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Chapter 6: Problem 86

Why does the density of water increase when it is cooled from \(6^{\circ} \mathrm{C}\) to \(4^{\circ} \mathrm{C}\) but then increase when it is cooled from \(4^{\circ} \mathrm{C}\) to \(2^{\circ} \mathrm{C} ?\)

Short Answer

Expert verified
Explain the role of the molecular structure and hydrogen bonds in these changes. Answer: When water is cooled from 6掳C to 4掳C, its density increases due to the hydrogen bonds forming and holding the water molecules closer together, creating a more ordered structure. However, when water is cooled from 4掳C to 2掳C, its density decreases as the water molecules form an open hexagonal structure, taking up more space and resulting in a lower density. The unique molecular structure and hydrogen bonding behavior in water is responsible for these changes in density.

Step by step solution

01

Discuss the molecular structure of water

Water is a polar molecule, which means that it has a positive and a negative end. The oxygen atom has a slightly negative charge, while the two hydrogen atoms have slightly positive charges. As a result, water molecules can form hydrogen bonds with other water molecules.
02

Define density and its relation to temperature

Density is defined as mass per unit volume. In general, when substances are heated, they expand and their density decreases. The same holds for a substance when it is cooled, it contracts and its density increases. However, water exhibits an unusual behavior due to the interaction between hydrogen bonds and the molecular structure of water.
03

Explain the density anomaly of water between 4掳C and 6掳C

When water is cooled from 6掳C to 4掳C, its density increases. This is because the hydrogen bonds between the water molecules are able to form and hold the molecules closer together. The water molecules are arranged in a more ordered structure at 4掳C, which results in a lower volume and thus a higher density.Shown in latex terms, it means \(蟻_{6^\circ C} < 蟻_{4^\circ C}\).
04

Explain the density anomaly of water between 2掳C and 4掳C

When water is cooled further, from 4掳C to 2掳C, its density starts to decrease. This is due to the formation of a more open hexagonal structure in water as it gets closer to freezing. The open structure of ice takes up more space than the liquid water, which leads to a decrease in density as the temperature continues to decrease. Therefore, \(蟻_{4^\circ C} > 蟻_{2^\circ C}\).
05

Conclusion

In conclusion, the density of water increases when it is cooled from 6掳C to 4掳C, but then decreases when it is cooled from 4掳C to 2掳C due to the unique molecular structure and the behavior of hydrogen bonds. As water is cooled from 6掳C to 4掳C, the hydrogen bonds cause the water molecules to be held closer together, resulting in a higher density. When water is further cooled from 4掳C to 2掳C, the formation of an open hexagonal structure causes the density to decrease as the volume increases.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Hydrogen Bonding
Water is unique in its ability to form hydrogen bonds. Each water molecule can connect with up to four other water molecules through strong hydrogen bonds. These bonds occur due to the polar nature of water.
The oxygen atom in the molecule is slightly negative, while the hydrogen atoms are slightly positive. This allows them to attract each other like tiny magnets, creating a network of connected water molecules.
  • Hydrogen bonds give water its cohesive and adhesive properties.
  • These bonds are responsible for the high boiling point of water compared to other molecules of similar size.
  • They significantly influence water's behavior as the temperature changes.
Without hydrogen bonding, water wouldn't have its unique characteristics, including its role in temperature and density variations.
Molecular Structure of Water
Water's molecular structure is at the core of its density anomaly. A water molecule, or H鈧侽, is shaped like a V with an angle of about 104.5 degrees. This bent shape contributes to the polarity of the molecule.
  • In liquid water, this polar molecule structure allows the molecules to pack closely.
  • When cooler temperatures limit the molecular motion, hydrogen bonds arrange the water molecules in a more orderly manner.
At 4掳C, water molecules are densely packed due to optimal hydrogen bonding. As temperature decreases further, these structures shift towards a hexagonal form that occupies more space. Understanding the molecular structure of water helps in grasping why water behaves unusually when cooled below 4掳C.
Temperature and Density Relationship
The relationship between temperature and density is inversely straightforward for most materials: as temperature decreases, density typically increases. However, water defies this rule within a narrow range.
From 6掳C down to 4掳C, water behaves as expected: it becomes denser due to decreased kinetic energy, which allows hydrogen bonds to hold molecules closer. But, from 4掳C to 2掳C, the formation of an open hexagonal structure as ice approaches causes water's density to decrease.
  • Between 6掳C and 4掳C: Hydrogen bonds pull molecules closer, increasing density.
  • Between 4掳C and 2掳C: Open hexagonal structures start forming, decreasing density.
This peculiar behavior results in water reaching its maximum density at 4掳C, which is crucial for aquatic life and environmental sciences.

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Most popular questions from this chapter

Which of the following molecules can hydrogen-bond with molecules of water? (a) methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right) ;\) (b) ethane \(\left(\mathrm{CH}_{3} \mathrm{CH}_{3}\right) ;(\mathrm{c})\) dimethyl ether \(\left(\mathrm{CH}_{3} \mathrm{OCH}_{3}\right) ;(\mathrm{d})\) acetic acid \(\left(\mathrm{CH}_{3} \mathrm{COOH}\right)\)

Why are dipole-dipole interactions generally weaker than ion-dipole interactions?

Why are hydrogen bonds considered a special class of dipole-dipole interactions?

Which of the following molecules can hydrogen-bond among themselves in pure samples of bulk material? (a) methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right) ;\) (b) ethane \(\left(\mathrm{CH}_{3} \mathrm{CH}_{3}\right) ;\) (c) dimethyl cther \(\left(\mathrm{CH}_{3} \mathrm{OCH}_{3}\right) ;\) (d) acctic acid \(\left(\mathrm{CH}_{3} \mathrm{COOH}\right)\)

Which of these compounds has the lowest boiling point: (a) \(\mathrm{CH}_{4},\) (b) \(\mathrm{CH}_{3} \mathrm{Cl},(\mathrm{c}) \mathrm{CH}_{2} \mathrm{Cl}_{2},\) (d) \(\mathrm{CHCl}_{3},\) (e) \(\mathrm{CCl}_{4}.\)
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