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Introduction to Matter and Energy in Science

This chapter explores the nature of science, including the scientific method, types of data, and the role of hypotheses in inquiry. It also covers the limitations of science, the difference between facts, laws, hypotheses, and theories, and the branches of chemistry.

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Introduction to Matter and Energy in Science

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  1. Chapter 1 Matter and energy

  2. The Nature of Science • Science • Law • Fact • Hypothesis • Theory Archimedes

  3. Scientific method Observing (Quantitative) (Qualitative) generalizing testing theorizing

  4. Types of Data (Recorded observations) • Quantitative or qualitative

  5. The Role of Hypotheses in Inquiry • Tentative answer to a well-framed question, an explanation on trial • Makes predictions that can be tested

  6. Hypothesis-Based Science • Inquiry that asks specific questions • proposing and testing of hypotheses

  7. The Myth of the Scientific Method • The scientific method is an idealized process of inquiry • Very few scientific inquiries adhere to the “textbook” scientific method

  8. The Nature of Science Science: observation of the world and the constant testing of theories against nature, with the requirement that everything that is to be called science must be testable The character of science matches the American character Practical, pragmatic, classless, based on evidence Healthy skepticism

  9. Rational approach to questions Dull slog through failures to reach a conclusion Answers lead to more questions What is a fact, law, hypothesis, theory? Can only address question that deal with the natural world

  10. What science is not Pseudoscience e.g. astrology

  11. Limitations of Science • Science cannot address supernatural phenomena • Hypotheses must be testable and falsifiable and experimental results must be repeatable

  12. Theories in Science • Broad in scope • Generate new hypotheses • Supported by a large body of evidence • Explain • Incorporates confirmed observations, laws, and successfully verified hypotheses

  13. Law – description of how a natural phenomenon will occur • Fact – natural phenomenon repeatedly confirmed by observation, e.g. Venus takes 225 days to go around the sun

  14. Chemistry: The Central Science biology physics chemistry ecology geology

  15. Natural Sciences • Biological (biology, ecology) – living things • Physical (chemistry, physics) - nonliving

  16. Branches of chemistry • Organic (carbon chemistry) • Inorganic • Physical • Biochemistry • Analytical

  17. Matter – anything that has mass & occupies space • Mass – measure of quantity of matter • Weight – measure of Earth’s gravitational attraction for matter

  18. Gravity – a product of the bending of spacetime

  19. Energy – ability to cause change or ability to do work • Kinetic (E of motion) • Potential (E of position)

  20. Interconversion of matter and energy • E = mc2

  21. Ecosystems and Energy Flow All the biotic and abiotic factors in a defined area

  22. Energy flows through ecosystems, while matter cycles within them

  23. Ecosystems and Physical Laws • Energy is conserved • The laws of physics and chemistry apply to ecosystems • Particularly in regard to the flow of energy • But degraded to heat during ecosystem processes

  24. States of matter • Solid (def. shape and vol. • Liquid (def. vol, fluid) • Gas (neither def. shape or vol.) • Plasma (gas w/ + particles & e-)

  25. Physical properties-can be measured w/o chg. In identity (e.g. BP) • Extensive – depends on amt. (e.g.length) • Intensive – doesn’t depend on amt. (e.g. BP)

  26. Physical change • Doesn’t result in chg. In identity

  27. Chemical properties • Change in identity

  28. Chemical change • One or more substances converted into diff. substances

  29. Chemical reaction • Reactants  Products

  30. Indications of chem. reaction • Evolution of heat and light • Production of a gas • Formation of precipitate

  31. Reaction types

  32. Mixtures- 2 or more kinds of matter, can be separated by physical means • Heterogeneous- not uniform, e.g. vegetable soup • Homogeneous- uniform, e.g. salt water, also called solutions

  33. Pure substance- homogeneous sample of matter, e.g. sugar • Every sample the same • Cannot be separated w/o changing ID • 2 types- elements : cannot be decomposed by chemical change, and compounds: can be decomposed

  34. Law of definite composition • A cmpd. contains the same elements in exactly the same proportions by mass

  35. Periodic table • Groups • Periods • Element symbols, e.g. Fe

  36. Types of elements • Metals – luster, reflectors, conduct electricity and heat, ductile, malleable • Nonmetals • Metalloids – semiconductors, char. of both

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