CHEMISTRY PHYSICAL BEHAVIOR OF MATTER CHEMISTRY Is the study of matter Based upon Composition, Structure and Properties Deals with Reactions.

CHEMISTRYCHEMISTRY

PHYSICAL BEHAVIOR OF MATTER

CHEMISTRYCHEMISTRY

Is the study of matterBased upon Composition, Structure and

Properties Deals with Reactions

Types of ChemistryTypes of Chemistry

Organic – Deals with Carbon compounds (life)


Physical Chemistry – Deals with energy and matter


Inorganic – Deals with non carbon compounds


Biochemistry – Deals with the chemistry of living things

Types of ChemistryTypes of ChemistryAnalytical – The identification of various

substances (labs)

Types of ChemistryTypes of ChemistryNUCLEAR

MATTERMATTER

Anything that has mass and volume. Mass- quantity of Matter

Volume-how much space something takes

up. Weight is a measure of the pull of gravity on

an object.

DENSITYDENSITY

How heavy an object is.Mass per Volume.Density = Mass divided by Volume

LAW of CONSERVATION of LAW of CONSERVATION of MATTER- MATTER-

Matter cannot be created nor destroyed by normal chemical means.

ELEMENT- ELEMENT-

Smallest unit of matter, cannot be decomposed.

The building blocks of matter: Calcium, Hydrogen

111 elements 88 natural

ELEMENTELEMENT

Atoms are the smallest part.

ELEMENTELEMENTArranged in the Periodic Table-

COMPOUND- COMPOUND- Two or more elements chemically combined. Can be decomposed by a chemical change. Elements are in a fixed ratio. Definite

composition. Properties differ from elements that make

them up.

COMPOUNDCOMPOUND

Binary Compound- Two elements that are chemically combined. Sodium chloride.

Ternary Compound- more than two elements.

MOLECULESMOLECULES

Molecules are the smallest part of a compound.

MIXTURE- MIXTURE-

Two or more substances are mixed together, but not chemically.

Substances retain their own properties.Aqueous (aq) are always mixturesNo set ratio-indefinite proportions.

MIXTURE-MIXTURE-

Heterogenious- The concentration is not the same throughout.

Homogenious- Substances are uniformly mixed throughout. Solutions.

PHYSICAL CHANGESPHYSICAL CHANGESPhysical changes-keeps material same

throughout (Cutting, phase change)Deal with Physical Properties: Color,

Melting Point

CHEMICAL CHANGES- CHEMICAL CHANGES-

Chemical changes-makes new substances with new properties.

Can be seen in a substance’s reactions. Combustion, oxidation.

SEPARATION OF SEPARATION OF MIXTURES-MIXTURES-

Chromatography- Separates substances by using their different adhesive forces.

SEPARATION OF SEPARATION OF MIXTURES- MIXTURES-

Distillation- Substances are separated by their different boiling points.

SEPERATION OF SEPERATION OF MIXTURES-MIXTURES-

Filtration- Separates solid

particles by passing through

a filter.

ENERGY- ENERGY-

The ability to do work.

ENERGYENERGY

Energy absorbed in breaking chemical bonds.

Energy released in making of chemical bonds.

Stronger bonds need more energy---- higher mp-bp

ENERGYENERGYPOTENTIAL ENERGY-stored energy

ENERGYENERGYKINETIC ENERGY-energy of motion.

ENERGY- ENERGY-

Exothermic- Energy is given off.

Releases heat. X + Y XY + Heat

condensation- freezing

ENERGY- ENERGY-

Endothermic- Energy is taken in.

XY + Heat -- X + Y

melting, vaporization

LAW of CONSERVATION of LAW of CONSERVATION of ENERGYENERGY

Energy cannot be created nor destroyed.

PHASES OF MATTER-PHASES OF MATTER-

SOLIDS-SOLIDS-

SOLIDS-SOLIDS-

Has a crystalline structure with a definite geometric shape.

