2007 Midterm

2007 Midterm - Dr Loza Chemistry 121 Thursday Autumn...

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Unformatted text preview: Dr. Loza Chemistry 121 Thursday Autumn Quarter 2007 October 18, 2007 FIRST MIDTERM EXAM 6:30 — 7:48 PM Name Lab. Instructor Signature Rec. Instructor 1. Fill out answer sheet as follows, using pencil only. (Ink will not record). a) Print your last name, starting at the far left, FILL IN THE CORRESPONDING LETTER UNDER EACH LETTER IN YOUR LAST NAME. b) Leaving one space after the last name, print your first name and FILL IN THE CORRESPONDING LETTER UNDER EACH LETTER IN YOUR FIRST NAME. c) MI means "middle initial". Leave one space after your first name, print your middle initial, FILL IN THE CORRESPONDING LETTER UNDER YOUR MIDDLE INITIAL. d) Place your signature on the line above your printed name. e) You MUST indicate your two-digit section number. 1. Locate your LAB day/time FIRST, 2. Find your TA'S NAME, 3. Fill in the TWO-DIGIT NUMBER for your section on the answer sheet starting in COLUMN "K" in the SPECIAL CODES SECTION. f) Fill in the IDENTIFICATION NUMBER starting in COLUMN A with your Carmen Student ID Number. g) DO NOT fill in sex or birth date. Find lab da /time, then TA. and enter two di it section number. Tuesday 8:30 or 9:30 Thursday 8:30 or 9:30 Monica Luo 38 Pat Bullinger Chris Check 39 Tamara Klotzback Kamala Kunchithapatham 40 Scott Burya Natalie Hage 41 Anita Chong Nick Durham 42 Dan Hyatt 43 Guang Li Morgan Weber 2. When the proctor gives the signal, but not before, check to see that there are 8 numbered pages, a Periodic Table and Solubility Guidelines. 3. There are 30 multiple choice questions for a total score of 175 points. 4. You must mark answers on the answer sheet in PENCIL. Fill in all answers COMPLETELY with PE_N(l. If you wish to change an answer, erase the unwanted mark COMPLETELY. 5. Use the blank page for scratch work, but note that only the marks you make on the answer sheet will be observed by the grading equipment. 6. The time allowed is 1 hour, 18 minutes. 7. At the end of the examination, you must hand in the ANSWER SHEET before leaving the room 1. (5 pts) Which of the following statements is correct? a) A compound may contain only one type of atom. b) A pure substance must contain only one type of atom. c) A heterogeneous mixture must contain at least three elements. d) A homogeneous mixture must be uniform. e) A mixture containing two compounds must be heterogeneous. 2. (6 pts) Calculate the following to the correct number of significant figures (4.26 x 72.3) x (0.038 + 2.000) a) 628 b) 627.7 c) 627.69 d) 630 e) 6.3 x102 3. (7 pts) A crucible is known to weigh 35.4273 9. Three students in the class determine the weight of the crucible by repeated weighings on a simple balance. Using the following information, which student has done the most accurate determination? Trial 1 Trial 2 Trial 3 Trial 4 Trail 5 a) 35.9 35.0 35.3 35.2 35.4 b) 35.9 36.0 35.9 36.0 35.9 c) 35.6 35.4 35.6 35.5 35.4 4. (6 pts) An empty graduated cylinder weighs 56.9854 9. After 20.0 mL of liquid is added, the cylinder and its contents weigh 83.6526 9. What is the density of the liquid in g/mL? a) 2.44 g/mL b) 2.444 g/mL c) 1.333 g/mL d) 1.33 g/mL e) 1.93 g/mL 5. (5 pts) Which statement below correctly describes the responses of alpha, beta and gamma radiation to an electric field? a) Both beta and gamma are deflected in the same direction, while alpha shows no response. b) Alpha and beta are deflected in opposite directions, while gamma shows no response. 