1. Properties and States of Matter

2. Chapter 3 Objectives Describe the two properties of all matter.
Section 1 Properties of Matter
Objectives
Describe the two properties of all matter.
Describe the difference between a pure substance and a mixture.
Define physical properties.
Define chemical properties.
Explain how matter is organized.

3. Chapter 3 What is Matter? Matter has mass and takes up space.
Section 1 Properties of Matter
What is Matter?
Matter has mass and takes up space.
Everything you can see in the universe is matter.
Atoms are the Building Blocks of Matter
All matter is made from particles called atoms.
Atom is the smallest unit of matter that has unique properties.

4. Flow Chart Of Matter MATTER MIXTURE PURE SUBSTANCE HOMOGENEOUS
physical change
PURE SUBSTANCE
HOMOGENEOUS
HETEROGENEOUS
solutions
chemical change
ELEMENT
COMPOUND

5. Chapter 3 Pure Substances
Section 1 Properties of Matter
Pure Substances
A pure substance consists of one type of atom or one type of molecule.
A pure substance may be an element or a compound.
A molecule is not necessarily a compound.

6. Pure Substances, continued
Chapter 3
Section 1 Properties of Matter
Pure Substances, continued
Elements: A Single Type of Atom
Elements cannot be broken down chemically or physically.
An element is a single kind of atom.
There are more than 100 different elements.
Three Major Categories of Elements
Metals
Metalloids
Non-metals

7. Chapter 3
Section 1 Properties of Matter

8. Pure Substances, continued
Chapter 3
Section 1 Properties of Matter
Pure Substances, continued
Molecules & Compounds
A Molecule is two or more atoms joined by chemical bonds
A molecule has a fixed composition
all of its molecules have the same atoms in the same proportion.
A compound is a molecule of two or more different atoms joined by chemical bonds.

9. Chapter 3
Section 1 Properties of Matter

10. Chapter 3 Mixtures A mixture contains two or more pure substances.
Section 1 Properties of Matter
Mixtures
A mixture contains two or more pure substances.
A homogeneous mixture is uniform throughout, such as apple juice.
A heterogeneous mixture is not uniformly mixed, such as salad dressing.
A mixture can be separated with physical methods

11. Chapter 3 Mixtures, continued
Section 1 Properties of Matter
Mixtures, continued
A Solution is a mixture that appears to be a single substance.
The particles are too small to be affected by gravity and do not separate.
Salt water
Many solutions are liquids, but may also be a gas or solid.
air

12. Chapter 3 Mixtures, continued Suspensions
Section 1 Properties of Matter
Mixtures, continued
Suspensions
A mixture where the particles eventually settle out.
May be gas or liquid.
Colloids
A mixture that has particles larger than a solution
Particles do not settle out.
May be solid, liquid, or gas.

13. Identifying Matter with Physical Properties
Chapter 3
Section 1 Properties of Matter
Identifying Matter with Physical Properties
A physical property is a characteristic of a substance that can be observed or measured.
Examples are mass, density, color, hardness, melting point, boiling point.

14. Identifying Matter with Physical Properties, continued
Chapter 3
Section 1 Properties of Matter
Identifying Matter with Physical Properties, continued
Mass and Weight
The amount of matter in an object is called mass.
Mass is constant at any place in the universe, because the amount of matter does not change.

15. Physical States of Matter
Solid
Liquid
Gas
Plasma

16. Solid Particles are tightly compact
Particles vibrate without the ability to move freely
Definite shape and volume
Solid Animation

17. Liquid
Particles are tightly compact, but able to move around close to each other
No definite shape, but definite volume
Liquid Animation

18. Gas Particles can easily spread out or move close together
Particle move freely and with a lot of energy
No definite shape or volume
Gas Simulation

19. Plasma
Why do you think this is the most common form/state of matter in the universe?
Exist at extremely high temperatures (several million degrees Celsius)
Particles are broken apart
Particles move freely and with extremely high energy
This form is not too common on earth, however it is the most common form of matter in the universe
No definite shape or volume?
Examples: Florescent and neon lights, lightning, aurora borealis

20. Energy and the States of Matter
The physical states of matter result from the amount of energy the particles composing the matter have. Basically, more energy means more movement for the particles and less energy means less movement.
Energy/Temperature and Matter
If you were to compare an ice cube and the steam created
from boiling water, which would you think has more energy?

