Anatomy & Physiology I Unit Two

1. Anatomy & Physiology I Unit Two

2. Basic Chemistry Definitions Matter – any thing that has mass and takes up space Therefore – all organisms as well as the visible or unseen physical world around them are made of matter

3. Basic Chemistry Definitions Atom – the smallest particle of an element that retains the characteristics of the element Element – a substance that cannot be changed into another substance

4. Atom Anatomy Electron – negative charge aaaaaaaaaaaaa Neutron – neutral charge Proton – positive charge

5. Periodic Chart Information Atomic Number (P#) 6 C 12.01 Chemical Symbol Atomic Mass (P# + N#)

6. Atom Examples

7. Basic Chemistry Definitions Isotopes –atoms of an element that have varying numbers of neutrons

8. Basic Chemistry Definitions Molecule – a particle made up of two or more atoms bonded together Diatomic molecule– two of the same type of atom bonded together such as O2 or N2

9. Basic Chemistry Definitions Compound – a substance made up of two or more elements bonded together Therefore – the smallest particle of a compound that retains its characteristics is a molecule (H2O or CO2)

10. Basic Chemistry Definitions Ion – an atom that has given up or gained electrons to achieve stability Cation – a positively charged ion that has given up electrons Anion – a negatively charged ion that has gained electrons

11. Basic Chemistry Definitions Electrolytes – salts that ionize in water and form solutions capable of conducting electricity Therefore – electrolytes (ions) carry a positive or negative charge

12. Basic Chemistry Definitions Free radical – a chemical particle carrying an odd number of electrons (O2-) Explanation – free radicals are formed from metabolic reactions, by radiation or chemicals

13. Basic Chemistry Definitions Free radical – a chemical particle carrying an odd number of electrons (O2-) Explanation – free radicals quickly combine with other molecules converting them into free radicals which will destroy more molecules

14. Basic Chemistry Definitions Antioxidant – a chemical that neutralizes free radicals Explanation – the body produces enzymes to convert free radicals and antioxidants are obtained through the diet

15. Ionic Bonds Bonds formed by the attraction between ions of opposite charges

16. Covalent Bonds Bonds formed by the sharing of electrons between atoms

17. Water - a covalently bonded, polar molecule aaaaaaaaaaaaa Molecules are said to be polar if they have slight opposite charges on either end

18. The slight attraction between the negative end of one molecule and the positive end of another results in a… aaaaaaaaaaaaaaaaa

19. The Relative Strengths of Chemical bonds Covalent bonds The undisputed champion!!! Ionic bonds The middleweight!! The weakest! Hydrogen bonds

20. Basic Chemistry Definitions Acid – a compound that releases hydrogen (H+) ions in solution Base – a compound that releases hydroxide ions (OH-) in solution

21. Basic Chemistry Definitions Salt – an ionic compound that does not contain H+ or OH-, obtained from an acid/base reaction Buffer – a chemical system that resists large changes in pH by taking up or giving off H+

22. Acid-Base Reaction Acid Base Salt Water HCl + KOH KCl + H2O Cl- K+ H+ OH-

23. Basic Chemistry Definitions pH – the measurement of the H+ concentration in a solution

24. pH – the measurement of the H+ concentration in solution

25. Buffers Remember – a buffer is a chemical system that resists large changes in pH by taking up or giving off H+ Therefore, a buffer is a homeostatic mechanism that helps to regulate the pH of blood and other body fluids

26. Buffers The pH range of blood is 7.35-7.45 It is extremely important that blood stay in this narrow range, making buffering systems necessary

27. Buffers The body has two types of buffering systems: < chemical < physiological A chemical buffer is a substance that removes or releases H+ from a system by binding to them or releasing them

28. Buffers A physiological buffer is a system that stabilizes pH by controlling the body’s output of acids, bases & CO2 The two systems that act as physiological buffers are the respiratory and urinary systems

29. Chemical Buffers The bicarbonate buffering system CO2 + H2O H2CO3 HCO3- + H+ The phosphate buffering system H2 PO4- HPO42-+ H+

30. Chemical Buffers The protein buffering system - COOH - COO-+ H+ OR - NH2 + H+- NH3+

31. Physiological Buffers The respiratory system is a two to three times stronger buffering system than chemical buffers The bicarbonate buffering system CO2 + H2O H2CO3 HCO3- + H+

32. Physiological Buffers The urinary system is most powerful buffering system in the body H+ are secreted from the blood into kidney tubules where they bind with HCO3-, HPO42- or ammonia

33. Physiological Buffers The bound and free H+ are then excreted in the urine The removal of free H+ is what makes this buffering system so powerful

34. Buffering Overview

35. Buffering Overview

36. Water - a covalently bonded, polar molecule aaaaaaaaaaaaa Molecules are said to be polar if they have slight opposite charges on either end

37. The slight attraction between the negative end of one molecule and the positive end of another results in a… aaaaaaaaaaaaaaaaa

38. Water aaaaa - Polarity leads to adhesion and cohesion • Adhesion and cohesion lead to capillary action and surface tension - High specific heat leads to temperature stability - High heat of vaporization leads to evaporative cooling

39. Water aaaaa - Spheres of hydration form electrostatic interactions, keeping ions from interacting with each other - This characteristic means water has a high degree of solvency and chemical reactivity

40. Water aaaaa - Water also ionizes into H+ and OH- which can be incorporated into other molecules or released from them

41. Water

42. Organic Chemistry The four types of organic compounds Carbohydrates Lipids Proteins Nucleic acids

43. Carbohydrates The general formula is CH2O The monomers are monosaccharides Functions: • Provide energy • Structural uses Examples: Plants - starch, cellulose Animals - glycogen, chitin

44. Lipids Functional group – COOH- (carboxyl) The monomers are fatty acids and alcohols Functions: • Storage energy • Structural uses • Regulation • Protection

45. Lipids Examples: • Fats (triglycerides) • Phospholipids • Steroids • Waxes

46. Lipids The two types of fatty acids • Saturated • Unsaturated

47. Proteins Two functional groups – COOH- (carboxyl) and NH2- (amine) The monomers are amino acids Functions: • Structural uses • Regulation • Protection • Provide energy

48. Proteins Examples: • Collagen • Hormones • Enzymes • Antibodies

49. Nucleic Acids The monomers are nucleotides Nitrogen base Functions: aaaaaaaaaaa • Heredity • Protein synthesis Phosphate group Pentose sugar

50. Nucleic Acids Examples: Single stranded with three forms – tRNA, rRNA, and mRNA Double stranded, double helix molecule • DNA • RNA