Lecture on Chemistry: Organic and Inorganic Compounds

Introduction

• Purpose of Lecture: To understand the basics of chemistry, focusing on organic and inorganic compounds, as a foundation for anatomy and physiology.
• Importance: Chemicals form cells, which form tissues, organs, systems, and organisms.
• Organic Compounds: Proteins, carbohydrates, and fats are essential for cell membranes.
• Inorganic Compounds: Water is a key component of the body.
• Metabolism: Consists of catabolism (breaking down) and anabolism (building up).

Chemistry Basics

• Matter: Anything with mass and takes up space.
  • Forms: Solid, liquid, gas.
  • Mass vs. Weight: Mass is the amount of matter; weight is gravity's force on mass.
• Elements: Cannot be split into simpler substances by ordinary means.
  • Chemical Symbols: E.g., Na for sodium.
  • Human Body Elements: 96% of body mass is composed of carbon (C), oxygen (O), hydrogen (H), and nitrogen (N).
  • Trace Elements: Include copper (Cu), selenium (Se), and zinc (Zn).

Cells and Antioxidants

• Cell Structure
  • Cytoplasm: Intracellular fluid.
  • Interstitial Fluid: Fluid between cells.
• Antioxidant System
  • Superoxide Dismutase (SOD): Protects cells from oxidation.
  • Mitochondrial Antioxidants: Manganese SOD protects mitochondria.
  • Other Antioxidants: Vitamin C, glutathione.

Atomic Structure

• Atoms: Smallest unit of matter with element properties.
  • Subatomic Particles: Protons, neutrons, electrons.
  • Electron Shells: Electron distribution around nucleus.
• Ions and Molecules
  • Ions: Atoms that have lost or gained electrons.
  • Molecules: Two or more atoms sharing electrons.
  • Compounds: Can be broken into simpler substances.

Chemical Bonds and Reactions

• Types of Bonds
  • Ionic Bonds: Losing or gaining electrons (e.g., NaCl).
  • Covalent Bonds: Sharing electrons (e.g., H2, O2).
  • Hydrogen Bonds: Attraction of oppositely charged molecules.
• Chemical Reactions
  • Synthesis: Combining elements to form larger molecules.
  • Decomposition: Breaking down into smaller components.
  • Exchange and Reversible Reactions: Reorganizing elements and reversible changes.
  • Oxidation and Reduction: Transfer of electrons (OIL RIG mnemonic).

Water and Solutions

• Properties of Water
  • Polar Molecule: Positive and negative poles.
  • Universal Solvent: Dissolves many substances.
  • Heat Capacity and Cohesion: Important for life and biochemical reactions.
• Solutions
  • Solvent and Solute: Water as solvent, substances dissolved are solutes.
  • Acids and Bases: Affect pH; acids donate H+, bases accept H+.

pH and Buffers

• pH Scale
  • Range: 0-14, 7 is neutral, below 7 is acidic, above 7 is basic.
  • Biological Importance: Blood pH (7.35-7.45), affects biochemical processes.
• Buffers
  • Function: Maintain pH balance in the body.

Conclusion

• The basics of chemistry and inorganic compounds have been covered, setting the stage for understanding organic compounds in the next lecture.