1. Chapter 8
What Is Matter?

2. Essential Questions
I can identify the parts of an atom and its purpose
I can explain why mixtures can be separated using physical properties.
I can classify elements and compounds according to their properties.
I can compare properties of different combinations of elements. ,

3. What is Matter? 8.1 Matter and Atoms Matter Anything that takes up
space and has mass.
Matter
What is Matter?

4. What is Matter Made Of… Atom
The smallest particle into which an element can be divided and still be the same element.

5. Center of the atom and
is made up of protons
and neutrons. Most of
the atom’s mass is in the
nucleus.
Nucleus

6. Protons
Neutrons
Electrons
The particles in the nucleus that
have a positive charge. (+)
Particles in the nucleus with a
neutral or no charge.
Are located around the edge of the
atom and have a negative charge.
(-) They can be easily removed.

7. Element
Elements
A pure substance that cannot be separated into simpler substances by physical or chemical means.
Ex. (Oxygen and hydrogen are both elements)
All of the oxygen atoms are
alike and all of the hydrogen
atoms are alike, but the
oxygen atoms are not
like the hydrogen atoms.

8. The elements are classified by their properties
Periodic Table
Is a chart containing 112
elements.
The elements are classified by their properties

9. Abbreviations for elements O=Oxygen H=Hydrogen
Chemical Symbols
Abbreviations for elements
O=Oxygen
H=Hydrogen
See pg. 224 (Old Book)

10. Is the number of protons in the nucleus. Each element
Atomic Number
Is the number of protons in
the nucleus. Each element
has a unique number of
protons in the nucleus. The
atomic number and number
of protons are the same.
Ex (Carbon has 6 protons, and Carbon’s atomic number is 6)

11. Atomic Mass
Dmitri Mendeleev
Is the number of protons plus
the number of neutrons.
Carbon has 6 protons and 6
neutrons, so 6 + 6=12. The
atomic mass will be 12.
The person who organized
the Periodic table.

12. Compounds
Compounds
A pure substance made of two or more elements that are chemically combined.

13. Sodium, hydrogen, carbon, & oxygen
Common Compounds
Compound
Elements Combined
Table Salt
Sodium & Chlorine
Water
Hydrogen & Oxygen
Carbon Dioxide
Carbon & Oxygen
Baking Soda
Sodium, hydrogen, carbon, & oxygen

14. Represent compounds the way chemical symbols
Chemical Formula
Subscript
Represent compounds the
way chemical symbols
represent elements. H2O is
water. It is a chemical
formula.
The number in a chemical
formula that tells how many
atoms we are talking about.
Ex (H2O)

15. Molecule
Is the number of compounds. 3
is the number of water molecules
and is written 3H2O.

16. Physical Change vs. Chemical change

17. 9.3 Physical and Chemical Changes
Is a change in size, shape or
form.
Ex (cutting paper into pieces or
changing water to ice)
The earth is shaped by physical
changes such as weathering
when water freezes and then
thaws and cracks rocks.

18. Chemical change
Chemical Change
When one or more substances are changed into new substances and have new and different properties.
Examples: Metal Rusting, Milk souring, fireworks, cooking Digesting your food, Using a battery

19. Baking a Cake, Chemical or Physical?
You take all of these ingredients, mix them and put them in the oven. =

20. Indicators of a Chemical Reaction
1.Formation of a Precipitate 2. Gas bubbles are released 3. It changes energy (Heat is added or released) 4. It may change color 5. A change in odor

21. Formation of a Precipitate
There is a formation of a solid when combining two solutions

22. Bubbles
The formation of a gas (bubbles or fizzing) is a clue that a chemical reaction is taking place.
Example: Alka-Seltzer dropped in water

23. Change in Energy (Heat)
A chemical reaction involves the breaking of bonds in the reactants and the forming of bonds in the product.
Endothermic (Temperature drops)- Absorb more energy than they release.
Exothermic (Temperature Increases) - Release more energy than they absorb.

24. Change in Color
In a chemical reaction there is often a change in color from the original substance to the new one.
(Examples: Rusting, Fireworks, Leaves changing

25. Change in Odor
Chemical reactions may give off a smell or new odor. (Example: Food rotting, such as rotten eggs)

26. Matter can’t be created or destroyed. It is just
Law of
Conservation of
Mass or Matter
Matter can’t be created or
destroyed. It is just
converted to another form.
Ex. (Burning wood)

27. Law of Conservation of Matter or Law of Conservation of Mass

28. What Do You See? What is its purpose?
When the pans are both at the same height, what does that mean if you have masses on both pans?
Keep this in mind as we continue

29. The Law
The law of conservation of matter states that matter (mass) can neither be created nor destroyed. It can, however, can be rearranged.
In a chemical reaction, the mass of the reactants must equal the mass of the products.
HUH?

30. Thinking of the balance?
Everything must be equal!
Remember the lab we just did?
When matter goes through a physical or chemical change, the amount (or mass) of the substances that you begin with must equal the amount (or mass) of the substances that you end with.
The before and after must balance
Why, you ask?
It’s the Law!!!!
The Law of Conservation of Matter (Mass)
Matter can neither be created, nor destroyed.

31. Lab Activity Let’s take a minute to think
(Demo: Add Sugar to water – determine mass before adding)
Just think about this…what will the mass be when we put it back on the balance?
Look at the before and after data
What do you notice about the sugar and the water?
Were any laws broken?
Explain

32. Law of Conservation of Matter (Mass)
If the amount of matter (mass) was not the same before and after the change
(remember, it is the law),
you must offer an explanation as to why.