1. Chapter 2 Biochemistry

2. Matter The “stuff” of the universe Anything that has mass and takes up space States of Matter Solid: has definite shape and volume Liquid: has definite volume but the shape is changeable. Gas: has a changeable shape and volume

4. Energy The capacity to do work (put energy into motion) Types of energy –Kinetic: energy in action (moving) –Potential: energy of position: stored (inactive or at rest) –Chemical: stored in the bonds of chemical substances

5. Types of Energy Continued –Electrical: results from the movement of charged particles –Mechanical: directly involved in moving matter –Radiant or electromagnetic: energy traveling in waves (visible light, ultraviolet light, and X-rays)

6. Law of Conservation of Energy This law states that energy is neither created nor destroyed it can only change its form. Energy is easily changed from one form to another During this conversion some energy may be lost in the form of HEAT.

7. Composition of Matter Elements: unique substances that cannot be broken down by chemical means Atoms: more or less identical building blocks for each element Atomic Symbol: one or two – letter chemical shorthand for each element

8. Properties of Elements Each element has unique physical and chemical properties Physical Properties: Those detected with our senses, (touch, smell, look, etc.) Chemical Properties: pertain to the way atoms interact with one another (burn, Explosive)

9. Elements of the Human Body Oxygen (O) 65% Carbon (C) 18.5% Hydrogen (H) 9.5% Nitrogen (N) 3.2 These all make up 96% of the body

10. Lesser Element Calcium (Ca) 1.5% Phosphorus (P) 1.0% Potassium (K).4% Sulfur (S).3% Sodium (Na).2% Chlorine (CL).2% Magnesium (Mg).1% Iodine (I).1% Iron (Fe).1% These elements make up 3% of the body

11. Trace Elements Trace elements make up less than.01% of the body. These elements are required in minute amounts, and are found as part of enzymes. Cr, Co, Cu, F, Mn, Mo, Se, Si, Sn, V, Zn

12. Atomic Structure The nucleus consists of neutrons and protons Neutrons: have no charge and a mass of one atomic mass unit (amu) Protons: have a positive charge and a mass of (1 amu) Electron are found orbiting the nucleus Electrons: have a negative charge and 1/2000 the mass of a proton (0 amu)

13. Models of Atoms Planetary Model: electrons move around the nucleus in fixed, circular orbits Orbital Model; regions around the nucleus in which electrons are most likely to be found

14. Models of Atoms

15. Identification of Elements Atomic number: equal to the number of protons Mass number: equal to the mass of protons and neutrons Atomic weight: average of the mass numbers of all isotopes Isotopes: atoms with the same number of protons but a different number of neutrons Radioisotopes: atoms that undergo spontaneous decay called radioactivity

16. Identification of Isotopes

17. Molecules and Compounds Molecules: two or more atoms held together by chemical bond. Compound: two or more different kinds of atoms chemically bonded together

18. Molecules and Compounds

19. Mixtures and Solutions Mixtures: two or more components physically intermixed (not chemically bonded ) Solution: homogeneous mixtures of components –Solvent: substance present in greatest amount the one that does the dissolving –Solute: substances present in smaller amounts the one that is dissolved

20. Mixture Solutions

21. Colloids and Suspensions Colloids (emulsions): heterogeneous mixtures whose solutes do not settle out ie: Blood Suspensions: heterogeneous mixture with visible solutes that tend to settle out

22. Colloids

23. Suspension

24. Chemical Bonds Electron shells, or energy levels, surround the nucleus of an atom Bonds are formed using electrons in the outermost energy level Valence shell : outermost energy level containing chemically active electrons Octet rule: except for the first shell which is full with two electrons, atoms interact in a manner to have eight electrons in their valence shell

25. Chemically Inert Elements Inert elements have their outermost energy level fully occupied by electrons

26. Chemically Reactive Elements Reactive elements do not have their outermost energy level fully occupied by electrons

27. Types of Chemical Bonds Ionic- donating of electrons Covalent- sharing of electrons Hydrogen- hydrogen bonded to selected elements

28. Ionic Bonds Ions are charged atoms resulting from the gaining or losing of an electron –Anion have gained one or more electrons –Cations have lost one or more electrons

29. Formation of Ionic Bond Ionic bonds form between atoms by transferring one or more electrons Ionic compounds form crystals instead of individual molecules Example: NaCl (sodium chloride)

30. Ionic Bond

31. Covalent Bond Covalent Bonds are formed by the sharing of two or more electrons Electron sharing produces molecules

32. Covalent Bond

33. Hydrogen Bonds Too weak to bind atoms together Common in dipoles such as water Responsible for surface tension of water Important as intermolecular bonds, giving the molecule a three- dimensional shape

34. Hydrogen Bonds

35. Patterns of Chemical Reactions Combination reactions: Synthesis reaction which always involve bond formation Synthesis means to produce A + B AB

37. Decomposition Reaction Decomposition reaction: Molecules are broken down into smaller molecules AB A +B

38. Decomposition Reaction

39. Exchange Reaction Exchange Reaction involves both synthesis and decomposition reaction During this reaction a switch is made between molecule parts AB + C AC + B and AB + CD AD +CB This reaction occurs when ATP reacts with glucose and transfers its end phosphate group to glucose, forming glucose- phosphate a

