Chem 42 Final Review Sheet Mr. J. Fassler Spring 2018
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1 Chem 42 Final Review Sheet Mr. J. Fassler Spring 2018 These problems are given to help you review concepts you may have forgotten. Old tests, quizzes and review sheets are also important in studying. Chapter 4 (Atoms and Ions) 1. Fill in the blanks for each ion. ion protons neutrons electrons 19 F 64 Cu 2+ Electron Configurations 2. Write ground state electron configurations for the following elements and ions: C F Al Ca 2+ Mn Br Chapter 5 (Nomenclature) 3. Name the following compounds. CaO Mg 3 (PO 4 ) 2 PCl 5 Cu 2 O PbO 2 NaHCO 3 CrO 3 Fe 3 (PO 4 ) 2 4. Write formulas from the following names, being sure that the charge is zero for each formula. carbon tetrachloride lead (II) chloride lithium carbonate copper (I) iodide ammonia magnesium sulfide ammonium chloride silver nitrate gold(i) cyanide hydrogen peroxide iron(iii) sulfate calcium hydroxide magnesium nitrate phosphorus trichloride
2 Writing chemical equations (Chapter 7) 5. Write and balance the complete molecular, complete ionic and net ionic equations for each of the following reactions. Refer to the solubility rules as needed. a. Aqueous sodium sulfate is mixed with aqueous calcium chloride. b. Aqueous ammonium phosphate is mixed with aqueous aluminum nitrate. c. Aqueous copper(ii) sulfate is mixed with sodium sulfide. d. Aqueous hydrochloric acid reacts with aqueous calcium hydroxide. Periodic Trends (Chapters 10 and 11) 6. What is electronegativity? 7. Which element is most electronegative? Least electronegative?
3 Lewis Structures/VSEPR (Chapter 6) 8. Draw Lewis structures for the following molecules and ions, including any formal charges and resonance structures. Also identify the of the molecule using VSEPR. PH 3 CO 3 2 O 2 SO 2 SO 3 C 2 H 4 C 2 H 2 H 2 N 2 Oxidation Numbers/Redox Reactions (Chapter 10) 10. Assign oxidation numbers and decide what substances are being reduced and oxidized in the reactions below. a. 2 HgO (s) à O 2 (g) + 2 Hg (l) b. 2 Al (s) + 3 FeO (s) à Al 2 O 3 (s) + 3 Fe (l)
4 Bonding & Intermolecular Forces (Chapter 7) 11. Explain the difference between an ionic bond and a covalent bond. 12. Explain the difference between bonds and intermolecular forces. 13. Use intermolecular forces to explain why H 2 O is a liquid, but H 2 S is a gas. 14. Use intermolecular forces to explain why Cl 2 is a gas, Br 2 is a liquid, and I 2 is a solid. Gases (Chapter 11) 15. For a friend's birthday, you buy a helium balloon with volume 4.20 L at 20. C. In order to get a better return on your investment, you decide to leave the balloon in a hot car until the temperature increases to 40. C. Assuming pressure is constant, find the new volume of the balloon. 16. In photosynthesis, the reaction 6 CO 2 (g) + 6 H 2 O (l) ¾ C 6 H 12 O O 2 (g) occurs. How many liters of oxygen at 20. C and 0.90 atm will be produced if 6.2 grams of water are consumed?
5 Solutions (Chapter 12) 17. What is the molarity of a solution of 3.2 moles of sugar in L? 18. If you dissolve 40.0 g CuSO 4 to a volume of 1.2 L, what is the concentration in moles/l? 19. How many liters of M Na2SO4 are needed to precipitate all the calcium ions in 6.24 L of M CaCl 2? CaCl 2 (aq) + Na 2 SO 4 (aq) à CaSO 4 (s) + 2 NaCl (aq) Acids and Bases (Chapter 15) 20. Write the Brønsted-Lowry definition of an acid and a base. 21. Identify the acid and its conjugate base in each of these reactions: HCl + H 2 O ¾ Cl + H 3 O + H 3 O + + OH ¾ H 2 O + H 2 O HS + OH ¾ S 2 + H 2 O H 2 PO 4 + HI ¾ H 3 PO 4 + I
6 22. Identify the acid and base in each forward reaction. a. CH 3 OH (aq) + HI (aq) CH 3 OH 2 + (aq) + I (aq) b. HSO 4 (aq) + HCO 3 (aq) H 2 CO 3 (aq) + SO 4 2 (aq) c. HSO 4 (aq) + HCO 3 (aq) CO 3 2 (aq) + H 2 SO 4 (aq) d. 2 CH 3 COO (aq) + H 3 PO 4 (aq) 2 CH 3 COOH (aq) + HPO (2 pts) Fill in the blanks (remember, conjugates differ by the presence of H + ). Acid CH 3 OH 2 + H 2 CO 3 Conjugate base SO 4 2 HSO (8 pts) Calculate the missing quantities: Solution [H 3 O + ] ph [OH ] poh Coke 2.5 acidic or basic? beer 3.16 x 10 7 bleach 2.00 x 10 2 seawater 5.78 pure water neutral Strong and weak acids/bases 25. Write definitions for weak acids/bases and strong acids/bases.
7 26. Write balanced equations that show the dissolution of: a. HCl in water b. Ca(OH) 2 in water 27. Calculate the ph, [OH ] and poh of a solution where [HCl] = 3.2 x 10 4 M. 28. Calculate the concentration of Ca(OH) 2 in a solution with ph
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