RadiumElectron Configuration, Bohr Model, Valence Electrons & Orbital Diagram

The electron configuration of Radium is written as 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p⁶ 4f¹⁴ 5d¹⁰ 6s² 6p⁶ 7s². Applying the Aufbau principle — filling orbitals from lowest to highest energy — plus the Pauli Exclusion Principle and Hund's Rule, we systematically place all 88 electrons: 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p⁶ 4f¹⁴ 5d¹⁰ 6s² 6p⁶ 7s². In the s-block, valence electrons fill spherical s-orbitals (maximum 2 electrons each). Radium's first shell is completely filled, forming a helium-like inert core of 2 electrons.

Radium follows the standard Aufbau filling order without exception. The noble gas shorthand [Rn] 7s² replaces the inner-shell electrons with the symbol of the preceding noble gas, highlighting that only the outer electrons — 7s² — 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, Radium's 88 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): 32 electrons; O-shell (n=5): 18 electrons; P-shell (n=6): 8 electrons; Q-shell (n=7): 2 electrons. The Q-shell (n=7) is the valence shell, containing 2 electrons.

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

The SPDF orbital model describes Radium'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. Radium's 88 electrons occupy 16 distinct subshells: 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p⁶ 4f¹⁴ 5d¹⁰ 6s² 6p⁶ 7s², governed by three quantum mechanical rules.

The Pauli Exclusion Principle ensures no two electrons in Radium 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 88 electrons would collapse into the 1s orbital. For Radium's s-electrons, only two quantum states exist per subshell (spin up ↑ and spin down ↓), so Hund's Rule has minimal impact — both electrons in an s-orbital must pair with opposite spins per the Pauli Exclusion Principle.

Following standard orbital filling, Radium 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 7s² subshell, making Radium a s-block element with 2 valence electrons in Group 2.

The outermost electrons — 7s² — are Radium's chemical agents. Understanding the 7s² occupancy — how many electrons, whether paired or unpaired, the orbital shape involved — is the foundation for predicting Radium's bonding geometry, oxidation behavior, and compound formation.

Radium's chemical reactivity is shaped by three interlocking properties: electronegativity (0.9 Pauling), first ionization energy (5.279 eV), and electron affinity (0.1 eV). Its electronegativity is very low (0.9) — strongly electropositive, a natural electron donor. Radium donates electrons to partners rather than accepting them — the hallmark of electropositive metals.

The first ionization energy of 5.279 eV is relatively low, confirming Radium's readiness to lose electrons — a quintessentially metallic trait. The electron affinity of 0.1 eV represents the energy released when Radium gains one electron, indicating a meaningful but moderate acceptance of electrons.

Radium reacts predictably with water, acids, and nonmetals by surrendering its two valence electrons, forming ionic or moderately polar compounds.

Placing Radium between Francium (Z=87) and Actinium (Z=89) reveals the incremental property changes that make the periodic table a predictive tool.

Francium → Radium: adding one proton and one electron increases nuclear charge by 1. Valence electrons shift from 1 to 2 (Group 1 → Group 2). Electronegativity: 0.7 → 0.9 | Ionization energy: 4.073 → 5.279 eV. Atomic radius decreases from 348 pm to 283 pm, consistent with increasing nuclear pull across a period.

Radium → Actinium: the additional proton and electron in Actinium changes the valence electron count from 2 to 3, crossing from Group 2 to Group 3. This boundary also marks a categorical transition from Alkaline Earth Metal to Actinide. These comparisons confirm that Radium sits at a well-defined chemical inflection point in the periodic table.