Are these things matter?

• Your book, your desk, your lunch, the air that you breathe and the water you drink?

• How do you know?

Matter is anything that has mass and volume.1. Mass is the amount of matter an object has.2. Volume is the amount of space an object takes up.

• Question: Will an inflated balloon weigh more, less, or the same as the same balloon deflated?

• Make a hypothesis, then test it. • Obtain the mass of a balloon, then inflate it, and

then obtain the new mass.

Mixtures: contain more than one type of matter and are physically

combined.

• Homogeneous Mixture– (Solution)

• uniform (same) throughout in composition

• Examples: coffee

air (mixture of gases) Alloys like: brass (Cu & Zn)steel (Fe & C)

• Heterogeneous Mixture

• not uniform (different) throughout in composition

• Examples:sand in watertea with ice cubesoil in waterchicken noodle soup

• Homogeneous• When you don’t see

the gas bubbles.

What is soda?Heterogenous or Homogeneous?

• Heterogeneous • When you see the

gas bubbles.

But if asked, say homogeneous!

Separation of MixturesMixtures can be separated by physical

means.

a) Filtration

b) Centrifuge

c) Chromatography

d) Distillation

e) Crystallization

Separate sand and salt?

Pure Substances: contain only one type of matter.

•Compounds – made from more than

one kind of atom– A molecule is the

smallest particle of a compound that retains its properties.

– Compounds cannot be separated by physical means! (only by chemical reactions)

Ex: salt, distilled water, sugar

• Elements– made of only one kind

of atom. – An atom is the

smallest part of an element).

Ex:

Separation of CompoundsCompounds can be separated chemical

means.

Examples:a) Electrolysis of waterwater hydrogen gas and oxygen gas

b) Chemical ReactionsMagnesium + Acid hydrogen gas

Mg + HCl (acid) MgCl2 + H2

So the properties of compounds may be similar or different than the properties of their elements!

Classify MatterElement, Compound, Homogenous mixture, or

Heterogeneous mixture

Boric Acid Solution

Oxygen gas (O2)

Carbon monoxide (CO)

Steel (Carbon, Iron)

Casserole

Homogeneous mixture

Element (molecule)

Compound

Homogeneous mixture

Heterogeneous mixture

Complete the classification chart now.

Skip the classification cards diagram below for now. You will do it later. Its due at end of class

Classify: Type of Matter:

1) charcoal (carbon)

  1) rock garden

  1) chlorine (Cl)

  1) air

Classify each of the following as either:(E) – Element (HomM) – Homogeneous Mixture(C) – Compound (HetM) – Heterogeneous Mixture

E

HetM

E

HomM

Starter

• Classify the following compounds

• Finish the yellow homework (exit ticket)

Classify: Type of Matter:

1) charcoal (carbon)

  1) rock garden

  1) chlorine (Cl)

  1) air

Properties of MatterProperty – a characteristic

Chemical properties: • characteristics of a

substance’s “ability” to change into a different substance.

• Gasoline is combustible and flammable

Physical properties: • characteristics that can

be observed or measured without changing the identity of the substance.

• Gasoline has a distinct odor, it is colorless, and a liquid at room temperature.

Hardness - resistance to scratching.

Elasticity – ability to be stretched or bounce

Which would you rather play “basketball” with?

A) bowling ballB) volleyball

luster – shine

Solubility – ability to dissolve in water

More examples

Brittleness –tendency to shatter

Malleability –be pounded into thin sheets.

Tensile Strength – the tension it can withstand before breaking.

Ductility – be drawn into thin wire.

More examples

Phase Change –change to and from solids, liquids and gasses.

Viscosity –the resistance to flow

Odor – the Smell.

Magnetism – attracted by a magnet.

More examples

Color – the current color.

CombustibilitY & Flammability – capable of catching fire and

burning .

reactivity – ability to react to form a new substance.

pH – measure of acidity.

