1. Matter and Atoms
By Mr. M

2. Sizes
Macroscopic refers to large scales like the universe Microscopic refers to small scale that we cannot see with our eyes alone Submicroscopic is so small we cannot see it with a microscope or other tools

4. Break down Everything is made of matter and energy
The universe breaks down into galaxies that break down into solar systems that break down into celestial bodies that break down into environments/ecosystems that break down into creatures that break down into organs/tissues that break down into cells that break down into organelles that break down into chemical compounds that break down into atoms that break down into subatomic particles that break down into…

5. chemicals Chemicals can be broken down into different categories
The breakdown is based on how the chemicals can be separated and what they are made of

6. What are some physical properties?
Physical: can be observed without changing the identity of the substance
What are some physical properties?
color
melting and boiling point
odor
Some physical changes would be
boiling of a liquid
melting of a solid
dissolving a solid in a liquid to give a homogeneous mixture — a SOLUTION.
Tearing something in half
Painting something

7. Chemical Chemical properties are hard to see Reactivity Toxicity
Entropy
Enthalpy
Stability
Chemical change or chemical reaction — transformation of one or more atoms or molecules into one or more different molecules.
Burning
Nuclear fission

8. Signs of a chemical reaction
Heat
Light
Gas made
Precipitate (a new solid that appears)
Color change

9. Physical vs. Chemical physical Examples: melting point chemical
flammable
density
magnetic
tarnishes in air

10. Matter Flowchart MATTER yes no MIXTURE PURE SUBSTANCE no yes no yes
Can it be physically separated?
MIXTURE
PURE SUBSTANCE
Is the composition uniform? no
yes
Can it be chemically decomposed? no
yes
Homogeneous Mixture
(solution)
Heterogeneous Mixture
Compound
Element
Colloids
Suspensions

11. atoms Everything is made of atoms
Compounds are made of different atoms
Elements are only one type of atom
Thus for every element there is a different type of atom
All of the elements (atoms) are listed on the periodic table
Each element can have different forms

12. States of matter
We say there are three states of matter; however, ….

13. Kinetic Molecular theory

15. Definitions
_______ — have rigid shape, fixed volume. External shape can reflect the atomic and molecular arrangement.
Reasonably well understood.
_______ — have no fixed shape and may not fill a container completely.
Not well understood.
_______ — expand to fill their container.
Good theoretical understanding

16. History of atom
The idea of the atom starts in 460 BC, but the actual terminology and acceptance of the atom does not begin until late 1700s

18. Models
Plum pudding
Billiard Ball

20. Atom parts
The nucleus is the center of the atom and the parts of the nucleus are called nucleons
Protons and neutrons are in this area
The outer layers of the atom have been called orbits, rings, energy levels, shells, and orbitals.
Electrons are in this area
You are expected to master electrons, protons, and neutrons…. If you think that is too much just look at the real parts

22. How to determine the three parts of the atom
To find out how many electrons, protons, and neutrons an atom has you need a periodic table
There are two (sometimes three numbers if a charge is included) that you need in each periodic table tile block.

23. Protons
The atomic number is actually the number of protons. If you add or subtract a proton you change the atomic number and thus the element’s identity
Protons have a mass of one amu
Protons have a charge of positive 1

24. Neutrons
The mass number is actually the neutrons plus the protons, so you must take the mass and subtract the protons to find neutrons
Atomic mass – atomic number
Neutrons have a mass of 1 amu
Neutrons have no charge
Neutrons are the glue of the atom
Atoms are held together by “the strong force”, weak forces, and electromagnetic

25. Electrons
Electrons are assumed to be equal to protons unless a charge is given
If a charge is present you find electrons with
Atomic number – charge
Example: H+1 is hydrogen with a charge of plus 1 so it is 1 -1 = 0 electrons
H -1 has a charge of negative one so =2 electrons
H with no charge is just 1 electron
Mass of 0
Charge of negative 1

26. Ions An element of molecule with a charge
Charges are given in the upper right hand corner
H+ or H-1

27. Isotopes
Different masses of the same element: Hydrogen-1 (1H) or hydrogen-2 (2H) or hydrogen-3 (3H)
caused by different amounts of neutrons
Many are radioactive
The mass on the table is an average of the isotope masses based on the percent abundance of each isotope

28. Finding the average atomic mass
If hydrogen 1 is 99 percent of all hydrogen and hydrogen 2 is 1 percent of all hydrogen, find the average atomic mass
(.99 X 1 amu) + (.01 X 2 amu) = 1.01 amu