1. Introduction to Matter

2. Think…Think…Think What is “stuff” made of?
What are the smallest bits of things?
If more than one kind of part makes up a thing, what are those parts?

3. Ancient cultures (Alchemists)

4. Think & Discuss: Ancient cultures
- wet when you cut it so it must have water
- grows from the ground so it has earth
makes smoke when it is burned so it must have air
can burn so it must contain fire

5. Think like an ancient person.
Potato

6. Think like an ancient person.
Silver

7. Think like an ancient person.
Feather

8. Limitations to the four elements.
Developed better systems to help classify matter.
There are more than just 4 elements.
Look at the Periodic Table

9. Classifying Matter Matter Pure Substances Mixtures milk, Gatorade
Homogeneous
Heterogeneous
Elements
Compounds
Cookie dough ice cream, muddy water
milk, Gatorade
Fe, O
H2O, CO2

10. MATTER Matter: anything that has mass and takes up space
Mass – the amount of matter in something
Volume – the amount of space something occupies
Which of the following is matter?
A car?
A box?
You?
Heat?
Fire?
Made up of different kinds of atoms
Includes all things that can be seen, tasted, smelled, or touched

11. Examples of Matter Cookies Oxygen You Water What is not matter? -Heat
-Energy
-Light

12. States of Matter
Matter can be in a solid, liquid, gas, plasma or Bose-Einstein condensates (BEC) state.

13. States of Matter
Four states:
Bill Nye:

16. In science, anything that has mass and takes up space is called matter
Everything in the universe is made of matter
A really loooooong time ago, the Greeks concluded that matter could be broken down into particles too small to be seen.
3 forms of matter: solid liquid, gas (pop quiz questions about this later)
Atom means indivisible
They called these particles
atoms

17. So, what’s an atom?
An atom is the smallest piece that matter can be broken down into
Okay, but I’ve never seen an atom Where are they?

18. Atoms are EVERYWHERE!! Atoms are in . . . plants hair desks boogers
CDs
Atoms are in . . .
hot dogs
chocolate
cheese
dirt
air
cars
and even underwear

19. Pop Quiz Question #1 What are the four main states of matter?
solid, water, freezing, boiling
Water, ice, air, steam
Solid, liquid, gas, plasma
earth, rain, air, fire
Correct answer is C

21. What is a property?
Property: a characteristic of a substance that can be observed

22. Physical versus Chemical Properties
The study of matter

23. Physical Properties melting point density
Physical property: a property that can be observed without changing the identity of the substance.
Examples of physical properties:
luster
malleability: the ability to be hammered into a thin sheet
ductility: the ability to be stretched into a wire
melting point
boiling point
density
solubility
specific heat

25. Examples of Physical Properties
Luster: shininess
Malleability: the ability to be hammered into a thin sheet
Ductility: the ability to be stretched into a wire

26. Physical Properties
Melting point: the temperature at which a substance changes from a solid to a liquid at a given pressure
water = 0oC
Boiling point: the temperature at which a substance changes from a liquid to a gas at a given pressure
water = 100oC

27. Special Physical Properties
Solubility: amount of a substance that can be dissolved in a given amount of solvent
Specific heat: amount of heat required to change a unit mass of a substance by one degree in temperature.
Density: the amount of mass per unit of volume

28. Density Density is the amount of mass per unit of volume.
Density can be used to identify a substance.
The density of water is 1.0g/mL

29. Density Calculations
Formula:
D = m/V = g/mL = g/cm3

30. Density Examples
#1: A cube has a mass of 3.0 g and occupies a volume of 6.0 ml. Would this object float or sink in water?
Mass = 3.0 g Volume = 6.0 mL
D = 3g/6 mL= 0.5 g/mL
This object would float in water because its density is less than water (1.0 g/mL).

31. More Density Calculations
#2: A liquid has a mass of 25.0 g and a volume of 10.0 mL. Use the table below to identify the substance.
M=25.0 g V=10.0 mL
D = 25 g/10 mL
D= 2.5 g/mL
The substance is potassium.
Potassium 2.5 g/ml

32. Chemical Properties
Chemical property: a property that can only be observed by changing the identity of the substance
Examples of chemical properties:
flammability
ability to rust
ability to tarnish
reactivity with vinegar

35. Compounds, Mixtures, Solutions and Reactions

36. Classifying Matter Matter Pure Substances Mixtures milk, Gatorade
Homogeneous
Heterogeneous
Elements
Compounds
Cookie dough ice cream, muddy water
milk, Gatorade
Fe, O
H2O, CO2

37. What is a Pure Substance?
A pure substance is a classification of matter that includes both elements and compounds
Pure substances cannot be separated by physical means such as distillation, filtration, or chromatography

38. Elements We will study elements in depth later, but be sure to know…
An element is made of one kind of atom
Found on the periodic table

39. What Is A Compound?
A compound is a pure substance that is created by 2 or more elements chemically reacting and joining together
Ex: NaCl, H2O, CO2, NH3, NaHCO3, and C6H12O6
Notice that elements combine in many ways to make compounds
Ex: H2O, H2O2, CO, and CO2

40. Why Do Compounds Form?
Compounds form to allow elements to become more stable
Na is flammable when it comes in contact with H2O, and Cl2 is a toxic gas
NaCl is a very stable compound that is neither flammable nor toxic (in normal quantities)
Compounds that are extremely unstable will break down to form the more stable elements

41. How Do Compounds Form?
Compounds form by the interaction between the nuclei and valence electrons of 2 or more elements.

