BELL RINGER

Explain, in terms of particles and energy, the different states of

matter.

MATTER & ENERGY

MATTER - anything that has mass and volume

ENERGY - the ability to do work

Heterogeneous Mixture

Matter

Can it be physically separated?

NOYES

Mixture

Can it be chemically

decomposed?

Pure Substance

Is the composition

uniform?

Yes No

Homogeneous Mixture

Yes No

Compound Element

BELL RINGER1.What does C6H12O6 (aq) mean?

Time (sec)

Tem

pera

ture

(ºC

)

2. Looking at the graph on the right, characterize each variable as independent or dependent.

Examples·Graphite -

·Pepper-

·Sugar(sucrose)-

·Paint-

· Milk-

element

Homogeneous mixture

compound

mixture

heterogeneous

Ne N2

SO3 Homogeneous Mixture

Practice

Practice

• Are constants about the substance

• Can use our senses to observe them

Physical Properties

Extensive

Intensive

depends on how much material you have

• Physical Changes does not alter the substance

– Can be reversed

A constant, does not matter how much

Chemical Properties· Properties substances adhere

to when they REACT with other substances

· Chemical Changes – · ID by color change, bubbles, heat Δ

· Examples· rust, burning a log, ice pack

ID the following as being intensive, extensive, or chemical properties

__________ The mass of copper wire is 325g.

__________ The boiling point of ethanol is 77.0 °C

__________ Baking soda reacts with vinegar to make CO2(g)

__________ The density of mercury is 13.6 g/ml.

__________ The solubility of sodium chloride in water is 40g/100 ml of water.

· Chemical Changes - Physical vs. Chemical

Mythbusters

Mentos Rocket

Heterogeneous Mixture

Matter

Can it be physically separated?

NOYES

Mixture

Can it be chemically

decomposed?

Pure Substance

Is the composition

uniform?

Yes No

Homogeneous Mixture

Yes No

Compound Element

BELL RINGER

1. Classify each type of mixture.

2. Determine the volume of Fe fillings used to produce mixture 2.

Mixture 1 (100 ml) Mixture 2 (100 ml)

Composition NaCl in H2O Fe fillings in H2O

Observations • Colorless liquid• No visible solid on

the beaker bottom

• Colorless liquid• Black solid on bottom of

beaker

Other Data • Mass of NaCl(s) dissolved = 2.9 g

• Mass of Fe(s) = 15.9g• Density of Fe(s) = 7.87g/cm3

NO, you don’t have to write down the chart

Made of two or more separate compoundsIn chemistry, this is usually a solid and a liquid

A. Types of mixtures

Largest particles

If left alone, particles will settle

Can also filter the mixture to remove particles

2. ColloidSmaller particles, may be invisible

Mixture is not transparentParticles do not settle. Cannot be filtered

Heterogeneous

Heterogeneous

Over 1 µm

Between 0.001 - 1 µm

1. Suspension

3. Solution

Smallest particles

Invisible - solution appears transparent

Particles cannot be filtered Must distill the solution to remove solids

B. Solutions

1. PartsSolute -

Solvent -

Smaller of the two materials – usually solidLarger quantity of the two – usually water or liquid

Solutions are labeled (aq)

CaCl2(aq) Calcium chloride dissolved in water

2. Solubility

How much solute can go into a solvent

Under 0.001 µm

Homogeneous

Tyndall Effect• Used to identify a colloidal solution or a

suspension, light is reflected by the dissolved particles

• Solutions particles are too small

Tyndall Effect

Heterogeneous Mixture

Matter

Can it be physically separated?

NOYES

Mixture

Can it be chemically

decomposed?

Pure Substance

Is the composition

uniform?

Yes No

Homogeneous Mixture

Yes No

Compound Element

suspensionscolloidssolutions

STATES OF MATTER•Solids•Liquids•Gases•Plasma

STATES OF MATTER

Atom MovementWhat happens to an atom when the kinetic energy changes? Click Here

Vibrational

Rotational

Translational

- about an axis, they flip over end to end

- particles are constantly vibrating

- particles move from place to place

STATES OF MATTER

•very low KE - particles can vibrate but not move

•fixed shape & volume

•Do Not conform to the container shape

•Vibrate only

SOLIDS -

STATES OF MATTER• Crystalline solid – arranged in a specific pattern such as diamonds, salt, or ice

• Amorphous solid – no molecular order as found in charcoal, plastics and glass

STATES OF MATTER

• low KE - particles can move around but are still close together

•variable shape but packed closely together

•fixed volume • (incompressible)