40. Exchange Reaction

41. Factors Influencing Rate of Chemical Reaction Temperature: chemical reaction proceed quicker at higher temperature Particle size: the smaller the particle the faster the chemical reaction Concentration: higher reacting particle concentrations produce faster reactions Catalyst: increase the rate of reaction without being chemically changed Enzyme: biological catalyst

42. Biochemistry Organic compounds Contain carbon, are covalently bonded, and are often large Carbohydrates, lipids, proteins, DNA, RNA, Nucleic Acids

43. Inorganic Inorganic compounds Do not contain carbon Water, salts, and many acids and bases

44. Organic Compounds

45. Inorganic Compounds Properties of Water High heat capacity: absorbs and releases large amounts of heat before changing temperature High heat of vaporization: changing from liquid to a gas requires large amount of heat Polar solvent properties: dissolves ionic substances, forms hydration layers around large charged molecules, and serves as the body’s major transport median

46. Properties of Water Reactivity: is an important part of hydrolysis and dehydration synthesis reaction Cushioning: resilient cushion around certain body organs

47. Salts Inorganic compounds Contain cations other than H + and anions other than OH - Electrolytes- they conduct electrical currents

48. Acids and Bases Acid release H + and are therefore proton donors HCl H + + Cl - Hydrochloric Acid Bases release OH - and are proton acceptors NaOH Na + + OH - Sodium hydroxide Acid releases H + ions in a solution Bases accepts H + ions in solution

49. Acid – Base Concentration pH Acidic solutions have higher H + concentration and, therefore, a lower pH Alkaline (Base) solution have a lower H + concentration and, therefore, a higher pH Neutral solutions have equal H + and OH - concentrations pH 7.0 distilled water

50. Acid – Base Concentration pH Acidic: pH 0 – 6.99 Basic: pH 7.01 – 14 Neutral: ph 7.00 Human blood and semen: 7.35 – 7.45

52. Buffers Systems that resist abrupt and large swings in the pH of body fluids Carbonic acid – bicarbonate system Carbonic acid dissociates, reversibly releasing bicarbonate ions and protons The chemical equilibrium between carbonic acid and bicarbonate resists pH changes in the blood.

53. Organic Compound Carbon Central Element Molecules unique to living systems contain carbon and hence are organic compound They include: Carbohydrates Lipids Protein Nucleic Acid

54. Carbohydrates Contain carbon, hydrogen, and oxygen Their major function is to supply a source of cellular food Main source of energy for your body Example: Monosaccharide, or simple sugar

55. Monosaccharide Glucose

56. Fructose

57. Galactose

58. Deoxyribose and Ribose

59. You also have disaccharides, or double sugars, as well as polysaccharides, or polymers, of simple sugars

60. Disaccharides

62. Lipids /Fats Contain C, H, and O, but the proportion of oxygen in lipids is less than in carbohydrates. Examples: Neutral Fats, or triglycerides (main fat) found in subcutaneous tissue and around organs Phospholipids found in cell membranes (phospholipid bilayer) Steroids; cholesterol, bile salts, vitamin D, sex hormones, adrenal cortical hormone

63. Function Fats are stored form of energy Insulation: maintain temperature for body organ Protection: cushion, shock absorbers Fat –soluble vitamins: vitamin A, D, E, and K

64. Amino Acids Building blocks of protein, containing an amino group and a carboxyl group Amino group NH 2 Carboxyl groups COOH 20 amino acids when combined in different combinations to form between 20 - 30 thousand different proteins

67. Protein Macromolecules composed of combinations of 20 types of amino acids bound together with peptide bonds

68. Fibrous and Globular Protein Fibrous protein Extended and strand – like Examples: Keratin, elastin, collagen, and certain contractile fibers (Keratin: skin epidermis, hair, nails) Globular protein Examples: antibodies (helps fight off infection), hormones, and enzymes

69. Protein Denaturation Reversible unfolding of proteins due to drops in pH and/ or increase in temperature Irreversibly denatured proteins cannot refold and are formed by extreme pH or temperature changes Denatured: –verb (used with object),-tured, - tur·ing. 1. to deprive (something) of its natural character, properties, etc. Biochemistry: to treat (a protein or the like) by chemical or physical means so as to alter its original state.

70. Characteristics of Enzymes Most are globular proteins that act as biological catalysts Holoenzymes consist of an apoenzyme (protein) and a cofactor (usually an ion) Enzymes are chemically specific

71. Characteristics of Enzymes Frequently named for the type of reaction they catalyze Enzymes names usually end in –ase Lower activation energy Examples of enzymes: amylase, lipase, hydrolase

72. Mechanism of Enzyme Action Enzyme binds with substrate Product is formed at a lower activation energy Product is released

73. Nucleic Acids Composed of carbon, oxygen, hydrogen, nitrogen, and phosphorus Their structural unit, the nucleotide, is composed of N – containing base, pentose sugar, and a phosphate group Five nitrogen bases contribute to nucleotide structure : adenine (A), guanine (G), cytosine(C), thymine (T), uracil (U)