Welcome to

1. Welcome to Jeopardy Unit 1 - Dimensional Analysis Unit 2 - Concepts of Matter and Atomic Structure

2. Physical or Chemical Extensive or Intensive Element or What? Dimensional Analysis Matter 100 100 100 100 100 200 200 200 200 200 300 300 300 300 300 400 400 400 400 400 500 500 500 500 500 600 600 600 600 600

3. Which statement is NOTa description of a chemical reaction? • A solid is dropped into a beaker of liquid and a gas is released. • B. Two liquids are mixed in a beaker and a solid forms at the bottom of the beaker. • C. A solid is dropped into a beaker of liquid and an explosion occurs. • D. A liquid is heated on a Bunsen burner and its temperature rises. D

4. Which of the following observed properties is most reliable in classifying a substance as a metal? A. Good conductor of heat B. Low melting temperature C. Unreactive with other elements D. Crumbles when hit by a hammer A

5. Which grouping identifies chemical properties? • A. Malleability, ductility, conductivity • B. Luster, hardness, texture • C. Combustibility, flammability, reactivity • D. Density, melting point, boiling point C

6. The MSDS of a chemical compound indicates that it is flammable. What does this tell you about the compound? A. It cannot be exposed to air. B. It evaporates at a very low temperature. C. It corrodes when exposed to air. D. It reacts with oxygen to release heat. D

7. Which is NOTan example of a physical change that takes place in the atmosphere? • A. A lightning strike forms ozone, O3, from oxygen gas. • B. Water vapor condenses to form a cloud. • C. The air temperature increases as energy is absorbed from the Sun. • D. The air pressure drops on a stormy day. A

8. What is a chemical property of water? • A. Water density is 1.00 g/cm3. • B. Water reacts readily with alkali metals. • C. Water is known as the universal solvent. • D. Water is a clear colorless liquid. B

9. An unknown silvery powder has a constant melting point and does not chemically or physically separate into other substances. The unknown substance can be classified as — A. an element B. a compound C. a mixture D. an alloy A

10. During an investigation, a student mixes two clear solutions together which form a white precipitate. The precipitate is then filtered, rinsed, filtered again and dried. The sample precipitate is identified as — • A. An element • B. A heterogeneous mixture • C. A compound • D. An alloy C

11. Which of the following statements describes a difference between a mixture and a pure substance? • A. A mixture tends to be homogenous, while a pure • substance tends to be heterogeneous. • B. A mixture has a specific melting point, while the melting • point of a pure substance can vary. • C. The density of a mixture can change with temperature, • but the density of a pure substance cannot change. • D. The composition of a mixture can vary from sample to • sample, but the composition of a pure substance is • always the same. D

12. A solid that forms in a solution during a chemical reaction is called a(n) A. element. B. precipitate. C. mixture. D. bond. B

13. In the following diagrams, the spheres represent particles. Different shadings represent different particles. Which of the following contains only one pure substance? B A D C C

14. Which of the following explains why saltwater is considered a mixture? A. It is composed of one element. B. It is composed of one compound. C. It is composed of two or more substances and has new chemical properties. D. It is composed of two or more substances that retain their own chemical properties. D

15. A chemistry student’s investigation is described below. The student determines that the unknown substance is sodium chloride. Which of the following is an extensive property of sodium chloride? A. Mass of 15 g B. White color C. Density of 2.17 g/cm3 D. Solubility in water A

16. A physical property of a system that does not depend on the system size or the amount of material in the system is called a/an. A. intensive B. extensive C. physical D. chemical A

17. A property of a system that does depend on the system size or the amount of material in the system is called a/an A. Intensive B. Extensive C. Physical D. Chemical B

18. Which of these is not an intensive property of matter ………. • A. Temperature • B. Luster • C. Volume • D. Hardness C

19. All of the following are examples of extensive properties except A. mass B. volume C. energy D. melting point D

20. All of the following are examples of intensive properties except A. viscosity B. heat C. melting point D. boiling point B

21. Which state of matter is characterized by having an indefinite shape, but a definite volume? • A. Gas • B. Liquid • C. Solid • D. Plasma B

22. Why did most of the alpha particles go straight through the gold foil in Rutherford’s experiment? • Most of an atom is empty space. • B. Alpha particles are positively charged. • C. Alpha particles move with high velocity. • D. The center of an atom is positively charged. A

23. Which state of matter has an indefinite volume and takes the shape of its container? • A. Solid • B. Liquid • C. Gas • D. Both B and C C

24. One way that mixtures differ from pure substances is in the methods that can be used to separate them into their components. Which of the following is a method used to separate the components of matter of some mixtures? A. A nuclear reaction B. A filtration process C. A chemical reaction D. An electrolysis process B

25. What are the differences between these isotopes of hydrogen shown below? 11H, 21H, and 31H A. number of electrons and atomic number B. number of protons and atomic number C. number of neutrons and mass number D. number of electrons and protons C

26. The two stable isotopes of copper have the following masses and percent abundance in nature: Using the table above, determine the average atomic mass of the element copper. A. 64.31 B. 65.33 C. 63.55 D. 127.86 C

27. Dimensional Analysis is • a problem-solving method that uses the idea • that any number or expression can be multiplied by one without changing its value. • B. is used to convert one unit of measurement to another unit of measurement usingconversion factors. • C. a method used to calculate the size of matter. • D. Both A and B. D

28. When using math in science you should always • Show all steps of your work. • Show all units of measure in all steps of your work. • Show all units of measure in your final answer. • All of these answers. D

29. If the values 2.54 centimeters and 1 inch are equal, then the conversion factor could be written • 2.54 centimeters / 1 inch • 1 inch / 2.54 centimeters • 1inch x 2.54 centimeters • Both A and B D

30. If 2.54 centimeters equals one inch and I wish to convert 27 inches into centimeters, how would I arrange the conversion factor so that centimeters would be cancelled? • Centimeters in the denominator • Centimeters in the numerator • Centimeters to be subtracted • Centimeters to be added A

31. When using the metric system, conversion can be completed by using the metric “ladder”, powers of 10, and simply moving your decimal. Using this method, how many meters are in 1,386 millimeters? A. 138.6 meters B. 13.86 meters C. 1.386 meters D. 0.1386 meters C

32. How many decigrams are in 84.96 kilograms? • 849.6 decigrams • 8,496 decigrams • 84,960 decigrams • 849,600 decigrams D