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CHMA11H3 Chapter Notes - Chapter 11: Coordination Number, Ion, Phase Diagram

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OC20962
18 Jun 2012
School
UTSC
Department
Chemistry
Course
CHMA11H3
Professor
Jamie Donaldson

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CHMA11H3 Full Course Notes
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CHMA11H3 Full Course Notes
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Document Summary

Chapter 11 liquids, solids, and intermolecular forces. 11. 2 solids, liquids, and gases: a molecular comparison. The densities of liquid (0. 998) and solid (0. 917) are greater than the density of gas (5. 90*10-4). This is due to the fact that the molecules of solid and liquid are closely packed together however on the other hand gas molecules have a lot of distance between one another. Water is in gaseous state at 100 c, liquid at 20 c, and solid at 0 c. Thermal energy overcomes the intermolecular forces in liquids and this allows them to more around one another. This is not possible in solids; they are locked in position and are only able to vibrate. Solids and liquids cannot be easily compressed since there is not much space between the particles but in gas since there is a large distance between the molecules it can be compressed.

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Related Questions

What are the main properties of liquids (in contrast to gases and solids)? Check all that apply.

Liquids have an indefinite shape and assume the shape of their container.

Liquids have much higher densities in comparison to gases.

Liquids are not easily compressed.

Liquids have an indefinite shape and do not assume the shape of their container.

Liquids are easily compressed.

Liquids have not a definite volume.

Liquids have a definite volume.

Liquids have lower densities in comparison to gases.

Which statement is true about intermolecular forces ofattraction between molecules?

A) Intermolecular forces affect the ability of particles in theliquid phase escaping into the gaseous phase.

B) There are various types of intermolecular attractions.

C) They tend to stick molecules together.

D) All of the above are true.

Between individual molecules of I2 in the solid state,which type of intermolecular forces would you expect to bedominant?

A) hydrogen bonding

B) ionic forces

C) dipole forces

D) London forces

Which statement is true regarding a liquid in a closedcontainer?

A) Once a particle leaves the liquid, it remains in the gaseousstate.

B) The attraction between the liquid particles prevents any ofthem from escaping into the gaseous state.

C) For every particle that leaves the liquid, another particlein the gaseous state replaces that particle.

D) The vapor pressure above the liquid does not change withtemperature.

Why is the enthalpy of vaporization for water much greater than its enthalpy of fusion? What does this say about the changes in intermolecular forces in going from solid to liquid to vapor? What do we mean when we say that a liquid is highly volatile? Do volatile liquids have large or small vapor pressures at room temperature? What strengths of intermolecular forces occur in highly volatile liquids?