Sana Sehar 
Thorium (Th) with atomic number 90, has the electron configuration [Rn] 6d² 7s². This indicates filled inner shells like radon (Rn), with two additional electrons in the 6d subshell and another two in the outermost 7s subshell.
How to write Orbital Diagram of Polonium? Polonium (Po), with 84 electrons, has a complex configuration: [Xe] 4f¹⁴ 5d¹⁰ 6s² 6p⁴. The key to its unique behavior lies in the outermost 6p subshell. Unlike most elements in its group, Polonium holds four electrons (6p⁴) instead of a full set.
How to write Orbital Diagram of Mercury? Mercury (Hg) packs 80 electrons uniquely. Unlike its group members, it fills its inner 5d subshell completely. Its configuration is [Xe] 4f¹⁴ 5d¹⁰ 6s² -. It fills electrons in inner shells before adding to the outer 6s subshell (6s²). This complete inner shell setup is believed to influence … Read more
How to write Orbital Diagram of Lead? Lead (Pb) possess 82 electrons. Unlike some elements, it fills its inner shells completely ([Xe] 4f¹⁴ 5d¹⁰ 6s². It fill shells in brackets as [Xe]) before adding to the outermost 6p subshell (6p²). This complete inner shell setup influences Lead’s high density and easy shaping (malleability).
How to write Orbital Diagram of Gold? Gold (Au) boasts 79 electrons. Its configuration, [Xe] 4f¹⁴ 5d¹⁰ 6s¹, reveals a twist. It has a full inner shell (5d¹⁰) and a single electron in the outermost shell (6s¹). This unique setup influences Gold’s metallic nature and remarkable resistance to tarnishing.
How to write Orbital Diagram of Bismuth? Bismuth (Bi), with 83 electrons, possesses an intriguing configuration ([Xe] 4f¹⁴ 5d³ 6s²). Unlike its group members, Bismuth hasa filled outermost shell (6s²) alongside partially filled inner orbitals (5d³). This unique arrangement influences Bismuth’s metallic properties and bonding behavior.
Californium (Cf) follows the trend of reactive transuranic elements. Its outer shell isn’t complete, containing electrons in the 5f and 7s subshells ([Rn] 5f¹⁰ 7s²). This partial filling, unlike noble gases with full outer shells, contributes to Californium’s chemical activity.
Americium (Am) joins the club of reactive elements. Its outer shell isn’t full, holding electrons in the 5f and 7s subshells ([Rn] 5f⁷ 7s²). This incomplete configuration, similar to Berkelium and Curium, makes Americium more prone to reactions compared to noble gases.
Curium (Cm) shares Berkelium’s reactive side. Its outer shell lacks a full configuration, with electrons in the 5f, 6d, and 7s subshells. This incompleteness, written as [Rn] 5f⁷ 6d¹ 7s², makes Curium chemically active, unlike the stable noble gases.
Berkelium (Bk) isn’t like the stable noble gases. Its outer shell isn’t full, instead having electrons in the 5f and 7s subshells. This incompleteness is reflected by its electron configuration, [Rn] 5f⁹ 7s², and makes Berkelium more reactive. The bracketed [Rn] represents filled inner shells, similar to Radon (Rn).