Definite shape and volume.Lowest kinetic energy.

SOLIDS-SOLIDS-Glass is not considered a true solid-It is

a Super cooled liquid. So are plastics.Both behave as highly viscous liquid.

SOLIDS-SOLIDS-

Melting-temperature of substance when it changes phases between solids and liquids.

SOLIDS-SOLIDS-

Normal melting point-melting of a solid at standard pressure.

Fusion-change from solid to liquid

STPSTP

Standard Thermal Pressure-Standard Temperature =

0 degrees Celsius

273 Kelvin

STPSTP

Standard Pressure =

101.3 kPa

1 Atmosphere

760 mm Hg

760 Torr

SOLIDS-SOLIDS-

Heat of Fusion- fusion means melting.This is the point where an object exists

as both a solid and a liquid. Heat of Vaporization- Energy required

to vaporize a liquid to a gas.

.

SOLIDS (ADVANCED) SOLIDS (ADVANCED) True Solids form Crystals. Sometimes this crystal has water combined

chemically inside of it. This is a HYDRATE.

SOLIDS (ADVANCED) SOLIDS (ADVANCED) HYDRATE- Crystal containing water inside of it. WATER of HYDRATION- The water inside. ANHYDROUS- Crystals without any water inside.

EFFLORESCENCE- When water of hydration is held very loosely. At room temperature this causes a spontaneous loss of water from the substance. Water leaves and it drys up.

SUBLIMATIONSUBLIMATIONSublimation-changes from a solid to a

gas. Iodine, CO2 ,

Napthalene, Di-ChloroBenzeneThese solids have unusually high vapor

pressures with weak inter-molecular forces.

LIQUIDS-LIQUIDS-

LIQUIDS- LIQUIDS- Definite volume, indefinite shape. Has less kinetic energy than gases.Includes Bromine and Mercury.

LIQUIDSLIQUIDS

Molecules can move about more freely .Take shape of container.

LIQUIDSLIQUIDS

Vapor pressure increases with temperature.

Boiling occurs when vapor pressure = atmospheric pressure.

LIQUIDSLIQUIDS

Vaporization-change from liquid to gas by adding heat.

Phases of MatterPhases of Matter

SOLIDS LIQUIDS GASES

Least space between particles

Most space between particles

Least Kinetic Energy

Most Kinetic Energy

Most Ordered Most Disorder

Strongest Bonds Weakest Bonds

Most Dense Least Dense

Least Movement Most Mol. Movement

PHASE CHANGES-PHASE CHANGES-

HEATING CURVE DIAGRAMHEATING CURVE DIAGRAM

HEATING CURVE DIAGRAMHEATING CURVE DIAGRAM Flat lines are where phase change occurs. Inclines/Declines are just change in

temperatures. Lowest flat line represents Fusion/Freezing. Highest flat line represents

Vaporization/Condensation. Kinetic Energy does not change during the flat

lines. Going up heating curves is endothermic. Going down cooling curves is exothermic.

PHASE CHANGE DIAGRAMPHASE CHANGE DIAGRAM

HEAT ENERGYHEAT ENERGY

Temperature measures average kinetic energy.

JOULES measure heat energy

FARENHEITFARENHEIT

Scale to record temperature that is based on two fixed points-

Freezing Point is the ice-water Equilibrium. Boiling Point is the water-steam Equilibrium. Freezing point = 32

Boiling point = 212Absolute Zero = -459.67

CELSIUSCELSIUS

Most commonly usedDeveloped by Andrew Celsius- 1742Freezing point = 0Boiling point = 100Absolute Zero= -273.15

Lord KelvinLord Kelvin

Proposed the concept of absolute zero.Absolute zero-the lowest possible

temperature where all molecular motion stops.

Everything would be a solid at this point.

KELVINKELVIN

Kelvin scale is based on:– Freezing point= 273.15– Boiling point= 373.15– Absolute Zero= 0

K= C + 273C = K – 273

The Kelvin & the Celsius degrees are equivalent, they are just off by 273 degrees.