0) Only alpha is deflected, while beta and gamma show no response. d) Both alpha and gamma are deflected in the same direction, while beta shows no response. e) Both alpha and beta are deflected in the same direction, while gamma shows no response. 6. (6 pts) Which of the following statements is(are) true? a) 18O and 19F have the same number of neutrons. b) 14C and 14N are isotopes of each other because their mass numbers are the same. 0) 1802' has the same number of electrons as 20Ne. d) a and b e) a and c 7. (5 pts) Which are the properties of metals? |. all solids IV. luster ll. brittle V. form ionic compounds Ill. conductor Vl. insulator a)|,||,lll b)|,|l|,V c)|l, IV, VI d)||,V,V| e)|||,|V,V 8. (5 pts) Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? 9. (6 pts) Which of the following does not occur as a diatomic molecule in the elemental form? a)oxygen b) nitrogen c)su|fur d) hydrogen e) bromine 10. (5 pts) An ion is formed a) by either adding or subtracting protons from the atom. b) by either adding or subtracting electrons from the atom. c) by either adding or subtracting neutrons from the atom. d )All of the above e) two of the above 11. (5 pts) What is the symbol for the phosphate ion? a) PO" b) P033' 0) P044" d) PO43' e) PO4' IN.) 12. (5 pts) What is the chemical formula for iron(l|l) sulfate? a) F92(SO4)3 b) FG3(SO4)2 C) F8(SO4)4 d) F63SO4 e) F8804 13. (5 pts) The correct name of P205 is a) phosphorous oxide b) diphosphorous pentoxide c) phosphoric oxide d) phosphorous oxide e) phosphorous pentoxide 14.(5 pts) HBrO4 is which of the following acids? a) hydrobromic acid b) perbromic acid 0) bromic acid d) bromous acid e) hypobromous acid 15. (7 pts) Balance the following equation for the oxidation of ammonia. What is the sum of the whole number coefficients of the reactants and products? _NH3(Q) + _02(g) —> _NO(9) + H20(g) a)11 b)14 c)19 d) 20 e)22 16.(6 pts) Determine the mass percent of nitrogen in copper(|l) nitrate to 3 significant figures. a) 3.55% b) 7.81% C) 11.5% d) 14.9% e) 18.3 0/o 17. (6 pts) How many atoms of gold are in 3.0 g of gold? 8) 9.2 x1021 atoms b) 2.3 x1020 atoms 0) 5.8 x 1022 atoms (:1) 1.9 x 1023 atoms e) 4.7 x1021 atoms 18. (6 pts) The mass percent of iron in an iron oxide is 77.7%. Find the empirical formula. a) F9203 b) Fe304 c) F8203 d) FeO e) None ofthese 19. (9 pts) Caproic acid, the compound responsible for the aroma of dirty gym socks and running shoes, contains carbon, hydrogen and oxygen. On combustion analysis, a 0.450 g sample of caproic acid gives 0.418 g water and 1.023 g carbon dioxide. What is the empirical formula of caproic acid? a) c4Hgo b) c3Hso C) C5H902 d) C4H1002 e) CaHaOz 20.(7 pts) Household bleach (sodium hypochlorite) is prepared by the reaction of sodium hydroxide and chlorine. How many grams of sodium hydroxide are needed to react with 50.0 g of chlorine? 2 NaOH(aq) + Cl2(g) —> NaOCl(aq) + NaCl(aq) + H20(l) 21. (7 pts) Magnesium metal reacts with oxygen to give MgO. If 5.00 g of Mg and 5.00 g of oxygen are allowed to react, what weight of MgO will be formed? 