1. I. Levels of Biological Organization
Smaller & simpler Subatomic particles (n, p, e)
Atoms
Molecules
Organelles
Cell
Tissues
Organs
Organ Systems
Organism
Population
Communities
Larger & more complex Ecosystem

2. Chemistry Review & Biochemistry

3. II. Introduction
A. But wait…isn’t this Biology? Yes, but we need to understand the basic structure of atoms, because atoms make up molecules.

4. B. Matter anything that has mass and takes up space
1. All matter is made out of the 115 or so elements, which are listed on the Periodic Table (PT)
2. Elements cannot be broken down into a substance with a different chemical or physical property, unlike molecules.
a. Example: water (H20) can be broken down into the elements hydrogen and oxygen. However, hydrogen and oxygen have totally different properties than water.

5. II. Atom smallest particle of an element that keeps the properties of the element
A. Structure
1. 3 particles (they’re called subatomic particles)
Abbreviation
Location
Mass (amu)
Charge
Proton
p+ or +
Nucleus 1 +1
Neutron
n0 or 0
Electron
e- or -
Energy levels
1/1840 -1

6. 2. Bohr Model
Nucleus e- e- p+ n0
Energy Levels

7. 3. 99% of the mass of an atom is in the nucleus
4. Electrons (e-) are always moving
5. e- in the outermost energy level are called valence electrons (VE)
6. To figure out how atoms will bond, we care about e- (especially VE)

8. 7. Drawings of atoms (Shell Drawings)
a. Oxygen atom 8 p+, 8n0, 8e-

9. b. Nitrogen atom 7 protons, 7 neutrons, 7 electrons

10. c. Sulfur atom __ protons, __ neutrons, __ electrons
16+
16 0
2 e- 8 e- 6 e-

11. d. Hydrogen 1 p+, 0 n0, 1 e-

12. III. The Periodic Table Organization
A. The Periodic Table (PT) lists all of the elements in the world
B. There are about ? elements. This means that everything in the whole world is made out of these elements!
C. The Periodic Table is organized into groups and periods. We number groups across the top and the periods along the side. There are 18 groups and 7 periods (see PT).

14. D. Comparing Oxygen and Sulfur
1. Look at the shell diagrams for Oxygen and Sulfur. What do these atoms have in common?
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2. Locate these 2 atoms on the PT. You should notice that these 2 elements are in the same group. Elements in the same group have the same number of valence electrons. Elements within the same group will act the same chemically.

15. IV. Interpreting the Periodic Table
A. Information you can figure out by looking at the Periodic Table:
Atomic Number
Element Symbol
Element Name
Atomic Mass 17 Cl
Chlorine
35.453

16. B. The atomic mass tells you the mass of an atom in amu (# of protons + # of neutrons).
C. The number of protons (at. number) will equal the number of electrons in an atom
D. # of neutrons = atomic mass – atomic number
E. Draw a shell diagram for a Chlorine atom, using the information from above.

17. F. Draw a shell diagram for a Carbon atom (use the PT)

18. G. Dot Diagrams for Atoms
1. In a dot diagram, the dots represent the valence electrons.
2. There will not be more than 8 valence electrons.
3. Each unpaired electron is a bonding site.
4. Dot Placement:
X O Cl C
1 5
3 7

21. V. Molecules A. 2 basic types of bonds:
1. Ionic chemical bond formed when e- are lost or gained; forms ions= atoms with a charge
a. Salt (NaCl)

22. 2. Covalent chemical bond formed when e- are shared between atoms
a. Water (H20)

23. 3. Why would atoms want to bond?
a. In order to become more stable (HAPPY!)
b. An atom defines stability as having 8 valence electrons—just like the Nobel gases
c. Covalent bonds form molecules. In molecules, atoms share e- to become stable.
d. Ionic bonds- atoms lose or gain e- to be just like the nearest Nobel gas

24. B. A closer look at water 1. Dot diagrams: H H O
2. Hydrogen always makes one bond (one unshared e-)
3. Oxygen always makes two bonds (2 unshared e-)
4. Carbon always makes four bonds (4 unshared e-)

25. C. Dot diagrams for some simple compounds
1. First draw the dot structures for the following atoms (remember: you will need to use the PT)
2. Next to each dot diagram, write the # of bonds that this atom will always make when it is a compound