BSC 2085: Anatomy and Physiology Part 1 - Introduction to Chemistry

Lecture Overview

• Professor Mariah Evans
• Focus: Basic Chemistry
• Course Context: Necessary for understanding biochemistry in anatomy and physiology
• Elements, molecules, compounds, electrons, protons, neutrons, chemical reactions, and bonds

Chemistry Basics

Matter and Energy

• Matter: Occupies space and has mass
  • Examples: humans, water, computers
  • Forms: Solid, liquid, gas
• Weight: Mass + effects of gravity
• Energy: Ability to do work
  • Potential Energy: Stored, inactive energy
  • Kinetic Energy: Active, in motion
  • Law of Thermodynamics: Energy cannot be created or destroyed, only transformed

Forms of Energy

• Chemical Energy: Stored in chemical bonds, released during digestion
• Electrical Energy: Movement of charged particles (ions)
• Mechanical Energy: Directly involved in moving matter
  • Example: Digestive system muscle contractions
• Radiant/Electromagnetic Energy: Travels in waves (X-rays, UV rays)

Elements and Atoms

• Periodic Table: List of all known elements
• Atomic Structure:
  • Protons: Positive charge
  • Neutrons: Neutral
  • Electrons: Negative charge
• Atomic Symbol: Short form of element name (e.g., C, O, H, N)
• Atomic Number: Number of protons
• Atomic Mass: Number of protons + neutrons
• Isotopes: Variants with different neutron numbers
• Atomic Weight: Average mass of isotopes

Chemical Bonds

Types of Bonds

• Ionic Bonds: Attraction between oppositely charged ions
  • Example: Sodium (Na) and Chlorine (Cl) form NaCl (table salt)
• Covalent Bonds: Sharing of electrons
  • Polar: Unequal sharing, e.g., water (H2O)
  • Nonpolar: Equal sharing, e.g., carbon dioxide (CO2)
• Hydrogen Bonds: Weak attractions, important in water molecules

Mixtures and Solutions

• Mixtures: Physically intermixed, not chemically bonded
  • Solutions: Homogeneous
  • Colloids: Heterogeneous, do not settle out
  • Suspensions: Particles settle out over time
• Solvent and Solute: Solvent dissolves solute, e.g., water is a universal solvent

Chemical Reactions

• Synthesis Reactions: Anabolic, building up
• Decomposition Reactions: Catabolic, breaking down
• Exchange Reactions: Swap components
• Redox Reactions: Electron transfer (oxidation and reduction)

Factors Affecting Reaction Rates

• Temperature: Higher temp increases rate
• Concentration: More reactants increase rate
• Particle Size: Smaller particles increase rate

Enzymes

• Biological catalysts that speed up reactions
• Lower activation energy
• Specific to substrates

Organic Compounds

Carbohydrates

• Monosaccharides: Simple sugars (glucose, fructose, galactose)
• Disaccharides: Two monosaccharides (sucrose, maltose, lactose)
• Polysaccharides: Many sugars (starch, glycogen, cellulose)

Lipids

• Triglycerides: Energy storage, insulation, protection
• Phospholipids: Cell membrane structure
• Steroids: Cholesterol, hormones

Proteins

• Polymers of amino acids
• Structure levels (primary, secondary, tertiary, quaternary)
• Functions: Enzymes, structural support, transport

Nucleic Acids

• DNA: Double-stranded, genetic blueprint
• RNA: Single-stranded, protein synthesis

Conclusion

• Next lecture: Cells 1 & 2
• Exam review and preparation

Note: This is a condensed summary of the lecture material designed for study and revision purposes.