Chemistry 200: General Chemistry I - Lecture
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1 Name Date Chemistry 200: General Chemistry I - Lecture Exam #2, 100 Points Total Form: A Read all directions carefully. Answers not conforming to the directions will be marked as incorrect! Section 1: Matching (10 points) Match the following concepts with the appropriate definitions or examples listed below. Make selections such that each term has its best possible match. Indicate your choices by marking your Scantron sheet (1-10) with the appropriate two-letter code. ionic bond H + amu cations electronegativity Lewis dot symbol molecular formula spectator ions theoretical yield binary acid BC. proton AE. held together by +/- charge attraction CD. mass unit for an atom or molecule AB. increases towards top right of periodic table AC. small, positively-charged particles BE. calculated via stoichiometry BD. do not participate in a reaction AD. way to represent an atom and its valence e s DE. contains only hydrogen and a nonmetal in its formula CE. nonreduced formula 1
2 Section 2: Multiple Choice (40 points) Choose the term or phrase that best completes the sentence or answers the question. Indicate your selection by marking the appropriate letter on your Scantron sheet. 11. In Al 2 X 3, the element X must belong to Group None of these 12. What volume of M BaCl 2 is required to react completely with 42.0 ml of M Na 2 SO 4 if the net ionic equation for the reaction is Ba 2+ (aq) + SO2 4(aq) BaSO 4(s)? 12.1 ml 72.6 ml 145 ml 290 ml 13. Upon analysis, a compound is found to contain 22.8% sodium, 21.8% boron, and 55.4% oxygen. What is its simplest formula? NaBO NaB 2 O 5 Na 2 B 4 O 7 Na 3 BO The oxidation state of chromium in Cr 2 O 2 7 is
3 15. Which of the following pairs would form a metallic bond? Mg, S N, O Na, H Li, Li 16. Which of the following oxyanions has 3 oxygens in its formula? sulfur trioxide sulfite iodite hypobromite 17. The number of atoms in 9.0 g of aluminum is the same as the number of atoms in. 8.1 g of magnesium 9.0 g of magnesium 12.1 g of magnesium 18.0 g of magnesium 18. How many carbon atoms are in a 1.0 carat diamond ring weighing 200 mg? None of these 19. Which of the following compounds is expected to have the highest melting point? NaCl AgI PCl 5 MgO 3
4 20. How many moles of iron react with 1.75 moles of oxygen gas? The equation for the reaction is: 3O 2(g) + 4Fe (s) 2Fe 2 O 3(s) mole 1.75 mole 2.33 mole 5.25 mole 21. Which of the following has a 1 charge? phosphate sulfate ammonium bicarbonate 22. Which of the following compounds contains the greatest percentage of nitrogen? C 6 H 3 N 3 O 7 (MW = 229 g/mole) CH 4 N 2 O (MW = 60.1 g/mole) LiNH 2 (MW = 23.0 g/mole) Pb(N 3 ) 2 (MW = 291 g/mole) 23. Ammonia, NH 3, reacts with the hypochlorite ion, OCl, to produce hydrazine, N 2 H 4 according to the reaction 2NH 3 + OCl N 2 H 4 + Cl + H 2 O. How many moles of hydrazine are produced from 5.85 moles of ammonia if the reaction has a 78.2% yield? 2.29 moles 2.92 moles 4.57 moles 9.15 moles 4
5 24. In the combustion analysis of C x H y N z, the moles of nitrogen in the formula would be found via. the combustion product NO 2 the combustion product N 2 conservation of mass Combustion analysis cannot be used for this compound. 25. The concept of electronegativity applies to which of the following? F NaF HF All of these 26. What is the molarity of a solution made by dissolving 8.56 g of sodium acetate (MW = g/mole) in water and diluting to ml? 5.30 M M M M 27. The oxidation state of C in C 2 O 2 4 is Which of the following can participate in ionic, covalent, and metallic bonding? oxygen, O iron, Fe samarium, Sm None of these 5
