A hypothetical element, $M$, from the 9 th period of the periodic table, is discovered to form a stable binary compound with fluorine, MF_n. This compound demonstrates unique magnetic properties and high thermal stability. Given the element's position in the periodic table and its interaction with fluorine, what is the most likely value of $\mathrm{n}$ in MF_n, and what type of chemical bonding predominantly occurs in MF_n? Options: a) $\mathrm{n}=2$, with bonding primarily ionic due to the high electronegativity difference between $M$ and fluorine. b) $n=4$, with a mixture of ionic and covalent bonding, involving the participation of $g$-orbitals in $M$. c) $n=6$, with bonding primarily covalent, involving hybridization of $f, d$, and $p$ orbitals of $M . d$ ) $n=8$, with a unique type of metallic bonding characterized by a delocalized electron cloud involving $f$ and $g$ orbitals of $M$.

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***C*** ∻Key Concept∻ ⚹Valence and Bonding⚹ ∻Explanation∻ ⚹Elements in the 9th period would likely have access to $f$, $d$, and $p$ orbitals for bonding, leading to a high coordination number with fluorine, such as 6, favoring covalent character due to orbital overlap.⚹◊What is the significance of the interaction between the hypothetical element M and fluorine in determining the most likely value of n in the compound MF_n?⍭ Generate me a similar question◊

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