SeleniumElectron Configuration, Bohr Model, Valence Electrons & Orbital Diagram

The electron configuration of Selenium is written as 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁴. Applying the Aufbau principle — filling orbitals from lowest to highest energy — plus the Pauli Exclusion Principle and Hund's Rule, we systematically place all 34 electrons: 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁴. The p-subshell adds three dumbbell-shaped orbitals (p_x, p_y, p_z) that collectively hold up to 6 electrons. In Selenium, these outermost p-orbitals are the seat of its chemical personality — more than half-filled, driving electron acceptance.

Selenium follows the standard Aufbau filling order without exception. The noble gas shorthand [Ar] 3d¹⁰ 4s² 4p⁴ replaces the inner-shell electrons with the symbol of the preceding noble gas, highlighting that only the outer electrons — 3d¹⁰ 4s² 4p⁴ — are chemically active. Note: for Period 4+ elements, the 4s orbital fills before 3d per Madelung's rule, even though 3d ends at a lower energy in the final atom.

Shell-by-shell, Selenium's 34 electrons are distributed as: K-shell (n=1): 2 electrons; L-shell (n=2): 8 electrons; M-shell (n=3): 18 electrons; N-shell (n=4): 6 electrons. The N-shell (n=4) is the valence shell, containing 6 electrons.

Chemically, this configuration places Selenium in Group 16 with oxidation states of 6, 4, 2, -2. This configuration directly predicts Selenium's bonding mode, reactivity toward oxidizing and reducing agents, and the stoichiometry of its most common compounds.

The SPDF orbital model describes Selenium's electrons not as planetary orbits but as three-dimensional probability clouds — each orbital a region of space where an electron is most likely to be found. Selenium's 34 electrons occupy 8 distinct subshells: 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁴, governed by three quantum mechanical rules.

The Pauli Exclusion Principle ensures no two electrons in Selenium share the same four quantum numbers (n, l, m_l, m_s). This is why the 1s orbital holds only 2 electrons, the full p-subshell holds 6, d holds 10, and f holds 14. Without this rule, all 34 electrons would collapse into the 1s orbital. Hund's Rule of Maximum Multiplicity is critical in Selenium's p-subshell: the three p-orbitals (p_x, p_y, p_z) must each receive one electron before any pairing occurs. This minimizes electron-electron repulsion and explains Selenium's 3 paired and 0 empty p-orbitals.

Following standard orbital filling, Selenium fills orbitals in the sequence: 1s → 2s → 2p → 3s → 3p → 4s → 3d → 4p → 5s → 4d → 5p → 6s → 4f → 5d → 6p → 7s → 5f → 6d → 7p. The final electron enters the 4p⁴ subshell, making Selenium a p-block element with 6 valence electrons in Group 16.

The outermost electrons — 4p⁴ — are Selenium's chemical agents. Understanding the 4p⁴ occupancy — how many electrons, whether paired or unpaired, the orbital shape involved — is the foundation for predicting Selenium's bonding geometry, oxidation behavior, and compound formation.

Selenium's chemical reactivity is shaped by three interlocking properties: electronegativity (2.55 Pauling), first ionization energy (9.752 eV), and electron affinity (2.021 eV). Its electronegativity is high (2.55) — strongly electronegative, preferring to accept bonding electrons. In bonds with less electronegative partners, Selenium attracts shared electrons toward itself, creating polar or ionic character.

The first ionization energy of 9.752 eV sits in the moderate range, allowing some ionic character in the right partner combinations. The electron affinity of 2.021 eV represents the energy released when Selenium gains one electron, an enormous exothermic release confirming the element's powerful oxidizing nature.

In standard chemical conditions, Selenium forms diverse compounds across multiple oxidation states, consistent with its 6 valence electrons and p-block character.

Placing Selenium between Arsenic (Z=33) and Bromine (Z=35) reveals the incremental property changes that make the periodic table a predictive tool.

Arsenic → Selenium: adding one proton and one electron increases nuclear charge by 1. Valence electrons shift from 5 to 6 (Group 15 → Group 16). Electronegativity: 2.18 → 2.55 | Ionization energy: 9.815 → 9.752 eV. Atomic radius decreases from 114 pm to 103 pm, consistent with increasing nuclear pull across a period.

Selenium → Bromine: the additional proton and electron in Bromine changes the valence electron count from 6 to 7, crossing from Group 16 to Group 17. This boundary also marks a categorical transition from Nonmetal to Halogen. These comparisons confirm that Selenium sits at a well-defined chemical inflection point in the periodic table.