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Chapter 7: Problem 18

Is it incorrect to say that molecules are motionless in the liquid phase? Explain.

Short Answer

Expert verified
It is incorrect to say that molecules are motionless in the liquid phase. Molecules in a liquid have more freedom to move around than in the solid phase, due to weaker and more temporary attractive forces, such as van der Waals forces or hydrogen bonding. Their constant movement includes random motion, vibrations, and rotations, allowing the liquid to flow and take the shape of its container.

Step by step solution

01

Understand the liquid phase characteristics

In the liquid phase, particles (molecules or atoms) are close together but have more freedom to move around than in the solid phase. Molecules in a liquid still experience attractive forces, such as van der Waals forces or hydrogen bonding, but these attractions are weaker and more temporary, allowing for more motion compared to the solid phase.
02

Assess the statement about molecular motion in the liquid phase

Since molecules in a liquid are not as tightly held together as in a solid, they have more freedom to move around each other. This movement is not uniform: it involves random motion, vibrations, and rotations. Therefore, to say that molecules are motionless in the liquid phase is incorrect.
03

Explain why the statement is incorrect

The statement that molecules are motionless in the liquid phase is incorrect because the particles in a liquid are constantly moving. They have enough kinetic energy to overcome some of the attractive forces between molecules, allowing them more freedom in movement compared to the solid phase. Their movement includes random motion, vibrations, and rotations. The motion of molecules in the liquid phase is also what allows the liquid to flow and take the shape of its container. So, it is false to claim that molecules are motionless in the liquid phase.

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Most popular questions from this chapter

Which of the molecules below would not form hydrogen bonds? (a) \(\mathrm{CH}_{3} \mathrm{OH}\) (b) \(\mathrm{CH}_{3} \mathrm{OCH}_{3}\) (c) \(\mathrm{CH}_{3} \mathrm{COOH}\) (d) \(\mathrm{NH}_{3}\) (e) None of these would form hydrogen bonds.

How is it possible for a nonpolar molecule to have a higher boiling point than a polar one?

Predict which compound in each pair will have the higher melting point, and explain why for each pair. (a) HI or KI (b) \(\mathrm{Na}_{2} \mathrm{O}\) or \(\mathrm{H}_{2} \mathrm{O}\) (c) \(\mathrm{CaF}_{2}\) or \(\mathrm{HF}\) (d) \(\mathrm{SiO}_{2}\) or \(\mathrm{CO}_{2}\)

What do we mean by induced dipole when discussing London forces?

Eicosane, \(\mathrm{C}_{20} \mathrm{H}_{42}\), has a higher melting point and a higher boiling point than water, even though water has hydrogen bonds between molecules and eicosane does not. Explain how this can be.
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