Biological Hazards in Outdoor Activities

Biological Hazards

• Ragweed, pollen, viruses, peanuts, bee stings: Examples of biological hazards.
• Camping biohazards: Include bee stings, deer ticks, toxic plants, bats, mouse droppings, and uncooked food.
• Bee stings: Can cause itching, allergic reactions.
• Deer ticks: Carry Lyme disease, causing body aches and fatigue, which is treatable with antibiotics.
• Toxic plants: Can cause injury or death.
• Bats: Can carry rabies.
• Mouse droppings: Can transmit hantavirus.
• Uncooked food: Can cause foodborne illnesses, such as E. coli or salmonella.

Biohazard Personal Protection Outdoors

• Clothing: Wear light-colored clothing, long pants, socks, and shoes.
• Tick Check: Check for ticks and use insect repellent.

Biohazards - Needles

• Locations: Can be found in schoolyards, parks, beaches, streets, and homes.
• Avoidance: Avoid contact with needles.

Sources of Biohazards

• People: A source of biohazards.
• Pets and wildlife: A source of biohazards.
• Insects: A source of biohazards.
• Food and water: Dirty food and water can be sources of biohazards.
• Needles: Dirty needles are a source of biohazards.

Infections – Spread

• Contaminated Materials: Infections spread when shared materials aren't properly cleaned.
• Airborne Infections: Eye infections are airborne and spread quickly.

Personal Hygiene - Sharing

• Avoid: Avoid sharing food, drinks, clothing, makeup, hairbrushes, etc.
• Handwashing: Always wash hands thoroughly after touching dirty or contaminated surfaces.

Chemical Hazards

• WHMIS: Workplace Hazardous Materials Information System.
• Purpose: To ensure awareness of health and safety hazards related to hazardous chemicals, and avoid unsafe use.
• Supplier Responsibility: Suppliers must provide labels and Material Safety Data Sheets (MSDS).
• Employer Responsibility: Employers must provide labels and train workers on WHMIS procedures.
• Worker Responsibility: Workers must inform employers of hazards.
• Information Sources: WHMIS information is provided through labels, MSDS, and instructional programs.

WHMIS Symbols

• 8 Distinctive Symbols: Compressed gas, flammable & explosive, oxidizing materials, poisonous & infectious, corrosive materials, dangerously reactive materials. (Infectious are divided into materials with immediate/serious toxic effects and other toxic effects).

Sustainability

• Definition: Resources that last for a long time.
• Sustainable Ecosystem: Natural, undisturbed areas. Characteristics are constant over time.
• Unsustainable Ecosystem: Unnatural, disturbed areas. Need care for survival.

Earth's Main Components

• Atmosphere: Layer of gases surrounding Earth. Contains water, carbon dioxide, ozone.
• Lithosphere: Solid outer layer (crust and upper mantle). Extends 100 km down. Includes soil.
• Hydrosphere: All water on Earth. Mostly saltwater oceans.
• Biosphere: Areas where life exists within the lithosphere, atmosphere, and hydrosphere.

The Sun

• Energy Distribution: 30% reflected, 44% heats surfaces, 25% evaporates water, 1% wind, 0.023% photosynthesis.

Trophic Levels

• 1st: Green plants (autotrophs).
• 2nd: Herbivores (e.g., bunnies, deer).
• 3rd: Carnivores (e.g., wolves, bears).

Food Chain Example

• Grass → grasshopper → frog → snake → hawk

Types of Organisms

• Autotroph: Makes its own food (e.g., plants).
• Heterotroph: Cannot make its own food. Includes herbivores, carnivores, and omnivores.

Chemical Formulas

• Photosynthesis: 6CO2 + 6H2O → C6H12O6 + 6O2
• Cellular Respiration: C6H12O6 + 6O2 → 6CO2 + 6H2O + ATP (heat)

Photosynthesis/Cellular Respiration

• Photosynthesis: Plants use sunlight to convert carbon dioxide and water into sugars and oxygen.
• Cellular Respiration: Organisms convert sugars and oxygen into carbon dioxide, water, and energy.

Food Webs/Energy Transfer

• Niche: Each species occupies a unique niche.
• Relationships: Feeding relationships are represented by food chains, food webs, and trophic levels.
• Energy Loss: Energy is continuously lost to the environment.
• Trophic Levels & Energy: Higher trophic levels have less available energy.
• Ecological Pyramids: Display energy, number, and biomass relationships.

