number: 16.00
- Symbol: O

2. Carbon (C)
- Atomic number: 6
- Mass number: 12.01
- Symbol: C

3. Neon (Ne)
- Atomic number: 10
- Mass number: 20.18
- Symbol: Ne

4. Potassium (K)
- Atomic number: 19
- Mass number: 39.10
- Symbol: K

#### Questions:
- What 2 parts of an atom does the atomic # represent?
→ The atomic number represents:
1. The number of protons in the nucleus.
2. The number of electrons in a neutral atom.

- How do you figure out the # of neutrons?
→ Use the formula:
\[
\text{Number of neutrons} = \text{Mass number} - \text{Atomic number}
\]

Example for Oxygen:
\(16 - 8 = 8\) neutrons

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Part 2: Creating Bohr Diagrams

#### Rules for arranging electrons:
1. The 1st energy level holds up to 2 electrons.
2. The 2nd energy level holds up to 8 electrons.
3. The 3rd energy level holds up to 8 electrons (for most atoms).

> Note: The 3rd level can actually hold up to 18 electrons in advanced chemistry, but in basic models, it's often capped at 8.

#### Term for electrons in the outermost energy level:
→ The term used is valence electrons.

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Sketching Atoms: Examples

Let’s go through each element and sketch a Bohr diagram.

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#### Example 1: Oxygen (O)
- Atomic number: 8 → 8 protons, 8 electrons
- Electrons arranged:
- 1st shell: 2 electrons
- 2nd shell: 6 electrons
- Valence electrons: 6

Bohr Diagram:
```
••
• •
• •
• •
••
```
(Inner circle: 2 e⁻, Outer circle: 6 e⁻)

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#### Example 2: Carbon (C)
- Atomic number: 6 → 6 protons, 6 electrons
- Electron configuration:
- 1st shell: 2 e⁻
- 2nd shell: 4 e⁻
- Valence electrons: 4

Bohr Diagram:
```
••
• •
• •
• •
••
```
(Outer ring has 4 electrons)

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#### Example 3: Neon (Ne)
- Atomic number: 10 → 10 protons, 10 electrons
- Configuration:
- 1st shell: 2 e⁻
- 2nd shell: 8 e⁻
- Valence electrons: 8 (full outer shell → noble gas)

Bohr Diagram:
```
••
• •
• •
• •
••
```
(Outer ring full with 8 electrons)

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#### Example 4: Potassium (K)
- Atomic number: 19 → 19 protons, 19 electrons
- Configuration:
- 1st shell: 2 e⁻
- 2nd shell: 8 e⁻
- 3rd shell: 8 e⁻
- 4th shell: 1 e⁻
- Valence electrons: 1

Bohr Diagram:
```
••
• •
• •
• •
••
•
```
(4th shell has just 1 electron)

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Summary of Key Concepts

| Element | Protons | Electrons | Neutrons | Valence Electrons |
|--------|--------|----------|---------|------------------|
| O | 8 | 8 | 8 | 6 |
| C | 6 | 6 | 6 | 4 |
| Ne | 10 | 10 | 10 | 8 |
| K | 19 | 19 | 20 | 1 |

> For potassium:
> Mass number ≈ 39, so neutrons = 39 - 19 = 20

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Final Answers to Worksheet Questions:

1. What 2 parts of an atom does the atomic # represent?
→ Number of protons and number of electrons (in a neutral atom).

2. How do you figure out the # of neutrons?
→ Subtract atomic number from mass number:
\( \text{Neutrons} = \text{Mass number} - \text{Atomic number} \)

3. Term for electrons in the outermost energy level?
→ Valence electrons

4. Bohr Diagrams: Follow the rules above and draw concentric circles with electrons placed accordingly.

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