1. CHAPTER 2 The Chemistry of Living Things

2. Slide 2.1 “atom” means “can’t be cut” by Greeks 2500 years ago. Atoms, the smallest functional unit of an element, consist of: All Matter Consists of Elements Made of Atoms

3. Atoms are made of Protons: positive charge, in nucleus, are heavy, “p + ” Neutrons: no charge, in nucleus, are heavy, “n 0 ” Electrons: negative charge, outside nucleus “electron cloud”, very light (1/1840 of a proton or neutron), “e - ”

5. Charges in an Atom The + charge on a proton is equal to the - charge on an electron. Atoms are neutral (have no overall charge) Therefore, the # of protons = # electrons in an atom.

6. Slide 2.2 Atomic number – determines the identity of the atom. – It tells us the number of protons in the atom. – It also tells us the number of electrons (b/c an atom is neutral in charge.) – Ex: atomic number of carbon, C = 6 – Question: how many protons? How many electrons? How many neutrons?

7. Isotopes The number of neutrons can vary from atom to atom in an element. Atoms of the same element w/different #s of neutrons are called ISOTOPES. In order to know how many neutrons in an atom you must be told. The mass number tells you how much mass the atom has. – Since p + and n 0 are the heavy parts, – mass # = # of p + ’s + n 0 ’s.

8. QUESTION: If the mass number of a carbon atom is 14, How many protons? How many electrons? How many neutrons? LET’S PRACTICE! – Whiteboard – Marker – Paper towel

9. Atomic Mass Units Atoms are weighed in a.m.u. 1 a.m.u. is based on the mass of a Carbon-12 atom. – it has 6 p+ and 6 n 0, – 1 a.m.u = 1/12 the mass of a carbon-12 atom.

10. IONS Electrons are in constant motion around the nucleus. e-s in the highest occupied level are called valence e-s. Some atoms lose or gain electrons in their valence level.

11. IONS When they do this, they get a charge. – If you lose an electron, the ion has a ___ charge – If you gain an electron, the ion has a ___ charge

12. ATOM v. ION ATOM – has no charge ION- has a charge (b/c e-s have been lost OR gained)

13. Slide 2.3. BONDING: Atoms Combine to Form Molecules Atoms want a stable arrangement For most atoms this is 8 e-s in the valence level (for small guys, it’s 2 in the valence) There are 2 ways to get the e-’s you need. Share Gain/lose

14. Table 2.1 Slide 2.4 Three Types of Chemical Bonds

16. Written NaCl NOT Na-Cl Ionic Bonds

17. Elements of Living Organisms Table 2.2 Slide 2.5

18. Life Depends on Water Water molecules are polar (they have slight electrical charges, like little magnets) o Biological solvent-ex: K+ for muscle contraction o Hydrogen bonds make it expand when frozen (animals in lakes can survive winter) o Water is liquid at body temperature o Water can absorb and hold heat energy o Water helps regulate body temperature Slide 2.6

19. Hydrogen bonds (dotted lines) a.k.a. van der Waals forces Oxygen slightly –ve charge Hydrogen slightly +ve

20. Properties of Water (b/c of hydrogen bonding) Cohesion- attraction between molecules of the same substance. (water-water attraction) Examples – Drops of water – Surface tension (Fig 2-8 p 41 of text)

21. Properties of Water (b/c of hydrogen bonding) Adhesion-attraction btwn molecules of different substances (water-other substance attraction) Examples – Capillary action-water drawn up a tube – “Meniscus”= the curve shape water has when in a tube

22. Water forms Important Mixtures Solutions when a substance dissolves in water Ex: Salt-water. NaCl is pulled apart into IONS by the water.

23. Figure 2.8 Slide 2.8 Water Keeps Ions in Solution

24. Water forms Important Mixtures (cont.) Suspensions Material does NOT dissolve, but separates into small pieces that remain floating Ex: blood w/red blood cells

25. ACIDS & BASES Water can form ions too! H 2 O  H + + OH - When by itself, water makes equal amounts of H + + OH -

26. ACIDS & BASES (cont.) Some things cause water to release many H+ ions. These are acids. Some things cause water to release many OH- ions. These are bases.bases pH is a measure of the H + concentration in a solution.

27. Figure 2.10 Slide 2.10 The pH Scale

28. BUFFERS (DON’T WRITE THIS) Remember homeostasis? WRITE THIS: All living things need to maintain a stable pH. – Humans need a pH between 6.5 & 7.5 – Otherwise, chemical reactions get messed up. They do this through buffers: weak acids or bases that prevent sharp, sudden changes in pH – Ex: ______ for an upset stomach. It absorbs extra H+ ions.

29. (Section 3): Carbon “Organic” Compounds Why is carbon so special? Carbon has 4 valence electrons, Allows it to bond to many other things at once. Pix of organic compounds important to living things Pix of organic compounds important to living things

30. Carbon, the building block of living things: Is 18% of human body by weight Forms four covalent bonds Can form single or double bonds Can build micro- or macromolecules (big chains) Slide 2.11 Section 3: Carbon (Organic) Compounds of Living Organisms

31. Figure 2.12 Slide 2.12 Carbon Can Bond in Many Ways

32. Figure 2.14 Slide 2.15 1: Carbohydrates MADE OF: C, H, O FUNCTION: energy & structure

33. 1. Sugars: short chains of Monosaccharides- 1 sugar ring Ex: glucose, galactose Disaccharides-2 attached sugar rings Ex: sucrose, fructose, lactose 2. Polysaccharides: thousands of monosaccharides joined in chains and branches Starch: made in plants; stores energy Glycogen: made in animals; stores energy Cellulose: undigestible polysaccharide made in plants for structural support Slide 2.16 Types of Carbohydrates

35. Lipids: Insoluble in Water TYPES OF LIPIDS Triglycerides: energy storage molecules – Fatty acids: saturated and unsaturated Phospholipids: cell membranes Steroids: carbon-based ring structures – Cholesterol: used in making estrogen and testosterone Slide 2.17 2: Lipids Made of: C,H,(O) Function: energy storage, waterproof coverings

38. Unsaturated triglyceride

39. Steroids (type of lipid)

40. Made of: C,H, O, N Function: building materials, enzymes Structure Made of monomers called amino acids The instructions for building proteins are in DNA Slide 2.18 Proteins: Complex Structures Contructed of Amino Acids

45. Hemoglobin (4 protein strands held together)

46. Enzyme Function Enzymes: – are proteins – function as catalysts (something that speeds up chem rxns) – facilitate chemical reactions Lower the activation energy (energy required to start a rxn.) The function of an enzyme is dependent on: – temperature – pH – ion concentration – presence of inhibitors Slide 2.19

47. Enzyme Action

48. Structure and Function of Nucleic Acids Functions – Store genetic information – Provide information used in making proteins Structure – Nucleotides consist of a phosphate group, a sugar, and a nitrogenous base – DNA structure is a double helix: two associated strands of nucleic acids – RNA is a single-stranded molecule Slide 2.20

49. Structure of DNA and RNA DNA: double-stranded – Sugar: deoxyribose – Nitrogenous bases: adenine, thymine, cytosine, guanine – Pairing: adenine-thymine and cytosine-guanine RNA: single-stranded – Sugar: ribose – Nitrogenous bases: adenine, uracil, cytosine, guanine – Pairing: adenine-uracil, cytosine-guanine Slide 2.21.

50. DNA nucleotides

52. RNA structure

53. Figure 2.25 Slide 2.22 Copyright © 2001 Benjamin Cummings, an imprint of Addison Wesley Longman, Inc. Structure and Function of Adenosine Triphosphate (ATP)