1calorie = 4.186 joules

SIG FIGSSIG FIGS

HEAT ENERGY PROBLEMS HEAT ENERGY PROBLEMS

HEAT ENERGY PROBLEMSHEAT ENERGY PROBLEMS

To determine the amount of heat gained or lost when there is a temperature change-

Q = MC ∆T Q = heat in either calories or joules C = specific heat ***water equals 4.18 J/g M = mass of the substance in grams ∆ T = change in temperature


How many Joules are needed to raise the temperature of 60.0 grams of water from 15.0 to 50.0 degrees Celsius?

Q = MC ∆ T

Q = 60.0 x 4.18 x 35.0

Q =


How much heat is needed to raise the temperature of 150.0 grams of water from 25.0 to 65.0 degrees Celsius?


How much water can 250. Joules of heat raise from 30.0 to 40.0 degrees Celsius?


What will be the final temperature when 375 Joules are added to 75.0 grams of water that is at 25.0 degrees Celsius?


How many calories are needed to change 5.0 grams of water from 20.0 to 35.0 degrees celsius?


What will be the new temperature when 209.0 Joules are taken away from 10.0 grams of water which starts at 90.0 degrees Celsius?


To determine the amount of heat lost or gained when there is a phase change-

Q = MHf Q = MHv

Hf = heat of fusion (solid to liquid) 334 J/g Hv = heat of vaporization (liquid to gas) 2260.

Joules/gram


How many Joules are needed to melt 13.0 grams of ice? How about to vaporize it?


Heat of Fusion is also equal to 80. cal/gramHeat of Vaporization is also equal to 540.

cal/gram

Calculate the energy in Calories for the last problem….


Calculate both Joules and Calories needed to vaporize 22 grams of water? Express your answer in KiloJoules and KiloCalories..


Calculate how many Kilo-Joules are needed to fully vaporize 3.0 grams of ice that starts at 273 Kelvin?


Do figure the last problem in calories?

QUIZ (6 points each)QUIZ (6 points each) 150. Joules will raise the temperature of 7.50 grams

of water to what degree Celsius when it starts at 25.0 degrees C? Sig Figs..

How many Joules will be released when 8 grams of water vapor undergoes condensation?

How many more Joules will it take, than Calories, to vaporize 13 grams of water?

750. Joules of Heat will increase how much water from 275 to 300. Kelvin? Sig Figs..

How many KiloJoules will it take to completely vaporize (this occurs at 100 degrees) 5 grams of ice that starts at 0 degrees Celsius? Remember that ice does not normally vaporize!

QUIZ 6 points eachQUIZ 6 points each 120. Joules will raise the temperature of 9.50

grams of water to what degree Celsius when it starts at 25 degrees C? Sig Figs..

How many Joules will be released when 7 grams of water vapor undergoes condensation?

How many more Joules will it take, than Calories, to vaporize 11 grams of water?

650. Joules of Heat will increase how much water from 275 to 300 Kelvin? Sig Figs..

How many KiloJoules will it take to completely vaporize (this occurs at 100 degrees) 4 grams of ice that starts at 0 degrees Celsius? Remember that ice does not normally vaporize!

QUIZQUIZ

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3

2

1

4

7

6

5

B

****Name three substances that normally Sublimate?

TEST

GASESGASESIndefinite shape and volume. Take shape of container.

GASES-GASES-

Particles are very far apart.Highest kinetic energy.

GASESGASESThese are affected by pressure

changes.

GASESGASES

Includes- Noble Gases and H,He, N,O,F,Cl.

Have the highest Entropy- disorder.

GASES-GASES-Much less density than solid and liquid.Gases tend to spread out and flow away

from one another (Diffusion).Diffuse better under conditions of high

temperature and low pressure.Most soluble at low temps & high

pressure

BarometerBarometer

Atmospheric pressure pushes Mercury up the barometric tube.

