Despite the fact that XeO_4 has a higher molecular mass than XeO_3, XeO_4 exists

Question

Despite the fact that XeO_4 has a higher molecular mass than XeO_3, XeO_4 exists as a gas at room temperature, where XeO_3 is a solid. Xe is the central atom in both molecules. Why is the boiling point of XeO_3 so much greater? XeO_3 is a polar molecule, but XeO_4 is non-polar. XeO_4 is a polar molecule, but XeO_3 is non-polar. XeO_3 has a lone pair on both Xe and O atoms, but XeO_4 has lone pairs only on O. XeO_4 has more double bonds than XeO_3 Which do you expect to have the highest boiling point? CH_4 H_2Se H_2S PH_3 NH_3

Explanation / Answer

1. Both XeO4 and Xe03 are polar, however Xe03 has more loan pairs, as Both Xe and O has loan, which does intermolecular bonding to make a solid, this is weaker in the case of Xe04 and exist as gas.

2.  NH3 have a smaller mass than PH3, it has a stronger interaction, namely, hydrogen bonds, that are formed in the sequence of N ... H - N where the dots represents the hydrogen bond and the trace represents the covalent bond. That type of interaction does not occur in elements other than F, O and N when hydrogen is present. And this type of interaction is many times stronger than the equivalent ones in other situations where these elements does not occur.

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