Science, Systems, Matter, and Energy

1. Chapter 3 Science, Systems, Matter, and Energy

2. Objectives • Science as a process for understanding • Components and regulation of systems • Matter: forms, quality, and how it changes; laws of matter • Energy: forms, quality, and how it changes; laws of energy

3. Ask a question Do experiments and collect data Interpret data Well-tested and accepted patterns In data become scientific laws Formulate hypothesis to explain data Do more Experiments to test hypothesis Revise hypothesis if necessary Well-tested and accepted hypotheses become scientific theories Science • Scientific Data • Hypothesis – based on observations • Scientific Theories - verified, widely accepted hypothesis • Scientific Laws - happens over and over in nature (Thermodynamics)

4. Scientists Use Reasoning • Inductive - specific observations to arrive at a general conclusion Example: drop several objects and conclude that all objects fall to the earth’s surface when dropped • Deductive - generalizations to arrive at a specific conclusion Example: all birds have feathers, therefore eagles have feathers

5. Two Types of Science • Frontier Science - not widely tested and accepted Example: herbal remedies • Consensus Science - widely accepted by expert scientists Example: gravity, thermodynamics, etc.

6. Systems • Set of components that … 1. function and interact in a predictable manner. 2. can be isolated for observation. • Components of systems are … 1. Inputs – what is put into the system. 2. Flows – what is within the system. 3. Stores – what is accumulating within the system. 4. Outputs – what flows out of the system.

7. How are Systems Regulated? • Positive Feedback - Change in one direction causes further change in the same direction. Example: money in the bank accumulating interest • Negative Feedback - Change leads to lessening of that change. Example: recycling aluminum cans

9. How do Time Delays affect Systems? • Can allow a problem to build up slowly until it reaches a threshold. • Can cause a fundamental shift in the system. • Examples: - leak from toxic waste dump - lung cancer 20 years after smoking cessation

10. How can Synergy affect Systems? • Synergy 1 + 1 = 3? - Combined affect is more than the sum of their separate effects. - Example: Moving a 300 lb. log Person 1 = 100 lbs. Person 2 = 100 lbs.

11. Matter: Forms, Structure, and Quality ■Element: building blocks of matter ■Compound: two or more elements combined ■Atom: smallest units of matter ■Ion: charged atom ■Molecule: two or more atoms combined

12. What’s in an Atom? • Protons + positive charge • Neutrons no charge • Electrons - negative charge • Atomic Number number of protons

13. Examples of Atoms Fig. 3-4 p. 48

14. Chemical Bonds Covalent – “sharing”

15. Chemical Bonds Ionic - “transfer of electrons”

16. Organic Compounds • Hydrocarbons – natural gas (CH4) • Chlorinated Hydrocarbons – • DDT (C14H9Cl5) • Chlorofluorocarbons – aerosals • and AC Coolant • Carbohydrates – glucose, sucrose, • fructose, galactose • Proteins – amino acids with • carbon backbones

17. The Four States of Matter • Solid • Liquid • Gas • Plasma

18. Which State of Matter is the Most Abundant? • Plasma - sun and stars - high energy mix of + and – particles - formed when electrons are taken from the nuclei of atoms (high energy process)

19. Matter • Matter Quality - Measure of how useful a form of matter is to us as a resource, based on its availability and concentration. • High Quality Matter 1. Fairly easy to extract and concentrated. 2. Found near the Earth’s surface. 3. Great potential for use as a resource.

20. Matter Continued • Low Quality Matter 1. Dilute 2. Deep underground or dispersed in the ocean (difficult to extract). 3. Little potential use as a resource. • Material Efficiency - Amount of material needed to produce each unit of goods or services.

22. Forms of Energy • Kinetic - energy in motion Examples: Wind, Flowing Streams, Electricity • Potential - stored energy Examples: Unlit Stick of Dynamite, Rock in Hand

23. Convection Conduction Radiation Heat from a stove burner causes atoms or molecules in the pan’s bottom to vibrate faster. The vibrating atoms or molecules then collide with nearby molecules, causing them to vibrate faster. Eventually, molecules or atoms in the pan’s handle are vibrating so fast it becomes too hot to touch. As the water boils, heat from the hot stove burner and pan radiates into the surrounding air, even though air conducts very little heat. Heating in the bottom of a pan causes the water to vaporize into bubbles. Because they are lighter than the surrounding water, they rise. Water then sinks from the top to replace the rising bubbles. This up and down movement (convection) eventually heats all of the water. Transfer of Heat Energy

24. Energy • Energy Quality - Energy source’s ability to do useful work. • High Quality Energy 1. Concentrated 2. Provides useful work Examples: Electricity, Concentrated Sunlight

25. Energy Continued • Low Quality Energy 1. Dispersed 2. Little useful work Example: Heat dispersed in the Atlantic Ocean.

