To determine which of the given molecules consists of atoms with stable configurations, we need to consider the valence electron configurations and whether they result in full outer shells for all atoms involved.
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NaCl2 (Sodium dichloride): Sodium (Na) has 1 electron in its outer shell and loses it to become stable (Na+), while chlorine (Cl) needs 1 electron to fill its outer shell (Cl-). However, having 2 Cl atoms for 1 Na atom is not a stable configuration because Na can only provide 1 electron. Thus, NaCl2 is not stable.
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CaBr2 (Calcium bromide): Calcium (Ca) has 2 electrons in its outer shell and loses both to achieve stability (Ca2+), while bromine (Br) needs 1 electron to fill its outer shell (Br-). In CaBr2, each Ca donates 2 electrons to 2 Br atoms, resulting in a stable configuration for both the calcium and the bromine atoms. Thus, CaBr2 is stable.
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PH4 (Phosphonium): Phosphorus (P) typically has 5 valence electrons and can form 4 bonds with hydrogen atoms, but having 4 hydrogen atoms does not provide a stable octet for the phosphorus atom. Therefore, PH4 does not represent a configuration with all stable atoms.
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SiO5 (Silicon pentoxide): Silicon (Si) can form bonds with oxygen atoms, but having 5 oxygen atoms for 1 silicon atom does not yield a stable configuration as oxygen also requires 2 electrons to fill its outer shell. Therefore, SiO5 is not a stable molecule.
Based on this analysis, the only molecule with all atoms having a stable configuration is:
CaBr2 (Calcium bromide).
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