Free Printable Electron Configuration Orbital Diagram Worksheets - Free Printable

Let's solve each element step by step, providing:

- Full electron configuration
- Short-hand (noble gas) electron configuration
- Orbital diagram (using arrows to represent electrons in orbitals)

We'll follow the Aufbau principle, Pauli exclusion principle, and Hund’s rule.

---

1. Nitrogen (N)

- Atomic number: 7 → 7 electrons

#### Full:
1s² 2s² 2p³

#### Short-hand:
[He] 2s² 2p³

#### Orbital Diagram:
```
1s: ↑↓
2s: ↑↓
2p: ↑ ↑ ↑
```

(Each box represents an orbital. The 2p subshell has three orbitals: 2px, 2py, 2pz. Electrons fill singly first before pairing.)

✔ Filling:
- 1s: 2 electrons (paired)
- 2s: 2 electrons (paired)
- 2p: 3 electrons — one in each of the three orbitals (unpaired, following Hund’s rule)

---

2. Sodium (Na)

- Atomic number: 11 → 11 electrons

#### Full:
1s² 2s² 2p⁶ 3s¹

#### Short-hand:
[Ne] 3s¹

#### Orbital Diagram:
```
1s: ↑↓
2s: ↑↓
2p: ↑↓ ↑↓ ↑↓
3s: ↑
```

- 1s, 2s, 2p are fully filled.
- 3s has one unpaired electron.

---

3. Chlorine (Cl)

- Atomic number: 17 → 17 electrons

#### Full:
1s² 2s² 2p⁶ 3s² 3p⁵

#### Short-hand:
[Ne] 3s² 3p⁵

#### Orbital Diagram:
```
1s: ↑↓
2s: ↑↓
2p: ↑↓ ↑↓ ↑↓
3s: ↑↓
3p: ↑↓ ↑↓ ↑
```

- 3p subshell has 5 electrons: two paired orbitals, one with a single electron (unpaired).

---

4. Calcium (Ca)

- Atomic number: 20 → 20 electrons

#### Full:
1s² 2s² 2p⁶ 3s² 3p⁶ 4s²

#### Short-hand:
[Ar] 4s²

#### Orbital Diagram:
```
1s: ↑↓
2s: ↑↓
2p: ↑↓ ↑↓ ↑↓
3s: ↑↓
3p: ↑↓ ↑↓ ↑↓
4s: ↑↓
```

- All orbitals up to 4s are filled.
- No unpaired electrons.

---

5. Gallium (Ga)

- Atomic number: 31 → 31 electrons

#### Full:
1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p¹

> Note: Order is 4s before 3d, but 3d fills after 4s.

#### Short-hand:
[Ar] 4s² 3d¹⁰ 4p¹

#### Orbital Diagram:
```
1s: ↑↓
2s: ↑↓
2p: ↑↓ ↑↓ ↑↓
3s: ↑↓
3p: ↑↓ ↑↓ ↑↓
4s: ↑↓
3d: ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓
4p: ↑
```

- 3d: 10 electrons → all paired
- 4p: 1 electron → unpaired

---

6. Krypton (Kr)

- Atomic number: 36 → 36 electrons

#### Full:
1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶

#### Short-hand:
[Kr] → This is a noble gas, so short-hand is just [Kr]

But since it's the element itself, we write the full configuration.

Wait: for Kr, short-hand would be [Kr], but that's redundant. So usually, we just write the full configuration.

Alternatively, if we're using noble gas shorthand for elements beyond Kr, we'd use [Kr]. But here, Kr is the noble gas, so its short-hand is just [Kr].

But for this exercise, we can write:

#### Full:
1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶

#### Short-hand:
[Kr] ← but since Kr is the element, this is correct as a shorthand representation.

Actually, short-hand for Kr is just [Kr] — no further abbreviation.

But in context, when writing configurations for other elements, we use [Kr], so here it's appropriate.

#### Orbital Diagram:
All orbitals filled up to 4p⁶.

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

- All orbitals are completely filled → no unpaired electrons.

---

✔ Final Answers:

---

1. Nitrogen (N)
- Full: 1s² 2s² 2p³
- Short-hand: [He] 2s² 2p³
- Orbital Diagram:
```
1s: ↑↓ 2s: ↑↓ 2p: ↑ ↑ ↑
```

---

2. Sodium (Na)
- Full: 1s² 2s² 2p⁶ 3s¹
- Short-hand: [Ne] 3s¹
- Orbital Diagram:
```
1s: ↑↓ 2s: ↑↓ 2p: ↑↓ ↑↓ ↑↓ 3s: ↑
```

---

3. Chlorine (Cl)
- Full: 1s² 2s² 2p⁶ 3s² 3p⁵
- Short-hand: [Ne] 3s² 3p⁵
- Orbital Diagram:
```
1s: ↑↓ 2s: ↑↓ 2p: ↑↓ ↑↓ ↑↓ 3s: ↑↓ 3p: ↑↓ ↑↓ ↑
```

---

4. Calcium (Ca)
- Full: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²
- Short-hand: [Ar] 4s²
- Orbital Diagram:
```
1s: ↑↓ 2s: ↑↓ 2p: ↑↓ ↑↓ ↑↓ 3s: ↑↓ 3p: ↑↓ ↑↓ ↑↓ 4s: ↑↓
```

---

5. Gallium (Ga)
- Full: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p¹
- Short-hand: [Ar] 4s² 3d¹⁰ 4p¹
- Orbital Diagram:
```
1s: ↑↓ 2s: ↑↓ 2p: ↑↓ ↑↓ ↑↓ 3s: ↑↓ 3p: ↑↓ ↑↓ ↑↓ 4s: ↑↓ 3d: ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ 4p: ↑
```

---

6. Krypton (Kr)
- Full: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶
- Short-hand: [Kr]
- Orbital Diagram:
```
1s: ↑↓ 2s: ↑↓ 2p: ↑↓ ↑↓ ↑↓ 3s: ↑↓ 3p: ↑↓ ↑↓ ↑↓ 4s: ↑↓ 3d: ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ 4p: ↑↓ ↑↓ ↑↓
```

---

📌 Tips for Drawing Orbital Diagrams:

- Each box = one orbital.
- Arrows (↑↓) = electrons; opposite spins.
- Fill orbitals from lowest energy to highest.
- In degenerate orbitals (like p, d), place one electron in each before pairing (Hund’s rule).
- Always check total electrons match atomic number.

Let me know if you'd like a printable version or visual diagrams!