1. Biochemistry Chapter 2 Pages 24-60

2. Biochemistry Biochemistry combines organic and inorganic chemistry and their interactions in living organisms.

3. Biochemistry Organic chemistry revolves around the carbon atom and the seemingly endless number of compounds it can form.

4. Biochemistry Organic chemistry revolves around the carbon atom and the seemingly endless number of compounds it can form. Inorganic chemistry involves all the other elements and includes the salts, acids and water.

5. Biochemistry Water is the single most important inorganic compound making up 60 to 70% of all living matter.

6. Biochemistry What are some of water’s unique properties:

7. Biochemistry What are some of water’s unique properties: –High Heat Capacity

8. Biochemistry What are some of water’s unique properties: –High Heat Capacity Water must absorb large quantities of energy for the temperature to change. This value is illustrated in its high specific heat.

9. Biochemistry What are some of water’s unique properties: –High Heat Capacity Water must absorb large quantities of energy for the temperature to change. This value is illustrated in its high specific heat. –High Heat of Vaporization

10. Biochemistry What are some of water’s unique properties: –High Heat Capacity Water must absorb large quantities of energy for the temperature to change. This value is illustrated in its high specific heat. –High Heat of Vaporization Water must absorb large quantities of heat to change from the liquid to gas phase

11. Biochemistry What are some of water’s unique properties: –Polar Solvent

12. Biochemistry What are some of water’s unique properties: –Polar Solvent Water is considered to be the universal solvent and serves as the aqueous environment for all cellular activities.

13. Biochemistry What are some of water’s unique properties: –Polar Solvent Water is considered to be the universal solvent and serves as the aqueous environment for all cellular activities. –Reactivity

14. Biochemistry What are some of water’s unique properties: –Polar Solvent Water is considered to be the universal solvent and serves as the aqueous environment for all cellular activities. –Reactivity Water not only serves as a medium for reactions but participates in almost all reactions in the cell, such as the dehydration synthesis and hydrolysis reactions.

15. Biochemistry What is responsible for water’s unique properties?

16. Biochemistry What is responsible for water’s unique properties? Hydrogen Bonding

17. Biochemistry Hydrogen Bonding This is a weak attraction between a hydrogen on one water molecule and an oxygen on an adjacent water molecule. This results in water molecules “sticking” to each other.

18. Biochemistry

19. Hydrogen bonding is most evident with surface tension.

20. Biochemistry Salts are made up of a + ion (cation) and a – ion (anion).

21. Biochemistry Salts are made up of a + ion (cation) and a – ion (anion). –The cation is usually a metal ion such as Na +

22. Biochemistry Salts are made up of a + ion (cation) and a – ion (anion). –The cation is usually a metal ion such as Na +

23. Biochemistry Salts are made up of a + ion (cation) and a – ion (anion). –The cation is usually a metal ion such as Na + –The anion is either an nonmetal ion such as Cl - or a complex radical such as phosphate (PO 4 -3 )

24. Biochemistry All ions are classified as electrolytes which means they can conduct an electrical current. Electrolytes are important for nerve conduction, muscle contraction and cell membrane polarity.

25. Biochemistry

26. Electrolyte imbalances can lead to heart arrhythmias or muscle fatigue.

27. Biochemistry Acid & Bases are also electrolytes but are derived from water itself. –An acid has a proton or H + as its only cation in an aqueous solution.

28. Biochemistry Acid & Bases are also electrolytes but are derived from water itself. –An acid has a proton or H + as its only cation in an aqueous solution. –A base has a hydroxy anion or OH - as its only negative ion in an aqueous solution.

29. Biochemistry The strength of an acid or base is measured using the pH scale.

30. Biochemistry An acid and base react to form a slat and water. This is known as a neutralization reaction.

31. Biochemistry pH of the body is very important. The body goes to great lengths to maintain the body's pH at 7.45.

32. Biochemistry pH of the body is very important. The body goes to great lengths to maintain the body's pH at 7.45. Deviations from this can lead to potentially fatal acid base imbalances.

33. Biochemistry

35. Buffers regulate pH changes within a cell and organism to prevent large fluctuations in pH.

36. Biochemistry Buffers regulate pH changes within a cell and organism to prevent large fluctuations in pH. Important buffers include: »Carbonic acid----Bicarbonate system »Phosphoric acid----Phosphate system

37. Biochemistry

38. Review 1. What are the two branches of chemistry that make up biochemistry?

39. Review 1. What are the two branches of chemistry that make up biochemistry? 2. What is organic chemistry?

40. Review 1. What are the two branches of chemistry that make up biochemistry? 2. What is organic chemistry? 3. What is inorganic chemistry?

41. Review 1. What are the two branches of chemistry that make up biochemistry? 2. What is organic chemistry? 3. What is inorganic chemistry? 4. Why is responsible for water’s properties?

42. Review 5. What makes up a salt?

43. Review 5. What makes up a salt? 6. What is an acid?

44. Review 5. What makes up a salt? 6. What is an acid? 7. What is a base?

45. Review 5. What makes up a salt? 6. What is an acid? 7. What is a base? 8. What is pH?

46. Review 5. What makes up a salt? 6. What is an acid? 7. What is a base? 8. What is pH? 9. Why are buffers important?

47. At the Clinic It was determined that a patient was in acidosis. What does this mean, and would you treat the condition that would raise or lower the pH?

48. At the Clinic Carbon dioxide concentration influences blood pH in the following manner: High levels of CO 2 increase the rate of formation of carbonic acid. If a patient has difficulty ventilating the lungs, as in emphysema would they be in acidosis or alkalosis?

49. At the Clinic Hugo, a patient with kidney disease, is unable to excrete sufficient amounts of hydrogen ions. Would he be hyperventilating or hypoventilating?