2 M9(S) + 02(9) —> 2 M90(S) 22. (5 pts) A weak electrolyte exists predominately as in solution. a) atoms b) ions 0) molecules d) electrons e) isotopes 23. (6 pts) Which of the following are strong electrolytes? HCI HCZH302 NH3 KCI Cu(N03)2 a) one of the above b) two of the above 0) three of the above d) four ofthe above e) all of the above 24. (6 pts) Will a precipitate reaction occur when aqueous solutions of CdCI2 and (NH4)2S are mixed? a) precipitation will occur forming one solid. b) precipitation will occur forming two solids. c) precipitation will not occur. d) no precipitation will occur but reduction of cadmium will occur. e) no precipitation will occur but oxidation of sulfur will occur. UI 25. (7 pts) The balanced net ionic equation for the reaction occurring when solutions of silver nitrate and sodium iodide are mixed is 8) Ag+(aQ) + |'(aq) —> Ag|(S) b) Ag+(aq) + NOs'(aQ) —> AQN03(S) 0) Ag+(aQ) + N03'(aQ) —> AgNOs(aq) d) AgNOg(aq) + Na|(aq) —> Agl(s) + NaN03(aq) e) AgN03(aq) + Na|(aq) —> Agl(aq) + NaNO3(s) 26. (5 pts) The oxidation number of chromium in Cr2072' is d) +4 e) +3 27. (6 pts) Consider the following reactions AgNOs(aQ) + Zn(s) —> Ag(s) + Zn(N03)2(aq) Zn(N03)2(aq) + Co(s) —> no reaction A9N03(aQ) + C0(3) —> Ag(s) + CO(N03)2(3CI) Which is the correct order of increasing activities for these metals? a) Ag<Zn<Co b) Co<Ag<Zn c) Co<Zn<Ag d) Ag<Co<Zn e) Zn<Co<Ag 28. (6 pts) What is the molarity of 0.195 g of cholesterol (027H4GO) in 100 mL of blood serum? a)5.0 x 10'3 M b) 8.6 x103 M c)9.8 x103 M d)3.0x10'4M e) 7.2 x10'4M 6 29.(7 pts) What is the molar concentration of I3' if 24.55 mL of 0.206 M Na28203 is needed for the complete reaction of 10.00 mL of the l3' solution? The net ionic equation is 2 32032'(aQ) + '3'(aQ) —* S4062'(a<1) + 3 Hal) a) 0.253 M b) 0.367 M c) 0.411 M d) 0.154 M e) 0.321 M 30.(4 pts) Which of the following is not a strong acid? a) HCI b) st04 c) HCIO4 d) HCN e) HNo3 Am Iv >853 ZEdvoa F» Wu Iv HESS: $553 E> H<> <> S> ENE Iv Wnrfifiw 3930 30mm? S 3 G a 3 055% NE a: U) a fi < O H wopo k5.0m RX mm Aflmm mob“? mmbo mu mm Lo 52 AN mmLh quN poN oNbH wmbh wmbH mm mm .N 1\. Om w» UPS Guam mu mm u 5) Wm NNmbN mu.wa N m E d mm H» d< Wm 3.3 50.8 59% :32 :3 a N3: >nnaamm 3 mm 3 i a a S a a a 2 H.» Om 3. Ga H6 6% mo ma HS 45.. F: a 5.2 $0.5 $9.2 . 55 E8 350 398 3va 398 5.? ES 3 8 ma 3 3 8 :5 :: H8 _. >n H: 08 WW Om mm Eu 3.» HH 1‘. .. ~58 a»? 3:: ~38 ~38 “3.3 8:; ~32 MS: “mm: 893 #3.: Soluble Ionic Compounds SolubilitYClUidelines tor Ionic-Compounds in _Water Important Exceptions N 03— C2H302_ Cl— Br— I_ 5042— Compounds containing None None Compounds of Agl‘, H32 2+, and Pb2+ Compounds of Ag+, Hg22+, and Pb2+ Compounds of Ag+, Hg“, and Pb2+ Compounds of 812+, Ba2+, Hg22+, and Pb2+ Insoluble Ionic Compounds Important Exceptions Compounds containing 82— C032‘ PO43— OH— Compounds of NH4+, the alkali metal cations, and Ca2+, 812+, and Ba2+ Compounds of NI-Lfr and the alkali metal cations Compounds of NH4,+ and the alkali metal cations Compounds of the alkali metal cations, and Ca2+, 813+, and Ba2+ ...
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This note was uploaded on 10/22/2008 for the course CHEM 121 taught by Professor Wyzlouzil during the Spring '07 term at Ohio State.

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2007 Midterm - Dr Loza Chemistry 121 Thursday Autumn...

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