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APES Unit 2 Abiotic and Biotic Parts of Ecosystems. La Ca ñ ada High School Living in the Environment by Miller, 11 th Edition. Matter and Energy Resources: Types and Concepts. 3-1: Matter: Forms, Structure, and Quality 3-2: Energy: Forms and Quality
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APESUnit 2Abiotic and Biotic Parts of Ecosystems La Cañada High School Living in the Environmentby Miller, 11th Edition
Matter and Energy Resources: Types and Concepts • 3-1: Matter: Forms, Structure, and Quality • 3-2: Energy: Forms and Quality • 3-3: Physical and Chemical Changes and the Law of Conservation of Matter • 3-4: Nuclear Changes • 3-5: The Two Ironclad Laws of Energy • 3-6: Connections: Matter and Energy Laws and Environmental Problems
MatterForms, Structure, and Quality • Matter is anything that has mass and takes up space. • Matter is found in two chemical forms: elements and compounds. • Various elements, compounds, or both can be found together in mixtures.
Atoms, Ions, and Molecules • Atoms: The smallest unit of matter that is unique to a particular element. • Ions: Electrically charged atoms or combinations of atoms. • Molecules: Combinations of two or more atoms of the same or different elements held together by chemical bonds.
What are Atoms? • The main building blocks of an atom are positively charged PROTONS, uncharged NEUTRONS, and negatively charged ELECTRONS • Each atom has an extremely small center, or nucleus, containing protons and neutrons.
http://mediaserv.sus.mcgill.ca/content/2004-Winter/180-Winter/Nuclear/frame0008.htmhttp://mediaserv.sus.mcgill.ca/content/2004-Winter/180-Winter/Nuclear/frame0008.htm
Atomic Number and Mass Number. • Atomic number • The number of protons in the nucleus of each of its atoms. • Mass number • The total number of protons and neutrons in its nucleus.
Elements are organized through the periodic table by classifications of metals, metalloids, and nonmetals
Inorganic Compounds • All compounds not Organic • Ionic Compounds • sodium chloride (NaCl) • sodium bicarbonate (NaOH) • Covalent compounds • hydrogen(H2) • carbon dioxide (CO2) • nitrogen dioxide (NO2) • sulfur dioxide (SO2) • Ammonia (NH3)
Inorganic Compounds • The earth’s crust is composed of mostly inorganic minerals and rock • The crust is the source of all most nonrenewable resource we use: fossil fuels, metallic minerals, etc. Various combinations of only eight elements make up the bulk of most minerals.
Nonmetallic Elements. • Carbon (C), Oxygen (O), Nitrogen (N), Sulfur (S), Hydrogen (H), and Phosphorous (P). • Nonmetallic elements make up about 99% of the atoms of all living things.
Ionic Compounds Structure • Composed of oppositely-charged ions • Network of ions held together by attraction Ionic bonds • Forces of attraction between opposite charges
Formation of Ionic Compounds • Transfer of electrons between the atoms of these elements • Atom that is metal loses electrons (oxidation) to become positive • Atom that is nonmetal gains electrons (reduction) to become negative • Results in drastic changes to the elements involved
Sodium Chloride • Sodium is a rather "soft" metal solid, with a silver-grey color • Chlorine is greenish colored gas • When a single electron is transferred between these elements, their atoms are transformed via a violent reaction into a totally different substance called, sodium chloride, commonly called table salt -- a white, crystalline, and brittle solid
Covalent Bonds • Formed by two non-metals • Similar electronegativities • Neither atom is "strong" enough to steal electrons from the other • Therefore, the atoms must share the electrons
Covalent Bonds • Chlorine atoms with valence electrons shown • Chlorine atom has seven valence electrons, but wants eight • When unpaired electron is shared, both atoms now have a full valence of eight electrons • Individual atoms are independent, but once the bond is formed, energy is released, and the new chlorine molecule (Cl2) behaves as a single particle
Organic Compounds • Compounds containing carbon atoms combined with each other with atoms of one or more other elements such as hydrogen, oxygen, nitrogen, sulfur, etc. • Hydrocarbons • Compounds of carbon and hydrogen • Chlorofluorocarbons • Carbon, chlorine, and fluorine atoms • Simple carbohydrates • carbon, hydrogen, oxygen combinations
Organic Compounds Hydrocarbons Chlorofluorocarbons
Biological Organic Compounds Carbohydrates (Glucose) Protein (Cytochrome P450)
Biological Organic Compounds Lipid(Triglyceride) Nucleic Acid (DNA)
Matter Quality • Matter quality is a measure of how useful a matter resource is, based in its availability and concentration. • High quality matter is organized, concentrated, and usually found near the earth’s crust. • Low quality is disorganized, dilute, and has little potential for use as a matter resource.
