AP Ch 10 Liquids and Solids.notebook

1

November 22, 2016

Mar 20­11:22 AM

Chapter 14Liquids and Solids

Mar 20­11:24 AM

Did you know?• Water vapor (gas) is 2000x less dense than liquid water.

• Water and ice have very similar densities

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 20­11:29 AM

Water and ice are more alike than water and steam. Why is this?

Mar 20­11:32 AM

13.1 Target: I can explain why water is so unique and valuable for life

­ the human body is 65% water

­ water is resistant to heating and cooling so it helps regulate body temperatures

­ it can dissolve many substances such as vitamins and nutrients

­ expands as it freezes so it floats on water protecting aquatic life below

See handout for explanations

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 20­1:24 PM

13.4 I can explain the difference between intermolecular and intramolecular forces and can recognize examples of each

Intramolecular forces

er ­ forces between molecules

­ forces within molecules or forces holding ions together3 types: ionic, covalent, metallic

Types: Hydrogen bonding, dipole­dipole, London Dispersion Forces

Feb 28­12:05 PM

Strength of forces

strongest weakestIonic metallic covalent network Hydrogen bonds dipole­ dipole London

dispersion

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 20­1:33 PM

13.6 I can explain the differences between the three types of intermolecular bonds: Hydrogen bonds, Dipole­Dipole Bonds, and London Dispersion Forces

13.7 If given a molecule, I can identify which type of intermolecular

forces it would exhibit

Dipole­Dipole forcesPolar molecules Non polar molecules

hydrogen bonding­ occurs when H is bonded to atoms of O,N or F

London Dispersion forces

London Dispersion forces

Below are the types of intermolecular forces that can exist

only

Mar 20­4:18 PM

Attractions Between Molecules

London dispersion forces­ the weakest of all ( caused by the motion of electrons)­ can occur between polar or nonpolar molecules

When electrons are on one side of the atom, it creates a temporary dipole and can induce a dipole on a nearby atom.

fluctuating dipole in a nonpolar molecule

*only type of attractive forces that can exist between nonpolar molecules

Non polar molecules:

London Dispersion forces become more significant as the sizes of the atoms or molecules increase. Larger size means more electrons available to form dipoles

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 20­4:42 PM

Polar molecules Dipole­Dipole forces­ attractions between negative and positive

ends of polar molecules

Dec 9­1:07 PM

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Feb 28­1:08 PM

What types of intermolecular forces would you expect between molecules of PCl3?

1 London Dispersion2 Dipole­Dipole3 Hydrogen bonding

a) 1 onlyb) 1 and 2c) 1,2 and 3d) 1 and 3e) 2 and 3

Feb 28­1:11 PM

What types of intermolecular forces would you expect between molecules of CO2?1 London Dispersion2 Dipole­Dipole3 Hydrogen bondinga) 1 onlyb) 1 and 2c) 1,2 and 3d) 1 and 3e) 2 and 3

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Feb 28­1:12 PM

What types of intermolecular forces would you expect between molecules of NH3?1 London Dispersion2 Dipole­Dipole3 Hydrogen bondinga) 1 onlyb) 1 and 2c) 1,2 and 3d) 1 and 3e) 2 and 3

Mar 3­9:18 AM

What types of intermolecular forces would you expect between molecules of C2H4?1 London Dispersion2 Dipole­Dipole3 Hydrogen bondinga) 1 onlyb) 1 and 2c) 1,2 and 3d) 1 and 3e) 2 and 3

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 3­9:04 AM

What types of intermolecular forces would you expect between molecules of CH3OH?1 London Dispersion2 Dipole­Dipole3 Hydrogen bondinga) 1 onlyb) 1 and 2c) 1,2 and 3d) 1 and 3e) 2 and 3

Mar 4­11:28 AM

What types of intermolecular forces would you expect between molecules of CH3OH?1 London Dispersion2 Dipole­Dipole3 Hydrogen bondinga) 1 onlyb) 1 and 2c) 1,2 and 3d) 1 and 3e) 2 and 3

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 4­11:13 AM

How many kJ need to be removed in order to freeze 50.0 grams of water at its freezing point? a. 16.7 c. 6.01b. 300.5 d. 40.69

a

specific heatsice = 2.1 J/gCwater=4.18 J/gCsteam=1.84 J/gCHf= 334 J/gHv= 2260 J/g

