Feb 10 Warm up – grab a packet from the black cart And Warm up - Get your lab notebook set it up...

Feb 10

• Warm up – grab a packet from the black cart

And

• Warm up - Get your lab notebook set it up for a demo

If you did not take the test or finish the test yesterday see me

Demo # 2 Kinetic Theory

• Introduction to unit 3

• Title = kinetic theory demo

• Question – is the kinetic theory of matter true??

Demo – Kinetic theory

• Main idea – all matter is made up of particles and these particles are always moving to some extent

• Crushing this can without using my hands is an example of this

Unit 3: Properties and States of Matter

Kinetic Theory

• The kinetic theory explains how particles move in different states of matter.

– All matter is composed of small particles (molecules, atoms, and ions).

– The particles are in constant, random motion.– The amount of motion is proportional to the

temperature. Increased temperature means increased motion.

– Solids, liquids and gases differ in the freedom of motion of their particles and the extent to which the particles interact.

Three states of matter

SOLID LIQUID GAS

•Definite Shape

•Definite Volume

•Cannot be compressed

•Cannot flow

•Definite Volume

•Can flow

•No definite Shape

•Cannot be compressed

•No definite Volume

•No definite Shape

•Can flow

•Can be compressed

Plasma

• The new fourth state of matter

• When any matter becomes tooo hot the electrons are stripped / fall off

• This matter shares properties of a gas and a liquid

• Examples - sun

Plasma TV

• Different type of plasma

• Here we have a gas that the electrons are just loose- not bound to any nucleus

• lightning

Kinetic Theory

• Motion in a gasThe constant motion of particles

in a gas allows a gas to fill any container

• Three Main points1. Particles of a gas are in constant, random motion2. The motion of one particle is unaffected by another

unless they collide3. The Forces of attraction among particles can be ignored

• POSITIVE AND NEGATIVE CHARGES

Ex) air freshener

Kinetic Theory

• Motion in a liquid– Particles in a liquid are more closely packed

than particles in a solid• Attractive forces apply

– A Liquid can take the shape of a container because the particles of a liquid can flow to new locations

• The Volume of a liquid is constant because of the attractive forces between particles keep them together

Kinetic Theory

• Motion in a solid– Solids have a definite shape and volume

because particles are in a solid vibrate in a fixed location

ex) People sitting in a theatre or a classroom

Warm-Up – get you lab notebook

• Put this in your lab notebook

• What state of matter has…– 1. Definite shape, definite volume– 2. No definite shape, no definite volume– 3. Definite volume, no definite shape

– Choices – solid, liquid , and gases

Schedule

• Warm up-fast fact

• Phase Changes

• Kinetic theory lab

• Phase change handout – in you packet from yesterday

Fast Fact - What is the origins of Valentines day

• 290 AD – Rome declared the soldiers could not be married

• Secretly went to Bishop Valentine to get married

• Became a saint and his day is Feb 14th

Kinetic theory lab – put this in lab note book

Title – kinetic theory lab

Problem – we need to understand what is a phase change

Data- leave space for a data table

Conclusion – “ answer questions from lab ”

Kinetic Theory Lab

• Remember– Every minute take a reading from the thermometer

– Once the beaker is on the hot plate DO NOT TOUCH IT

– Mark , highlight when the ice has completely turned into water, and when water begins to boil

– Continue to take data until the water has completely boiled for 5 minutes

ExampleData Table in notebook

time (min) temperature (C)

0 1

1 5

2 11

3 12

4 13

5 14

6 15

7 15

After your done with the water

• Build your graph

• Answer the conclusion questions

Honors

• You must write a formal lab on this experiment

Thermal Energy

• Thermal energy is heat. It can also be defined as the sum of the kinetic energy of the particles in a substance. Has to do with temperature and mass.

– Temperature is a measurement of the average kinetic energy of a substance.

• Increases kinetic energy (speed of particles)• Higher Temperature = molecules moving faster

– Solid < Liquid < Gas

Phase Change

• Definition – the reversible physical change that occurs when a substance changes from one state of mater into another

• The temperature does not change during a phase change

• Energy is either stored or released during a phase change

Phase Change Graph

Common Phase changes

• 1. Melting solid -> liquid• 2. Freezing liquid -> solid• 3. Vaporization liquid -> gas , endothermic

• 4. Evaporation liquid -> gas , below boiling point

• 5. Condensation gas - > liquid, cloudy bathroom mirror

• 6. Sublimation solid - > gas, dry ice

• 7. Deposition Gas -> solid, Frost on a window

Freezing / Melting point

• Freezing point– Temperature in which a liquid becomes a

solid• Molecules become more closely packed together• Water – below 0 degrees C

• Melting Point – temperature in which a solid become a liquid– Every solid has a different MP

