trial for biochem lec

• Biochemistry is sometimes called biological chemistry. It can be seen as a study of the components and composition of living things and how they come together to become life.
• Biochemistry


  The study of chemical processes that give rise to the complexity of life
• Scope of Biochemistry

  • Cell Biology
  • Molecular Biology
  • Molecular Genetics

  
• Three Principal Areas of Biochemistry

  • Structural Biochemistry
  • Metabolic Biochemistry
  • Genetic/Molecular Genetic Biochemistry

  
• Importance of Biochemistry

  • To understand life in molecular terms
  • Essential to all life sciences
  • Basis for health and diseases
  • Applied to medicine, dentistry, and veterinary medicine

  
• Applications of Biochemistry

  • Pharmacology
  • Physiology
  • Microbiology
  • Clinical Chemistry
  • Food Science - Nutrition
  • Agriculture
  • Toxicology
• Major Causes of Diseases

  • Physical agents
  • Chemical agents, including drugs
  • Biologic agents
  • Oxygen lack
  • Genetic disorders
  • Immunologic reactions
  • Nutritional imbalances
  • Endocrine imbalances
• Biochemistry is a description of life at the molecular level that includes a description of all the complex interrelated chemical changes within the cell called metabolism.
• Biochemistry involves a study of the molecules that make up all living things which are inherently interesting and help us better understand how organisms operate and therefore covers wide application.

  
• Biochemistry makes significant contributions to the fields of cell biology, physiology, immunology, microbiology, pharmacology, and toxicology, as well as the fields of inflammation, cell injury, and cancer.

  
• Water


  The most abundant molecule in cells, accounting for 70% or more of total cell mass
• Properties of Water

  • Polarity
  • Dipole
  • Molecular Interactions
  • Hydrogen Bonding
  • Hydrogen Bonds vs. Covalent and Ionic Bonds
  • Multiple Hydrogen Bonds
  • Cohesion, Adhesion and Surface Tension
  • Heat Capacity (heat storage)
  • Heat vs Temperature
  • Solubility

  
• Types of Solutes

  • Hydrophobic (Heterogenous)
  • Hydrophilic (Homogenous)
• A water balance must be maintained within the body. If the water loss significantly exceeds the intake, the body experiences dehydration. If the intake significantly exceeds the water loss, water builds up in the body and causes edema (fluid retention in tissues).

  
• Life's chemistry is tied to water! Life first evolved in water. All living things require water. The chemical reactions of our body occur in cells consisting of 70-95% water.
• Surface tension


  Caused by cohesion of water to itself and lack of adhesion to air
• Heat Capacity (heat storage)


  Water has an extremely high specific heat (amount of energy needed to raise the temperature)
• Heat Capacity (heat storage)


  Energy is stored in hydrogen bonds and molecular motion
• Heat Capacity (heat storage)


  Water moderates temperature
• Heat


  The total kinetic energy stored in an object (related to mass)
• Temperature


  The average kinetic energy (mass doesn't matter)
• Solubility


  Water dissolves a huge range of compounds (universal solvent) due to its molecular interactions

  
• Solution


  Evenly distributed mixture of 2 or more substances
• Solvent


  Dissolving substance (usually water)
• Solute


  Dissolved substance
• Hydrophobic (Heterogenous)


  • Hydrophobic substances do not form hydrogen bonds with water (oils, membranes, some proteins, etc)

  
• Hydrophilic (Homogenous)


  • Hydrophilic substances form hydrogen bonds with water (ions, sugars, cellulose, some proteins)

  
• Water


  A bent molecule, not linear. The hydrogen atoms have a partially positive charge; the oxygen atom has partially negative charge

  
• Water

  The charge distribution is due to the electronegativity difference between hydrogen and oxygen atoms (the attraction that an atom has for a bonding pair of electrons)

  
• Dipole-dipole force


  Intermolecular force in which the positive end of one molecule attracts the negative end of another molecule
• Hydrogen bonds


  Stronger-than-expected intermolecular forces (stronger than dipole-dipole forces) due to the very high electronegativity of oxygen combined with the fact that a hydrogen atom has only one electron

  
• Hydrogen bond


  The overall interaction of hydrogen atom bonded to either oxygen, nitrogen, or fluorine atoms with an oxygen, nitrogen or fluorine on another molecule (intermolecular) or the same molecule (intramolecular)

  
• Oxidation-reduction


  Important because they are the principal sources of energy on this planet, both natural or biological and artificial
• VDGEHROA

  When the Valence of an element Decreases that means it Gained Electrons/Hydrogens, it was Reduced and its compound is the Oxidizing Agent
• VILEHORA

  If the Valence of an element Increases that means it Lost Electron/Hydrogen, it was Oxidized and its compound acts as the Reducing Agent
• VanderWaalsForces / London Force

  • Weak force
  • Brought about by the fluctuating charge of the molecule due to electron distribution
  • Results in a temporary dipole causing induced polarization
  • Occurs in neutral, non-polar molecules
  • Increases with number of carbons, decreases with branching
• Dipole-dipole

  • Observed among partly ionic or polar molecules
  • Brought about by the interaction of two charges at both ends – one is slightly positive and the other is slightly negative
  • The greater the polarity, the stronger the dipole-dipole interaction
  • Induces polarization causing a positive charge to be negative
• Hydrogen Bonding


  • Strongest type of intermolecular force
  • Can either be intramolecular or intermolecular
  • Intermolecular H-bonding raises the boiling point of organic compounds
  • Intramolecular H-bonding lowers the boiling point
  • Occur between polar covalent molecules that possess a hydrogen bonded to an extremely electronegative element, specifically -N, O, and F

  
• Type of Force

  • Van der Waals
  • Dipole-Dipole
  • Hydrogen Bonding

  
• Relative Strength

  • Weak
  • Moderate
  • Strong