21. Properties of Matter Chemical Property
Any property of matter that describes a substance based on its ability to change into a new substance
Examples
flammability
reactivity with vinegar
reactivity with oxygen
Iron + Oxygen  Iron oxide (rust)
2Fe + 3O2  Fe2O3

22. Chemical or Physical Property?
Paper is white
Boiling point of H2O is 100oC
Zinc reacts with hydrochloric acid and creates hydrogen gas
Nitrogen does not burn
Sulfur smells like rotten eggs
Physical Property
Physical Property
Chemical Property
Chemical Property
Physical Property

23. Comparing Physical and Chemical Properties
Substance/Matter
Physical Property
Chemical Property
Helium
Less dense than air
Nonflammable
Wood
Grainy texture
Flammable
Baking soda
White powder
Reacts with vinegar to produce bubbles
Powdered sugar
Does not react with vinegar
Rubbing alcohol
Clear liquid
Red food coloring
Red color
Reacts with bleach and loses color
Iron
Malleable
Reacts with oxygen

24. Changes in Matter Physical Change
a change in shape, size, color, or state
a change without a change in chemical composition
a change that is reversible
The Mixtures Lab
Examples
tearing paper
cutting your hair
change in state

25. Changes in States (Physical Changes)
Plasma
Plasma
Plasma
Disposition
Vaporization
(Evaporation/Boiling)
Gas
Gas
Gas
Gas
Liquid
Liquid
Liquid
Liquid
Condensation
Melting
Solid
Freezing
Sublimation
All changes in state require a change in energy
All changes in state require a change in energy

26. States of Matter Simulation
This is what happens when energy is added and taken away

27. combining sulfuric acid and sugar
Changes in Matter
Chemical Change
a change in which a substance becomes another substance having different properties
a change that is not reversible using ordinary physical means
Changes that usually cause heat, sound, light, odor, fizzing/foaming, color changes
You usually need more than one of the above characteristics to be considered a chemical change!
Examples
combining sulfuric acid and sugar
burning a piece of wood
soured milk

28. Chemical or Physical Change?
Bending a Paper Clip
Baking a cake
The sublimation of carbon dioxide
Crushing an aluminum can
Vinegar and baking soda combining to create salt and water
Physical Change
Chemical Change
Physical Change
Physical Change
Chemical Change

29. Chapter 3
Section 1 Properties of Matter

30. Chapter 3 Section 2 Objectives Define the law of conservation of mass.
Section 2 Physical and Chemical Changes
Chapter 3
Section 2 Objectives
Define the law of conservation of mass.
Describe the difference between physical and chemical changes.
Explain why some changes are reversible and some are not.

31. Chapter 3 Conservation of Mass
Section 2 Physical and Chemical Changes
Chapter 3
Conservation of Mass
Mass is not created or destroyed in ordinary chemical or physical changes.
In ordinary physical or chemical changes, the amount of matter, which is called mass, does not change.

32. Conservation of Mass Lab
Weigh a clean, dry cup: _________
Add a small amount of vinegar and re-weigh: ____
Amount of Vinegar = (#2 - #1) = ______________
Weigh a 2nd clean, dry cup:_________
Add a small amount of baking soda and re-weigh:_______
Amount of Baking soda = (#5 - #4) = __________
Total Mass of reactants: (#6 + #3) = __________
SLOWLY add the baking soda to the vinegar. If it overflows, you have to start over.
Weigh the resulting mixture and cup: _______
Total Mass of Products (#9 - #1)= ___________
Was Conservation of Mass upheld? Does #10 = #7? Explain why or why not.

33. Physical Changes in Our World
Section 2 Physical and Chemical Changes
Chapter 3
Physical Changes in Our World
A physical change is any change in which the properties of a substance, but not the identity of the substance, change.
The next slide shows the physical changes that occur when sulfur and salt are separated.

34. Section 2 Physical and Chemical Changes
Chapter 3

35. Physical Changes in Our World, continued
Section 2 Physical and Chemical Changes
Chapter 3
Physical Changes in Our World, continued
Physical Changes in Nature
Movement of soil and rock
Ponds freezing
Water freezing or melting
Physical Changes in Industry
Making sugar
Building furniture

36. Chemical Change in Our World
Section 2 Physical and Chemical Changes
Chapter 3
Chemical Change in Our World
A chemical change occurs when new substances are formed
Different identity
Different physical properties.
A Chemical Change producing new substances are also called chemical reactions.