More examples

How many properties did you come up with?

combustibility

flammability

reactivity

pH (acidity)

Ex: Silver will tarnish because of reactivity

melting point

boiling point

freezing point

viscosity

magnetism

odor

color

solid

liquid

gas

densityhardness luster solubilityelasticity brittleness malleability ductility tensile strength Electricalconductivity

Changes of Matter

Chemical Changes: • A change that does

produce a new substance.

• Usually not reversible.• Ex: Iron rusts forming iron

oxide.

Physical Changes: • A change that does not

produce a new substance.

• Usually reversible.• Ex: Ice melts into water.

How do you know a chemical change has occurred?

Evidence of aChemical Change:

1. Energy (Heat): absorbed energy (endothermic) released energy (exothermic)

• Gas is produced (bubbles) • Solid (precipitate) forms • Odor or color change occurs

New substances are formed

Physical & Chemical Changes

Physical• Plant loses water

through evaporation• Toothpick is broken• Sugar dissolves• Ice cube melts• Food coloring• Copper wire is cut

Chemical• Energy ATP• Match burns• Bike rusts• Gasoline burns• Silver tarnishes• Leaves change color• Food is digested• Acid + Base Salt

Why are these chemical changes?

Tea Party Properties

• In an envelope provided by the teacher are– Physical and Chemical Properties (Orange Cards)– Physical and Chemical Changes (Blue or White

Cards)

• Organize the orange cards into two piles: Physical and Chemical Properties.

Identify the following as a physical property, a chemical property, a physical change, or a chemical change.

Ice melting

Tarnishing in moist air

Silver in color

Conducts electricity

Ability to explode

Recycled aluminum can

Ability to react with acid

Burned the popcorn

Physical change

Chemical change

Physical property

Physical property

Chemical property

Physical change

Chemical property

Chemical change

Do Worksheets

Starter• Quiz today Pick up white and green handout. Pick up returned HW.

• What are each of these? HomM, HetM, Compound or Element?

What are each of these? ChemC, PhysC, ChemP or PhysP?

 1 • tap water (H2O, minerals) 2 • salt water solution 3 • quartz sand (SiO2) 4 • vegetable soup 5 • table salt (NaCl) 6 • sugar (C6H12O6) 7 • hydrochloric acid solution 8 • neon gas (Ne)

1. aluminum is malleable __________2. ability of sodium to react with chlorine__________3. leaf turning red __________4. a pond freezes over__________5. iron rusting __________6. paper being torn __________7. TNT is explosive __________8. acetone is volatile (vaporizes easily)__________

Video: States of Matter

Oobleck

MythBusters

States of MatterPhase Shape Volume Fluidity

Solid Definite Definite Fixed position

Liquid Indefinite Definite Fluid

Gas Indefinite Indefinite Fluid

Plasma – “charged gas”.

Plasma• Plasma is a gas

containing charged particles such as electrons and ions.

• It is the most common state of matter in the universe.

Changes of State

What is meant by “change of state”?

Change of State: a physical change between states of matter.

(Boiling)

• Temperature influences changes of state.

• As temperature increases, the internal energy increases.

• S L GClick Here and run applet

S & L

L & G

1. Phase changes require a gain or loss of Energy.

2. During a phase change, the temperature does NOT change.

3. When can two states coexist? During a phase change.

Temp is

constant

Temp is constant

• Solid: Substance with a definite shape and volume• Liquid: Substance with a definite volume but not a definite

shape• Gas: Substance with no definite volume or shape• Plasma: Substance that is extremely high in energy and is rare

on earth but common in stars

Phase changes in matter are:

• Melting: change from a solid to a liquid• Freezing: change from a liquid to a solid• Vaporization: the change from liquid to gas• Evaporization: vaporization from the surface of a

liquid.• Boiling: vaporization from within as well as from

the surface of a liquid• Condensation: change from a gas to a liquid • Sublimation: change from a solid to a gas• Deposition: change from gas to solid

Real World Experiences!

• How does it feel when you put rubbing alcohol on your skin? Why?

• What happens to “dry ice” when left on the counter? Why?

• What happens to “moth balls” left in storage trunks?

Your skin feels cold because when alcohol evaporates, it absorbs heat energy from your skin.