26. Why is There No “Away”? Law of Conservation of Matter • We cannot destroy atoms. • We can only rearrange them into different spatial patterns (physical) or into different combinations (chemical). • Everything we think we have “thrown away” is still here in one form or another.

27. Example • DDT - banned, but still residues in imported coffee, tea, fruit, and other foods. - or as fallout from air masses moved long distances by wind. • Law of Conservation of Matter - means we will always face the problem of what to do with wastes and pollutants.

28. Pollution 3 Factors that Determine the Severity of a Pollutant’s Chemical Effects: 1. Chemical Nature 2. Concentration - parts per million (ppm) 3. Persistence - measure of how long the pollutant stays in the air, water, soil, or body. Classification of Pollutants: • Degradable (reduced to acceptable levels) • Slowly Degradable (decades or longer-DDT) • Nondegradable (natural processes cannot break down -lead, arsenic)

29. Nuclear Changes • Matter undergoes a nuclear change: 1. natural radioactive decay 2. nuclear fission 3. nuclear fusion

30. Natural Radioactive Decay • A nuclear change in which unstable isotopes spontaneously emit fast- moving particles (matter), high-energy radiation, or both at a fixed rate. • Unstable Isotopes are called “radioactive isotopes” - radioactive decay continues until isotope becomes stable. • Isotopes have a different number of neutrons but the same number of protons.

31. Natural Radioactive Decay Continued • Radiation emitted by radioisotopes is damaging ionizing radiation. • Gamma Rays – a form of high-energy electromagnetic radiation emitted from radioisotopes. You do not want to be exposed to these waves. • Alpha/Beta Particles – high-speed ionizing particles emitted from the nuclei of radioisotopes.

33. What is Half-Life? • The amount of time needed for one-half of the nuclei in a given quantity of a radioisotope to decay and emit their radiation to form a different isotope. • Decay continues, often producing a series of different radioisotopes, until a stable, nonradioactive isotope is formed. • The half-life estimates how long a sample of radioactive isotope must be stored in a safe container before it decays to a safe level and can be released into the environment.

34. Half-Life Continued • A general rule is that such decay to a safe level takes about 10 half-lives. • Example: Plutonium-239 has a half-life 24,000 years. It is produced in nuclear reactors and used in nuclear weapon production. It must be stored safely for 240,000 years (10 x 24,000). • Plutonium-239 can cause lung cancer when its particles are inhaled in minute amounts. • Ionizing radiation exposure from alpha particles, beta particles, and gamma rays can damage cells by genetic damage (mutations of DNA) or somatic damage (tissue damage).

35. Nuclear Fission • Neutrons can split apart the nuclei of certain isotopes with large mass numbers and release a large amount of energy. 1. Neutron hits the nucleus of an isotope. 2. Nucleus splits and releases 2 or 3 more neutrons and ENERGY. 3. Each of these neutrons can go on to cause additional fission. • Multiple fissions create a chain reaction which releases an ENORMOUS AMOUNT OF ENERGY.

36. Examples of Nuclear Fission • Atomic Bomb – An enormous amount of energy is released in a fraction of a second in an uncontrolled nuclear fission chain reaction. • Nuclear Power Plant – The rate at which the nuclear fission chain reaction takes place is controlled. In conventional nuclear fission reactors, the splitting of uranium- 235 nuclei releases energy in form of heat, which produces high-pressure steam to spin turbines and thus generate electricity.

39. Nuclear Fusion • Nuclear fusion is a nuclear change in which extremely high temperatures force the nuclei of isotopes of some lightweight atoms to fuse together and form a heavier nucleus which in turn releases large amounts of energy. • Extremely high temperatures (at least 100 million oC) are needed to force the positively charged nuclei (protons strongly repel one another) to fuse. • Source of energy in sun and stars.

41. Sun-hydrogen isotopes fuse to make helium-energy and heat.

42. What are Nuclear Reactions used for? • Energy Production: nuclear power plants generate electricity for our homes. • Medical Technology: cancer treatment, X-rays. • Nuclear Weapons: atomic bomb, hydrogen bomb.

43. Nuclear Power Plant

44. Atomic Bomb

45. Laws of Thermodynamics 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. • Energy input always equal energy output. • You cannot get something for nothing in terms of energy quantity. 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, usually heat.