Free Printable Electron Configuration Orbital Diagram Worksheets - Free Printable

To solve the problem, we need to determine the complete and short-hand electron configurations for each element listed and fill in the corresponding orbital diagrams. Let's go through each element step by step.

---

1. Nitrogen (N)

- Atomic Number: 7
- Electron Configuration:
- Full: \(1s^2 \, 2s^2 \, 2p^3\)
- Short-hand: \([He] \, 2s^2 \, 2p^3\)

- Orbital Diagram:
- \(1s\): Fully filled with 2 electrons.
- \(2s\): Fully filled with 2 electrons.
- \(2p\): Contains 3 electrons, following Hund's rule (each orbital gets one electron first before pairing).

```
1s: ↑↓
2s: ↑↓
2p: ↑ ↑ ↑
```

---

2. Sodium (Na)

- Atomic Number: 11
- Electron Configuration:
- Full: \(1s^2 \, 2s^2 \, 2p^6 \, 3s^1\)
- Short-hand: \([Ne] \, 3s^1\)

- Orbital Diagram:
- \(1s\): Fully filled with 2 electrons.
- \(2s\): Fully filled with 2 electrons.
- \(2p\): Fully filled with 6 electrons.
- \(3s\): Contains 1 electron.

```
1s: ↑↓
2s: ↑↓
2p: ↑↓ ↑↓ ↑↓
3s: ↑
```

---

3. Chlorine (Cl)

- Atomic Number: 17
- Electron Configuration:
- Full: \(1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^5\)
- Short-hand: \([Ne] \, 3s^2 \, 3p^5\)

- Orbital Diagram:
- \(1s\): Fully filled with 2 electrons.
- \(2s\): Fully filled with 2 electrons.
- \(2p\): Fully filled with 6 electrons.
- \(3s\): Fully filled with 2 electrons.
- \(3p\): Contains 5 electrons, following Hund's rule.

```
1s: ↑↓
2s: ↑↓
2p: ↑↓ ↑↓ ↑↓
3s: ↑↓
3p: ↑ ↑ ↑ ↑ ↑
```

---

4. Calcium (Ca)

- Atomic Number: 20
- Electron Configuration:
- Full: \(1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2\)
- Short-hand: \([Ar] \, 4s^2\)

- Orbital Diagram:
- \(1s\): Fully filled with 2 electrons.
- \(2s\): Fully filled with 2 electrons.
- \(2p\): Fully filled with 6 electrons.
- \(3s\): Fully filled with 2 electrons.
- \(3p\): Fully filled with 6 electrons.
- \(4s\): Fully filled with 2 electrons.

```
1s: ↑↓
2s: ↑↓
2p: ↑↓ ↑↓ ↑↓
3s: ↑↓
3p: ↑↓ ↑↓ ↑↓
4s: ↑↓
```

---

5. Gallium (Ga)

- Atomic Number: 31
- Electron Configuration:
- Full: \(1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^{10} \, 4p^1\)
- Short-hand: \([Ar] \, 3d^{10} \, 4s^2 \, 4p^1\)

- Orbital Diagram:
- \(1s\): Fully filled with 2 electrons.
- \(2s\): Fully filled with 2 electrons.
- \(2p\): Fully filled with 6 electrons.
- \(3s\): Fully filled with 2 electrons.
- \(3p\): Fully filled with 6 electrons.
- \(4s\): Fully filled with 2 electrons.
- \(3d\): Fully filled with 10 electrons.
- \(4p\): Contains 1 electron.

```
1s: ↑↓
2s: ↑↓
2p: ↑↓ ↑↓ ↑↓
3s: ↑↓
3p: ↑↓ ↑↓ ↑↓
4s: ↑↓
3d: ↑↓ ↑↓ ↑↓ ↑↓ ↑↓
4p: ↑
```

---

6. Krypton (Kr)

- Atomic Number: 36
- Electron Configuration:
- Full: \(1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^{10} \, 4p^6\)
- Short-hand: \([Ar] \, 3d^{10} \, 4s^2 \, 4p^6\)

