1. B ASIC AND O RGANIC C HEMISTRY Chapters 2, 3, 4 and, 5

2. M ATTER * Anything that takes up space or has mass * it is made up of elements which are substances that cannot be broken down * elements can combine together and create compounds Element mattercompounds

3. E LEMENTS IN THE H UMAN B ODY Oxygen Carbon Hydrogen Nitrogen Calcium Phosphorus Potassium Sulfur Sodium Chlorine Magnesium

4. E LEMENTS HAVE PROPERTIES Element properties are controlled by the type of ATOM that it is. An atom is the smallest unit of matter that still retains the properties of the element. In an element there are protons neutrons and electrons The atomic mass of an atom is the protons plus neutrons The number is also the atomic number When the number of neutrons change in an atom the atoms is known as an isotope

5. E NERGY IN ATOMS Protons and electrons within an atom carry a charge : protons (+) electrons (-) Energy as a whole is the capacity to cause change Potential Energy: energy that matter possesses because of its location or structure Electrons give atoms potential energy Electrons are in electrons shells around the nucleus of the atom that gives them their energy level. Valence electrons are electrons that are on the outermost shell

6. C HEMICAL B ONDING AND R EACTIONS Chemical bond – an attraction between atoms that holds them close together. Strongest Covalent Ionic

7. C OVALENT B ONDS - The sharing of valence electrons between two or more atoms. - When a bond is made between two or more atoms it is a MOLECULE when there is one covalent bond (H 2 ) it is a single bond where there are two it is double bond (O 2 )

8. Electronegativity : is the attraction of an atom to form a covalent bond. TYPES OF COVALENT BONDS NON-POLAR COVALENT Electrons are shared equally POLAR COVALENT Electrons are not equally shared (CH 4 )

9. I ONIC B ONDS When the electron is completely taken from one atom and given to the other. (NaCl) This creates a charged atom or an ION. CATION is the ion with the positive charge or the atom that gives away the electron ANION is the ion with the negative charge or the atom that takes the electron The attraction that causes this and the resulting bond is an IONIC BOND The resulting compound is an IONIC COMPOUND or SALT

10. W EAK B ONDS Hydrogen Bonds: hydrogen covalently bonds to an electrongative atom Van der Waals interaction: weak attractions that occur in moving molecules

11. C HEMICAL R EACTION Making and or breaking of chemical bonds Reactants: starting material of the reaction Products: ending material of the reaction Chemical equilibrium: reactions that are occurring but at the same rate

12. P OLAR M OLECULES AND B ONDING Water is a polar molecule this means that it has opposite charges at opposite ends.

13. F OUR PROPERTIES OF W ATER Cohesion: a phenomenon that describes hydrogen bonding in water, pulls water into small vessels, responsible for water tension Moderation of temperature: water has a high specific heat, when hydrogen bonds form minimizes temperature Insulation of water: ice is less dense than liquid water and hydrogen bonding is organized Solvent : the polarity allows it to dissolve substances

14. W ATER AND P H Water is a neutral when it breaks down it creates H+ and OH- ions. Acid is an over abundance of H+ molecules (0-7) Base is an over abundance of OH- molecules (7- 14) Organisms need to maintain their own pH level

15. O RGANIC C HEMISTRY The study of carbon compounds Carbon bonding : remember that carbon has an atomic number of 6 which means it has 6 electrons in the electron orbital 4 of which are valence electrons

16. Hydrocarbon: organic molecules consisting only of carbon and hydrogen Isomers: compounds that have the same numbers of atoms of the same elements but different structures and different properties Structural isomers differ in covalent bonds Geometric isomers differ in spacing Enantiomer is a mirror image

17. F UNCTIONAL G ROUPS Components of organic molecules that are most commonly involved in chemical reactions ATP : adenosine triphosphate : ENERGY!

18. R ECALL MACROMOLECULES In Biology I should have done a lot with macro’s we are going to spend a short amount of time reviewing Remember the macro’s are: Carbohydrates Lipids Proteins Nucleic Acids

19. C ARBOHYDRATES Are for short energy storage in the cell and immediate source of fuel (MARATHON RUNNERS!) Polysaccharides include starch, glycogen and cellulose

20. L IPIDS Are for energy storage that is why it collects around organs and places in the body Saturated – maximum number of attached H Unsaturated – several double bonds to avoid H’s Cholesterols Steroids

21. P ROTEINS Used to build other structures in the body specifically amino acids Have varying structures and functions

22. N UCLEIC ACIDS Make up DNA and RNA which controls all functions of the body

23. E NZYMES