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Chapter 11: Problem 20

True or false: (a) Molecules containing polar bonds must be polar molecules and have dipole-dipole forces. (b) For the halogen gases, the dispersion forces decrease while the boiling points increase as you go down the column in the periodic table. (c) In terms of the total attractive forces for a given substance, the more polar bonds there are in a molecule, the stronger the dipole-dipole interaction. \(\mathbf{d}\) ) All other factors being the same, total attractive forces between linear molecules are greater than those between molecules whose shapes are nearly spherical. (e) The more electronegative the atom, the more polarizable it is.

Short Answer

Expert verified
(a) False: Molecules with polar bonds can still be nonpolar if the overall molecular geometry cancels out the dipoles. (b) False: Dispersion forces and boiling points both increase as you go down the column for halogen gases. (c) True: More polar bonds can result in a larger overall dipole moment and stronger dipole-dipole interactions. (d) True: Linear molecules have greater attractive forces due to their extended surface area. (e) False: More electronegative atoms are generally less polarizable.

Step by step solution

01

a) Molecules containing polar bonds must be polar molecules and have dipole-dipole forces

This statement is false. While it is true that molecules with polar bonds can have dipole-dipole forces, a molecule with polar bonds can still be nonpolar if the overall molecular geometry allows for the dipoles to cancel each other out, resulting in no net dipole moment.
02

b) For the halogen gases, the dispersion forces decrease while the boiling points increase as you go down the column in the periodic table

This statement is false. As you go down the column in the periodic table, the dispersion forces actually increase due to an increase in the number of electrons and a larger electron cloud, which makes the atoms more polarizable. The boiling points of halogen gases also increase as you go down the column, so both dispersion forces and boiling points increase.
03

c) In terms of the total attractive forces for a given substance, the more polar bonds there are in a molecule, the stronger the dipole-dipole interaction

This statement is true. The presence of multiple polar bonds in a molecule can result in a larger overall dipole moment, leading to stronger dipole-dipole interactions between molecules.
04

d) All other factors being the same, total attractive forces between linear molecules are greater than those between molecules whose shapes are nearly spherical

This statement is true. Linear molecules tend to have greater attractive forces due to their extended surface area available for interaction with other molecules. Spherical molecules, on the other hand, have a smaller surface area available for contact and thus smaller total attractive forces.
05

e) The more electronegative the atom, the more polarizable it is

This statement is false. Electronegativity refers to the ability of an atom to attract bonding electrons, while polarizability refers to an atom's susceptibility to distortion by an external electric field. In general, more electronegative atoms are less polarizable, as their electron clouds are held more tightly and are less easily distorted.

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Most popular questions from this chapter

Which type of intermolecular force accounts for each of these differences? (a) Acetone, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{CO},\) boils at $56^{\circ} \mathrm{C} ;\( dimethyl sulfoxide or DMSO, (CH \)\left._{3}\right)_{2}$ SO, boils at \(189^{\circ}\) C. (b) \(\mathrm{CCl}_{4}\) is a liquid at atmospheric pressure and room temperature, whereas \(\mathrm{CH}_{4}\) is a gas under the same conditions. \((\mathbf{c})\) \(\mathrm{H}_{2} \mathrm{O}\) boils at \(100^{\circ} \mathrm{C}\) but \(\mathrm{H}_{2} \mathrm{~S}\) boils at \(-60^{\circ} \mathrm{C}\). (d) 1 -propanol boils at \(97^{\circ} \mathrm{C}\), whereas 2 -propanol boils at \(82.6^{\circ} \mathrm{C}\).

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Freon, \(\mathrm{CCl}_{2} \mathrm{~F}_{2},\) and dichloromethane, \(\mathrm{CH}_{2} \mathrm{Cl}_{2},\) are common organic substances. Freon is a gas with a normal boiling point of \(-29.8^{\circ} \mathrm{C}\); dichloromethane's normal boiling point is \(39.6^{\circ} \mathrm{C}\). Which statement is the best explanation of these data? (a) Dichloromethane can form hydrogen bonds, but freon cannot. (b) Dichloromethane has a larger dipole moment than freon. (c) Freon is more polarizable than dichloromethane.

Based on the type or types of intermolecular forces, predict the substance in each pair that has the higher boiling point: (a) propane \(\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)\) or \(n\) -butane \(\left(\mathrm{C}_{4} \mathrm{H}_{10}\right),(\mathbf{b})\) diethyl ether $\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OCH}_{2} \mathrm{CH}_{3}\right)\( or 1 -butanol \)\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{OH}\right)$ (c) sulfur dioxide \(\left(\mathrm{SO}_{2}\right)\) or sulfur trioxide \(\left(\mathrm{SO}_{3}\right)\), (d) phosgene \(\left(\mathrm{Cl}_{2} \mathrm{CO}\right)\) or formaldehyde \(\left(\mathrm{H}_{2} \mathrm{CO}\right)\). Look up and compare the normal boiling points and nor-

(a) Which type of intermolecular attractive force operates between all molecules? (b) Which type of intermolecular attractive force operates only between polar molecules? (c) Which type of intermolecular attractive force operates only between the hydrogen atom of a polar bond and a nearby small electronegative atom?
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