Textbook Question
Contrary to expectation, the addition of more fluorines to ethane lowers the boiling point. Explain this phenomenon.
2. Molecular Representations
Intermolecular Forces
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Hydrogen bonds are important for which of the following reasons?
A
They significantly increase the boiling points of compounds.
B
They are responsible for the color of organic compounds.
C
They are the primary force in ionic bonding.
D
They decrease the solubility of compounds in water.
Verified step by step guidance1
Understand the nature of hydrogen bonds: Hydrogen bonds are a type of dipole-dipole interaction that occurs when a hydrogen atom covalently bonded to a highly electronegative atom, such as oxygen, nitrogen, or fluorine, interacts with another electronegative atom.
Consider the effect of hydrogen bonds on boiling points: Hydrogen bonds increase the boiling points of compounds because they require additional energy to break these interactions during the phase transition from liquid to gas.
Evaluate the role of hydrogen bonds in solubility: Hydrogen bonds generally increase the solubility of compounds in water, as they allow for better interaction with water molecules, which are also capable of hydrogen bonding.
Analyze the relationship between hydrogen bonds and ionic bonding: Hydrogen bonds are not the primary force in ionic bonding. Ionic bonds are formed through the electrostatic attraction between oppositely charged ions, which is a different type of interaction.
Assess the impact of hydrogen bonds on the color of organic compounds: Hydrogen bonds do not directly influence the color of organic compounds. The color is typically related to the presence of conjugated systems and the absorption of specific wavelengths of light.
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