1. 2.1 Chemical Elements Chemistry as it related to biology

2. A. Matter What is matter?

3. B. Atomic Structure

4. The atomic mass of an atom: All atoms of an element have:

5. Interactive Periodic TableInteractive Periodic Table | Cartoon Periodic TableCartoon Periodic Table

6. Isotopes Definition:

7. Carbon 14 - Break it Down! Carbon- 12 is the most common form of carbon: Carbon 14:

8. A carbon with eight rather than six neutrons is unstable; it releases rays and subatomic particles and is a radioactive isotope. Sample Question: A 200 g sample of tashonian is left in a container, the half life of tashonian is 1 hour. How much of the sample will be left after 4 hours? Answer:

9. Quick Activity: The Half Life of Twizzlers http://www.biologycorner.com/worksheets/decay_twizzlers.html

10. Low levels of radiation such as radioactive iodine or glucose allow researchers to trace the location and activity of the atom in living tissues; therefore these isotopes are called tracers which are used in CAT scans

11. High levels of radiation can cause cancerous tissues and destroy cells; careful use of radiation in turn can sterilize products and kill cancer cells.

12. E. Electrons and Energy Electrons occupy an orbital at some level near or distant from the nucleus of the atom.

13. 4. When atoms absorb energy during photosynthesis, electrons are __________________________. 5. The innermost shell of an atom is complete with _____electrons; all other shells are complete with _____electrons.

14. DRAW IT! QUICK!! 1. Draw six protons in the nucleus of the atom. 2. Draw six neutrons in the nucleus of the atom. 3. Draw two electrons in the first energy level and label them with their charge. 4. Draw four electrons in the second energy level and label them with their charge. 5. What element is it!? __________ (the future of the human race depends on it!)

15. 2.2 Elements and Compounds A. Compounds When two or more different elements react or bond together, they form a compound (e.g., H2O). Electrons possess energy and bonds that exist between atoms in molecules contain energy. Glycine

16. B. Ionic Bonding

18. C. Covalent Bonding

19. Carbon has amazing bonding properties, as we will learn in the next chapter on BIOCHEMISTRY

20. D. Nonpolar and Polar Covalent Bonds 1. In nonpolar covalent bonds, sharing of electrons is ________. 2. With polar covalent bonds, the sharing of electrons is ________. a. In water molecule (H2O), sharing of electrons by oxygen and hydrogen is not equal; the oxygen atom with more protons dominates the H2O association. *The oxygen then assumes a small negative charge *

21. E. Hydrogen Bonding 1. Hydrogen bond definition: 2. Many hydrogen bonds taken together are relatively strong. 3. Hydrogen bonds between complex molecules of cells help maintain structure and function. Hydrogen bonds create surface tension.

23. Chemistry of Water A. First Cells Evolved in Water 1. All living things are 70.90% water. 2. Because water is a polar molecule, water molecules are hydrogen bonded to each other. 3. With hydrogen bonding, water is liquid between 0 C and 100 C which is critical for life.

24. B. Properties of Water 1.

25. 2. Water has a high heat of vaporization. a. Hydrogen bonds between water molecules require a large amount of heat to break. b. This property moderates earth's surface temperature; permits living systems to exist here. c. When animals sweat, evaporation of the sweat takes away body heat, thus cooling the animal.

26. 3. Water is ______________, facilitates chemical reactions both outside of and within living systems.. a. Water is a universal solvent because it : b. Ionized or polar molecules attracted to water are hydrophilic. c. Nonionized and nonpolar molecules that cannot attract water are hydrophobic. Solvents dissolve other substances (solutes) and do not lose their own properties. If we use a simple and easy example, we can get a handle on the idea. Take a glass of warm water, put a teaspoon of table salt in it, and stir it. The salt will dissolve in the water and "disappear" from view. The water is the solvent here, the salt is the solute in this example, and the resulting salt water is a solution that we created. It's that simple.

27. C. Acids and Bases 1. Covalently bonded water molecules ionize; the atoms dissociate into ions. 2. When water ionizes or dissociates, it releases a small (107 moles/liter) but equal number of H+ and OH ions; thus, its pH is neutral. 3. Water dissociates into hydrogen and hydroxide ions:

28. 4. Acid molecules dissociate in water, releasing hydrogen ions (H+) ions: HCl ¨ H+ + Cl-. 5. Bases are molecules that take up hydrogen ions or release hydroxide ions. NaOH ¨ Na+ + OH-. See also: Acid & Base ColoringAcid & Base Coloring

29. 6. The pH scale indicates : 1) One mole of water has 107 moles/liter of hydrogen ions; therefore, has neutral pH of 7. 2) Acid is a substance with pH less than 7; base is a substance with pH greater than 7. 3) As logarithmic scale, each lower unit has 10 times the amount of hydrogen ions as next higher pH unit; * Buffers keep pH steady and within normal limits in living organisms..