• Vibrate & Rotate

LIQUIDS -

STATES OF MATTER

•high KE - particles can separate and move

throughout the container

•Variable shape & volume

•Fluid and Compressible

• Vibrate, Rotate, Translate

GASES -

STATES OF MATTER

•Very high KE - particles collide with enough energy to break into charged particles (+/-)

•variable shape & volume

•Stars, fluorescent light bulbs

PLASMA -

STATES OF MATTER

Very good display of the differences in states of

matter

Animation

HEAT vs. Temperature

Heat- flow of energy from a higher temperature object to a lower temperature object

Temperature- the measure of an object’s average kinetic energy

- the more an object moves, the higher the temperature

Heat Transfer

Endothermic -

Exothermic - Heat given off during a reaction

Heat absorbed during a reaction

ThinkUsing the following graph, draw a line, representing the temperature of a substance as it is heated constantly starting as a solid all the way through to a gas.

Time

Tem

pera

ture

(K

E)

BELL RINGERWhich of the following phase

changes are exothermic?

1. CO2(s) + heat CO2(g)

2. NH3(g) NH3(l) + heat

3. Cu(s) + heat Cu(l)

4. Hg(l) + heat Hg(g)

Just right down the correct choice!

Heating CurveTe

mpe

ratu

re (

KE

)

Time

KE

KE

KE

PHASE

PHASE

Heating CurveTe

mpe

ratu

re (

KE

)

Time

q=mc T

q=mc T

q=mc Tq=mHv

q=mHf m = mass

c = specific heat [4.18]

q = heat loss/gain

Heat Energy ProblemsHow much heat energy, in joules, is absorbed by 24.8 grams of water when it is heated from

21.2ºC to 28.3 ºC? Get the formula from Reference Tables

q = mcΔT

q = 24.8g (4.18J/g•ºC) 7.1ºC

q = 736 J

q = 740J

Heat Energy ProblemsHow much heat energy is absorbed when

11.3g of ice melts to form liquid water at the same temperature?

Get the formula from Reference Tables

q = mHf

q = (11.3 g) (334J/g)

q = 3774.2 J

q = 3770 J

Heat Energy ProblemsIf it takes 273.3 J of energy to condense 19.2 g of a substance, what is the heat of vaporization

of a substance

Get the formula from Reference Tables

q = mHv

273.3J = (19.2 g) (x)

Hv = 14.2 J/g

The temperature of a piece of copper with a mass of 95.4 g increases from 25.0°C to

48.0°C when the metal absorbs 849 J of heat. What is the specific heat of copper?

q = mcΔT

849J =

c = 0.387 J/g•K

BELL RINGER

(95.4 g) (c) (23.0 K )

Cooling Curve Lab

Heat Energy ProblemsHow much heat is absorbed when 70.00 g of

water is completely vaporized at its boiling point?

Get the formula from Reference Tables

q = mHv

q = (70.0 g) (2260J/g)

q = 158200 J

BELL RINGER

What

Cooling Curve for Lauric Acid

0

20

40

60

80

0 2 4 6 8 10

Time (min)

Tem

per

atu

re (

C)

AB C

D

Which line segment represents a phase change only?

What is the melting point of lauric acid?

At which point do the particles of lauric acid have the highest kinetic energy?

What phase change occurs during this 10-minute graph?

Lauric Acid is starting as a

liquid

Just sketch the graph!

Quiz

Heat Problems

Remember: The energy to melt the

ice only comes from the warm water!!!!!!!!!

BELL RINGER

If it takes 22.0 kj of energy to change 43.2 g of a

substance to a liquid, what

is its heat of fusion? 509 Joules/gram

Since the components of a mixture are different substances, with at least some physical properties that are unique to each substance, mixtures can be separated by physical means into their components by techniques such as …

Filtration

Distillation

Decanting

Chromatography

And many others

Separation Techniques

FiltrationIs the process of

removing ‘straining’ a solid, precipitate, from a liquid using a porous paper

Mixture ofsolid andliquid

Stirring rod

Filtrate (liquidcomponentof the mixture)

Filter papertraps solid

Funnel

• For separation of substances in different phases

• Ex – Air filters, coffee filters, fuel filters

• Decanting

• Immiscible liquids – separation by differing densities use a separatory funnel

Filtration

decanting• Pouring a liquid off of a solid

• carefully pouring a solution from a container, leaving the precipitate in the bottom of the container.

