Arrange the following compounds in the increasing order of their boiling points:
Butane, 1-Bromobutane, 1-Iodobutane, 1-Chlorobutane
Ans. To determine the increasing order of boiling points for the given compounds, we need to consider the strength of intermolecular forces present in each compound. Generally, stronger intermolecular forces lead to higher boiling points.
The intermolecular forces in the compounds mentioned arise from London dispersion forces, dipole-dipole interactions, and hydrogen bonding (if applicable).
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Butane (C4H10): Butane is a nonpolar molecule and exhibits only London dispersion forces between its molecules.
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1-Chlorobutane (C4H9Cl): 1-Chlorobutane is polar due to the C-Cl bond and can exhibit dipole-dipole interactions in addition to London dispersion forces.
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1-Bromobutane (C4H9Br): Similar to 1-chlorobutane, 1-bromobutane is also polar and can exhibit dipole-dipole interactions in addition to London dispersion forces.
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1-Iodobutane (C4H9I): 1-Iodobutane is also polar and can exhibit dipole-dipole interactions in addition to London dispersion forces.
Now, considering the strength of intermolecular forces:
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Butane has only London dispersion forces.
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1-Chlorobutane, 1-Bromobutane, and 1-Iodobutane have stronger intermolecular forces due to dipole-dipole interactions in addition to London dispersion forces.
