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The webpage "Water Science Basics | Physics, Chemistry, Biology, Geology" from KnowYourH2O.com serves as an introductory hub for understanding foundational concepts in water science, emphasizing physics, inorganic chemistry, organic chemistry, and biology to interpret water quality issues within environmental science. It uses an informal, accessible style with anecdotes, simplifications, and occasional tangents to engage readers without requiring advanced knowledge. The content notes its limitations—it is not exhaustive, may include over-simplifications or errors, and invites feedback for improvements. Geology is mentioned in the title but not detailed in the sections. The page acts as a gateway with links to deeper subpages for each topic.

Article Sponsor: Jase Medical (Know Your H20 partner) 

Introduction and Structure

The introduction stresses that water quality interpretation requires reviewing basics from physics (atomic structure and radiation), chemistry (inorganic and organic compounds), and biology (organisms affecting water). It positions these as building blocks for broader environmental understanding, with informal narratives to maintain interest. The page outlines four main areas, with internal links to detailed subpages:

• Physics: Covers atomic basics, isotopes, radiation, and measurement.
• Inorganic Chemistry: Explains electron shells, bonds, polarity, and oxidation states.
• Organic Chemistry: Details carbon-based compounds, functional groups, and water contaminants.
• Biology: Discusses life classification, terminology, problem organisms, bacteria, and biological half-life.
  

Physics:

This section provides a refresher on physical sciences relevant to water, including atoms, isotopes, electromagnetic radiation, nuclear stability, radiation types, sources, effects, and measurement. Key applications include isotope tracing in groundwater and radiation in water supplies.

• Atoms and Elements: Atoms consist of electrons orbiting a nucleus of protons and neutrons. Atomic number (protons) defines the element (e.g., hydrogen: 1, carbon: 6). Atomic mass includes protons and neutrons. Isotopes vary in neutrons (e.g., hydrogen: protium ¹H, deuterium ²H, tritium ³H). Notation includes symbols like ²³⁸U. Water variants like D₂O (heavy water) are used as tracers or moderators.

• Electromagnetic Radiation: Electrons occupy discrete energy levels; excitation and drops emit radiation across the spectrum (radio waves to gamma rays). Emission/absorption spectra identify elements in water (e.g., via Atomic Absorption Spectrophotometer for metals like arsenic).
  
  
• Stability and Decay: Unstable isotopes decay via alpha (He nucleus ejection), beta (neutron to proton), or fission. Half-life measures decay time (e.g., tritium: 12.3 years; U-238: 4.5 billion years). Decay chains (U-238 to Pb-206) produce radon in water.

• Sources and Measurement: Natural sources include granite (U, Th); human-made from reactors. Units: Curie/Becquerel (activity), eV/Joules (energy), Roentgen (exposure), Rad/Gray (dose), REM/Sievert (equivalent dose accounting for biological effectiveness).

Example: Radon standards (4 pCi/L air), background radiation (~10 µR/h).

Inorganic Chemistry: Building on physics, this covers electron behavior, bonding, polarity, and oxidation, with water examples like rusting and solubility.

• Energy Levels/Electron Shells: Electrons fill subshells (s:2, p:6, d:10, f:14). Configurations determine bonding (e.g., oxygen: 1s²2s²2p⁴, needs 2 electrons). Noble gases (full shells) are inert.

• Electromagnetic Spectrum and Ionization: Absorption/emission of photons excites/ionizes atoms. Ionizing radiation (UV+) breaks bonds; fluorescence detects water substances.

• Ions, Bonds, and Polarity: Ions form by gaining/losing electrons (cations +, anions -). Ionic bonds (unequal sharing, e.g., NaCl); covalent (equal, e.g., CH₄). Water is polar (bent H-O-H, partial charges), enabling dissolution of salts and soaps.

• Oxidation States: Elements change states in redox reactions (e.g., Fe⁰ to Fe³⁺ in oxic water, causing stains). Rules for calculation (H:+1, O:-2); examples: H₂SO₄ (S:+6), CH₄ (C:-4). Table of common states (e.g., N: -3 to +5).
  

Organic Chemistry: Focuses on carbon compounds as water contaminants, with structures and nomenclature.

• Carbon Atom: Forms 4 bonds (tetrahedral); enables chains/rings. Distinguishes organic from inorganic.

• Hydrocarbons: Alkanes (e.g., methane CH₄, ethane C₂H₆); isomers (e.g., n-butane vs. isobutane). Alkenes (double bonds, e.g., ethylene C₂H₄).

• Functional Groups: Building blocks like –OH (hydroxyl), –CH₃ (methyl), –Cl (chloride). Halogenated methanes (e.g., CHCl₃ chloroform from chlorination).

• Ethers, Cyclics, Aromatics: MTBE (ether), cyclohexane (cyclic, e.g., Lindane insecticide), benzene (aromatic, modified to toluene, TNT).

• Organic Acids and Triazine: Carboxyl –COOH (e.g., acetic CH₃COOH, 2,4-D herbicide). Atrazine (triazine ring with Cl, amino groups).

Afterword notes emerging contaminants like 6PPD-quinone.

Biology: Covers life classification, terms, water problems, bacteria, and half-life.

• Classification: Six kingdoms (Animalia, Plantae, Fungi, Protista, Bacteria, Archaea); three domains (Eukaryota, Bacteria, Archaea). Hierarchy: Kingdom to Species (e.g., Homo sapiens).

• Terminology: Microorganism/microbe (invisible life); viruses (debated as alive, need hosts).

• Problem Causers: In water: bacteria (e.g., Legionella), protozoa, parasites, viruses. Algal blooms, mosquitoes.

• Bacteria: Shapes: coccus (round), bacillus (rod), vibrio (comma), spirillum/spirochete (spiral). Diseases: cholera (Vibrio), E. coli (some strains). Iron-reducers like Crenothrix cause stains/smells.

• Biological Half-Life: Time to eliminate half a substance (e.g., lead: 28-36 days in blood; iodine-131 effective: 5.5 days).

Overall, the resource educates on water science fundamentals, linking to subpages for depth, and highlights practical implications like contamination and treatment.

Glossary:  https://www.knowyourh2o.com/indoor-3/glossary

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