“Dry ice” (solid carbon dioxide) does not disappear, but it sublimes into a gas.

“Moth balls” (solid napthalene) do not disappear, but it sublimes into a gas. The fumes kill the moths.

Starter

1. In which of these materials do particles have the slowest motion and MOST ordered arrangement?

A. a gas such as nitrogen C. a solid compound such as baking soda

B. a liquid such as salt water D. a mixture such as coke a cola

2. How can scientists separate elements in compounds and in mixtures?

A. By heating them to their gaseous state.

B. By chemical reactions that recombine or rearrange atoms

C. They separate elements in compounds by chemical reactions, and elements in mixtures by physical processes.

D. They separate elements in compounds by physical reactions and elements in mixtures by physical processes.

3. At a Halloween party students observe dry ice at room temperature. The solid sublimes directly to the gas state. This sublimation is accompanied by which change in the carbon dioxide?

A. decrease in volume C. increase in mass

B. decrease in particle number D. increase in particle motion

Pick up green handout. Pick up homework and grades back tables.

Turn in white notes from last class and green demo lab pick up a calculator

Matter is anything that has mass and volume.1. Mass is the amount of matter an object has.2. Volume is the amount of space an object takes up.

• Question: Will an inflated balloon weigh more, less, or the same as the same balloon deflated?

• Make a hypothesis, then test it. • Obtain the mass of a balloon, then inflate it, and

then obtain the new mass.

Mass vs. Weight• Amount of matter• Use a balance• Kg• Doesn’t change

with location

• Pull of gravity• Use a scale• Newton• Does change with

location

Which has more mass?

A) 1 kilogram of feathers

B) 1 kilogram of bricks

They are the same!

1 kg = 1 kg

Which takes up more space?

A) 1 kilogram of feathers

B) 1 kilogram of bricks

The Feathers

Measure matter by finding the density!

Which has the greater density?A) steel bar B) steel paper clip

The density of steel is the same! Size doesn’t matter!

Density of Steel

steel bar

Units for Density

Metric Units:

Solid: g/cm3

Liquid: g/mL

Density of water is 1g/mL (at 4º C)

Memorize This!

• Density of Water: 1.00 g/mL

• Density of Ice: 0.92 g/mL

Which one floats? Why?

Which of the following will float on water?Why is it good to know the density?

All those lessthan 1.0 g/mL

Density helps you identify a substance

Predict the correct “floating order” of the substances as they would appear in the “Density Column”.

Substance Density g/cm3

Copper 8.8

Corn oil 0.925

Corn syrup 1.38

Glycerin 1.26

Mercury 13.6

Plastic 0.93

Rubber 1.34

Tar 1.02

Water 1.00

Wood 0.7

Make your own density column

• Get out your density column handout.

• Get some colored pencils, scissors and glue sticks

• Color and arrange your density columns with the least dense on top and most dense on bottom

• You have 15 minutes

Calculating Density• Obtain mass using a balance.

• Obtain volume by any of these methods.– Ruler: Volume = L x W x H– Graduated cylinder– Water displacement

d

m

v“Magic Circles”

d = m/vm = d x vv = m/d

1) Is the bar really gold or fool’s gold?Find the density of the bar if the mass is 1891.4 g and the dimensions are 3.5 cm by 3.5 cm by 8.0 cm.

• Gold has a density of 19.3 g/cm3

V = L x W x H

D = M/V

1891.4 g / 98 cm3

= 19.3 g/cm3 Yes it’s gold!

d

m

v

D = M/V

16.98 g / 21.5 mL

= 0.79 g/mL It is alcohol!

2) Is this liquid water, alcohol, or kerosene?

Find the density of the liquid if the mass is 16.98 g? Water 1.0 g/mLAlcohol 0.79 g/mLKerosene 0.82 g/mL

• Read the volume

d

m

v

Starter

1. 100 grams of a liquid completely fill a 200 mL bottle. What is the density of the liquid?

2. Mrs Butterworths pancake syrup has a density of 1.5 g/mL. What would be the approximate mass of the syrup in a 500 mL bottle?

