1. MATTER
Chapter 3

2. Section 3.1 The Particulate Nature of Matter
Objective:
Learn about the composition of matter

3. Matter Matter is anything that:
a) has mass, and
b) takes up space
Mass = a measure of the amount of “stuff” (or material) the object contains (don’t confuse this with weight, a measure of gravity)
Volume = a measure of the space occupied by the object

4. States of Matter
Objective:
To define the 3 states of matter

5. States of matter
Solid- matter that can not flow (definite shape) and has definite volume.
Liquid- definite volume but takes the shape of its container (flows).
Gas- a substance without definite volume or shape and can flow.
* Vapor- a substance that is currently a gas, but normally is a liquid or solid at room temperature. (Which is correct: “water gas”, or “water vapor”?)

6. States of Matter Definite Volume? Definite Shape? Solid Liquid Gas
Result of a TemperatureIncrease?
Definite Volume?
Definite Shape?
Will it Compress?
Small Expands.
Solid
YES
YES NO
Small Expands.
Liquid NO NO
YES
Large Expands.
Gas NO NO
YES

7. Three Main Phases
Solids – molecule are locked into fixed positions….little movement to move
Liquids – molecules can slide past one another
Gas – a free to move randomly about

8. Copper Phases - Solid

9. Copper Phases - Liquid

10. Copper Phases – Vapor (gas)

11. Condense
Freeze
Melt
Evaporate
Solid
Liquid
Gas

12. 4th state: Plasma - formed at high temperatures; ionized phase of matter as found in the sun

13. Ever heard of a Bose-Einstein Condensate???

14. Section 3.2 Physical/Chemical Properties and Changes
Objective:
To distinguish between physical and chemical properties
To distinguish between physical and chemical changes

15. Properties are… Words that describe matter (adjectives)
Physical Properties- a property that can be observed and measured without changing the material’s composition.
Describes individual characteristics
Examples- color, hardness, m.p., b.p.
Chemical Properties- a property that can only be observed by changing the composition of the material.
Describes social characteristics
Examples- ability to burn, decompose, ferment, react with, etc.

16. Physical vs. Chemical Change
Physical change will change the visible appearance, without changing the composition of the material.
Boil, melt, cut, bend, split, crack
Is boiled water still water?
Can be reversible, or irreversible
Chemical change - a change where a new form of matter is formed.
Rust, burn, decompose, ferment

17. Recognizing Chemical Changes
Energy is absorbed or released (temperature changes hotter or colder)
Color changes
Gas production (bubbling, fizzing, or odor change; smoke)
formation of a precipitate - a solid that separates from solution (won’t dissolve)
Irreversibility - not easily reversed
But, there are examples of these that are not chemical – boiling water bubbles, etc.

18. Section 3.5 Separation of Mixtures
Objective:
Learn 2 methods of separating a mixture

19. Separation of a Mixture
Objective:
Learn 2 methods of separating mixtures

20. Separating Mixtures- (talk more about mixtures is tomorrow)
Some mixtures can be separated easily by physical means: rocks and marbles, iron filings and sulfur (use magnet)
Differences in physical properties can be used to separate mixtures.
Filtration - separates a solid from the liquid in a heterogeneous mixture (by size) – Figure 2.7, page 46

21. Filtration separates a liquid from a solid.

22. Separation of a Mixture
Distillation: takes advantage of different boiling points.
NaCl boils at 1415 oC

23. Another view of Distillation

24. Separation of a sand-saltwater mixture
To separate sand-saltwater mixture:
first use filtration to separate sand from saltwater
then use distillation to separate salt and water

25. Section 3.3 Elements and Compounds
Objective:
The difference between a element & compound

26. What about atoms? All matter is made up of tiny particles called ATOMS
Although objects look quite continuous and uniform, they are really particulate in nature
Atoms are not all alike
About 100 different types of atoms make up all the different types of matter
Think of the alphabet (atoms) and words (matter)

27. Element, Compound or Molecule
Elements simplest kind of matter
cannot be broken down any simpler and still have properties of that element!
all one kind of atom.
Compounds are substances that can be broken down only by chemical methods
when broken down, the pieces have completely different properties than the original compound.
made of two or more different atoms, chemically combined (not just a physical blend!)
Molecules are substances that can be broken down only by chemical methods
made of two or more atoms, chemically combined (not just a physical blend!)

28. A molecule is what you get when any atoms join together.
I am not clear on what a molecule is. If water is a molecule, is it also a compound because the hydrogen and oxygen have been chemically combined? If so, how do you determine whether a substance is a compound or a molecule?
A molecule is what you get when any atoms join together.
A compound is what you get when atoms of two or more different elements join together.
All compounds are molecules, but not all molecules are compounds.
Water is a molecule because it is made from atoms that have been chemically combined. It is also a compound because the atoms that make water are not all the same - some are oxygen and some are hydrogen.
Oxygen in the atmosphere is a molecule because it is made from two atoms of oxygen. It is not a compound because it is made from atoms of only one element - oxygen. This type of molecule is called a diatomic molecule, a molecule made from two atoms of the same type.

29. Elements vs Compounds Currently, there are 117 elements
Elements have a 1 or two letter symbol, and compounds have a formula.
An element’s first letter always capitalized; if there is a second letter, it is written lowercase: B, Ba, C, Ca, H, He
Some names come from Latin or other languages

30. Compounds vs Elements
Compounds can be broken down into simpler substances by chemical means, but elements cannot.
Compounds always contain atoms of different elements…..Always in the same composition
Ex. Water is always found as 2 hydrogen atoms combined with 1 oxygen atom

31. Section 3.4 Mixtures vs Pure substance
Objective:
To distinguish between mixtures and pure substances

32. Mixtures
Mixtures - are a physical blend of at least two substances; have variable composition. They can be either:
Heterogeneous – the mixture different it is not uniform in composition
Chocolate chip cookie, gravel, soil.
2.) Homogeneous - same composition throughout; called “solutions”
Kool-aid, air, salt water
Every part keeps it’s own properties.

33. Solutions are homogeneous mixtures
Mixed molecule by molecule, thus too small to see the different parts
Can occur between any state of matter: gas in gas; liquid in gas; gas in liquid; solid in liquid; solid in solid (alloys), etc.
Thus, based on the distribution of their components, mixtures are called homogeneous or heterogeneous.

34. Alloy – mixture of metals
Twenty-four-karat gold is an element Eighteen-karat gold is an alloy. Fourteen-karat gold is an alloy. *An alloy is a mixture or metallic solid solution composed of two or more elements

35. Tie together some of the information
What is the difference then between a mixture and a compound????

36. Compound vs. Mixture Compound Mixture Made of one kind of material
Made of more than
one kind of material
Made by a
chemical change
physical change
Definite
composition
Variable

37. Pure Substances Pure substances – always have same composition
Either elements or compounds
Ex pure water is a pure substance – it only contains H2O molecules
Tap water is a mixture – it contains H2O and other minerals such as calcium and magnesium

38. Classification of Matter

39. Which is it?

40. Element

41. Which is it?

42. Compound/molecule

43. Which is it?

44. Mixture

45. Which is it?

46. CANNOT be a compound. WHY????
Molecule.
CANNOT be a compound. WHY????

47. Chapter 3
The End