• Water – Above 0 Celsius• Mercury - -32 C

Boiling Point / Condensation

• Boiling point – Temperature where a liquid becomes a gas

• Water 90-100 degrees C

Surface area – part of water that is exposed

Larger surface area – faster reaction

• Condensation– A Gas cools to become a liquid– Water on a mirror after a shower

Sublimation

• Were a solid changes into a gas

• Dry ice

• Endothermic reaction – need energy

• Dry ice absorbed the heat energy from its environment and transformed straight into a gas

After Lab

• Vocab – now its late

• Phase change handout

• Was in back of packet

• Atomic Model Project is due Monday

Liquid Nitrogen

• Beaker: What is the boiling point?

• Balloons: Do you see the three phases?

• Apples and Bananas: Solids are Brittle

• Placed in a bottle: Can Anyone Explain?

Composition of Matter

Matter

• Anything that has mass and takes up space

• pure substance or mixture

Pure Substance

• A pure substance can not be broken down physically into anything else. –Element–Compound

Element

• Element – on periodic table

• Elements are composed of only one type of atom

• Has one capital letter– Na– Cl– F

• Atom – smallest particle of an element

Compound or Molecule

• Compound – combo of 2 or more elements

• Two or more capital letters– NaCl– H2O– MgO2

– CO2

• Molecule – smallest part of a compound

Pure Substances

• Compound

– properties differ from those of individual elements

– EX: table salt (NaCl)

Pure Substances

• For example…

Two different compounds, each has a definite composition.

Inorganic vs. Organic Compounds

• Inorganic compounds have no Carbon– NaCl, H2O, NH4

• Organic compounds have carbon– C6H12O6 C2H6

Biological Organic Compounds

• Proteins – egg, meat

• Carbohydrates – bread, sugar, pasta

• Lipids – lard, butter, oil

Quick Quiz

On A separate piece of paper answer the following question using your notes

1. What is the difference between the melting phase and the freezing phase?

2. List the qualification of a liquid?3. Write an example of a substance in each phase of

matter?4. What is the difference between an Element and a

compound?5. What is the difference between a organic and inorganic

compound?

Mixtures

• two or more substances that can be physically separated

Heterogeneous Mixtures

• Heterogeneous mixture: See component parts

• Examples

–Granite

–Concrete

–Dry Soup Mix

Homogeneous Mixtures

• Homogeneous mixture: cannot see component parts

• Examples:

–Kool Aid

–Sweet Tea

Mixtures can be…

• Gas in Gas (air) – what we breath

• Gas in Liquid (soda) the carbonation

• Liquid in Liquid (mixed fruit juices)

• Liquid in Solid (Iced Tea) – energy needs to be implied

• Solid in Solid (Concrete, Alloys)

A “microscopic” view

Classifying Matter

1. Classify the following as an element, compound, or mixture (heterogeneous or homogeneous).

• _____ air _____ oxygen• _____ tin can _____ sugar• _____ Windex _____ Salad dressing• _____ sand and sugar _____ gummi bear

2. A white solid is dissolved in water. The resulting colorless, clear liquid is boiled in a beaker until dryness. White crystals remain in the beaker. The liquid can be classified as a(n) ______________.

HO E

E OC

HO HE

HE HO

Homogeneous mixture

-Which box represents an element, a compound and a mixture?

Quiz

Complete Identification and Separation Lab

• Example– Saltwater

Composition

Homo mixture

Type of Mixture

Solid/liquid

Identify each of the items as an element, an inorganic compound, an organicCompound, a homogeneous mixture, or a heterogeneous mixture. If it is a Mixture, tell the type (gas/gas, gas/liquid, etc)

Review Lab

Mixtures can be separated by…

• Dissolving

• Filtering

• Evaporating

• Magnetic Separation

• Chromatography

Unit 6 Quiz

Warm Up

• Please place your formal lab report on the front table.

• What type of substance can be separated using physical means such as evaporating, distilling, filtering, chromatography, or magnetic separation?

– Answer choices: elements, compounds, or mixtures

Review Quiz

• More Practice Identifying Matter

Physical/Chemical Properties Lab

• Label the top of the next full page in your composition notebook with the title above and today’s date (2/21/2008).

• Write the definition for Physical and Chemical properties.