3. These 4 liquids are poured into a graduated cylinder. What order would you pour them to keep them separate?

4. The air you breath everyday is what?

A compound, mixture, solution or

element?

Honey 1.48 g/ml

Alcohol 0.79 g/ml

Water 1.00 g/ml

Shampoo 1.06 g/ml

Pick up HW, and yellow handout. Today we finish green. Yellow is HW

3) Is the “Silver Surfer” really made of silver? We obtained a sample with a mass of 262.5 g. Platinum 21.5 g/cm3

Silver 10.5 g/cm3

Tin 7.3 g/cm3

Find the volume by water displacement.

d

m

v

d = m/v

= 262.5 g / 25 cm3

= 10.5 g/cm3 It is Silver!

4) What is the volume in mL of this syrup if it has a density of 0.63 g/mL and a mass of 78 g?

v = m/d= 78g ÷ 0.63 g/mL= 123.8 mL d

m

v

5) What is the mass in grams of this lead pipe if it has a density of 11.4 g/cm3 and a volume of 55 cc?

m = d x v= 11.4 g/cm3 x 55 cc= 627 g

d

m

v

Starter 10/7/13

• Work questions 3 and 4 on the yellow HW problems.

• The quiz will have the same sort of problems.

Boats are made so that they have a lower

density than water.

The upward force exerted on an object immersed in a fluid is called the “buoyant force”.

Click on picture for demo.

Buoyant Force

Draw a vector to show the buoyant force (up) and the weight force (down).

Weight Force (Gravity)

Buoyant Force

Which liquid exerts a greater buoyant force on the block?Blue or Clear?

Blue (greater)Blue (greater)

Why does a block of steel sink, but a steel boat float?

The Titanic Sinks

What two forces are involved?

When will an object sink or float?

Sink• Weight Force >

Buoyant Force

• Density of object > density of fluid

Float• Weight Force <

Buoyant Force

• Density of object < density of fluid

(greater than) (less than)

Archimedes Principle The buoyant force exerted

on an object in a fluid is equal to the weight of the fluid displaced by the object.

It explains: the buoyancy of ships the rise of a balloon in the

air the loss of weight of objects

underwater. 2 N

2 N

buoyancy.html

Sink of Float

Archimedes’ Principle Practice:

• Rock weighs 2.25 N• In water, the rock weighs

1.8 N• The water displaced by

the rock:• 2.25N – 1.8 N = 0.45 N.• So, the buoyant force

exerted on the rock is 0.45 N.

0.45 N

Do all fluids exert the same buoyant force on an object?

Mercury

Which liquid exerts a greater buoyant force?

0.45 N 0.53 N

NO

2.25 N

Buoyant force of stacked liquids?

• If I stacked the liquids which liquid would have the greatest buoyant force on the tar ball?

A.Water

B.Glycerin

C.Corn syrup

D.Mercury

Buoyancy and FluidHow do Submarines work?

Buoyancy and GasesWhy do hot air balloons

float?• A balloon will float

when the weight of the balloon is less than the weight of the volume of air displaced.

• Air in the balloon is heated to make it less dense than the surrounding air.

The beach ball and the basketball each contain the same amount of air.

• Which has the greater amount of pressure and why?

The basketball has greater pressure than the beach ball because it has less volume causing the air particles to have less space.

flows slower?Starter

etchor Molasses?

Why does ketchup flow so slow?Viscosity is the resistance to flow due to:

• Large, bumpy molecules

• Strong attraction between molecules

How does temperature affect viscosity?

• As a liquid gets warmer, its viscosity __________.

• Ex: cold honey vs. warm honey

• As a gas gets warmer, its viscosity ___________.

• Why?

decreasesincreases

Because the number of collisions increase causing friction which slows the molecules down.

Why do companies want you to heat up your syrup before using

it?

• Increase temperature…

• Decrease Viscosity…

• Use more syrup!!

• Buy more syrup!!

Viscosity Lab

• Compare the viscosity of different fluids.

• Observe the effects of temperature on viscosity.

Viscosity