APES Unit 2 Abiotic and Biotic Parts of Ecosystems

1. APESUnit 2Abiotic and Biotic Parts of Ecosystems La Cañada High School Living in the Environmentby Miller, 11th Edition

2. 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

3. 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.

4. Solid, Liquid, and Gas

5. 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.

6. 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.

7. 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

8. 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.

9. Elements are organized through the periodic table by classifications of metals, metalloids, and nonmetals

10. 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)

11. 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.

12. 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.

13. Ionic Compounds Structure • Composed of oppositely-charged ions • Network of ions held together by attraction Ionic bonds • Forces of attraction between opposite charges

14. 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

15. http://www.emc.maricopa.edu/faculty/farabee/BIOBK/redox.gif

16. 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

17. 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

18. 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

19. 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

20. Organic Compounds Hydrocarbons Chlorofluorocarbons

21. Biological Organic Compounds Carbohydrates (Glucose) Protein (Cytochrome P450)

22. Biological Organic Compounds Lipid(Triglyceride) Nucleic Acid (DNA)

23. Earth’s Crust

24. 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.

25. High quality & Low quality LOW QUALITY HIGH QUALITY

26. 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.

27. Electromagnetic Spectrum • The range of electromagnetic waves, which differ in wavelength (distance between successive peaks or troughs) and energy content.

28. 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.

29. Potential energy • Potential energy is stored energy that is potential available for use. • Potential energy can be charged to kinetic energy.

30. 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.

31. 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

32. 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

33. Alpha, Beta, Gamma rays

34. 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

35. Click to see QuickTime Movie of Fissionhttp://www.atomicarchive.com/Movies/Movie4.shtml

36. 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

37. 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

38. 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.

39. 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

40. 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

41. 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!

42. Goals of Matter Recycling Societies To allow economic growth to continue without depleting matter resources or producing excess pollution

43. 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

44. Low Waste Societies • Works with nature to reduce throughput • Based on energy flow and matter recycling

45. 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

46. Low Waste Societies Function • Reduce unnecessary consumption • Emphasize pollution prevention and waste reduction • Control population growth

47. Unit 2, Chapter 4 Ecology, Ecosystems, and Food Webs

48. 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

49. 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

50. 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