1. CHEMISTRY COMES ALIVE Chapter 2

2. Definition of Concepts Matter = anything that occupies space and has mass. SolidLiquidGas Energy = the ability to do work Potential energy Kinetic energy

3. COMPOSITION OF MATTER Matter is composed of elements, 92 of which occur naturally. Elements cannot be broken down or subdivided by ordinary chemical means. 98% of the body is composed of the elements CHNOPS

4. COMPOSITION OF MATTER Atoms = smallest indivisible unit of an element. Molecule = two or more atoms of the same element held together by chemical bonds Compounds = two or more atoms of different elements held together by chemical bonds.

5. ATOMIC STRUCTURE

6. PLANETARY MODELS

7. PERIODIC CHART

8. INERT ELEMENTS

9. ACTIVE ELEMENTS

10. RULES OF BONDING Atoms in the periodic chart are said to be neutral atoms = that is they have no charge because they possess the same number of protons (+) as electrons (-). Ions = charged particles because of uneven numbers of protons and electrons. –Cation = positively charged –Anion = negatively charged

11. IONIC BONDS

12. COVALENT BONDS

15. POLAR versus NON-POLAR

16. HYDROGEN BONDS

17. BIOLOGICALLY IMPORTANT COMPOUNDS Inorganic compounds = those that lack carbon such as water, salt, hydrochloric acid, etc. Organic compounds = those that contain carbon such as carbohydrates, lipids, proteins, etc.

18. INORGANIC COMPOUNDS Water is the most important biological inorganic compound. –Polar –High heat capacity –High heat of vaporization –Exhibits adhesion and cohesion –Liquid water is denser than solid water –Cushioning

19. INORGANIC COMPOUNDS Electrolytes = any substance that disassociates in solution to form ions that are able to conduct electrical currents. –Salts –Bases –Neutrals –Acids –Buffers

20. SALTS Electrolyte that disassociates to form two of the most notable ions in current conduction. NaClNa + + Cl -

21. ACIDS Release H+ ions Considered to be proton donors pH of less than 7.0 Example: HCl H + +Cl - HCl H + +Cl -

22. BASES Release OH- ions Considered to be proton acceptors pH greater than 7.0 Example: NaOHNa + +OH -

23. BUFFERS Buffers resist abrupt and large swings in pH of body fluids by releasing hydrogen ions when pH begins to rise and also binding hydrogen ions when pH begins to fall. HCl + NaHCO 3 H 2 CO 3 + NaCl NaOH + H 2 CO 3 NaHCO 3 + H 2 O

24. ORGANIC COMPOUNDS Organic compounds contain carbon units put together by covalent bonds. There are four types of organic compounds: –Carbohydrate –Lipid –Protein –Nucleic acid

25. CARBOHYDRATES

26. CARBOHYDRATES

27. CARBOHYDRATES

28. LIPIDS

29. LIPIDS

30. LIPIDS

31. PROTEINS

32. PROTEINS

33. PROTEINS

34. PROTEINS

35. NUCLEIC ACIDS