Fundamental Chemistry Concepts for Anatomy & Physiology

Study Guide - Smart Notes

Tailored notes based on your materials, expanded with key definitions, examples, and context.

Understanding matter and energy is essential for grasping the chemical basis of life processes in Anatomy & Physiology.

Matter: Anything that has mass and occupies space. Examples include solids, liquids, and gases.
Energy: The capacity to do work or cause change. Exists in various forms such as chemical, electrical, mechanical, and radiant energy.
Potential Energy: Stored energy due to position or structure (e.g., water held behind a dam).
Kinetic Energy: Energy of motion (e.g., water flowing down a river).

Kinetic or Potential Energy	Example
Potential energy	Food molecules in the stomach
Kinetic energy	The passage of food to the stomach
Potential energy	A stretched rubber band
Kinetic energy	The release of a stretched rubber band
Potential energy	Water held behind a dam
Kinetic energy	Water flowing down a river

Types of Energy:

Elements are the simplest forms of matter, and atoms are their basic building blocks.

Chemical element: A pure substance composed of only one type of atom.
Major elements in the body: Oxygen (O), Carbon (C), Hydrogen (H), Nitrogen (N) – together make up about 96% of body mass.

Subatomic particle	Located in the nucleus?	Charge	Mass (atomic mass units)
Proton	Yes	+1	1 amu
Neutron	Yes	0	1 amu
Electron	No	-1	Negligible

Example: Hydrogen has three isotopes: Protium (1 proton), Deuterium (1 proton, 1 neutron), Tritium (1 proton, 2 neutrons; radioactive).

Molecules and compounds are formed by atoms bonding together, while mixtures are physical combinations of substances.

Molecule: Two or more atoms bonded together (e.g., O2).
Compound: Molecule containing two or more different elements (e.g., H2O).
Mixture: Physical combination of substances without chemical bonding (e.g., air, salt water).

Type of mixture	Description or example
Solution	Solute particles are very small, do not settle out, and do not scatter light (e.g., salt water)
Colloid	Solute particles scatter light but do not settle out (e.g., cytosol in cells)
Suspension	Solute particles are very large, settle out, and may scatter light (e.g., sand in water)

Chemical bonds hold atoms together in molecules and compounds, affecting their properties and behavior.

Ionic bond: Attraction between oppositely charged ions (e.g., NaCl).
Covalent bond: Sharing of electron pairs between atoms (e.g., H2O).
Hydrogen bond: Weak attraction between a hydrogen atom and an electronegative atom (e.g., between water molecules).

Chemical bond type	Description or example
Hydrogen bond	Attraction between a hydrogen atom carrying a partial positive charge and an electronegative atom with a slightly negative charge
Covalent bond	Sharing of pairs of electrons
Ionic bond	Attraction between oppositely charged ions

Octet rule: Atoms tend to gain, lose, or share electrons to achieve eight electrons in their outer shell.
Polar covalent bond: Unequal sharing of electrons (e.g., H2O).
Nonpolar covalent bond: Equal sharing of electrons (e.g., O2).

Chemical reactions are processes in which chemical bonds are formed, broken, or rearranged.

Synthesis reaction: Atoms or molecules combine to form a larger, more complex molecule.
Decomposition reaction: A molecule is broken down into smaller molecules or atoms.
Exchange reaction: Parts of molecules are exchanged to form new molecules.
Oxidation-reduction (redox) reactions: Involve the transfer of electrons between molecules; important in energy production.

Type of chemical reaction	Example or Equation
Synthesis	Nucleotides are joined together to form a DNA molecule
Decomposition	Protein is broken down into amino acids
Exchange	The transfer of a phosphate group from creatine phosphate to ADP produces ATP and creatine

Irreversible reactions: Many chemical reactions in the body proceed in one direction due to removal of products or energy changes.

The rate of chemical reactions in the body is influenced by several factors.

Particle size: Smaller particles react faster.
Concentration: Higher concentration of reactants increases reaction rate.
Temperature: Higher temperature increases reaction rate.
Catalysts (enzymes): Biological catalysts that speed up reactions without being consumed.

Example: Cellular respiration equation:

Water and inorganic compounds are vital for maintaining homeostasis in the body.

Water: Polar molecule; excellent solvent; high heat capacity prevents sudden temperature changes.
Salt: Ionic compound that dissociates in water to form ions (electrolytes).
Electrolytes: Substances that conduct electricity in solution; essential for nerve and muscle function.

Ion	Function in the body
Na+ (sodium)	Nerve impulse transmission, muscle contraction
K+ (potassium)	Maintaining cell membrane potential
Ca2+ (calcium)	Muscle contraction, blood clotting

Acid: Substance that releases hydrogen ions (H+) in solution.
Base: Substance that accepts hydrogen ions or releases hydroxide ions (OH-).
Buffer: Substance that minimizes changes in pH.
pH scale: Measures concentration of H+ ions; ranges from 0 (acidic) to 14 (basic).

Example: If [H+] = mol/L, then pH = 7 (neutral).

*Additional info: Some explanations and examples have been expanded for clarity and completeness.*