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ANYTHING WITH MASS AND VOLUME

MATTER

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MATTER. ANYTHING WITH MASS AND VOLUME. Classification of Matter. Elements. Pure Substances. Draw this chart!, leave space to define the terms. Compounds. Matter. Homogeneous. Mixtures. Heterogeneous. Mixtures and Pure Substances. - PowerPoint PPT Presentation

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Page 1: MATTER

ANYTHING WITH MASS AND VOLUME

Page 2: MATTER

Matter

Pure Substances

Mixtures

Elements

Compounds

Homogeneous

Heterogeneous

Draw this chart!, Draw this chart!, leave space to leave space to define the termsdefine the terms

Page 3: MATTER

Mixtures and Pure Substances

• A pure substance is made of only one kind of material and has definite properties.

• Matter that consists of two or more substances mixed together but not chemically combined is called a mixture.

Page 4: MATTER

Pure Substances:• Elements are the simplest pure

substance. – Examples: hydrogen, carbon,

and oxygen.

• The smallest particle of an element that has the properties of that element is called an atom.

Page 5: MATTER

Pure substances:• Compounds are pure substances that

are made of more than one element bound together.– Examples: water (H2O), and carbon

dioxide.

A molecule is formed when two or more atoms combine.Example: water (H2O), O2

Page 6: MATTER

MIXTURESHeterogeneous vs. Homogeneous

• Homogeneous matter (solutions): matter that has identical properties throughout. – Examples: Sugar, salt water, and whipped

cream

• Heterogeneous matter: matter that has parts with different properties. – Examples: granite, soil, potpourri

Page 7: MATTER

EXAMPLES

• What type of matter are each of the following… ?

Page 8: MATTER

SAND

Page 9: MATTER

SAND

Heterogeneous mixtureHeterogeneous mixture

Page 10: MATTER

Salt (NaCl)

Page 11: MATTER

Salt (NaCl)

COMPOUNDCOMPOUND

Page 12: MATTER

Air

Page 13: MATTER

Air

• Homogeneous mixture of: Nitrogen, N2 78.08%Oxygen, O2 20.95%Argon, Ar 0.93%Carbon dioxide, CO2 0.033%Neon, Ne 0.0018%Helium, He 0.00052%Methane, CH4 0.0002%Krypton, Kr 0.00011%Nitrogen(I) oxide, N2O 0.00005%Hydrogen, H2 0.00005%Xenon, Xe 0.0000087%Ozone, O3 0.000001%

Many gases make up mixture, Many gases make up mixture, but it looks like it is all one but it looks like it is all one gas.gas.

Page 14: MATTER

Gold

Page 15: MATTER

GoldELEMENT: AuELEMENT: Au

Page 16: MATTER

Bronze

Page 17: MATTER

Bronze

Homogeneous Homogeneous mixturemixture of of copper and tin copper and tin (alloy: mixture (alloy: mixture of metals)of metals)

Page 18: MATTER

Salad Dressing

Page 19: MATTER

Salad Dressing: Heterogeneous

Page 20: MATTER

Conservation• Law of Conservation of Matter

(Mass): matter cannot be created or destroyed.

• Law of Conservation of Energy: Energy cannot be created or destroyed; it may only change from one form to another.

Page 21: MATTER

Matter and energy MUST be conserved; it’s the LAW!

Page 22: MATTER

Virtually everything that is, is made up of atoms.

Page 23: MATTER

From the very large...

Page 24: MATTER

To the very small...

Page 25: MATTER

We are all made of atoms…and only atoms.

This includes you and me!

Page 26: MATTER

Making stuff nature

never dreamed of.

The Elements Song

Currently we have about 115 kinds of atoms. In the natural world there exists 88 different kinds of atoms.

The others have been artificially produced in laboratories.

Page 27: MATTER

We call each kind of atom an element, and give it a specific name and symbol.

Copper Cu

Gold Au

Page 28: MATTER

Periodic Table

Page 29: MATTER

Abundance of the elements,

by weight

Page 30: MATTER

The Earth’s interior is rich in iron

Page 31: MATTER

Sand is made of

Silicon & Oxygen

Page 32: MATTER

The ocean waters are

made of oxygen & hydrogen

Page 33: MATTER

Atoms are made up of protons, neutrons, and electrons.

Protons and neutrons are found in the nucleus of atoms -- roughly at the center

Electrons travel around the nucleus.

Of course real atoms don’t look anything

like this!

Page 34: MATTER

Different kinds of atoms, or elements, are different because they have different numbers of protons.

They don’t look anything like this either!

Page 35: MATTER

We list the elements by their atomic numbers - the number of protons

they have.

Hydrogen, number 1 Helium, number 2

In several cases the atomic weights are in parentheses.  This indicates that these elements have no stable isotopes; that is, they are radioactive.  The value In several cases the atomic weights are in parentheses.  This indicates that these elements have no stable isotopes; that is, they are radioactive.  The value enclosed in parentheses and used for the atomic weight is the atomic mass number of the most stable known isotope, as indicated by the longest half-life. enclosed in parentheses and used for the atomic weight is the atomic mass number of the most stable known isotope, as indicated by the longest half-life.

Page 36: MATTER

Physical Properties• Physical properties: characteristics that

can be observed without changing the identity of the substance.

• Examples: – mass– volume– color – shape – texture– density

Page 37: MATTER

Physical Changes

• Physical change: a change in the physical form or properties of a substance that occurs without a change in composition.