Average pressure at sea level = 1 atm

= 760 mmHg

= 760 Torr

Invented in the mid 1600’s by Evagelista

Torricelli

MANOMETERSMANOMETERS

Measures gas within a confined container. It is a U-tube containing mercury.

MANOMETERSMANOMETERS

KINETIC-MOLECULAR KINETIC-MOLECULAR MODEL- MODEL-

Gas made of molecules - diatomic.Large spaces in between molecules.Constant random motion-no shape.Molecules display no attraction or

repulsion for one another .

Based on ideal gases


COLLISIONS:


High temperature means high kinetic energy \ more collisions

Molecules move - More collisions means More pressure.

IDEAL GAS- IDEAL GAS-

A gas that conforms exactly to the Kinetic Molecular Theory.

Real gases have attractions and have volume

IDEAL GAS- IDEAL GAS- In reality- There are no ideal gases, only

real.

IDEAL GAS-IDEAL GAS-

Hydrogen & Helium are the closest to being ideal.

The lighter the gas, The more ideal- the quicker it moves.

Most ideal at high Temp and low Pressure

The GAS LAWSThe GAS LAWS

BOYLE’S LAW CHARLES’ LAW GAY-LUSSAC’S LAW COMBINED GAS LAW GRAHAM’S LAW DALTON’S LAW AVOGADRO’S LAW IDEAL GAS LAW

BOYLES LAWBOYLES LAW

Robert Boyle 1662

Relates Pressure

& Volume


If you increase pressure- the volume will decrease.


Volume is in an inverse proportion to pressure.

PV=K

P 1 V 1 = P 2 V 2


Find the new volume when the original volume is 50. ml, and the Pressure changes from 2.0 atm to 4.0 atm?


A 2.0 liter sample of gas exerts a pressure of 2.0 atm. Find the new pressure when the Gas expands to a volume of 16 Liters?


A 24.0 ml sample of gas has a pressure of 100. Kpa. Find the volume at standard pressure?


Find the new volume when 1.20 Liters of a gas goes from 760. Torr to 780. Torr?


A 24. Liter sample of gas has a pressure of 190. Torr. Find the Volume at STP?

CHARLES LAWCHARLES LAW

Jacques Charles (late 1700's)


Volume of gas is in direct proportion to temperature.

If you increase temperature- the volume will too.

Always use Kelvin

V 1 / T 1 = V 2 / T 2


Find the new volume when 200.ml is changed from 100.K to 200.K ?


Find the volume when 30.0 ml of gas goes from 27.0 to 127 degrees Celsius?

JOSEPH GAY-LUSSACJOSEPH GAY-LUSSAC

Developed Gay-Lussac’s Law:There is a direct proportion between

pressure and temperature

P1/T1 = P2/T2

Verified Charles’ LawContributed to hot-air ballooning

COMBINED GAS LAWCOMBINED GAS LAW

Relates all the Gas Law

P 1 V 1 / T 1 = P 2 V 2 / T 2

STP- Standard Thermal Pressure

273 Kelvin, 101.3 kPA 0 Celsius, 1 Atm.

Constants, Kelvin, & STP

GAS LAW PROBLEMSGAS LAW PROBLEMS

At 27C , a pressure of 303.9 kPA, and a volume of 60.0 ml- Find the new volume at STP?


What's the new temperature when 1.0 atm of gas, with a volume of 25 liters , and a temp of 27C is changed to .50 atm and 50. liters?

*** Remember to convert to Kelvin-

Gas Law ProblemGas Law Problem

At constant Temperature, Find the new volume when 5.00 ml of a gas is changed from 300. mmHg to 500. mmHg.


At what temperature in Celsius degrees, would you need to change the volume of Oxygen gas from 24.0 to 50.0 Liters when the pressure goes from 1.0 atm to .40 atm. The starting Temperature is at 27 degrees Celsius?


