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Chem 1B > Unit 3: Phases And Phase Changes > Flashcards

Unit 3: Phases And Phase Changes Flashcards

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1
Q

If you put a sample of 100.0g of Water at 25.0 Degrees Celsius and a sample of 100.0g Water at 90 degrees Celsius, which will freeze first?

A

The 100g sample of water at 90 degrees Celsius.

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2
Q

What conditions need to be met for a molecule to be polar?

A

There must be a difference in Electronegativity and arrows leading to a net direction.

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3
Q

Molecules with a net dipole would have _____ IMFs.

A

Stronger

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4
Q

Define London Dispersion Forces

A

IMFs w/ molecules that have no net molecular dipole. Instantaneous temporary dipoles are created; the larger the molecules, the stronger the LDFs (easier for the temporary dipoles to form).

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5
Q

What is the difference between Intramolecular and Intermolecular Forces?

A

Intramolecular is WITHIN

Intermolecular is BETWEEN

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6
Q

Define characteristic of a Gas

A

Molecules far apart and disordered; negligible interactions occur between the molecules.

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7
Q

Define characteristics of Liquids

A

Intermediate Situation

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8
Q

Define characteristics of Solids

A

Molecules are close together and ordered; strong interactions occur between the molecules.

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9
Q

Increase in temperature implies that there is an increase in _____.

A

Heat Energy

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10
Q

What happens in Melting/Freezing?

A

Melting is Solid to Liquid and Freezing is Liquid to Solid.

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11
Q

What happens in Boiling/ Condensation?

A

Liquid to Gas is Boiling and Gas to Liquid is Condensation.

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12
Q

What is the difference between Evaporation and Boiling?

A

Evaporation typically occurs at the boiling point; molecules escape the gas phase at lower temperatures.

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13
Q

Define Boiling Point

A

Boiling point is when the vapor pressure is EQUAL TO OR GREATER THAN the atmospheric pressure.

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14
Q

What happens in Sublimation/Deposition?

A

In sublimation, solid goes to gas; in deposition, gas goes to solid.

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15
Q

What is freeze drying?

A

Lowering the pressure (vacuum) with water.

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16
Q

Can you always predict the degree of the boiling point based off the present IMFs?

A

No; the important thing is to be able to recognize trends.

17
Q

Can hydrogen bonds be considered a chemical bond? What can they be considered?

A

No, it’s not a chemical bond; it’s an IMF.

18
Q

A hydrogen bond is an intermolecular force _____ 2 water molecules.

A

Between

19
Q

What happens when the hydrogen bond in water is broken?

A

A physical change occurs.

20
Q

Why does warmer water freeze faster than colder water?

A

In the liquid state, there are more disordered molecules; however, considering the disorder, the water molecules are CLOSER to one another than in solid ice. (the unique structure of solid water requires a larger distance in between molecules).

Warmer water will have more disorder, and more distance between molecules; will be easier to form lattice structure which has more distance between molecules.

21
Q

What are some factors that affect boiling points?

A

IMFs, Polarity, difference in electronegativity.

22
Q

Why does the phase change from liquid to gas require so much more heat than the phase change from solid to liquid?

A

Converting liquid to gas requires the complete breaking of IMFs, whereas converting solid to liquid requires only partial disruption of IMFs.

23
Q

Heat of fusion entails the _____ of IMFs whereas the heat of vaporization entails the _____ of IMFs.

A

Partial Disruption- Complete Disruption

24
Q

Phase Diagrams are a plot of what?

A

Pressure vs. Temperature (T on the x-Axis and P on the Y-Axis)

25
Q

To get water to sublime, pulling a _____ lowers the pressure.

A

Vacuum

26
Q

Why is the negative slope for the Solid/Liquid line in water unique?

A

Because solid H2O is less dense than liquid H2O.

27
Q

Define Supercritical Point

A

High pressure and high temperature state that we call a supercritical fluid; has properties of both liquids and gases (fluid nature w/low viscosity).

28
Q

What does Low Viscosity mean?

A

Means it has a low density, and if you drop something in it, it would pass through very easily.

29
Q

Define Triple Point

A

Combination of temperature and pressure where solid, liquid, and gas co-exist.

30
Q

What is Dry Ice?

A

Solid CO2

31
Q

Define Boiling Point?

A

When the temperature is high enough to allow the vapor pressure to be higher than atmospheric pressure.

32
Q

Define Vapor Pressure

A

The ability of surface molecules to escape that’s related to temperature.

33
Q

What is the relationship between Temperature and Vapor Pressure?

A

Direct

34
Q

What is the relationship between IMFs and Vapor Pressure?

A

Inverse

35
Q

What is the relationship between Vapor Pressure and Boiling Point?

A

Inverse

Chem 1B (6 decks)

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