42. What Do Compounds Have To Do With My Life?
Compounds are the substances that make up ALL living and non-living things
Examples: Where would you be without:
H2O—water
NaCl—table salt
C3H8O—rubbing alcohol
C55H98O6—an example of an
unsaturated fat

43. Classifying Matter Matter Pure Substances Mixtures milk, Gatorade
Homogeneous
Heterogeneous
Elements
Compounds
Cookie dough ice cream, muddy water
milk, Gatorade
Fe, O
H2O, CO2

44. What Is A Mixture?
A mixture is the physical combination of 2 or more substances
A mixture is not chemically combined
Mixtures can be separated by physical means such as filtration, distillation, and chromatography
Mixtures can be divided into 2 groups
Homogenous mixtures
Heterogeneous mixtures

45. How Do Mixtures Form?
Mixtures form by physically “junking” 2 or more substances together
Remember no chemical change is occurring
The formation of a mixture is not a result of lowering energy

46. What Is a Homogenous Mixture?
A homogeneous mixture is a mixture that is evenly distributed
commonly called solutions
Solution = Solute + Solvent
Solute: “stuff” being dissolved
Solvent: “stuff” doing the dissolving
The solvent is present in greater quantity
The solute is present in the lesser quantity
Ex: Salt water: Salt=solute, Water=solvent

47. What Is a Heterogeneous Mixture?
A heterogeneous mixture is a mixture that is unevenly distributed.
Examples:
Cookie dough ice cream: The chunks of dough are not evenly distributed throughout the ice cream
Chex Mix: You may find a different number of pretzels or Chex cereal in each handful; therefore, the mixture is unevenly distributed

48. How Are Mixtures Important To My Life?
We encounter mixtures everywhere in our lives
Where would you be without:
Ice cream
Kool-aid
Shampoo
Soap
Milk
Orange juice

49. Pop Quiz Question #1 Place an S beside each solution
and an M beside each mixture
_____ seawater
_____ steel
_____ salad
_____ air
_____ handful of skittles S S M S M

50. Changes in Matter

51. Physical Change Examples
Physical change: a change that occurs that does not alter the identity of the substance
Melting ice
Freezing Kool-aid
Tearing paper
Boiling water

52. An indicator is something that produces an observable physical change but still retains its original form.
Some of these changes may include the appearance or disappearance of a color.

53. Chemical Change Examples
Chemical change: a change that occurs causing the identity of the substance to be changed.
Burning paper
Digesting food
Electrolysis of water
A chemical change is called a chemical reaction
Cannot be undone (not reversible)

54. Chemical Changes Cont’d
Indicators of a chemical change:
Production of light
Production of heat
Production of a gas
Color change
Formation of a precipitate
*Precipitate: an insoluble substance that is produced as result of a chemical reaction

55. Is it Physical or Chemical?
Change
Physical
Chemical
Melting cheese
Burning wood
Milk souring
Shredding paper
Bicycle rusting

56. How Can We Change Matter Into New Substances?
Chemical reaction (also known as a chemical change) is a change in a substance or substances that results in a totally new substance
Ex: 2H2(g) + O2(g)  2H2O(g)
Notice that the reactants (the substances you start with) combine to form a new substance (the product)

57. Why Do Chemical Reactions Occur?
Chemical reactions occur to produce a more stable product than the existing reactants
Ex: 2Na(s) + Cl2(g)  2NaCl(s)
*The sodium is highly unstable and the chlorine gas is somewhat unstable. The resulting Sodium Chloride is VERY stable.
**It is important to understand that the products have totally different properties than the reactants

58. Where Does The Matter Go?
It is important to understand that when matter undergoes a chemical reaction (a chemical change) it does not disappear or appear
The atoms are rearranged and form new bonds, but no matter is lost nor gained
This is called the Law of Conservation of Matter

59. What Kind of Chemical Reactions Do I Experience?
The acidic milk and basic baking soda that produce CO2 gas when a cake bakes
Paper burning to produce ashes, CO2, and H2O vapor
Hydrogen peroxide decomposing to produce water and oxygen gas

60. Exothermic Reactions A reaction in which energy is released
Often produces an increase in temperature
Reactants = Products + Energy

61. Exothermic Examples
Glow sticks- work by a chemical reaction that releases energy as light
Fireflies- light up by a reaction that takes place between oxygen and a chemical called luciferin

62. Endothermic Reactions
A reaction in which energy is absorbed
Often produces a decrease in temperature
Reactants + Energy = Products

63. Endothermic Examples Instant cold pack Photosynthesis
Baking a cake- The cake batter will not bake unless it absorbs energy

64. Simple Chemical Reactions
Explain 3 chemical reactions on your paper
Bill Nye – Simple Chemical Reactions