• Examples:– melting– freezing– grinding– dissolving

Page 38: MATTER

Chemical Properties

• Chemical property: describes a substance’s ability to change into a different substance.

• Examples: – flammability– reactivity

Page 39: MATTER

Chemical Changes• Chemical change: occurs

when a substance changes composition by forming one or more new substances. (bonds are broken and bonds are formed)

• Example:– HCl + NaOH NaCl + H2O

Page 40: MATTER

Indications of a Chemical Change…

Flames

Gas is given off (not to be confused with boiling)

Color Change

Page 41: MATTER

Evaporation is a physical change

Page 42: MATTER

Breaking is a physical change.

Page 43: MATTER

Boiling is a change of state, and therefore a

physical change!

Page 44: MATTER

Rusting is a Chemical Change

Page 45: MATTER

Burning is a Chemical Change

Page 46: MATTER

• NOTETAKERS:

• PHASES of MATTER

Page 47: MATTER

Kinetic Theory

• All matter is made of atoms and molecules that act like tiny particles.

• These tiny particles are always in motion. The higher the temp., the faster the particles move.

• At the same temp., more massive (heavier) particles move slower than less massive (lighter) particles.

Page 48: MATTER

SOLIDS

• Definite shape?• YES

• Definite volume?• YES

• Molecules in a solid are tightly packed and constantly vibrating.

Page 49: MATTER

LIQUIDS

• Definite shape?• NO

• Definite volume?• YES

• Some liquids flow more easily than others. The resistance of a liquid to flow is called viscosity. – Honey has a high viscosity compared to water.

Page 50: MATTER

GASES

• Definite shape?• NO

• Definite volume?• NO

• The particles in a gas are spread very far apart, but can be compressed by pumping them into a restricted volume.

Page 51: MATTER

Phase Changes (Changes of State)

• Changes in phase are examples of physical changes.

• Melting: solid liquid• Freezing: liquid solid• Vaporization: liquid gas• Condensation: gas liquid• Sublimation: solid gas• Deposition: gas solid

Page 52: MATTER

Changes of State

GAS

SOLID

Deposition

Sublimation

VaporizationCondensation

Melting

Freezing

LIQUID

Melting

Page 53: MATTER

• ENERGY is the ability to change or move matter.

• Energy is ABSORBED when substances melt or evaporate.– NOTE: our bodies cool down when our sweat

evaporates.

• Energy is RELEASED when substances freeze or condense.

Page 54: MATTER

Melting

• The change of state from solid to liquid.

• Energy (heat) is absorbed by the substance that is melting.

Page 55: MATTER

Freezing• The change of state from liquid to

solid. Opposite of melting. • Energy (heat) is released by the

substance undergoing freezing.

Page 56: MATTER

Evaporation• The change of state at the surface of a liquid as it passes to a vapor.

This results from the random motion of molecules that occasionally escape from the liquid surface.

– Energy (heat) is absorbed by the liquid

– Can happen at any temperature

Page 57: MATTER

Condensation

• The change of state from gas to liquid. The opposite of evaporation.– Energy (heat) is released by the gas to become a liquid.

Page 58: MATTER

Boiling• Change from state from a liquid to a gas.• Occurs throughout the liquid.

– boiling point/temperature is determined by pressure

– Energy (heat) is absorbed by the liquid for it to boil and produce gas.

Page 59: MATTER

*Boiling & freezing points depend on the pressure.*Boiling & freezing points depend on the pressure.

Page 60: MATTER

Water at normal pressure (1 atm):

• For water at normal (every day) pressures:

• Melting/freezing point:

• Condensing/boiling point:

0 oC (32oF)

100 oC (212oF)

Label the points & temperatures on your graph.

Page 61: MATTER

*Boiling & freezing points depend on the pressure.*Boiling & freezing points depend on the pressure.

00°C°C

100°C100°C

Page 62: MATTER

*Boiling & freezing points depend on the pressure.*Boiling & freezing points depend on the pressure.

00°C°C

100°C100°C

Potential Energy = flat lines (stored energy)

Page 63: MATTER

*Boiling & freezing points depend on the pressure.*Boiling & freezing points depend on the pressure.

00°C°C

100°C100°C

Kinetic Energy = slanted lines (energy of motion, temperature is changing)

Page 64: MATTER

Change the pressure Change the Boiling Point

Page 65: MATTER

VIDEO

• Bill Nye: Phase Changes

Page 66: MATTER

Phase Diagrams• a phase diagram shows the equilibria

pressure-temperature relationship among the different phases of a given substance

Page 67: MATTER

Draw Phase Diagrams

Water CO2

Label SOLID, LIQUID, GAS phases

Label points A, B, C, D (show on board)

Page 68: MATTER

triple point = Point ______The point at which all 3 phases of a substance (solid, liquid, gas) can coexist at equilibrium.

critical point = Point ______The combination of critical temperature and critical pressure.

A

C

D

critical temp = temp. above which a gas cannot be liquefied. (H2O=374ºC)

critical pressure = press. required to liquefy a gas at its critical temperature. (H2O=218 atm)

Page 69: MATTER

AB = AC = AD =

C

WATERWATER Carbon DioxideCarbon Dioxide

Page 70: MATTER

AB = AC = AD =

C

meltingcurve

Page 71: MATTER

AB = AC = AD =

C

meltingcurve

sublimationcurve

Page 72: MATTER

AB = AC = AD =

C

meltingcurve

sublimationcurve

vaporpressurecurve

Page 73: MATTER

Activity

• Triple Point of Carbon Dioxide