1. Course: Biological Chemistry I (CHEM 5360) Instructor: Gabriel Fenteany

2. Introduction

3. Periodic Table of Elements

6. Common Functional Groups in Biochemistry

11. Example of a Protein: An Immunoglobulin G Antibody

15. Cells

24. Noncovalent Bonding

43. Water and the Hydrophobic Effect

50. Acid-Base Chemistry

52. pH = -log[H+]
or more precisely
pH = -log[H3O+]

56. Henderson-Hasselbalch Equation
pH = pKa + log [A-]/[HA]

60. The Energetics of Life

61. Enthalpy (H) ∆H = ∆E + P∆V where ∆E = q - w
(internal energy change = heat absorbed by system from surroundings - work done by system on surroundings)
In most biochemical reactions, ∆H  ∆E  q

62. Entropy (S)

63. Gibbs Free Energy Change
∆G = ∆H - T∆S

69. Adenosine Triphosphate (ATP)
Thermodynamically unstable, but kinetically stable
Westheimer, F.H Why nature chose phosphates. Science 235,