6 29. Which of the following bonding modes involve the formation of cations? ionic covalent metallic ionic and metallic 30. Which of the following is a strong electrolyte? cadmium sulfide lead(ii) bromide barium hydroxide sodium sulfate 6
7 Section 3: Long Answer (10 points each) 31. Hydrochloric acid reacts with sodium carbonate according to the equation below. 5 points. If 14.0 ml of a M HCl solution reacts with g of Na 2 CO 3, how many grams of carbon dioxide will form? 5 points. How much of the excess reagent (in units of volume or mass, depending on which reagent is in excess) remains after the reaction? 2HCl (aq) + Na 2 CO 3(s) 2NaCl (aq) + H 2 O (l) + CO 2(g) 7
8 32. 4 points. Show the step-by-step formation of the bonding that occurs between sulfur and fluorine. 4 points. Show the step-by-step formation of the bonding that occurs between sodium and nitrogen. 2 points. Explain the reason behind the differences in the bond formation in your answers above. If there are no differences in the way you showed the formation of the bonding, write, None. 8
9 33. A ml sample of sulfuric acid is being titrated with a M potassium hydroxide solution. 5 points. Write the balanced molecular equation (including states) for the titration reaction. 5 points. If the equivalence point occurs at ml, what is the molarity of the sulfuric acid solution? 9
10 34. Complete the table below with the correct formula or name for the indicated compounds. Formula Name Ca(CN) 2 Co 2 O 3 GeCl 4 H 2 SO 3 selenium trioxide copper(ii) phosphate perbromic acid molybdenum(vi) sulfate 10
11 35. 6 points. Complete the two reactions below and balance the resulting equations. Remember to include states in the products. CdCl 2(aq) + AgNO 3(aq) Cr 2 (SO 4 ) 3(aq) + NaOH (aq) 4 points. below. Identify the reducing agent and the oxidizing agent in the reaction 2NaOH (aq) + Cl 2(aq) NaCl (aq) + NaClO (aq) + H 2 O (l). Reducing agent: Oxidizing agent: 11
12 Answer Key for Exam A Section 1: Matching (10 points) AE ionic bond BC. proton BC H + AE. held together by +/- charge attraction CD AC AB AD CE BD BE DE amu cations electronegativity Lewis dot symbol molecular formula spectator ions theoretical yield binary acid CD. mass unit for an atom or molecule AB. increases towards top right of periodic table AC. small, positively-charged particles BE. calculated via stoichiometry BD. do not participate in a reaction AD. way to represent an atom and its valence e s DE. contains only hydrogen and a nonmetal in its formula CE. nonreduced formula 1
13 Section 2: Multiple Choice (40 points)
14 Section 3: Long Answer (10 points each) 31. Answer: g of CO g of Na 2 CO 3 remains unreacted. 32. Answer: Three step drawing showing one Lewis dot structure of S and Lewis dot structures of F with lone electrons circled between the S and each F leading to a drawing of S connected to each F with single lines with lone pair electrons surrounding each atom leading to the formula SF 2. Three step drawing showing three Lewis dot structures of Na and one Lewis dot structure of N with harpoons drawn from Na s lone electrons to half-filled sites on the N leading to 3[Na] + and [N] 3 with the N surrounded with 4 electron pairs leading to the formula Na 3 N. In, the bond being formed is covalent, so sharing is indicated by circling electrons. In, the bond being formed is ionic, so electrons are shown as being transferred from the metal to the nonmetal. 33. Answer: H 2 SO 4(aq) + 2KOH (aq) K 2 SO 4(aq) + 2H 2 O (l) M H 2 SO Answer: calcium cyanide, cobalt(iii) oxide, germanium tetrachloride, sulfurous acid, SeO 3, Cu 3 (PO 4 ) 2, HBrO 4, Mo(SO 4 ) Answer: CdCl 2(aq) + 2AgNO 3(aq) 2AgCl (s) + Cd(NO 3 ) 2(aq). Cr 2 (SO 4 ) 3(aq) + 6NaOH (aq) 3Na 2 SO 4(aq) + 2Cr(OH) 3(s). Reducing agent: Cl 2(aq). Oxidizing agent: Cl 2(aq). 3
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