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Study Guide for Unit 4 Exam

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Study Guide for Unit 4 Exam Study Guide for Unit 4 Exam Directions: Write the answers to the following questions on a separate sheet of paper. For the best chance of success for this test, study all notes, worksheets and bell work for the unit. Use the book and the internet for additional resources. While doing this worksheet will be helpful, it may not be enough to do your best. THIS REVIEW MUST BE TURNED IN ON THE DAY OF THE TEST. IT WILL BE COUNTED AS AN ASSIGNMENT. This is due: _____________________________________________ 1. What is an ion? 2. What does the octet rule state? 3. What is the difference between oxidation and reduction? 4. What is an oxidation state? 5. What is the oxidation state for elements in group 1, group 2, group 3, groups 3-12, group 13, group 14, group 15, group 16 & group 17, respectively? 6. Which of the following elements will lose electrons (become oxidized), and which will gain electrons (become reduced)? Na, Cl, Br, Ba, Sr, As, N 7. How does an atom become a cation? 8. Give two cation examples. 9. How does an atom become an anion? 10. Give two anion examples. 11. Is hydrogen a metal or a non-metal? Explain. 12. What is the difference (chemically) between an organic and inorganic compound? 13. Why do atoms bond? 14. What are the four types of bonding? Describe each type of bonding. 15. What are the properties of ionic compounds? 16. What is an ionic compound? Give an example. 17. What are the properties of covalent compounds? 18. What is the main difference between an ionic and a covalent bond? What are the other differences between an ionic and covalent bond/compound? a. What types of elements are they composed of? b. What happens to the electrons in each type of compound? c. What are the properties of the two types of compounds? d. Which type conducts when dissolved in water? 19. How can you tell if the bond between two atoms will be ionic or covalent? 20. Which type of bond is strongest (ionic or covalent)? 21. Which of the following sets of ions would have the strongest attraction to each other in an ionic compound? Why? a. Na+ + Cl- b. Ba 2+ + O 2- c. Na+ + Ba 2+ 22. Which of the following pictures is ionic? Which is covalent? 1 23. Describe what keeps elements together (bonded) in an ionic compound. 24. Describe what keeps elements together (bonded) in a covalent compound. 25. Describe the atoms present in a metallic bond. 26. What are the properties of polyatomic compounds? 27. Nomenclature: 28. Be able to write the names/symbols for the elements on the periodic table. o Write the names for: . O, H, C, P, etc o Write the symbols for: . Antimony, Tin, Iron, Copper 29. Write the names/symbols for the diatomics. 30. Write the names/symbols for the cations. 31. Write the names/symbols for the anions. 32. Explain how to write ionic compound formulas using the criss cross method. Show an example. Ca + F Rubidium and Oxygen 33. Write the Lewis dot diagrams (structural formulas) for the compounds listed above. 34. Complete the following table chlorine Sulfur hydroxide carbonate Strontium Magnesium Fe (II) Ammonium 35. What is the difference between a monoatomic ion and a polyatomic ion? 36. Explain how to name ionic compounds: NaBr K2O 37. Explain how to write ionic formulas with polyatomics: Cs + NO3 Aluminum Acetate 2 38. Explain how to name ionic compounds with polyatomics: Li2CO3 Be3(PO4)2 39. Explain how to write ionic formulas with transition metals: Copper (II) Nitrate Iron (III) Oxide 40. Explain how to name ionic compounds with transition metals: HgCl2 CoSO3 41. What are the charges for Ag, Zn, and Cd? 42. Explain how to write the names/formulas for covalent compounds. 43. What are the ten greek prefixes and what number do they correspond to? 44. Be able to write covalent formulas: Diphosphorus Petoxide Trinitrogen Hexasulfide Carbon Trioxide 41. Be able to name covalent compounds: NO2, SO3, CO 45. What are the correct names for CH4, H2O, and NH3? 46. Name the following compounds: N2O6, CO, CF4, B2O10 47. Write formulas for the following compounds: Water (dihydrogen monoxide) Carbon tetrachloride Ammonia (nitrogen trihydride) Tricarbon decafluoride 48. Draw structural formulas (Lewis dot formulas) for the following: SO3 CO CS2 CCl4 N2O NI3 PCl3 47. What is an acid? 48. Know how to name an acid: HCl H2S H3PO4 49. Know how to write an acid: Hydrobromic Acid Phosphorous Acid 50. What is a hydrate? Give an example. 51. Know how to name and write hydrates: NaCl * 4H2O Lithium Bromide Decahydrate 3 .
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