• Precipitate – solid formed in a solution during a chemical reaction

decanting

chromatography• Separation of a mixture based upon bonding preferences or size of molecules

• Tie-dye

• Pen ink

• Chlorophyll

• Paternity testing

Separation of MixturesChromatography• separation of

substances based on their attraction for substances not in the mixture

• Gas

• Paper

Distillation

Coolingwater out

Coolingwater in

Run hoseinto sinkConnect hoseto cold watertap

• The separation of a mixture based upon boiling point differences.

• The substance with the lower boiling point will vaporize and re-condense as a purified substance

• Used to purify liquids

• Distilled water

DistillationCoolingwater out

Coolingwater in

Run hoseinto sink

Connect hoseto cold watertap

• separation of substances by their boiling point

• Miscible liquids

• Solutions

• Volatility – measure of the speed at which a

substance evaporates

DistillationFractional Distillation

Distillation

SHAKE TEST

White Board ReviewWhat would be the temperature change if 3.00g of water absorbed 29.2 J of energy?

White Board ReviewAt 1.00 atm of pressure, 25.0 g of a compound at its normal boiling point are converted to a gas by the addition of 34400.J What is the heat of vaporization of this substance?

White Board ReviewIf 122.3 J are added to 32.8 g of water at 30.0°C, what will be the final temperature of water?

White Board Review23422 J of energy was used to change the temperature of 162.8g substance from 13.2°C to 19.4°. What is the specific heat of the substance?

White Board ReviewA 14.3g sample of liquid water at 100.0°C is cooled to solid water at 0.0°C. How much energy was released?

BELL RINGER

Describe how to separate ammonia from hydrogen and nitrogen.

Gas Boiling Point Melting PointSolubility in

Water

Nitrogen -196ºC -210ºC Insoluble

Hydrogen -252ºC -259ºC Insoluble

Ammonia -33ºC -78ºC Soluble

Law of Conservation of Energy

=energy is not created nor destroyed

REMEMBER: Heat energy always travels from the higher temperature to the lower temperature until both

temperatures are the same.

Temperature ScalesTemperature• measures how fast

an object’s molecules are moving = KE

• Different scales have been developed

• Only need two fixed points to develop your own scale

Temperature ConversionsOn Reference Tables

K = °C + 273

A 1.0 °C change = 1.0K change

Some Test Topics:Matter Classification

PE vs. KE (how measured, when changing)

Separation Techniques

Temperature Conversions

Heat Formulas

Phase Changes (aqueous)

Heating/Cooling Curves - interpret

BELL RINGER

How can you tell if a physical change has

occurred?

Separation by Chromatography

samplemixture

a chromatographic column

stationary phaseselectively absorbs

components

mobile phasesweeps sampledown column

detector

http://antoine.frostburg.edu/chem/senese/101/matter/slides/sld006.htm

Separation by Chromatography

samplemixture

a chromatographic column

stationary phaseselectively absorbs

components

mobile phasesweeps sampledown column

detector

http://antoine.frostburg.edu/chem/senese/101/matter/slides/sld006.htm

_________ CurveTe

mpe

ratu

re (

KE

)

Time

Label Everything!

Pure Substances

–contain only ONE kind of atom–Ex - copper gold

Element

Pure Substances• COMPOUND

– composed of 2 or more elements in a fixed ratio

–new properties different from individual elements

The compound has completely different properties than the element

NaClNa

Cl2

Heat (Joules)

BELL RINGER

0 80 240 320 740

-20

0

20

40

60

80

100

120

0 200 400 600 800 1000

Heat (Joules)

Tem

p (C

)

The graph shows the heating curve of 2.0 gram of a solid as it is heated at a constant rate, starting below its melting point. What is the heat of vaporization and along which line on the graph is it measured?

A

BC

DE

Heat Problems

Problem #3 back of sheet

from last class

0 ° C

100 ° C

Analysis By Separation Lab

 

X 100%

Analysis By Separation Lab

Write-Up

1. Procedure – replaces the purpose

2. Safety

3. Data: ALL Data and calculations

4. Questions – answered in complete

sentences

5. Summary

Exam

BELL RINGER

A student has a flask containing two immiscible liquids. One of

the liquids is a solution of a solid in water. Describe how you

would separate the mixture into

its three separate components?

BELL RINGER

If it S

Specific Heat Lab

BELL RINGER

How many phases of matter exist? What are they?

BELL RINGER

How can you tell if a physical change has

occurred?

BELL RINGER

1. What is the freezing point of the substance in the above graph?

2. In a box on your paper, draw at least 9 particles (•) of the substance during the first 3 minutes of heating.

0

20

40

60

80

100

120

0 10 20 30 40

Time (min)

Tem

pera

ture

(C

)Just sketch the graph!

Precision and Accuracy