Mar 4­11:29 AM

What types of intermolecular forces would you expect between molecules of H2S?1 London Dispersion2 Dipole­Dipole3 Hydrogen bondinga) 1 onlyb) 1 and 2c) 1,2 and 3d) 1 and 3e) 2 and 3

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Dec 9­8:22 AM

Dec 9­8:24 AM

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Dec 9­8:25 AM

Dec 9­8:26 AM

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Dec 9­8:29 AM

Dec 9­8:29 AM

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Dec 9­8:30 AM

Dec 9­8:32 AM

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Dec 9­8:33 AM

Mar 27­2:03 PM

MeltingEndothermic

vaporizationEndothermic

freezingExothermic

CondensationExothermic

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 4­8:32 AM

Mar 4­8:39 AM

Energy and Phase Changes

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 4­8:16 AM

Heat of Fusion of Water (Hf = 334 J /g)

Heat of Fusion­the amount of heat required to convert unit mass of a solid into the liquid without a change in temperature. (or released for freezing)

Melting or Freezing

How much energy is required to melt 10.g of ice at its melting point?

Exq = m Hf

Mar 4­8:21 AM

Boiling and CondensingHeat of Vaporization­the amount of heat required to convert unit mass of a liquid into the vapor without a change in temperature.

Heat of Vaporization of Water Hv = 2260 J /g

How much energy is required to vaporize 10.g of water at its boiling point?

How much energy is released when 20. g of steam is condensed at 100oC?

q= m Hv

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 4­9:00 AM

The specific heat of water is 4.18J/gCThe specific heat of ice is 2.1 J/gCThe specific heat of steam is 1.84 J/gC

Recall q=mc t

Mar 4­8:32 AM

How much energy does it take to warm 50 g of water from 20 C to 50 C? (specific heat of water is 4.18J/gC).

Recall q=mc t

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 21­3:22 PM

0

100

q=mc t

q=mc t

q=mc t

heat of fusion

heat of vaporiztion

4.184 (water sp. heat)

1.7(steam sp. heat)

2260 J/g

334 J/g

waterHeating curve for

mHf

mHv

2.1

Mar 4­9:08 AM

Example:

How many Joules of heat are required to heat a 360 g of water from ­5C to steam at 110 C?

Ice from ­5 to 0 melt ice heat from 0 to 100 vaporize heat from 100 to 110

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 4­9:11 AM

Clickers

Mar 4­11:15 AM

How many kJ are required to boil 100. grams of water at its boiling point?a. 226 c. 40.67b. 4067 d. none of the above specific heats

ice = 2.1 J/gCwater=4.18 J/gCsteam=1.84 J/gCHf= 334 J/gHv= 2260 J/g

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 4­11:11 AM

c

How much energy (J) is required to convert a 15.5 g ice cube at ­5.0 C to water vapor at 180 C?a. 56000 c. 49000b. 11000 d. 27000

specific heatsice = 2.1 J/gCwater=4.18 J/gCsteam=1.84 J/gCHf= 334 J/gHv= 2260 J/g

Mar 5­9:08 AM

What type of intermolecular forces are present in FCN?1 London Dispersion2 Dipole­Dipole3 Hydrogen bondinga) 1 onlyb) 1 and 2c) 1,2 and 3d) 1 and 3e) 2 and 3

Would you expect it to have a relatively high or low boiling point?

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 28­12:44 PM

Strength of intermolecular forces influence MP and BP

The key thing to consider here is that boiling points reflect the strength of forces between molecules. The more they stick together, the more energy it will take to blast them into the atmosphere as gases.

The relative strength is in the following order:

Ionic > hydrogen bonding > dipole­dipole > London dispersion forces

Higher BP and MP Lower BP and MP

13.8 I can explain the concepts of evaporation, condensation and vapor pressure and the influence intermolecular forces have on them.

Target 13.7: If given a molecule, I can identify which type of intermolecular bond it would exhibit

Apr 1­8:39 AM

Liquids with high vapor pressures:

• The intermolecular bonds are weak so evaporating rate is very high

What kind intermolecular forces would you expect?