37. Chemical Change in Our World, continued
Section 2 Physical and Chemical Changes
Chapter 3
Chemical Change in Our World, continued
Chemical Changes in Nature
Photosynthesis
Digestion.
Physical Changes in Industry
Making metal
Refining oil for gasoline.

38. Are Physical and Chemical Changes Reversible?
Section 2 Physical and Chemical Changes
Chapter 3
Are Physical and Chemical Changes Reversible?
Most physical changes are reversible
Physical changes only affect the matter’s form.
Most chemical changes are not reversible.

39. Chapter 3 Section 3 Objectives
Section 3 States of Matter
Section 3 Objectives
Explain why particles in matter are always in motion.
Compare the properties of solids, liquids, and gases.
Explain the behavior of gases.
Describe plasma.

40. Particles of Matter in Motion
Chapter 3
Section 3 States of Matter
Particles of Matter in Motion
There are movements in matter that are too small to see or feel.
Particles in matter are always in motion because particles have energy.

41. Particles of Matter in Motion, continued
Chapter 3
Section 3 States of Matter
Particles of Matter in Motion, continued
States of Matter Determined by Particle Energy The more energy a particle has, the faster it moves.
Particle energy and movement determines the physical forms of matter, or the states of matter.
Four states of matter are solid, liquid, gas, and plasma.
They are physically different because their particles have different amounts of energy.

42. Chapter 3
Section 3 States of Matter

43. Physical Differences Between States of Matter
Chapter 3
Section 3 States of Matter
Physical Differences Between States of Matter
Solids Have Rigid Structure
Particles are fixed into place
water molecules in ice.
Does not change shape or size.
Temperature measures the energy of the particles.
The temperature at which a solid change to liquid is called its melting point.

44. Physical Differences Between States of Matter, continued
Chapter 3
Section 3 States of Matter
Physical Differences Between States of Matter, continued
Liquids
A liquid assumes the shape of its container.
Molecules are in contact with each other, but are not held rigidly in place.
A liquid has a definite volume but no definite shape.

45. Physical Differences Between States of Matter, continued
Chapter 3
Section 3 States of Matter
Physical Differences Between States of Matter, continued
Gas
The particles of matter have enough energy to escape their attraction to each other.
Due to their high energy and rapid motion, particles of a gas fill whatever volume is available.
A gas has no definite shape and no definite volume.

46. Physical Differences Between States of Matter, continued
Chapter 3
Section 3 States of Matter
Physical Differences Between States of Matter, continued
Changing from One State to Another
Changes occur when energy is added to or removed from a substance.
The change from a liquid to a gas is called evaporation or boiling.
Energy is added to the liquid to cause its molecules to escape the attraction to one another.

47. Physical Differences Between States of Matter, continued
Chapter 3
Section 3 States of Matter
Physical Differences Between States of Matter, continued
When a gas is cooled, attractions between the particles becomes stronger and the gas condenses into a liquid.
When a liquid changes to a solid, it freezes. The liquid cools enough for attractions between the particles to lock the particles into fixed positions.

48. Chapter 3
Section 3 States of Matter
Solid, Liquid and Gas

49. Chapter 3 Behavior of Gases
Section 3 States of Matter
Behavior of Gases
The volume of a gas is the amount of space taken up by the gas particles in a container.
Temperature Heat causes a gas to expand because the molecules have more energy. Cold causes the gas to contract because the molecules move slower.

50. Behavior of Gases, continued
Chapter 3
Section 3 States of Matter
Behavior of Gases, continued
Volume The volume of a gas depends on the container that holds the gas.
Pressure measures the amount of force exerted per unit area of a surface. When air particles collide within a container, they exert more pressure.
In the next slide, the beach ball has less pressure because it has fewer gas particles.

51. Chapter 3
Section 3 States of Matter

52. Plasma: A Fourth State of Matter
Chapter 3
Section 3 States of Matter
Plasma: A Fourth State of Matter
Plasma is a state of matter that starts as a gas and then becomes ionized. Its properties differ from those of a solid, liquid, or gas.
Plasma is created when energy is added to a gas. Plasma is similar to a gas in that it has no fixed shape, but it is different in that it conducts electric current and is attracted to magnetic fields.

53. Chapter 3 Concept Mapping
Properties and States of Matter
Concept Mapping
Use the terms below to complete the concept map on the next slide.
changes of state
melting
evaporating
solid
liquid
condensing
chemical formulas

54. Chapter 3
Properties and States of Matter

55. Chapter 3
Properties and States of Matter

56. End of Chapter 3 Show Chapter menu Resources
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