Virtual Lab - Quantum numbers

⚛ QUANTUM NUMBERS LABORATORY

Explore orbitals • Select electrons • Discover all four quantum numbers

🔬 1. Select Your Orbital and Electron

Select Orbital / Subshell 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 7s 7p

Select Electron Number

Important: Select a subshell first. Then select the electron number in that subshell. The simulation follows Hund's rule and the conventional left-to-right orbital-box order.

🎯 2. Orbital Box Diagram

Select an orbital to begin.

Select an electron to see its position in the orbital.

🌈 3. All Four Quantum Numbers

Principal Quantum Number ? n – Main energy level

Azimuthal Quantum Number ? l – Subshell shape

Magnetic Quantum Number ? mₗ – Orbital orientation

Spin Quantum Number ? mₛ – Electron spin

The four quantum numbers will appear here automatically.

📘 4. Understand the Four Quantum Numbers

Principal quantum number (n)
It indicates the main energy level or shell of an electron. Its values are 1, 2, 3, 4 and so on.

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Azimuthal quantum number (l)
It indicates the subshell. For s, l = 0; for p, l = 1; for d, l = 2; for f, l = 3.

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Magnetic quantum number (mₗ)
It indicates the orbital orientation. Its values range from minus l to plus l, including zero.

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Spin quantum number (mₛ)
It indicates the spin of the electron. Its possible values are plus one-half and minus one-half.

🧠 5. Quantum Number Practice

Test your understanding with automatically generated questions.

📌 6. Important Rules to Remember

Rule 1: The value of n is always a positive integer.
Rule 2: The value of l ranges from 0 to n − 1.
Rule 3: The value of mₗ ranges from −l to +l.
Rule 4: The value of mₛ is either +1/2 or −1/2.
Rule 5: Each orbital can accommodate a maximum of two electrons with opposite spins.
Rule 6: According to Hund's rule, electrons occupy degenerate orbitals singly with parallel spins before pairing.

Interactive Chemistry Learning Laboratory
Learn • Explore • Experiment • Understand