• Probably LDF

The pressure of the vapor present at equilibrium with its liquid is called the vapor pressure of the liquid

Target 13.8: I can explain the concepts of evaporation, condensation, and vapor pressure and the influence intermolecular forces have on them

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Apr 1­8:40 AM

What is another name for a liquid with a high vp?

• A volatile liquid

Examples of volatile liquids:

• Perfumes, gasoline, alcohol

Apr 1­8:41 AM

Liquids with low vapor pressures:

• Intermolecular forces pretty strong, evaporation rate low

What kinds of intermolecular forces would you expect?

• Dipole­dipole and/or Hydrogen bonds

Therefore: the stronger the intermolecular forces, the lower the vapor pressure

The lower the vapor pressure, the higher the boiling point.

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Apr 10­8:04 AM

FCNBH3

CH3Cl

Which has stronger LDF, Ar or H2What happens to BP if you increase the air pressure?

NCl3

What type of forces are present in a substance with low vapor pressure?

What type of forces are present in substances with high vapor pressure? LDF

dipole-dipole

Apr 1­8:52 AM

Examples of non volatile liquids.

• Wax, water, molasses

Ex. 3 Predict which substance in each of the following pairs will show the largest vp at a given temp

A. HOH, CH3OH

Water contains two polar O­H bonds; methanol has only one. Therefore water would have a lower vapor pressure.

B. CH3OH, CH3CH2CH2CH2CHOH

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 10­10:47 AM

Apr 5­8:56 AM

London Dispersion

forces become more

significant as the sizes

of the atoms or

molecules increase.

Larger size means more

electrons available to

form dipoles

Ex.

Which of the following

would you expect to

have a lower melting

point, F2, Cl2, Br2, orI2?

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 5­1:22 PM

Which of the following would you expect to have the highest vapor pressure?A) H2OB) CO2

C) NH3

D) SO2

Mar 5­1:32 PM

State why the normal melting point of ICl (27.2°C) is so much higher than that of Br2 (-7.2°C). a) ICl has hydrogen bonding

b) ICl molecules have a lower molecular weightc) Iodine in ICl is more electronegative than Bromined) ICl molecules are polar

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 5­3:08 PM

.Which of the following will have stronger London Dispersion forces?

a. H2b. Hec. Ned. Kr

Mar 5­3:12 PM

Place the following compounds in order of decreasing strength of intermolecular forces, starting withthe strongest forces.HF O2 NCl3A) O2 > NCl3 > HFB) HF > NCl3 > O2C) NCl3 > O2 > HFD) NCl3 > HF > O2E) HF > O2 > NCl3

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 5­3:19 PM

Place the following substances in order of increasing vapor pressure at a given temperature, startingwith the smallest vapor pressure.NF3 NH3 BCl3

A) NH3 < NF3 < BCl3B) NF3 < NH3 < BCl3C) BCl3 < NH3 < NF3

D) NH3 < BCl3 < NF3

E) BCl3 < NF3 < NH3

Mar 5­3:15 PM

Which of the following would you expect to have the lowest boiling point?

A) HFB) Br2c) NCl3

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 22­9:26 AM

Target 13.9: I can identify and explain the different parts to a Phase Diagram

Demo

NO phase diagrams on AP test

Mar 20­1:31 PM

Let’s say that, for some reason, you want to know what phase of matter a substance will be under some conditions of pressure and temperature. If you want this info, you need a phase diagram.

The lines: Each line that marks the border between two phase changes denotes the conditions under which both phases of matter can stably exist. The normal melting point: The temperature at which the compound melts at a pressure of one atmosphere. In this diagram, the normal melting point is 0 C. The normal boiling point: The temperature at which the compound boils at a pressure of one atmosphere. In this diagram, the normal boiling point is 100 C. Triple point: The conditions of temperature and pressure at which all three phases of matter can stably exist. For water, the triple point is 0.06 atm and 0.01 C, which is why you’ve never seen all three phases of water in equilibrium. Critical point: The conditions of temperature and pressure past which it’s impossible to distinguish between the liquid and gas phase of the material. This occurs because the material has too much energy to stick together (which is true of gases) but is crammed so tightly together that intermolecular forces between the particles are strong. Under these conditions, the material is said to be a supercritical fluid.

Phase Diagrams

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 5­3:25 PM

solid liquid

gas

What is the normal freezing point of the substance?

