In a groundbreaking experiment, a synthetic element, $Q$, with an atomic number of 140 , is observed to form a stable diatomic molecule, $Q 2$, under extreme laboratory conditions. This molecule demonstrates unusual bonding characteristics that challenge conventional bonding theories. Considering its high atomic number and the observed stability of Q2, which of the following theoretical models best explains the bonding in Q2? Options: a) Traditional covalent bonding with a modified Lewis structure, incorporating expanded octet theory. b) A unique type of metallic bonding exclusive to superheavy elements, involving a "sea" of delocalized electrons. c) Bonding involving a molecular orbital approach with significant involvement of $g$ and $h$ atomic orbitals. d) lonic bonding with a high degree of covalent character due to the polarization effects of large nuclear charges. Don't use chat gpt.

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***C*** ∻Key Concept∻ ⚹Molecular Orbital Theory with Involvement of g and h Orbitals⚹ ∻Explanation∻ ⚹For an element with such a high atomic number as 140, traditional bonding theories may not suffice due to the involvement of orbitals beyond f (such as g and h). Molecular orbital theory can accommodate these higher orbitals, which likely play a role in the bonding of superheavy elements like Q.⚹◊What are the unique bonding characteristics of the stable diatomic molecule $Q_2$ formed by the synthetic element Q with atomic number 140 under specific laboratory conditions?⍭ Generate me a similar question◊

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