ℹ️ How to use: Enter an atomic number (1-118), specify orbital configuration, set maximum electrons, and click calculate. Visual orbital diagram appears below results.
Visualize electron configurations and master quantum mechanical principles instantly
An orbital box diagram shows electrons arranged in boxes. Each box represents one orbital. One orbital holds maximum two electrons. Electrons are shown as arrows. Arrows pointing up and down indicate electron spin.
These diagrams help visualize electron distribution around atoms. They make complex quantum concepts easier to understand. Students can predict chemical behavior through orbital patterns.
Each square box represents a single atomic orbital. The filling order follows the Aufbau principle strictly. Hund's rule guides electrons into orbitals with parallel spins.
Energy levels increase from lower to higher orbitals. Electrons fill lower energy orbitals first always. Each level can contain different maximum electron numbers.
S orbitals hold maximum two electrons only. P orbitals hold maximum six electrons in total. D orbitals hold maximum ten electrons in complete configuration. F orbitals hold maximum fourteen electrons when fully filled.
Orbital diagrams predict bonding and reactivity patterns. They help explain why elements form specific compounds. Scientists use them to understand molecular structure.
Quantum numbers describe electron position and energy. Principal quantum number defines energy level shells. Azimuthal quantum number determines orbital shape characteristics.
Transition metals often show irregular electron configurations. Some elements have half-filled d orbital stability advantages. Fully filled orbitals provide extra stability to elements.
Electrons exhibit intrinsic angular momentum called spin. Spin generates magnetic moment in electron behavior. Paired electrons have opposite spins canceling magnetic effects.
Orbital hybridization explains molecular bonding phenomena clearly. Hybrid orbitals form when atomic orbitals mix. Carbon forms sp3, sp2, and sp hybrid orbitals.
The quantum mechanical model replaced Bohr's atomic model. Orbitals represent electron probability regions, not exact paths. Electrons exist as wave-particle duality entities.
Wave functions describe electron behavior mathematically. Probability density shows electron location likelihood regions. Squaring the wave function gives probability density.
Penetration describes how electrons approach the nucleus. S-orbitals penetrate more than p-orbitals effectively. Inner electrons shield outer electrons from charge.
Aufbau principle guides electron filling order systematically. Electrons fill lowest energy orbitals first always. Orbital energy depends on both n and l.
Pauli exclusion prevents identical quantum state occupation. Maximum two electrons share one orbital only. Electrons must have different spin quantum numbers.
Term symbols describe atomic states concisely. They incorporate spin and orbital angular momentum. Spectroscopy reveals orbital transition information directly.
Unpaired electrons create paramagnetic behavior in atoms. Paired electrons create diamagnetic behavior patterns. Magnetic susceptibility depends on unpaired electron counts.
Ionization energy increases across each period generally. It decreases down each group predictably. Noble gases show highest ionization energy values.
| Orbital Type | Shape | Number of Boxes | Max Electrons | Angular Momentum (l) | First Appearance |
|---|---|---|---|---|---|
| s | Spherical | 1 | 2 | 0 | 1s |
| p | Dumbbell-shaped | 3 | 6 | 1 | 2p |
| d | Cloverleaf-shaped | 5 | 10 | 2 | 3d |
| f | Complex multi-lobed | 7 | 14 | 3 | 4f |
S-block elements fill s-orbitals as valence electrons. Group 1 elements have one valence electron. Group 2 elements have two valence electrons. These form alkali and alkaline earth metals.
P-block elements fill p-orbitals as valence electrons. Group 18 elements complete p-orbital shells fully. These include nonmetals, halogens, and noble gases.
D-block elements fill d-orbitals progressively systematically. These are called transition metals scientifically. Many show multiple oxidation states due to electrons.
F-block elements fill f-orbitals in inner shells. Lanthanides are called rare earth elements. Actinides include most radioactive elements known.
1s² → 2s² → 2p⁶ → 3s² → 3p⁶ → 4s² → 3d¹⁰ → 4p⁶ → 5s² → 4d¹⁰ → 5p⁶ → 6s² → 4f¹⁴ → 5d¹⁰ → 6p⁶ → 7s² → 5f¹⁴ → 6d¹⁰ → 7p⁶
Note: This is the Aufbau (building-up) sequence. Follow diagonal rule visually. Superscripts show maximum electrons per orbital.
Aufbau Principle: Electrons fill orbitals from lowest to highest energy systematically.
Pauli Exclusion Principle: No two electrons can have identical quantum numbers.
Hund's Rule: Electrons occupy empty orbitals before pairing up.
Orbital: Region of space where electrons have high probability of existing.
Quantum Number: Values describing electron energy and position properties.
Electron Spin: Intrinsic angular momentum of electrons (up or down).
Electronegativity: Element's tendency to attract bonding electrons.
Diamagnetic: Material not attracted to magnetic fields weakly.
Hydrogen (H) has one electron total. Its configuration is 1s¹. Try entering atomic number 1.
Carbon (C) has six electrons total. Its configuration is 1s² 2s² 2p². Try entering atomic number 6.
Iron (Fe) has twenty-six electrons total. Its configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁶. Try atomic number 26.
Chromium (Cr) has special electron configuration arrangement. It's 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ 4s¹ instead. Half-filled d orbitals provide stability.
Copper (Cu) also shows configuration exceptions. Its configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s¹. Filled d-orbitals enhance stability greatly.
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