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Hydrogen bonding Transitional Reasoning Practice

Chemistry · States of Matter & Solutions · Chemistry · Intermolecular Forces

1 Chemistry practice questions on Hydrogen bonding. Questions that build towards applied reasoning.

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Questions

  1. 1.

    A chemistry student compares two constitutional isomers having the same molecular formula, C2H6O: ethanol (CH3CH2OH) and dimethyl ether (CH3OCH3). Although both compounds have identical molar masses, ethanol is a liquid at room temperature with a boiling point of 78 °C, whereas dimethyl ether is a gas that boils at -24 °C. Based on molecular structure and intermolecular interactions, which statement best explains this significant difference in boiling points?

    • A) Ethanol exhibits much stronger London dispersion forces than dimethyl ether because it has a greater total number of electrons.
    • B) Ethanol molecules form intermolecular hydrogen bonds due to the hydrogen atom covalently bonded to oxygen, requiring more energy to separate them during boiling.
    • C) Dimethyl ether cannot participate in dipole-dipole attractions because its central oxygen atom has no partial negative charge.
    • D) The covalent bonds holding together dimethyl ether molecules are weaker and break more readily upon heating than those in ethanol.

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