– Physical Properties: Any characteristic of a material that you can observe directly or measure with a tool without changing the composition of the substance. (It does not change chemically)

– Chemical Properties: Any characteristic of a material that indicates whether it can undergo change that will alter the composition of the substance. (It does change chemically)

Make a table like this in your composition notebook to record

your data

Physical/Chemical Properties Lab

• You and your lab partner must go around to each station and identify whether the property being demonstrated is a physical or chemical property and state why.

• boiling point, combustion, freezing/melting point, density, oxidation, solubility, viscosity, conductivity, corrosion, acid or base

These are the properties you have to choose from

Warm-Up

• Please make a list of physical and chemical properties:

Physical Properties (7) Chemical Properties (3)

Boiling pointMelting/freezing pointSolubilityConductivityDensityViscosityAcid or base

OxidationCorrosionCombustion

Physical Property

• Any characteristic of a material that you can observe directly or measure with a tool without changing the composition of the substance. (It does not change chemically)

• Examples: boiling point, freezing/melting point, density, solubility, viscosity, electrical conductivity.

Viscosity

• A fluid’s resistance to flow– High viscosity fluids take longer to pour.– Viscosity may change with temperature.

• Viscosity Demo

Conductivity

• Ability to transmit electrons (electricity)– Conductors vs. insulators

• Metals – good conductors• Non metals – insulators• Some solutions are good conductors that contain

dissolved ions (electrolytes).

Solubility

• Ability to dissolve or be dissolved

• Solubility increased by:

1. Temperature

2. Surface Area

3. Stirring

Density

• Density – the amount of mass of an object related to its volume

• Density = mass (Kg) / volume (cm3)

Complete Density Lab

• When finished let me see your data.

• Once I check your data:

• Work on the density problems on the last page of your packet.

• HW: Density Drill (In your packet) front side only

Review Density Lab

Density Problems

• HW: Lab Report and Density Sheet due tomorrow

Warm-Up

• What is the density of a piece of wood that has a mass of 24.0 grams and a volume of 12.0 cm3?

– What would the density be if the piece of wood were cut in half?

• A  piece of wood that measures 3.0 cm by  6.0 cm by 4.0 cm has a mass of 36.0 grams. What is the density of the wood? Would the piece of wood float in water?  (volume = L x W x H)

• The volume of a solution went from 40 ml to what you see above in a graduated cylinder after putting in a gold ring. If the mass of the gold ring is measured to be 30 grams, what is the density of the gold ring?

Review Density Lab

1 cm3 = 1mL = 1 g

Acids and Bases• Acids

– Form hydrogen (H+) ions in solution

– Low pH ( < 7 )– Sour/tart taste– electrolytes– React with metals to

form H2 gas– Corrosive – tissue

damage/burns – Change color of

indicators– React with bases to

form salt & water

• Bases– Form hydroxide (OH-) ions

in solution– High pH ( > 7 )– Bitter taste– electrolytes– Feel slippery– Often crystalline solids

when undissolved– Corrosive – burns– Change color of indicators– React with acids to form

salt & water

pH

• pH is a measure of the concentration of H+ ions in solution (0-14)– Acids < 7– Neutral = 7– Bases > 7

• pH meter uses electrodes to read electrical conductivity in solution

• pH paper changes color when exposed to acids/bases– match pH paper color to a chart to get pH– Follows ROYGBIV A-B

Litmus

• Litmus paper is another common indicator– Acids turn it red – Bases turn it blue

Common Examples

• Acids– Citric– Lactic– Acetic (vinegar)– Carbonic (carbonated

drinks)– Hydrochloric (HCl –

stomach acid)– Sulfuric, Nitric,

Phosphoric (fertilizers)

• Bases– Ammonia– Clorox– Magnesium Hydroxide

(antacid)– Sodium hydroxide

(soap, oven/drain cleaners)

– Aluminum Hydroxide (antacid, water purification, color-fast fabrics)

LAB: Acids and Bases

Warm Up

• Get started on Acid-Base WS from your packet.– Omit #’s 7, 13, 15 on front and compound B

on the back

Neutralization

• Acids and Bases neutralize each other– Acid + Base Salt + Water

• HCl + NaOH H2O + NaCl

Chemical Property

• Characteristic of a material that indicates whether it can undergo change that will alter the composition of the substance. (It does change chemically)

• Examples: Oxidation, Corrosion, Combustion

Oxidation

• Ability to bind with oxygen during a reaction– Iron rusting

• Iron + Oxygen Iron oxide

2 Fe + O2 2 FeO

Combustibility

• Ability to burn– Cremora Demo

Corrosion

• Ability to break down a metal– Silver Tarnishing

• Silver + Sulfur Silver Sulfide

Ag + S AgS

Decomposition

React/Not react with acids

Warm Up

• Get out practice test and get ready for review.