Here are the electronic configurations for elements 1-30, following the Aufbau principle and Hund's rule:

Element | Atomic Number | Electronic Configuration

------- | -------- | --------

Hydrogen (H) | 1 | 1s¹

Helium (He) | 2 | 1s²

Lithium (Li) | 3 | 1s² 2s¹

Beryllium (Be) | 4 | 1s² 2s²

Boron (B) | 5 | 1s² 2s² 2p¹

Carbon (C) | 6 | 1s² 2s² 2p²

Nitrogen (N) | 7 | 1s² 2s² 2p³

Oxygen (O) | 8 | 1s² 2s² 2p⁴

Fluorine (F) | 9 | 1s² 2s² 2p⁵

Neon (Ne) | 10 | 1s² 2s² 2p⁶

Sodium (Na) | 11 | 1s² 2s² 2p⁶ 3s¹

Magnesium (Mg) | 12 | 1s² 2s² 2p⁶ 3s²

Aluminum (Al) | 13 | 1s² 2s² 2p⁶ 3s² 3p¹

Silicon (Si) | 14 | 1s² 2s² 2p⁶ 3s² 3p²

Phosphorus (P) | 15 | 1s² 2s² 2p⁶ 3s² 3p³

Sulfur (S) | 16 | 1s² 2s² 2p⁶ 3s² 3p⁴

Chlorine (Cl) | 17 | 1s² 2s² 2p⁶ 3s² 3p⁵

Argon (Ar) | 18 | 1s² 2s² 2p⁶ 3s² 3p⁶

Potassium (K) | 19 | 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹

Calcium (Ca) | 20 | 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²

Scandium (Sc) | 21 | 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹

Titanium (Ti) | 22 | 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d²

Vanadium (V) | 23 | 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d³

Chromium (Cr) | 24 | 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁵ (exception)

Manganese (Mn) | 25 | 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁵

Iron (Fe) | 26 | 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁶

Cobalt (Co) | 27 | 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁷

Nickel (Ni) | 28 | 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁸

Copper (Cu) | 29 | 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d¹⁰ (exception)

Zinc (Zn) | 30 | 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰

Important Notes:

* Aufbau Principle: Electrons fill orbitals in order of increasing energy.

* Hund's Rule: Within a subshell, electrons fill each orbital individually before pairing up.

* Exceptions: Chromium and Copper have slightly different electronic configurations due to the stability associated with half-filled and completely filled d-orbitals.