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ChLM Final Review Name: Period: 9. For generic element “X”, define what goes in each location in the symbol (hint: remember these are all whole numbers). Base Knowledge 1. Classify the following as observations or inferences a) The liquid is green because food coloring was added. b) The beaker has green liquid in it. c) The beaker can hold up to 250 mL. d) The beaker will be the best tool for this lab. 2. Measure the following, circle your estimated digit and include units X 10. Complete the following table. Element Symbol Atomic Mass mass number Atomic # of number p+ # of n0 # of e- Neon a) b) Atoms 3. What part of an atom determines which element it is? __________________ 4. Which particle determines the chemical reactivity of an atom? ____________________ 5. What does the word “neutral” mean? When is an atom neutral? Nickel Ions 11. What happened to the electrons to make a cation? ___________ 12. What happened to the electrons to make an anion? ___________ 13. What is the difference between a magnesium atom and a magnesium ion (+2)? 14. What is different between a fluorine atom and a fluoride ion (-1)? 6. Define the following words, use equations when helpful: a) Atomic Number b) Mass Number c) Atomic Mass 7. How do you get from Atomic Mass to Mass Number? _________________________________ 8. How do you find the number of neutrons in an atom? 15. Complete the following table. Element Symbol Mass Number Silver 108 + 47 Iodine 127 53 Oxygen 16 8 Ag I O Protons Neutrons Electrons 10 Periodic Table 16. On the Periodic Table, which type of elements make cations? Which type make anions? 17. List three metals. 18. List three nonmetals. 19. List two halogens. How many valence electrons do the halogens have? 20. List two alkaline earth metals. How many valence electrons do the alkaline earth metals have? 21. Why don’t the noble gases react with anything? 22. Draw arrows showing where periods and groups are on the periodic table. 23. Use the periodic table to identify the element in period 3, group 17. What do you know about this element? (What is the name of its group? How many valence electrons does it have? 24. As you move left to right in a period, what happens to the mass of the elements? Rutherford 25. What kind of particles did Rutherford shoot at the thin gold foil? _________________ 26. What did we learn about atomic structure because of Rutherford’s experiment? Isotopes 27. How many protons, neutrons and electrons are in one neutral atom of each of the following isotopes? a) Beryllium-9 p = b) Silicon-28 p= c) Silicon-29 p= n= n= n= e= e= e= 28. Write the complete symbols for neutral atoms of Potassium-39 and Potassium-40. 29. Which of the above isotopes is the most common? How did you decide this? 30. The less common isotope in #10 is radioactive. What does it mean if something is radioactive? Use the words “stable,” “nucleus,” and “decay” in your answer. Radioactive Decay 31. What are the three types of radioactive decay you learned about? Write the symbol for each (include all relevant numbers). 32. Which part of the atom changes during radioactive decay? Half-Life 33. Use the following graph to determine the half-life of Uranium-238. Ionic/Covalent 38. What kinds of elements are in ionic bonds? _____________ & ________________ 39. What kinds of elements are in covalent bonds? ________________ & ______________ 40. Ionic Formulas & Naming – give the appropriate name or formula for the following ionic compounds. Chemical Name Chemical Formula (make sure your ratio is correct) Potassium iodide 34. If you started with 100 g of Uranium-238, how many grams would be left after 9000 million years? How many half-lives is 9000 million years? Calcium nitride Rb2O Al2S3 Electromagnetic Spectrum 35. What is the highest energy color of visible light? Which is the lowest? Bohr Model 36. How many electrons can fit on the first energy level of the Bohr model? _____ How many on the second? _____ 41. Covalent Formulas & Naming – give the appropriate name or formula for the following covalent compounds. (remember prefixes in your notes) Chemical Name Chemical Formula Sulfur hexafluoride Dihydrogen monoxide CH4 37. Draw the complete Bohr model for Beryllium and Magnesium (remember to show protons & neutrons). What do the electrons have in common between these two elements? P2Cl5 Which of the following compounds would you expect to have a lower melting point? How did you decide? a) LiBr or NO2 b) PCl3 or MgCl2 43. Which of the following compounds would you expect to conduct electricity when dissolved in water? How did you decide? a) LiBr or NO2 b) PCl3 or MgCl2 42. 44. What do we call one unit of a covalent compound? 45. How are covalent compounds held together? Balancing 46. Which side of a chemical equation are the reactants on? The products? 47. ___(NH4)2S (aq) + ___ZnCl2 (aq) ___ ZnS (s) + ___NH4Cl (aq) Reaction type: _________________ 48. ___Na2CO3 (s) ___ Na2O (s) + ___CO2 (g) Reaction type: _________________ 49. ___H2 (g) + ___I2 (s) ___ HI (g) Reaction type: _________________ 50. ___Rb (s) + ___HCl (aq) ___ RbCl (aq) + ___H2 (g) Reaction type: _________________ 51. ___C9H20 (l) + ___O2 (g) ___ H2O (l) + ___CO2 (g) Reaction type: _________________