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Transcript of CHEMISTRY PHYSICAL BEHAVIOR OF MATTER CHEMISTRY Is the study of matter Based upon Composition,...
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)
Types of ChemistryTypes of Chemistry
Physical Chemistry – Deals with energy and matter
Types of ChemistryTypes of Chemistry
Inorganic – Deals with non carbon compounds
Types of ChemistryTypes of Chemistry
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
HEAT ENERGY PROBLEMSHEAT ENERGY PROBLEMS
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 =
HEAT ENERGY PROBLEMSHEAT ENERGY PROBLEMS
How much heat is needed to raise the temperature of 150.0 grams of water from 25.0 to 65.0 degrees Celsius?
HEAT ENERGY PROBLEMSHEAT ENERGY PROBLEMS
How much water can 250. Joules of heat raise from 30.0 to 40.0 degrees Celsius?
HEAT ENERGY PROBLEMSHEAT ENERGY PROBLEMS
What will be the final temperature when 375 Joules are added to 75.0 grams of water that is at 25.0 degrees Celsius?
HEAT ENERGY PROBLEMSHEAT ENERGY PROBLEMS
How many calories are needed to change 5.0 grams of water from 20.0 to 35.0 degrees celsius?
HEAT ENERGY PROBLEMSHEAT ENERGY PROBLEMS
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?
HEAT ENERGY PROBLEMSHEAT ENERGY PROBLEMS
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
HEAT ENERGY PROBLEMSHEAT ENERGY PROBLEMS
How many Joules are needed to melt 13.0 grams of ice? How about to vaporize it?
HEAT ENERGY PROBLEMSHEAT ENERGY PROBLEMS
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….
HEAT ENERGY PROBLEMSHEAT ENERGY PROBLEMS
Calculate both Joules and Calories needed to vaporize 22 grams of water? Express your answer in KiloJoules and KiloCalories..
HEAT ENERGY PROBLEMSHEAT ENERGY PROBLEMS
Calculate how many Kilo-Joules are needed to fully vaporize 3.0 grams of ice that starts at 273 Kelvin?
HEAT ENERGY PROBLEMSHEAT ENERGY PROBLEMS
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
llll
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
KINETIC-MOLECULAR KINETIC-MOLECULAR MODEL- MODEL-
COLLISIONS:
KINETIC-MOLECULAR KINETIC-MOLECULAR MODEL- MODEL-
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
BOYLES LAWBOYLES LAW
If you increase pressure- the volume will decrease.
BOYLES LAWBOYLES LAW
Volume is in an inverse proportion to pressure.
PV=K
P 1 V 1 = P 2 V 2
BOYLES LAWBOYLES LAW
Find the new volume when the original volume is 50. ml, and the Pressure changes from 2.0 atm to 4.0 atm?
BOYLES LAWBOYLES LAW
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?
BOYLES LAWBOYLES LAW
A 24.0 ml sample of gas has a pressure of 100. Kpa. Find the volume at standard pressure?
BOYLES LAWBOYLES LAW
Find the new volume when 1.20 Liters of a gas goes from 760. Torr to 780. Torr?
BOYLES LAWBOYLES LAW
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)
CHARLES LAWCHARLES LAW
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
CHARLES LAWCHARLES LAW
Find the new volume when 200.ml is changed from 100.K to 200.K ?
CHARLES LAWCHARLES LAW
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?
GAS LAW PROBLEMSGAS LAW PROBLEMS
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.
GAS LAW PROBLEMSGAS LAW PROBLEMS
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?
GAS LAW PROBLEMSGAS LAW PROBLEMS
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.
GRAHAM’S LAWGRAHAM’S LAW
M = Molar MassV or R = Rates of Effusion
GRAHAM’S LAWGRAHAM’S LAW
Calculate how many times faster Hydrogen will Effuse than Carbon Dioxide?
GRAHAM’S LAWGRAHAM’S LAW
Calculate how the rates of Effusions of Carbon Tetra-Chloride (CCl4) and of Methane (CH4) compare?
GRAHAM’S LAWGRAHAM’S LAW
Calculate how the rates of Effusions of Carbon DiOxide (CO2) and of Chlorine gas (Cl2) compare?
GRAHAM’S LAWGRAHAM’S LAW
Calculate how the rates of Effusions of Helium and of Fluorine gas compare?
GRAHAM’S LAWGRAHAM’S LAW
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……….
DALTON’S LAW OF DALTON’S LAW OF PARTIAL PRESSURESPARTIAL PRESSURES
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……….
DALTON’S LAW OF DALTON’S LAW OF PARTIAL PRESSURESPARTIAL PRESSURES
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