A) 100 CB) 340 CC) 825 CD) 175 CE) 825 C

Mar 10­7:40 AM

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 5­3:32 PM

solid liquid

gas

What is the normal Boiling point of the substance?

A) 100 CB) 340 CC) 825 CD) 200 CE) 825 C

Mar 22­9:26 AM

What is the normal boiling point?a) 37 C b) ­62 C c)­80 C d) it does not have a normal boiling point

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 5­3:36 PM

Lab­ Triple point

Mar 6­9:02 AM

How much of a grasp do you feel you have on today's target?a) very well, lets move onb) I have a pretty good grasp but need a little more practicec) I am totally clueless

Target 14.9: I can identify and explain the different parts to a Phase Diagram

Scroll up for more clicker practice

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 5­3:34 PM

Scroll up and do more clickers on intermolecular forces

Mar 20­12:44 PM

Target 13.11 I can distinguish between the 4 types of crystalline solids: Ionic, Molecular, Atomic, and Metallic

Many solids are crystalline­ which means they have a regular arrangement

Quartz rock salt pyrite­ FeS2

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November 22, 2016

Mar 20­12:58 PM

can be ionic, molecular or atomic

Mar 20­1:01 PM

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 20­1:09 PM

Ionic solids­ Generally have high melting points ­ held together by strong electrostatic forces

Crystalline solids have different properties because of the types of bonds that hold them together.

Molecular solids ­ Generally have low melting points ­ held together by either London

Dispersion forces if (nonpolar)or

Dipole­dipole forces ( if polar )and/or Hydrogen bonding- if H is bonded to N,O or F

­ form a regular pattern called crystal lattice

Apr 3­1:07 PM

Molecular Solids

S8 molecules P4 moleculesSulfur White phosphorus

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Apr 3­11:10 AM

Atomic SolidsThe properties of atomic solids vary greatly

Example: Diamond (pure carbon) has extremely high M.P. because ­ each carbon atom forms 4 covalent bonds with other carbon

atoms­ the entire crystal is really just one giant carbon molecule Silicon and Boron both bond with themselves to form giant molecules also

Substances like these are called network solids

Network solid ­ the atoms are bonded covalently in a continuous network. In a network solid there are no individual molecules and the entire crystal is the molecule.

Apr 3­11:58 AM

Metal solids

­Difficult to separate metal atoms but easy to slide them past each other

­bonding is strong but nondirectional

In metals, the valence electrons are free to roam through out the entire material forming an "electron sea"

Electron Sea model

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Apr 3­12:09 PM

Alloy­ A mixture of elements with metallic properties

2 TypesSubstitutional alloy

Interstitial alloy

some of host atoms are replaced with atoms of similar size

Some holes between atoms are occupied by much smaller atoms

Ex­ brass ( Cu and Zn)sterling silver ( Ag and Cu )

Ex­ Steel ( Fe and C )

Carbon ­ Iron bonds are directional, which makes the steel stronger and less malleable.The more carbon, the harder the steel

Apr 3­12:51 PM

Ex. 4 Name the type of Crystalline solid formed by each of the following substances:

A. Ammonia

B. Iron

C. Cesium fluoride

D. Argon

E. Sulfur

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Apr 3­11:33 AM

Type of Solid Interaction Properties Examples

Ionic IonicHigh Melting Point, Brittle, Hard

NaCl, MgO

Molecular

Hydrogen Bonding,Dipole­Dipole,London Dispersion

Low Melting Point, Nonconducting

H2, CO2

Metallic Metallic Bonding

Variable Hardness and Melting Point (depending upon strength of metallic bonding), Conducting

Fe, Mg

Network Covalent Bonding

High Melting Point, Hard, Nonconducting

C (diamond),SiO2 (quartz)

Apr 3­11:58 AM

Allotropes different structural modifications of an element

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 5­3:18 PM

Test TuesdayReview Monday

Mar 11­12:34 PM

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 11­1:03 PM

How much heat is needed to change 50 g ice at ­12 C to steam at 100C

Nov 21­10:55 AM

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Nov 21­10:58 AM

Nov 21­11:02 AM

AP Ch 10 Liquids and Solids.notebook

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November 22, 2016

Mar 2­11:09 AM

Go to Solutions chapter 11 smart notebook after this one is finished. Ch 10 and 11 are tested together

Nov 21­10:32 AM