Biogeochemical Cycles

• Cycling of Matter: Matter is cycled through ecosystems via biogeochemical cycles.
• Water Cycle: Water exists in all states during the water cycle.
• Carbon Cycle: Carbon moves between abiotic and biotic components via photosynthesis and cellular respiration.
• Nitrogen Cycle: Nitrogen is removed from the atmosphere by microorganisms, fixed, and returned by denitrifying bacteria.

Biotic/Abiotic Factors

• Population Limits: Many factors limit population sizes.
• Tolerance Ranges: Describe physical conditions where a species can survive.
• Ecosystem Factors: Ecosystem type is influenced by abiotic factors like light, water, and temperature.
• Species Interactions: Include competition, predation, mutualism, parasitism, and commensalism.
• Carrying Capacity: Maximum population size an ecosystem can sustain.

Major Terrestrial Ecosystems

• Biome Factors: Precipitation and temperature influence biome formation.
• Biome Characteristics: Distinct biotic and abiotic characteristics.
• Canadian Biomes: Tundra, boreal forest, grassland, temperate deciduous forest, mountain forest.
• Boreal Forest: Largest biome in Canada.

Aquatic Ecosystems

• Freshwater/Marine: Aquatic ecosystems are either freshwater or marine.
• Productivity: Most productive ecosystems are shallow, warm, nutrient-rich.
• Intertidal Zones: Abiotic conditions continuously alternate.
• Intertidal Species: Can survive varying abiotic conditions.

Ecosystem Products

• Examples: Maple syrup (maple trees), henna (plant extracts), waxes (carnauba palm leaves), aspirin (willow trees).

Ecosystem Services

• Protection: Ecosystems protect from physical threats (diseases, etc.).
• Regulation/Maintenance: Ecosystems maintain abiotic and biotic features.
• Cultural Services: Benefits from enjoying the environment.
• Products: Provide wood fiber, medicines, and food.

Equilibrium & Change

• Equilibrium: Most ecosystems are in a state of equilibrium.
• Stability: Equilibrium is maintained by stable abiotic conditions.

Ecological Succession

• Disturbances: Succession is initiated by disturbances (e.g., fire).
• Primary Succession: Occurs on soil or bare rock without prior life.
• Secondary Succession: Follows a disturbance but not total loss of life.

Species/Organisms

• Monoculture: Growing only one crop.
• Dominant Species: Affect ecosystem health.
• Indicator Species: Show changes in the environment (e.g., frogs).
• Biodiversity: Variety of animals and organisms in an environment.
• Speciation: Increase in biodiversity when one species splits into two or more.
• Extinction: Decline in biodiversity when a species disappears.
• Extinction Rates: Currently higher than speciation rates.
• Invasive Species: Non-native species with growing populations that harm the environment.
• Native/Non-native species: Native originate from the area, while non-native are introduced.

Impact of Invasive Species

• Ecological: Outcompeting native species, pollution.
• Economical: Costs from damage.
• Health: Transmission of viruses.
• Control Methods
• Chemical: Pesticides used on pests with economic value reducing crop damage but polluting air, water and soil
• Mechanical: Physical removal or barriers
• Pest/Pesticide: Pest = organism competing with or harming crops pesticide = kills pests
• Broad/Narrow Spectrum: Broad pesticide = toxic to a wide range of species Narrow pesticide = toxic to a limited number of species
• Herbicide: Pesticide that kills plants

Bioaccumulation/Bioamplification

• Bioaccumulation: Substances building up in organisms through consuming food.
• Bioamplification: Substances increasing as they move up a food chain.

Acid Precipitation

• Causes: Sulfur dioxide and nitrogen dioxide from industrial processes and fossil fuel burning.
• Effects: Species decline, nutrient depletion in soil, damaged vegetation and slower growth.

Waste & Water

• Oil Spills: Oil is toxic, slow to break down, and forms large slicks.
• Cleanup Methods: Skimming, burning, and dispersal agents to clean oil spills.

Plastics at Sea

• Persistence: Plastic does not degrade, lasting for hundreds/thousands of years.
• Production: Billions of tons produced annually; recycling is a small fraction.
• Garbage Patches: Massive plastic mats in the ocean, notably the North Pacific Garbage Patch.
• Impact: Fragments are ingested by fish and seabirds, causing blockage.

