IndiumElectron Configuration, Bohr Model, Valence Electrons & Orbital Diagram

The electron configuration of Indium is written as <strong>1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p¹</strong>. Applying the Aufbau principle — filling orbitals from lowest to highest energy — plus the Pauli Exclusion Principle and Hund's Rule, we systematically place all 49 electrons: 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p¹. The p-subshell adds three dumbbell-shaped orbitals (p_x, p_y, p_z) that collectively hold up to 6 electrons. In Indium, these outermost p-orbitals are the seat of its chemical personality — partially filled, enabling versatile bond formation.

Indium follows the standard Aufbau filling order without exception. The noble gas shorthand <strong>[Kr] 4d¹⁰ 5s² 5p¹</strong> replaces the inner-shell electrons with the symbol of the preceding noble gas, highlighting that only the outer electrons — 4d¹⁰ 5s² 5p¹ — 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, Indium's 49 electrons are distributed as: K-shell (n=1): <strong>2</strong> electrons; L-shell (n=2): <strong>8</strong> electrons; M-shell (n=3): <strong>18</strong> electrons; N-shell (n=4): <strong>18</strong> electrons; O-shell (n=5): <strong>3</strong> electrons. The O-shell (n=5) is the valence shell, containing 3 electrons.

Chemically, this configuration places Indium in Group 13 with oxidation states of 3. This configuration directly predicts Indium's bonding mode, reactivity toward oxidizing and reducing agents, and the stoichiometry of its most common compounds.

The SPDF orbital model describes Indium'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. Indium's 49 electrons occupy 11 distinct subshells: <strong>1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p¹</strong>, governed by three quantum mechanical rules.

<strong>The Pauli Exclusion Principle</strong> ensures no two electrons in Indium 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 49 electrons would collapse into the 1s orbital. <strong>Hund's Rule of Maximum Multiplicity is critical in Indium'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 Indium's distribution of electrons across separate p-orbitals.</strong>

Following standard orbital filling, Indium 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 <strong>5p¹</strong> subshell, making Indium a p-block element with 3 valence electrons in Group 13.

The outermost electrons — <strong>5p¹</strong> — are Indium's chemical agents. Understanding the 5p¹ occupancy — how many electrons, whether paired or unpaired, the orbital shape involved — is the foundation for predicting Indium's bonding geometry, oxidation behavior, and compound formation.

Indium's chemical reactivity is shaped by three interlocking properties: electronegativity (1.78 Pauling), first ionization energy (5.786 eV), and electron affinity (0.404 eV). Its electronegativity is low-to-moderate (1.78) — predominantly metallic character, electropositive tendency. This mid-scale electronegativity enables Indium to participate in both polar covalent and ionic bonding depending on its partner.

The first ionization energy of 5.786 eV is relatively low, confirming Indium's readiness to lose electrons — a quintessentially metallic trait. The electron affinity of 0.404 eV represents the energy released when Indium gains one electron, indicating a meaningful but moderate acceptance of electrons.

In standard chemical conditions, Indium forms predominantly +3 oxidation state compounds, consistent with its 3 valence electrons and p-block character.

Placing Indium between Cadmium (Z=48) and Tin (Z=50) reveals the incremental property changes that make the periodic table a predictive tool.

Cadmium → Indium: adding one proton and one electron increases nuclear charge by 1. Valence electrons shift from 12 to 3 (Group 12 → Group 13). Electronegativity: 1.69 → 1.78 | Ionization energy: 8.994 → 5.786 eV. Atomic radius decreases from 161 pm to 156 pm, consistent with increasing nuclear pull across a period.

Indium → Tin: the additional proton and electron in Tin changes the valence electron count from 3 to 4, crossing from Group 13 to Group 14. Both elements share Post-Transition Metal character, with Tin exhibiting slightly higher electronegativity. These comparisons confirm that Indium sits at a well-defined chemical inflection point in the periodic table.