1. Basic chemistry Why learn it? Life depends on chemistry. If the first task of an architect is to understand building materials, then the first job of a biologist is to understand the chemistry of life. Where? Chapter 2 of your textbook

2. What? In order: 1.The basics: Atoms and Compounds (small) 2.Properties of Water 3.Macromolecules (big) 4.Enzymes: how they get things done I anticipate a number of lab activities, at least 1 project, and 1 vocab assignment. There will also be some small homework assignments.

3. Atoms Atoms – The basic unit of matter. Atoms are very small, made up of subatomic particles that are even smaller than the atom. Atoms are usually neutral, meaning they have no charge.

4. Protons Protons-  Have about the same mass as a neutron.  Have a positive charge  Contained in nucleus in the center of the atom Atoms have the same number of protons as electrons

5. Neutrons  Have about the same mass as a proton.  Have no charge = neutral Contained in nucleus in the center of the atom

6. Electrons  Negatively charged particle  Electrons are in constant motion  They move around the out side of the nucleus  Atoms have the same number of protons as electrons  Electrons are in orbits around the nucleus  The first orbit can hold 2 electrons The second orbit can hold up to eight electrons

7. Element Element-  is a substance composed of only one type of atom  more than 100 elements  Elements are represented by one or two letter symbol Sum of protons and neutrons in nucleus is called atomic mass

9. Periodic Table Atomic Number - Simply refers to the number of protons present in the atom. Element Symbol - This is the symbol that chemical formulas or equations use to indicate that certain element. Atomic Mass - The average mass of one atom of that element in amu's (Atomic Mass Units).

10. Compounds Chemical compounds  Substance formed by two or more elements  Formed in definite proportions  Properties of compound is different that the elements its formed by  Hydrogen and oxygen are gases at room temperature, when combined they form water, a liquid, at room temperature.

11. Bonding Chemical Bonds-  Atoms in a compound are held together by chemical bonds  Bonds are formed by the electrons in the area around the nucleus The electrons that are available to from bonds are called valence electrons

12. Bonding Covalent bonds  Strongest bonds  Shared electrons

13. Two electrons are shared Single covalent Bond

14.  Double covalent bond Four electrons are shared

15. Ions  Ions are formed by giving up or receiving an electron  Ions can have a positive charge or negative charge  If atom gives an electron it has a positive charge called a Cation If atom gains an electron it has an negative charge called an Anion

16. Ionic Bonds  Formed when one or more electrons are transferred from one atom to the other

17. Isotopes Isotopes-  Have different number of neutrons  They have the same number of electrons & protons All chemical properties such as bonding remain the same

18. Van der Waals Forces  Not all electrons are shared equally when bonds are formed  When sharing is unequal, one end of a molecule may be slightly more positive or negative than the other  A slight attraction between molecules can develop because of oppositely charged regions

19. Van der Waals forces