Endangered Species

• Extinction: Natural or human-caused elimination of a species.
• COSEWIC: Committee on the Status of Endangered Wildlife in Canada; assesses and designates endangered species.
• Human Causes: Habitat destruction, overhunting/fishing, animal products, pollution.

Particle Theory

• Nature of Matter: All matter is made of tiny particles with spaces between them.
• Substance Differences: Different substances have different types of particles.
• Motion: Particles are in constant, random motion.
• Temperature & Motion: Particles move faster at higher temperatures.
• Attraction: Particles attract each other.

Pure Substances/Mixtures

• Pure Substances: Made of only one type of particle (e.g., tap water).
• Mixtures: Made of two or more types of particles, and can be solid, liquid, or gaseous.

Mechanical Mixtures/Solutions

• Mechanical Mixtures: Mixtures in which different types of matter are easily distinguishable.
• Solutions: Uniform mixtures in which different particles are not visibly distinguishable.
• Clarity Distinction: Clear liquids/gases are solutions; murky mixtures are mechanical.
• Alloy: Solid solutions of two or more metals (e.g., solder).

Physical Properties

• Definition: Characteristics determined without altering composition.
• Observation & Measurement: Observed using senses and instruments.
• Qualitative Properties: Non-numerical characteristics (color, odor, texture).
• Quantitative Properties: Numerical characteristics (temperature, mass).
• Viscosity: Fluid resistance to flow.
• Physical Change: Change in form without changing the composition.
• Chemical Properties: Describe ability to undergo chemical changes.
• Chemical Change: Change in substances and formation of new substances.
• Evidence of Chemical Change: Color change, odor change, bubbling (gas production), formation of a solid, temperature or light change.
• Precipitate: Solid that separates from a solution.
• Characteristic Physical Properties: Unique characteristics that identify a substance.
• Density: Mass per unit volume.
• Melting Point: Temperature for solid to liquid state change.
• Freezing Point: Temperature for liquid to solid state change.
• Boiling Point: Temperature for liquid to gas state change.
• Water Density: Water in solid state (ice) is less dense than liquid water.

Matter

• Definition: Anything with mass and volume.
• Categories: Elements and compounds.
• Elements: Pure substances (e.g., iron, copper, carbon).
• Compounds: Two or more elements chemically joined (e.g., water, sugar).
• Elements vs. Compounds: Elements are made of only one type of atom; compounds are made of two or more different elements joined.
• Molecule: A unit of a compound made of two or more atoms.
• Mixtures: Combinations of two or more substances (elements/compounds).
• Heterogeneous Mixtures: Components are visible and can be separated. Includes mechanical mixtures and suspensions.
• Mechanical Mixtures: Easily separated components (e.g. granola bar).
• Suspensions: Small particles suspended in another substance (e.g. salad dressing).
• Homogeneous Mixtures: Components are blended and not distinguishable. Includes solutions (one substance dissolving into another).
• Solvent: Dissolving substance (e.g. water).
• Solute: Dissolved substance (e.g. sugar).
• Solution Clarity: A solution will appear clear; a mechanical mixture looks murky.

Density

• Definition: Mass per unit volume.

Table of Elements

• Element: Pure substance that cannot be broken down.
• Element Symbol: Abbreviation for an element.
• Compound: Pure substance made of two or more elements.
• Metal: Lustrous, malleable, ductile, conducts heat/electricity.
• Non-metal: Usually gas or dull solid; doesn't conduct heat/electricity.
• Metalloid: Has properties of both metals and nonmetals.
• Chemical Family: Column of elements with similar properties. (alkali metal, alkaline earth metal, halogen, noble gas)
• Period: Row on the periodic table.

Atomic Structure

• Atom: Smallest unit of an element.
• Electron: Negatively charged particle.
• Proton: Positively charged particle (in the nucleus).
• Neutron: Neutral particle (in the nucleus).
• Atomic Number: Number of protons in an atom.
• Mass Number: Number of protons + neutrons.
• Isotope: Atoms with the same number of protons but different numbers of neutrons.
• Atomic Mass: Mass of an atom in atomic mass units.
• Bohr-Rutherford Diagram: Simple drawing showing protons, neutrons, and electrons.

Bohr-Rutherford Diagrams

• Model of Atom: Depicts atomic components.
• Component Identification: Protons = atomic number; Neutrons = difference between mass number and atomic number; Electrons = number of protons (neutral atom).

