1. Atoms
Atom – smallest particle of an element that retains the characteristics of that element.
Element – the most simple chemical substance
Arranged in the periodic table
Columns and rows
Each element is identified via 1 letter or 2 letter abbreviation

2. Structure of an Atom 18 in 3rd shell Composed of a Nucleus
Contains Protons (p+)‏
Contains Neutrons (n0)‏
Protons + Neutrons = Atomic Mass
# protons = atomic number
Surrounded by Electrons (smaller particles) with negative (e-) charges.
Travel in regions called energy levels
2 in 1st shell
8 in 2nd shell
18 in 3rd shell

3. Crash course on the Periodic Table
Columns go up and down
Rows go left and right
Metals are left of the zigzag, Nonmetals to the right (except H)‏
Elements are uncharged, which means the number of protons MUST EQUAL the number of electrons
Column numbers tell you valence shell electron number (I.e. their bonding pattern)‏
Valence shell electrons are the outermost electrons on an atom.
Hydrogen 1, 1 valence e-
Oxygen 16, 6 valence e-
Carbon 14, 4 valence e-
Nitrogen 15, 5 valence e-
What element am I? _____________________atom am I?

5. Bonding - Ionic
Elements become “happy” when they have a full valence electron shell
2, 8, 18, etc
With elements only 1 or 2 electrons away from a full shell will lose or gain electrons.
Bonds between metals and nonmetals.
The charge between the elements keeps them attracted together (ions)‏
Compound – atoms held together by ionic bonds.

7. Common Bonds in Biology
Covalent Bonds are the most common in Biology.
Organic in biology means “made of Carbon.”
Isotopes – atoms of the same element that contain different numbers of neutrons.

8. Bonding - Covalent
When elements have about 4 electrons to gain or lose, they elect to share electrons!
Saves energy, easier to do than to steal!
Occurs between nonmetals.
Water uses covalent bonds.
Molecule – atoms held together by covalent bonds.

10. Properties of Water
Consists of 1 Oxygen atom and 2 Hydrogen atoms per 1 water molecule.
Water resists temperature change (insulator)‏
Has three phases:
Solid (ice), liquid, gas (vapor)‏
Carries substances via Osmosis.
Serves as material transportation
Blood, plant sap
Water makes up 70-95% of organisms.
Cycles through the kidneys and eliminated out of the body

11. Hydrogen Bonds Water – a polar molecule Because of its polarity…
Means it has a slightly positive (+) end and a slightly negative (-) end.
Because of its polarity…
Bonds to other water molecules through Hydrogen Bonds
- Holds large molecules like proteins together
Sticks together (+ and – attract) to create a cohesion via surface tension
Good solvent
Can adhere creep up tubes via capillary action.
- From ground to tops of trees.
- The meniscus in a graduated cylinder

12. Mixtures
A mixture is a combination of substances where both substances keep their original properties.
Physically mixed, not chemically mixed.
Solution – one or more substances (solutes) are distributed evenly in another substance (solvent) (water)‏
The more solute in a solvent, the higher the concentration.
Organisms need to maintain a certain concentration for life processes, called homeostasis.
Suspensions – mixtures of water and non dissolved particles
Example: Blood

13. pH Scale pH – a measure of how acidic or basic something is.
Use pH paper to test
Acidic range is 0-6
Acids form H+ ions in water
Example: Lemon (2)‏
Neutral is 7
Example: Pure water and blood (7)‏
Basic range 8-14
Bases form OH- ions in water
Example: Ammonia (12)‏
Buffers – weak acids and weak bases that react with strong acids or bases to prevent sudden changes in pH.
Neutralization reaction:
HCl + NaOH → HOH + NaCl