Consider a hypothetical element, $Z$, which has an atomic number of 122 and is located in a newly discovered row of the periodic table. Element $Z$ forms an oxide, ZO_3, which exhibits both ionic and covalent character. The oxide is a solid at room temperature and has a high melting point. In the context of modern chemical theories, which of the following statements is most likely to be true about the bonding and structure of ZO_3? Options: a) ZO_3 has a molecular structure with sp^2 hybridization in Z and forms a lattice similar to silicon dioxide. b) ZO_3 forms a polymeric structure with resonance-stabilized Z-O bonds and has $\mathrm{sp}^{\wedge} 3$ hybridization in Z. c) ZO_3 exhibits a metallic bonding character due to the delocalization of electrons from $Z$ to the oxygen atoms. d) ZO_3 has an ionic lattice with partial covalent character, where $\mathrm{Z}$ exhibits an oxidation state uncommon for its period.

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***B*** ∻Key Concept∻ ⚹Hybridization and Bonding⚹ ∻Explanation∻ ⚹Given the high atomic number of Z, it is likely to have access to d and f orbitals, allowing for expanded octets and complex hybridizations. The description of ZO_3 suggests a polymeric structure with resonance stabilization, which is consistent with $\mathrm{sp}^{3}$ hybridization in Z, as it allows for the formation of multiple bonds with oxygen, leading to a three-dimensional network similar to that found in silica (SiO_2). This structure would account for the high melting point and the solid state at room temperature due to the extensive covalent bonding within the network.⚹◊What is the relationship between the atomic number of an element and its chemical properties, particularly in the context of bonding in compounds like ZO3?⍭ Generate me a similar question◊

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