1. Intro to Matter

2. Matter
EVERYTHING IN THE UNIVERSE IS EITHER MATTER OR ENERGY

3. Matter
MATTER – Anything that has mass and takes up space (volume).

4. Matter
MATTER MAKES UP THINGS THAT ARE VERY LARGE & VERY SMALL.

5. LAW OF CONSERVATION OF MATTER
MATTER CANNOT BE CREATED OR DESTROYED IT JUST CHANGES FROM ONE FORM TO ANOTHER.
(MATTER GETS RECYCLED)

6. Physical and Chemical Properties
All matter has different characteristics or
properties. These properties can be either
physical or chemical properties.
A. Physical properties: properties that can be
observed or measured. (color, mass, length,
volume, density, state, etc)
B. Chemical Properties: properties describe the ability of an object to change into a new substance. (flammability, reactivity)

7. Physical Properties COLOR STATE (PHASE) SHAPE ODOR (SMELL) TEXTURE
Observable PHYSICAL properties of matter (You can sense them):
COLOR
STATE (PHASE)
SHAPE
ODOR (SMELL)
TEXTURE
HARDNESS

8. Chemical Properties
Chemical Properties: properties describes the ability of an object to change into a new substance. (flammability, reactivity)

9. Elements & Compounds ELEMENTS ARE MADE OF ONLY 1 KIND OF ATOM
ELEMENTS & COMPOUNDS ARE THE BASIC BUILDING BLOCKS OF MATTER
EACH ELEMENT & COMPOUND HAS SPECIFIC PROPERTIES
ELEMENTS ARE MADE OF ONLY 1 KIND OF ATOM
SOME COMMON ELEMENTS:
HYDROGEN (H), HELIUM (He), OXYGEN (O),
CARBON (C), IRON (Fe), CALCIUM (Ca),
NITROGEN (N), SULFUR (S), SODIUM (NA)
CHLORINE (Cl), SILICON (Si), POTASSIUM (K) GOLD (Au). MERCURY (Hg)

10. Elements & Compounds + = Table Salt
COMPOUNDS ARE MADE OF 2 OR MORE DIFFERENT KINDS OF ELEMENTS.
COMPOUNDS ARE IDENTIFIED BY A CHEMICAL FORMULA
THE ELEMENTS THAT COMBINE TO MAKE THE COMPOUND CHANGE PROPERTIES + =
Table Salt

11. What is a Mixture? Mixture: is a combination of 2 or more
elements or compounds that are not
chemically combined. They are just mixed.
Examples of Mixtures:

12. Characteristics of Mixtures
No chemical change occurs (the substances keep their identity).
THE SUBSTANCES CAN BE SEPARATED!!!!!

13. Separating Mixtures
Filtration – filter out one substance to leave the other. Separating the soluble from the insoluble.
Chromatography – used to separate out mixtures of dyes. Shows all the colors used to make certain dyes
Evaporation – Used when you wish to collect a solute from a solution. Evaporate a LIQUID to leave the SOLID behind.
Magnet – use a magnet to remove the metal substances from nonmetal substances.

14. Types of Mixtures
Heterogeneous- the different substances are visible in the mixture. Homogeneous – The mixture looks the same and has the same characteristics throughout.

15. Physical Properties
Some measurable PHYSICAL properties of matter (You have to have equipment to measure):
Volume
Mass
Weight
Density
Temperature
Length
Height
Speed

16. Measurable Physical Properties
Measurable Properties – Properties that a
tool is needed to measure.
Mass – the amount of matter in an object. This is different than weight!!!!!
Weight – is the amount of gravity pulling on an object
For example: A human’s mass will never change. But if we traveled to the moon, our weight would change because there is less gravity than on Earth.

17. Measurable Properties of Matter
VOLUME – is the amount of space an object takes up (no matter what object).

18. Volume of a Liquid X MENISCUS - bottom of the curve.
LIQUID VOLUME : Use a graduated cylinder to find the volume
How to read a graduated cylinder
Must be at eye level to read.
Must read to bottom of the curve.
MENISCUS - bottom of the curve. X

19. Calculating the Volume of a Regular Solid
CALCULATE Volume = Length X Width X Height
EQUIPMENT: Ruler
UNIT : We will use cubic centimeters (cm3).
(Any unit of length can be cubed. IN3, FT3, M3)
Which of these objects below are regular solids?

20. Calculating the Volume of an Irregular Solid
Because you cannot measure the length, width, and height, you have to use Water Displacement to find the volume.
Place 50 ml water in a cylinder.
Drop in object to see how much the water rises.
The number of ml it rises is the volume of the object.

21. (Mass divided by volume)
Density
Density - the amount of matter in a given space or volume.
Calculate : mass
Density =
volume
(Mass divided by volume)

22. Density (physical property)
Density is used to identify substances.
All substances ALWAYS have the same density no matter how big or small the piece.
The density of water is 1g/ml.
Anything with a density higher than 1 will sink in water. Anything with a density less than 1 will float in water.
UNITS: g/cm3 for solids, g/ml for liquids
Density of gold = 19.32g/cm3
Density of silver = 10.50g/cm3
Density of ice = .9g/cm3

23. BELL RINGER Calculate the density for the following objects:
Mass= 10g Volume= 5ml
Mass= 16g Volume= 8cm
Mass= 5g Volume= 10ml
Mass= 12g Volume= 12 cm
Which object is water? Which object will
float in water? Which objects will sink in
water?
2g/ml sinker
2g/cm3 sinker
0.5g/ml floater
1g/cm3 water

24. Density objects!!!! When does the density of an object change?
Only when heat (energy) is added or taken away!!!!
ADDING HEAT – spreads out molecules = LESS
dense
Take AWAY heat – molecules come together = MORE dense.
Hot objects are less dense than cool
objects!!!!