High quality & Low quality LOW QUALITY HIGH QUALITY
Energy • Energy is the capacity to do work and transfer heat. • Energy comes in many forms: light, heat, and electricity. • Kinetic energy is the energy that matter has because of its mass and its speed or velocity.
Electromagnetic Spectrum • The range of electromagnetic waves, which differ in wavelength (distance between successive peaks or troughs) and energy content.
Kinetic energy. • Kinetic energy is the energy that matter has because of its mass and its speed or velocity. • It is energy in action or motion. • Wind, flowing streams, falling rocks, electricity, moving car - all have kinetic energy.
Potential energy • Potential energy is stored energy that is potential available for use. • Potential energy can be charged to kinetic energy.
Energy Quality • Very High: Electricity, Nuclear fission, and Concentrated sunlight. • High: Hydrogen gas, Natural gas, and Coal. • Moderate: Normal sunlight, and wood. • Low: Low- temperature heat and dispersed geothermal energy.
Natural Radioactive Decay • A nuclear change in which unstable isotopes spontaneously emit fast moving particles, high energy radiation, or both at a fixed rate • The unstable isotopes are also known as radioactive isotopes or radioisotopes
Natural Radioactive Decay • The decay continues until the original isotope becomes a stable, nonradioactive isotope • Until then, the radiation emitted is damaging ionizing radiation • Gamma rays • Alpha particles • Beta particles • After ten half-lifes, the material is said to be clean
Nuclear Fission • Nuclear change in which nuclei of certain isotopes with large mass numbers are spilt apart into lighter nuclei when struck by neutrons • Each fission releases two or three more neutrons and energy
Click to see QuickTime Movie of Fissionhttp://www.atomicarchive.com/Movies/Movie4.shtml
Critical Mass Enough fissionable nuclei available for multiple fission reactions to occur Chain Reaction Multiple fissions within a critical mass Releases huge amounts of energy Atomic Bomb or Nuclear Power Plant Nuclear Fission
The “Law of Conservation of Matter and Energy” • In any nuclear change, the total amount of matter and energy involved remains the same. • E = mc2 • The energy created by the release of the strong nuclear forces for 1 kilogram of matter will produce enough energy to elevated the temperature of all the water used in the Los Angeles basin in one day by 10,000oC
What is Nuclear Fusion? • Nuclear Fusion is a nuclear change in which two isotopes of light elements, such as hydrogen, are forced together at extremely high temperatures until they fuse to form a heavier nucleus, releasing energy in the process.
First Law of Thermodynamics • In all physical and chemical changes • Energy is neither created nor destroyed • But it may be converted from one form to another
Second Law of Thermodynamics • When energy is changed from one form to another • Some of the useful energy is always degraded to lower-quality, more dispersed, less useful energy • Also known as Law of Entropy
High Waste Societies • People continue to use and waste more and more energy and matter resources at an increasing rate • At some point, high-waste societies will become • UNSUSTAINABLE!
Goals of Matter Recycling Societies To allow economic growth to continue without depleting matter resources or producing excess pollution
Advantages Saves Energy Buys Time Disadvantages Requires high-quality energy which cannot be recycled Adds waste heat No infinite supply of affordable high-quality energy available Limit to number of times a material can be recycled Matter Recycling Societies
Low Waste Societies • Works with nature to reduce throughput • Based on energy flow and matter recycling
Low Waste Societies Function • Reuse/recycle most nonrenewable matter resources • Use potentially renewable resources no faster than they are replenished • Use matter and energy resources efficiently
Low Waste Societies Function • Reduce unnecessary consumption • Emphasize pollution prevention and waste reduction • Control population growth
Unit 2, Chapter 4 Ecology, Ecosystems, and Food Webs
Chapter 4Ecology, Ecosystems, and Food Webs • 4-1 Ecology and Life • 4-2 Earth’s Life-Support Systems • 4-3 Ecosystem Concept • 4-4 Food Webs and Energy Flow in Ecosystems • 4-5 How do Ecologists learn about Ecosystems? • 4-6 Ecosystem Services and Sustainability
4-1 Ecology and Life • Ecology- study of relationships between organisms and their environment • Ecology examines how organisms interact with their nonliving (abiotic) environment such as sunlight, temperature, moisture, and vital nutrients • Biotic interaction among organisms, populations, communities, ecosystems, and the ecosphere
Distinction between Species • Wild species- one that exists as a population of individuals in a natural habitat, ideally similar to the one in which its ancestors evolved • Domesticated species- animals such as cows, sheep, food crops, animals in zoos