- Orbital Diagram:
- \(1s\): Fully filled with 2 electrons.
- \(2s\): Fully filled with 2 electrons.
- \(2p\): Fully filled with 6 electrons.
- \(3s\): Fully filled with 2 electrons.
- \(3p\): Fully filled with 6 electrons.
- \(4s\): Fully filled with 2 electrons.
- \(3d\): Fully filled with 10 electrons.
- \(4p\): Fully filled with 6 electrons.

```
1s: ↑↓
2s: ↑↓
2p: ↑↓ ↑↓ ↑↓
3s: ↑↓
3p: ↑↓ ↑↓ ↑↓
4s: ↑↓
3d: ↑↓ ↑↓ ↑↓ ↑↓ ↑↓
4p: ↑↓ ↑↓ ↑↓
```

---

Final Answers

1. Nitrogen (N)
- Full: \(1s^2 \, 2s^2 \, 2p^3\)
- Short-hand: \([He] \, 2s^2 \, 2p^3\)
- Orbital Diagram:
```
1s: ↑↓
2s: ↑↓
2p: ↑ ↑ ↑
```

2. Sodium (Na)
- Full: \(1s^2 \, 2s^2 \, 2p^6 \, 3s^1\)
- Short-hand: \([Ne] \, 3s^1\)
- Orbital Diagram:
```
1s: ↑↓
2s: ↑↓
2p: ↑↓ ↑↓ ↑↓
3s: ↑
```

3. Chlorine (Cl)
- Full: \(1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^5\)
- Short-hand: \([Ne] \, 3s^2 \, 3p^5\)
- Orbital Diagram:
```
1s: ↑↓
2s: ↑↓
2p: ↑↓ ↑↓ ↑↓
3s: ↑↓
3p: ↑ ↑ ↑ ↑ ↑
```

4. Calcium (Ca)
- Full: \(1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2\)
- Short-hand: \([Ar] \, 4s^2\)
- Orbital Diagram:
```
1s: ↑↓
2s: ↑↓
2p: ↑↓ ↑↓ ↑↓
3s: ↑↓
3p: ↑↓ ↑↓ ↑↓
4s: ↑↓
```

5. Gallium (Ga)
- Full: \(1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^{10} \, 4p^1\)
- Short-hand: \([Ar] \, 3d^{10} \, 4s^2 \, 4p^1\)
- Orbital Diagram:
```
1s: ↑↓
2s: ↑↓
2p: ↑↓ ↑↓ ↑↓
3s: ↑↓
3p: ↑↓ ↑↓ ↑↓
4s: ↑↓
3d: ↑↓ ↑↓ ↑↓ ↑↓ ↑↓
4p: ↑
```

6. Krypton (Kr)
- Full: \(1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^{10} \, 4p^6\)
- Short-hand: \([Ar] \, 3d^{10} \, 4s^2 \, 4p^6\)
- Orbital Diagram:
```
1s: ↑↓
2s: ↑↓
2p: ↑↓ ↑↓ ↑↓
3s: ↑↓
3p: ↑↓ ↑↓ ↑↓
4s: ↑↓
3d: ↑↓ ↑↓ ↑↓ ↑↓ ↑↓
4p: ↑↓ ↑↓ ↑↓
```

Boxed Final Answer

\[
\boxed{
\begin{array}{l}
\text{1. N: Full: } 1s^2 \, 2s^2 \, 2p^3, \text{ Short-hand: } [He] \, 2s^2 \, 2p^3 \\
\text{2. Na: Full: } 1s^2 \, 2s^2 \, 2p^6 \, 3s^1, \text{ Short-hand: } [Ne] \, 3s^1 \\
\text{3. Cl: Full: } 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^5, \text{ Short-hand: } [Ne] \, 3s^2 \, 3p^5 \\
\text{4. Ca: Full: } 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2, \text{ Short-hand: } [Ar] \, 4s^2 \\
\text{5. Ga: Full: } 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^{10} \, 4p^1, \text{ Short-hand: } [Ar] \, 3d^{10} \, 4s^2 \, 4p^1 \\
\text{6. Kr: Full: } 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^{10} \, 4p^6, \text{ Short-hand: } [Ar] \, 3d^{10} \, 4s^2 \, 4p^6 \\
\end{array}
}
\]