25. THEORY OF KINETIC ENERGY (or Changing States of Matter)
1. ATOMS ARE ALWAYS MOVING
THE MORE ENERGY ADDED TO THE ATOMS, THE FASTER & FARTHER APART THEY MOVE
ENERGY ADDED
ENERGY ADDED

26. States (or Phases) of Matter
State of matter is a physical property!!!!
MATTER CAN BE FOUND IN 4 STATES (PHASES)
SOLID
LIQUID
GAS
PLASMA

27. Physical Changes
Physical Changes: a property of matter that can be observed or measured without changing the identity of the matter.
IN OTHER WORDS
A CHANGE IN STATE
A CHANGE IN SIZE, SHAPE, MASS
DOES NOT CHANGE THE CHEMICAL MAKE UP OF THE MATTER
YOU HAVE WHAT YOU STARTED WITH JUST IN A DIFFERENT FORM

28. Examples of Physical Change
PAPER TORN INTO PIECES
SUGAR DISSOLVED INTO TEA
SALT DISSOLVED INTO WATER
NAILS OR HAIR CUT

29. Physical Changes Types of Phase Changes Melting Evaporation Boiling
A change in phase is a physical change.
Types of Phase Changes
Melting
Evaporation
Boiling
Condensation
Sublimation
ALL PHASE CHANGES ARE CAUSED BY
ADDING OR TAKING AWAY ENERGY!!!

30. Remember…
CHANGING STATES DOES NOT CHANGE THE CHEMICAL MAKE UP OF THE MATTER
YOU HAVE WHAT YOU STARTED WITH JUST IN A DIFFERENT FORM
ICE WATER WATER VAPOR

31. Melting Energy is added
1. MELTING – GOING FROM A SOLID TO A LIQUID
Energy is added
When more heat (energy) is added to matter the particles move faster till the bonds break.

32. Evaporation GOING FROM A LIQUID TO A GAS AT THE SURFACE
ENERGY IS ADDED TO SURFACE OF LIQUID
THE PARTICLES AT THE SURFACE MOVE FASTER BREAKING BONDS.

33. Boiling GOING FROM A LIQUID TO A GAS ALL THROUGHOUT THE LIQUID
ENERGY IS ADDED TO ALL OF LIQUID
PARTICLES MOVE FASTER ALL THROUGH THE LIQUID
SOME PARTICLES MOVE FAST ENOUGH TO CHANGE TO GAS WHILE THEY ARE IN THE MIDDLE OF THE LIQUID
Water boils at 212 F, 100C.
EX: pan of liquid on the stove

34. Condensation THE PARTICLES MOVE SLOWER
CHANGING FROM A GAS TO A LIQUID
ENERGY IS REMOVED
THE PARTICLES MOVE SLOWER
THE ATTRACTION BETWEEN THE PARTICLES BEGAN TO PULL THE PARTICLES CLOSER TOGETHER & THE MATTER TURNS INTO A LIQUID
Ex: dew in the lawn, water running down mirror, ring on table under glass

35. Freezing CHANGING FROM A LIQUID TO A SOLID ENERGY IS REMOVED
THE PARTICLES MOVE EVEN SLOWER
THE ATTRACTION BETWEEN THE PARTICLES BEGAN TO PULL THE PARTICLES CLOSER TOGETHER & THE MATTER TURNS INTO A SOLID
Water freezes at 32 F, 0 C
EX: water to ice, wax or chocolate hardening

36. Examples of Sublimation: Snowflakes, dry ice, frost
Substance goes straight from a solid to a gas or from gas to solid. DRY ICE!!!!
Heat added or taken away rapidly
Molecules speed up and spread out
Examples of Sublimation: Snowflakes, dry ice, frost

37. Chemical Change
CHEMICAL CHANGE – occurs when 2 or more substances are combined into entirely new substance with all new properties. CANNOT CHANGE IT BACK!!!!!

38. Signs of a Chemical Change
FIZZES OR BUBBLES
COLOR CHANGE
HEAT GIVEN OFF
LIGHT GIVEN OFF
ODOR
HEAT REQUIRED FOR REACTION
NEW SUBSTANCE FORMED
Precipitate (solid)
Gas (bubbles)

39. Examples of a Chemical Change
BAKING BREAD – NO LONGER HAVE FLOUR, EGGS, MILK, YEAST
ALKA-SELTZER
BAKING SODA & VINEGAR
RUST
TARNISH

40. Law of Conservation of Matter (again!)
Law of Conservation of Matter – Law states that the number of atoms must be the same on each side of the equation

41. Chemical Changes through Chemical Reactions
A chemical reaction – Process in which the physical and
chemical properties of the original substance change as
new substances with different properties are formed
Baking soda and
vinegar

42. Parts of a Chemical Reaction
Products – Substances produced in the reaction
Reactants – Substance that begins the equation
Plus sign – added together
Arrow - equals
Reactants
Product