Ch2 and 3 Chem Enzymes INK

Chemistry's Relevance: Understanding chemistry is fundamental as it plays a crucial role in biological processes, influencing health and illness.
Cholesterol Levels:
- Cholesterol levels and interpretation based on lab results:
  - Total Cholesterol: 168 (Goal: <200)
  - HDL (Good) Cholesterol: 46 (Goal: >40)
  - LDL (Bad) Cholesterol: 86 (Goal: <160)
  - Triglycerides: 182 (Goal: <150)
- Conclusion: Cholesterol readings are good.
- Electrolytes:
  - Sodium: 138 (Normal: 135-148)
  - Potassium: 4.8 (Normal: 3.5-5.5)
  - Chloride: 105 (Normal: 96-109)
  - CO2: 24, BUN: 18, Creatinine: 1.11, Glucose: 89, Calcium: 9.6 (All values normal)
  - Conclusion: kidney function is normal.
- White Blood Cells: 7.4 (Normal: 3.5-10)
  - Hemoglobin: 11.7 (Normal: 13-17)
  - Hematocrit: 34.1 (Normal: 38.5-52)
  - Platelets: 339 (Normal: 150-450)
  - Interpretation: Mild anemia noted.

Experiment:
- Activity conducted on Phet Build an Atom simulation.
- Partner discussions on findings and conclusions drawn from simulations.

Matter:
- Definition: Anything with mass that occupies space.
- Three Forms: Solid, Liquid, Gas.
Elements:
- Defined as substances that cannot be broken down into simpler substances.
- Atoms of Key Elements:
  - Four primary elements that constitute 96.5% of the human body weight:
    - Oxygen: 65.0%
    - Carbon: 18.6%
    - Hydrogen: 9.7%
    - Nitrogen: 3.2%
- Trace elements include Calcium, Phosphorus, Potassium, Sodium, and others.

Periodic Table Highlights:
- Provides atomic number and atomic mass, essential for identifying elements and their properties.
Atomic Structure Components:
- Subatomic Particles: Protons (+), Neutrons (0), Electrons (-).
- Atomic number reflects the number of protons.
- Atomic mass equals protons + neutrons.
- Example: 9 protons and 9 neutrons indicate the element Fluorine (Atomic number 9).

Types of Chemical Bonds:
- Ionic Bonds: Formed through transfer of electrons between atoms, resulting in charged ions (cations and anions).
- Covalent Bonds:
  - Atoms share one or more pairs of electrons.
  - Types of Covalent Bonds:
    - Single covalent bonds (e.g., H2O)
    - Double covalent bonds (e.g., CO2)
    - Polar vs. Nonpolar covalent bonds.

Properties:
- Weak attractions between a hydrogen atom and a more electronegative atom.
- Important for the structure of proteins and DNA.
- Hydrogen bonds contribute to the unique properties of water.

Unique Properties:
- Cohesion: Water molecules sticking together.
- Adhesion: Water molecules sticking to other substances.
- Surface Tension: Water’s ability to resist external forces.
- High Specific Heat and Heat of Vaporization: Important in temperature regulation.
- Solubility: Water as a universal solvent; polar substances dissolve well in it.

Electrolytes:
- Substances that dissociate into ions in solution, essential for bodily functions.
- Distinction between electrolytes (e.g., Na+, Cl-) and nonelectrolytes (e.g., pure water).
Chemical Reactions:
- Interaction of atoms, ions, and molecules: Reactants converting into products (A + B → AB).
- Types of Chemical Reactions:
  - Dehydration synthesis (Anabolism): Requires energy to form bonds.
  - Hydrolysis (Catabolism): Energy-releasing reactions that break down compounds.

pH Scale Overview:
- Range of pH values indicates the concentration of hydrogen ions in a solution.
- Acids (pH < 7) release H+, bases (pH > 7) release OH-.
- Blood pH is maintained around 7.35-7.45, crucial for metabolism and enzymatic functions.
- Buffers: Substances that help maintain pH stability in biological systems, example: bicarbonate buffer system.

Organic Compounds:
- Include carbohydrates, lipids, proteins, and nucleic acids.
- Enzymes: Proteins that catalyze reactions, with a unique active site that binds specific substrates.
- Denaturation can affect enzyme functionality.

A whimsical approach to remembering concepts related to atoms, their structure, and importance in chemistry.