1. Properties and States of Matter
Chapter 3.1
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. 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.

5. 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

6. Chapter 3
Section 1 Properties of Matter

7. 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.

8. Chapter 3
Section 1 Properties of Matter

9. 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

10. 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

11. 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.

12. 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.

13. 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.

14. Identifying Matter with Physical Properties, continued
Chapter 3
Section 1 Properties of Matter
Identifying Matter with Physical Properties, continued
Mass and Weight
The force of gravity on an object is called weight.
Weight is sometimes confused with mass.
Weight varies depending on where you are in the universe.
Weight on moon is 1/6th of weight on earth
Mass on moon is the same as on earth

15. Comparing Mass and Weight
Chapter 3
Section 1 Properties of Matter
Comparing Mass and Weight

16. Identifying Matter with Physical Properties, continued
Chapter 3
Section 1 Properties of Matter
Identifying Matter with Physical Properties, continued
Volume
The amount of space matter occupies is called volume.
Density
The mass of an object per unit of volume is called its density.
Density is found by dividing mass by volume.

17. Identifying Matter with Physical Properties, continued
Chapter 3
Section 1 Properties of Matter
Identifying Matter with Physical Properties, continued
Other Important Physical Properties can help identify and classify matter.
Malleability substances are soft, such as aluminum – how well it can be shaped.
Conductivity - how well a substance conducts electricity.
boiling point.

18. Identifying Matter with Chemical Properties
Chapter 3
Section 1 Properties of Matter
Identifying Matter with Chemical Properties
Chemical Properties describe matter based on its ability to participate in chemical reactions and form new substances.
Reactivity is the ability of substances to combine and form one or more new substances.

19. Categories of Matter and Their Properties
Chapter 3
Section 1 Properties of Matter
Categories of Matter and Their Properties
Classification
based on the chemical and physical properties of matter.
Properties of Pure Substances
All pure substances have the same composition, and exactly the same physical and chemical properties.

20. Categories of Matter and Their Properties, continued
Chapter 3
Section 1 Properties of Matter
Categories of Matter and Their Properties, continued
Pure substances are either elements or compounds.
Elements are composed of the same atoms.
Compounds are composed of the same molecules.

21. Categories of Matter and Their Properties, continued
Chapter 3
Section 1 Properties of Matter
Categories of Matter and Their Properties, continued
Properties of Mixtures The physical and chemical properties of a mixture can vary.
A mixture is a blend of pure substances which retain their identity and properties.
All matter can be classified according to the categories shown on the next slide.

22. Chapter 3
Section 1 Properties of Matter

23. 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.

24. 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.

25. 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.

26. 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.

27. Section 2 Physical and Chemical Changes
Chapter 3

28. 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

29. 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.

30. 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.

31. 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.

32. 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.

33. 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.

34. 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.

35. Chapter 3
Section 3 States of Matter

36. 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.

37. 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.

38. 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.

39. 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.

40. 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.

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

42. 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.

43. 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.

44. Chapter 3
Section 3 States of Matter

45. 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.

46. 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

47. Chapter 3
Properties and States of Matter

48. Chapter 3
Properties and States of Matter

49. End of Chapter 3 Show Chapter menu Resources
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