History of the Atom

• Rutherford Experiment: Most particles passed through gold foil, some were deflected.
• Nucleus Idea: Small, dense, positive nucleus at the center of the atom.
• Empty Space: Most of an atom is empty space.
• Electron Cloud: Negatively charged electrons surround the nucleus.
• Proton Discovery: Rutherford credited with discovering protons.
• Neutron Discovery: Chadwick discovered neutrons.
• Bohr Model: Electrons orbit the nucleus, definite energy levels.
• Energy Level Transitions: Electrons absorb/release energy as light when they move between orbits.

Structure of Atoms

• Atom's Components: Extremely small nucleus with electrons surrounding it.

Patterns in the Periodic Table

• Chemical Families: Columns with similar properties.
• Periods: Rows on the table.
• Mendeleev's Organization: Elements grouped similarly.
• Predictions: Use of organization to predict undiscovered elements' attributes.

Charcoal/Diamond/Graphite

• Charcoal: Disorganized carbon structure; soft black solid.
• Graphite: Organized carbon structure; layered hexagons; good conductor.
• Diamond: Organized, interconnected carbon structure; extremely hard.
• Structural Differences: Impact hardness, density, and conductivity.

Molecular Elements/Compounds

• Diatomic Molecules: Seven elements naturally occurring as pairs of atoms (H2, N2, O2, F2, Cl2, Br2, I2).
• Chemical Formulas: Subscripts indicate the number of each atom.
• Varied Ratios: Same elements can form different compounds in different ratios.
• Ozone: Highly reactive; filters harmful UV light.

Ionic Compounds

• Non-molecular Compounds: Made of ions rather than molecules.
• Formation: Atoms lose or gain electrons to form charged ions.
• Cations/Anions: Positively/negatively charged ions formed by gaining/losing electrons.
• Charge Balance: Compounds have an overall neutral charge.

Metals/Nonmetals

• Alloys: Mixtures of metals.
• Formation: Created by mixing molten metals.
• Ionic Compounds (Metal/Nonmetal): Metals lose electrons ("cations") and nonmetals gain electrons (anions).
• Covalent Bonding (Nonmetal/Nonmetal): Atoms share electrons.

Breaking Molecules Apart

• H2O2 Decomposition: Hydrogen peroxide breaks down into water and oxygen.
• Catalysts: Substances that speed up reactions without being consumed.

Electricity

• Atomic Structure and Charge: Balanced atoms have equal protons and electrons.
• Charged Objects: Electrons gained/lost give objects net charge (positive/negative).
• Static Electricity: Accumulation of charge on a surface.
• Electroscopes: Instruments for detecting charges.
• Pith Ball/Leaf Electroscope: Used for charge detection.
• Charge Interaction: Like charges repel; opposite charges attract.
• Charging by Friction: Transfer of electrons from one material to another.
• Charging by Conduction: Transfer of electrons by direct contact.
• Charging by Induction: Transfer of electrons without direct contact.
• Grounding: Removing charge by transferring electrons to the ground.
• Electrostatic Precipitators: Remove particles from air using electrostatic charges.
• Conductors / Insulators: Conductors allow easy electron flow, whereas insulators impede it.
• Electric Circuits: Continuous conductive pathways and energy source.
• Loads: Devices transforming electrical energy.
• Switches: Devices to control electron flow in a circuit..
• Electric Current: Measurement/rate of electron flow.
• Ammeter: Measures electric current (connected in series with the component).
• Potential Difference (Voltage): Difference in potential energy per unit charge.
• Voltmeter: Measures potential difference (connected in parallel).
• Electrical Resistance: Material's opposition to current flow (measured in Ohms).
• Ohm's Law: Voltage = Current * Resistance.
• Series Circuits: Single electron pathway.
• Parallel Circuits: Multiple electron pathways.

Outer Space

• Celestial Objects: Stars, planets, moons.
• The Sun: Massive, hot gas radiating energy.
• Solar Activity: Nuclear fusion reactions generate energy. Solar flares and prominences.
• Solar Wind: Stream of high-energy particles.
• Planets: Inner (rocky, similar to Earth) and outer (gas giants).
• Dwarf Planets: (e.g. Pluto)
• Asteroids/Meteoroids: Rocky/metallic objects.
• Comets: Icy bodies.
• Comets & Sublimation: Comets form a tail when their outer surface sublimate (turn from solid to gas).
• Astronomical Units (AU): Convenient way to measure distances.