Find the new volume when 12 Liters of Methane gas at 300.K and 2.0 atm is changed to 400.K under a pressure of 1140 Torr?

GRAHAM’S LAWGRAHAM’S LAW

Diffusion is the spreading of a gas This is also called Effusion. Gases diffuse at a rate inversely proportional

to the square roots of their densities Lighter gases diffuse faster then heavier ones. Graham’s Law is used to calculate rates of

effusion of two gases relative to one another..

Developed by Tom Graham in 1829.


M = Molar MassV or R = Rates of Effusion


Calculate how many times faster Hydrogen will Effuse than Carbon Dioxide?


Calculate how the rates of Effusions of Carbon Tetra-Chloride (CCl4) and of Methane (CH4) compare?


Calculate how the rates of Effusions of Carbon DiOxide (CO2) and of Chlorine gas (Cl2) compare?


Calculate how the rates of Effusions of Helium and of Fluorine gas compare?


Find the mass of gas Q when Carboin Dioxide is 3 times faster than it!

DALTON’S LAW OF DALTON’S LAW OF PARTIAL PRESSURESPARTIAL PRESSURES

Developed by John Dalton in 1805The total pressure of a mixture is equal to

the sum of all of its gases.Pressure total = P1 + P2 + P3……….


Find the Total Pressure in Torr when:Carbon Monoxide has a pressure of 1.5atmChlorine gas has a pressure of 500 mmHgNeon gas has a pressure of 101.3 Kpa Pressure total = P1 + P2 + P3……….


What is the pressure of Argon gas in mmHg when the total pressure is 3 Atms and the other gas has a pressure of 1700 Torr.

DALTON’S LAW OF PARTIAL DALTON’S LAW OF PARTIAL PRESSURESPRESSURES

If the total pressure equals 900 Torr, Find the Partial pressures of both Oxygen and Chlorine gases.

There are 1 mole of Oxygen gas and 4 moles of Chlorine gas.

Gases Over WaterGases Over Water

Some of the water contributes to the total pressure.

You must subtract the partial vapor pressure of the water vapor to find the total pressure.

Total pressure = gas pressure +water vapor pressure

Gases Over Water ProblemGases Over Water Problem

Hydrogen is collected in a 250 ml container over water at 30 degrees Celsius.

H2 over water is really hydrogen + water vapor.Total Pressure = 764.8 torrTotal Pressure = PresH2O + PresH2

Gases Over Water ProblemGases Over Water Problem

Total Pressure = 764.8 torrTotal Pressure = PresH2O + PresH2

Vapor Pressure of water at 30.C = 31.8 torr

At 800 Torr and 303 kelvin, calculate the pressures of:

2 moles of CO2 (g)

3 moles of N2 (g)

****** Please note that they are over water.

AVOGADRO’S LAWAVOGADRO’S LAW

VOLUME is Directly proportional to the number of gas particles

V1/n1 = V2/n2

AMADEO AVOGADRO

AVOGADRO’S HYPOTHESISAVOGADRO’S HYPOTHESIS

Equal volumes of all gases contain equal number of particles.

# of particles of a Liter of Hydrogen equal # of particles of Oxygen.

602000000000000000000000.

AVOGADRO’S NUMBERAVOGADRO’S NUMBER

602000000000000000000000.602000000000000000000000.

A MOLE (n) is a unit used to count particles, molecules, atoms..

23

1 Mole = 6.02 x 10

At STP, one mole of particles occupies a volume of 22.4 Liters

IDEAL GAS LAWIDEAL GAS LAW

IDEAL GAS LAWIDEAL GAS LAW

IDEAL GAS LAW PROBLEMSIDEAL GAS LAW PROBLEMS

.25 moles of an ideal behaving gas will have what volume under .200 atms and a temperature of 600.K

CHEMISTRY PHYSICAL BEHAVIOR OF MATTER CHEMISTRY Is the study of matter Based upon Composition, Structure and Properties Deals with Reactions.

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