2. Chemistry For Life Matter - occupies space and has mass Elements - C,H,O,N,S,Fe,Ca,Na,Cl,K; make up matter and can’t be decomposed by ordinary chemical means Atoms Protons Neutrons Electrons

3. location weight charge Protons - nucleus 1 + Neutrons - nucleus 1 none Electrons - orbit 0 -

4. Atomic number - number of protons Atomic weight - protons + neutrons Ions - cations (+ ions that have lost an electron), anions (- ions that have gained an electron)

5. Isotope - same atomic number, different atomic weight - thus the number of neutrons differs Radioisotopes - break down and emit radiation that may be of clinical value

7. Covalent - sharing of a pair of electrons

9. Ionic - giving and taking electrons

10. Hydrogen - weak attraction between the positive part of one polar molecule and the negative part of another polar molecule; provides stability to large molecules

11. Atomic Combinations Molecules - stable combination of 2 or more elements Polar - electrons are unequally shared Nonpolar - electrons are equally shared Compounds - stable combination of 2 or more different kind of elements

12. Synthesis - anabolism - building molecules Decomposition - catabolism - breaking molecules downDecomposition - Exchange - buffers Reversible - goes in both directions depending on the conditions Oxy-Redox - leo the lion goes ger

13. Factors Influencing Reactions Temperature - rises increase speed of reactions to a point and vice versa Concentration - same as temp. Particle size - smaller ones act faster Catalysts - speed up reactions

14. Kinetic energy (being used) and potential energy (being stored) Chemical - in bonds Mechanical - muscles moving body Radiant - heat or light Electrical - flow of electrons in nerve impulses

15. Inorganic Compounds Lack carbons bonded to hydrogens Water - 60-80% of our weight Acids - release H ions when dissociating in water; tastes sour Bases - release OH ions when dissociating in water; tastes bitter

16. pH - a measure of how acidic or basic a substance is. It runs from 0, which is most acidic, to 14, which is most basic. 7 is neutral. Buffers - maintain the pH of a particular region by forming weaker acids or bases Salts - dissociates into cations and anions, which are not H or OH ions, when in water

17. Organic Compounds Compounds containing carbon bonded to hydrogen and oxygen

18. C, H, O Monosaccharides Glucose - blood sugar Fructose - the sweetest sugar Ribose - part of RNA Disaccharides Lactose - milk sugar

19. Sucrose - table sugar Maltose - in beer Polysaccharides Starch - our most abundant dietary carbohydrate Glycogen - our stored carbohydrate in our muscle and our liver Cellulose - a fiber that keeps us regular

20. C, H, O Fats and oils - glycerol + 3 fatty acids, a triglyceride; SFA, MUFA, PUFA Eicosanoids such as prostaglandins which influence the cells that produce them Phospholipids - build cell membranes Sterols - cholesterol, sex hormones Vitamins - A, D, E, K

21. C, H, O, N Amino acids - amino, carboxyl, hydrogen and radical around a C; they bind by peptide bonds to make polypeptides peptide Enzymes are all proteins – they catalyze reactions and often require coenzymes (vitamins or minerals); work like a lock and key

22. Other Organic Compounds Nucleic acids - DNA, RNA

23. ATP Structure

24. ATP - the energy compound Cyclic AMP - involved in hormone and neurotransmitter action