<p>Chapter 1-3 Study Guide Chemistry These are possible test questions, some of these are exactly the same as the questions on the test. Some will be changed a little. Ch. 1 1. What is the study of matter and the changes that occur in matter? 2. Explain these terms and how they relate to each other: observation, hypothesis, experiment, theory, scientific law. 2.1 3. Define these terms: a. Matter, b. atoms, c. a compound, d. molecule, e. an element, f. a solid, g. a liquid, h. a gas 4. What is the difference between a molecule and a compound? Can a molecule be a compound? Give an example. 5. Draw a picture of a. an atomic element, b. a molecular element, c. a compound. 2.2 6. Classify the following as a chemical or physical change: a. Liquid water is boiled and becomes a gas. b. An egg is cooked. 7. Give an example of a physical property of the floor in the chemistry classroom. 8. Give an example of a chemical property of the floor in the chemistry classroom. 9. In your own words, define a physical change using the words “atom” and “molecule.” Give an example of a physical change. 10. In your own words, define a chemical change using the words “atom” and “molecule.” Give an example of a chemical change. 2.3 11. Define these terms: a. Mixture, b. alloy, c. pure substance, d. homogeneous mixture, e. solution, f. heterogeneous mixture, g. distillation, h. filtration 12. Give an example of: a. a homogeneous mixture, b. a heterogeneous mixture. 13. List steps in how you could separate a mixture of sand, salt and water into its components. 14. Draw a picture on the molecular level of a: a. homogeneous mixture, b. heterogeneous mixture and c. pure substance 3.1 15. What contributions did alchemists make to the development of chemistry? 16. What is the most abundant element in the Earth’s crust (by % mass)? 17. What is the chemical symbol of silver? 18. How did the elements get their names? 3.2 19. a. (2 pts) State the Law of Constant Composition in your own words. b. (3 pts) How did Dalton’s atomic theory help explain the Law of Constant Composition? 20. What is a subscript in a chemical formula? 3.2 21. (2 pts) What is the formula for a molecule with two boron atoms and six hydrogen atoms? 3.3 22. What are the relative mass and charge of each subatomic particle? 23. Fill in this table: Name Symbol Atomic Mass # of # of # of Number Number Protons Neutrons Electrons 20 41 20</p><p>24. Define these terms: a. Electron, b. Nucleus, c. Proton, d. Neutron, e. Isotope, f.Atomic number, g.Mass number 25. (5 pts total) JJ Thomson conducted experiments with the cathode ray tube. In one experiment, he used charged plates. Draw and label a diagram of the experiment (2 pts), write his observation (2 pts), and his conclusion for this observation (1 pt). 26. (5 pts total) Draw a labeled diagram of the plum pudding model of the atom and describe it in one or two sentences. Why did JJ Thomson assume that there must be a positive charge in atoms? 27. (5 pts total) Draw a labeled diagram of Ernest Rutherford’s gold foil experiment. Label the source of α particles, the gold foil, the screen and the scattered α particles (2pts). What did Rutherford observe (1 pt)? What did he conclude from this (2 pts)? 3.4 28. Define these terms: a. Periodic table e. Halogens i. Metals b. Groups f. Noble gases j. Nonmetals c. Alkali metals g. Transition metals k. Metalloids d. Alkaline earth h. Diatomic metals molecules </p><p>29. What elements are gases at room temperature? Liquids? Solids? 30. Calcium is a metal / nonmetal / metalloid. 3.5 31. Define these terms: a. Ion c. Anion b. Cation d. Ionic compound 32. Fill in this table: Cation Anion Formula of compound Al3+ N3- Ca2+ P3-</p><p>33. Fill in this table: Ion Number of Number of protons electrons Fe3+ F- </p>