Understanding the Scientific Method and Measurements in Science

1. General Science I Sem. Review Final Jeopardy

2. The Scientific Method 100 • Define hypothesis. • A testable statement. • Ex) If you wear high heels instead of running shoes, then you won’t run as far. Back

3. The Scientific Method 200 • Define observation. • A statement made using the senses. • Ex) The flame is blue and 700oC Back

4. The Scientific Method 300 • What is the difference between a qualitative observation and a quantitative observation? • Qualitative- qualities of the object • Quantitative- quantities/numbers of the object Back

5. The Scientific Method 400 • Is the following a qualitative or a quantitative observation:There are 82 paper clips on the ground. • Quantitative- there was a quantity or numbers involved. Back

6. The Scientific Method 500 • In an experiment, you control things and you vary things. Define control and variable. • Control- everything you keep the same in the experiment. • Variable- the ONE thing you change in the experiment. Back

7. Measurement 100 • What is each letters’ metric prefix? K H D _ d c m • Kilo- ; Hecto- ; Deka- ; _ ; deci- ; centi-; milli-; Back

8. Measurement 200 • DAILY DOUBLE!!!! • Convert 50cm to m. • KHD_dcm m is in the middle… 0.5 m Back

9. Measurement 300 • What is the unit for temperature in science? • Celsius Back

10. Measurement 400 • Define mass. • The amount of matter in an object. Back

11. Measurement 500 • Define volume. • How much space an object takes up. Back

12. The Gas Laws 100 • Define diffusion. • When particles move from an area of high concentration to low concentration. Back

13. The Gas Laws 200 • State Boyle’s Law • “Boyle is at PV” • As pressure goes up, volume goes down. They’re opposites. Back

14. The Gas Laws 300 • State Charles’ Law • “Charles had a TV” • As temperature goes up, volume goes up. They do the same thing. Back

15. The Gas Laws 400 • Boyle’s Law or Charles’ Law?A hot-air balloon • Charles law (increase T of air in the balloon, it inflates; hot air rises, so balloon goes up in the air. Cool it down, it slowly sinks) Back

16. The Gas Laws 500 • Charles Law or Boyles’s Law?A bicycle pump • Boyles’s (Decrease the volume of the launcher and pressure builds up, shooting the potato) Back

17. The Atom/PT 100 • Atomic number = Atomic mass - what? • Atomic number = Atomic mass - NEUTRONS. Back

18. The Atom/PT 200 • What is an isotope? • An atom with a different number of neutrons. Back

19. The Atom/PT 300 • Rows on the PT are called _______ and columns are called ___________. • Rows are “periods” and columns are “families” or “groups” Back

20. The Atom/PT 400 • What goes is the blank with the “?” • 56; Atomic # and Proton # are equal Back

21. The Atom/PT 500 • The most reactive metal is ______. • Francium, sodium, or potassium? • Francium Back

22. Ionic and Covalent Bonds 100 • Ionic bonds _______ (share/transfer) electrons and bond with a _______ (metal/nonmetal) and a _____ (metal/nonmetal) • Transfer electrons and bond with a metal and a nonmetal Back

23. Ionic and Covalent Bonds 200 • Covalent bonds form between a _____ (metal/nonmetal) and a ____ (metal/nonmetal) • Covalent bonds always form between two nonmetals Back

24. Ionic and Covalent Bonds 300 • Write the formula for Sodium bromide. Is this an ionic or covalent bond? • NaBr… ionic Back

25. Ionic and Covalent Bonds 400 • Write the formula for dicarbon hexahydride; is this ionic or covalent • di=2; hexa=6; C2H6 prefixes mean covalent bond Back

26. Ionic and Covalent Bonds 500 • List one property of ionic compounds and one property of covalent compounds. • Ionic: high melting point, conduct electricity, brittleCovalent: low melting point, poor conductors of electricity Back

27. Final Jeopardy • Chemical ReactionsMAKE YOUR WAGER! • Cl2 + 4 NaBr  2 NaCl+ 2 Br2 Balanced? No Back