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Anatomy & Physiology: Foundational Concepts and Chemistry for Life

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Chapter 1: Introduction to Anatomy & Physiology

Definitions and Relationships

  • Anatomy is the study of the structure of body parts and their relationships to one another.

  • Physiology is the study of the function of body parts and how they work to carry out life-sustaining activities.

  • Structure and Function Relationship: The structure of an organ or cell is closely related to its function. For example, the structure of a phospholipid allows it to interact with both water and fat, making it ideal for forming cell membranes.

  • Example: The heart's muscular walls (structure) enable it to pump blood (function).

Levels of Organization

  • Organization in the body proceeds from chemical level to cellular, tissue, organ, organ system, and organism.

  • Example: Chemical atoms combine to form molecules, which make up organelles within cells.

Fundamental Life Processes

  • Metabolism: All chemical reactions in the body, including catabolism (breaking down) and anabolism (building up).

  • Responsiveness: Ability to sense and respond to stimuli.

  • Movement: Includes motion of the whole body, organs, cells, and cell structures.

  • Growth: Increase in body size or cell number.

  • Reproduction: Formation of new cells or organisms.

Homeostasis

  • Definition: The maintenance of a stable internal environment.

  • Example: Regulation of body temperature and blood glucose levels.

  • Homeostasis is maintained by feedback systems.

Feedback Systems

  • Components: Receptor, control center, effector.

  • Negative Feedback: Reverses a change to keep conditions within normal limits (e.g., regulation of blood pressure).

  • Positive Feedback: Strengthens or reinforces a change (e.g., childbirth contractions).

  • Example Table:

Feedback Type

Direction of Response

Example

Negative

Opposes change

Body temperature regulation

Positive

Amplifies change

Blood clotting

  • Homeostatic Imbalances: Can lead to disorders, diseases, or death.

  • Signs vs. Symptoms: Signs are objective and measurable (e.g., fever), symptoms are subjective (e.g., pain).

Chapter 2: Chemistry for Anatomy & Physiology

Basic Chemical Concepts

  • Matter: Anything that occupies space and has mass.

  • Elements: Substances that cannot be broken down by ordinary chemical means.

  • Atoms: Smallest units of elements, composed of protons, neutrons, and electrons.

  • Chemical Symbols: Abbreviations for elements (e.g., H for hydrogen).

Atomic Structure

  • Protons: Positively charged particles in the nucleus.

  • Neutrons: Neutral particles in the nucleus.

  • Electrons: Negatively charged particles orbiting the nucleus.

  • Atomic Number: Number of protons in an atom.

  • Mass Number: Sum of protons and neutrons.

  • Isotopes: Atoms of the same element with different numbers of neutrons.

  • Radioactive Isotopes: Unstable isotopes that decay over time.

Chemical Bonds

  • Ionic Bonds: Formed by transfer of electrons from one atom to another, resulting in charged ions.

  • Covalent Bonds: Formed by sharing electrons between atoms. Can be single, double, or triple bonds.

  • Polar Covalent Bonds: Unequal sharing of electrons, leading to partial charges.

  • Hydrogen Bonds: Weak attractions between polar molecules, important in water and biological molecules.

Types of Chemical Reactions

  • Synthesis: Building larger molecules from smaller ones.

  • Decomposition: Breaking down molecules into smaller components.

  • Exchange: Rearrangement of parts between molecules.

  • Reversible Reactions: Can proceed in both directions.

Energy in Chemical Reactions

  • Forms of Energy: Potential and kinetic energy; chemical energy stored in bonds.

  • Law of Conservation of Energy: Energy cannot be created or destroyed, only transformed.

  • Activation Energy: Minimum energy required to start a reaction.

  • Endergonic vs. Exergonic Reactions: Endergonic absorb energy; exergonic release energy.

Water, Solutions, and pH

  • Properties of Water: High heat capacity, solvent abilities, cohesion, and adhesion.

  • Solution: Homogeneous mixture of solute dissolved in solvent.

  • pH Scale: Measures hydrogen ion concentration; ranges from 0 (acidic) to 14 (basic).

  • Acid: Releases hydrogen ions () in solution.

  • Base: Accepts hydrogen ions or releases hydroxide ions ().

  • Buffer: Helps maintain stable pH in the body.

Organic Molecules and Biochemistry

  • Carbon: Versatile element, forms four covalent bonds, backbone of organic molecules.

  • Monomers and Polymers: Monomers are building blocks; polymers are chains of monomers.

  • Dehydration Synthesis: Joins monomers by removing water.

  • Hydrolysis: Breaks polymers into monomers by adding water.

Macromolecules

  • Carbohydrates: Sugars and starches; provide energy.

  • Lipids: Fats, oils, and steroids; store energy and form cell membranes.

  • Proteins: Made of amino acids; perform structural, enzymatic, and regulatory functions.

  • Nucleic Acids: DNA and RNA; store and transmit genetic information.

Enzymes

  • Definition: Biological catalysts that speed up chemical reactions.

  • Structure: Most are proteins with specific active sites.

  • Function: Lower activation energy, highly specific, can be regulated or inhibited.

  • Denaturation: Loss of enzyme structure and function due to changes in temperature or pH.

ATP (Adenosine Triphosphate)

  • Structure: Composed of adenine, ribose, and three phosphate groups.

  • Function: Main energy currency of the cell.

  • ATP Hydrolysis: Releases energy for cellular processes.

  • Equation:

Additional info:

  • Some content was inferred and expanded for clarity and completeness, such as detailed definitions, examples, and the structure of feedback systems.

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