1. Atoms Atom- The smallest particle that can be called an element.
All matter is made up of atoms.
Made up of Protons(+), Neutrons, and Electrons (-)

2. Elements A pure substance
All atoms of an element have the same # of protons.
An element can not be broken into another substance
No two elements are the same in their properties

3. Element Examples Element Hydrogen Oxygen Nitrogen Carbon
Made up of Elements
Water
Air
Rock

4. Concentrations The most abundant element in: The Universe
Hydrogen (H) – 98%
In the Earths Crust
Oxygen- 47%
Silicon- 28%

5. Three Atomic Particles
Proton
a. Found in the Nucleus
b. Positively Charged (+)
c. Is the Atomic #/whole # which = identity (C=6)
2. Electron
a. Found in a cloud around the Nucleus
b. Negative Charge (-)
c. Same # as the Atomic Number (C = 6)
d. Can be lost or gained to create charged particles (ions).
e. Determine how elements will bond/react.

6. Neutrons
a. Found in the Nucleus with the Protons.
b. Neutral/No charge
c. Creates Isotopes which are different versions of the same element
(i.e.C14 vs. C12)
d. Can be calculated by subtracting the atomic # from the atomic mass.
Decimal # rounded - Whole # = # of neutrons
(i.e. C = 12 – 6 = 6 neutrons)

8. Properties of Matter
Physical Property- How a substance looks, feels, tastes, etc.
Ex. Sugar is white, sweet and granular.
Chemical Property- How a substance reacts to the world round it.
Ex. Sugar will turn to a black solid when mixed with Sulfuric Acid.

9. How Matter Changes
Conservation of Mass- Matter is neither created nor destroyed it just changes form.
Physical Change- A change in form that does not result in a new substance.
Ex. Sugar dissolves in water or any state change.
Chemical Change- A change/reaction that creates a new substance. An indication this is happening is when you see a color change, heat, light, smoke/gas and a new byproduct.
Ex. Oxidation (rust), Combustion (burning) or any Photosynthesis and Cellular Respiration.

10. Metals Physical Shininess Conduct Heat and Electricity Chemical
High Density (Heavy)
Ductile (Can be made into wire)
Malleable (Can be flattened)
All solids except Hg and H
Chemical
Tend to lose electrons to make positive ions.
Tend to bond with non-metals like oxygen and water.(Corrosion)

11. Non Metals Physical Not Shiny Do not conduct electricity or heat
Low Density (lighter)
Brittle (not ductile or malleable)
Can be gas, solid or liquid
Chemical
Tend to gain electrons to make negative ions
Tend to bond with metals

12. Alkali Metals First Column
Never found alone in nature because they are so reactive.
React violently with water due to only having 1 valence electron

13. Halogens Second to last Column Never found alone in nature
Highly reactive with Alkali Metals due to 7 electrons in the valence shell

14. Nobel Gases Last Column
Do not react with anything due to having 8 valence electrons
All gases

15. Valence Electrons Electrons in the outer most shell
Can be determined by the column # (group) that the element exists in.
All atoms trying to reach the magic 8 number of valence electrons. (Octet Rule)
Number of valence electrons determines how reactive an element is and what type of bonds they form.

16. Ionic Bonding
An ion is formed when an atom gives up an electron and becomes positive (+) or an atom gains an electron an becomes negative (–)
An ionic bond is formed when two opposite charged atoms come in contact and stick to together.
This the strongest of the chemical bonds

17. Covalent Bonding Bond created when two atoms share electrons
Not as strong as ionic bonds (easier formed and easier broken)
Carbon makes a lot of these

19. Electron Dot Model Determine the # of valence electrons
Draw the atomic symbol
Starting at “12 o’clock” place a dot at 12, 3, 6 and 9
If there are more than 4 valence electrons you then start pairing electrons at each spot.
Bonding sites are all non-paired electrons