Fall 2007 October 18,2007

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1 Chemistry 121 Exam 1 Fall 2007 October 18,2007 Oregon State University Dr. Richard Nafshun Instructions: You should have with you several number two pencils, an eraser, your 3" x 5" note card, a calculator, and your University ID Card. If you have notes with you, place them in a sealed backpack and place the backpack OUT OF SIGHT or place the notes directly on the table at the front of the room. Fill in the front page of the Scantron answer sheet with your test form number (listed above), last name, first name, middle initial, and student identification number. Leave the class section number and the test form number blank. This exam consists of 25 multiple-choice questions. Each question has four points associated with it. Select the best multiple-choice answer by filling in the corresponding circle on the rear page of the answer sheet. If you have any questions before the exam, please ask. If you have any questions during the exam, please ask the proctor. Open and start this exam when instructed. When finished, place your Scantron form and note card in the appropriate stacks. You may keep the exam packet, so please show your work and mark the answers you selected on it. 1 inch = 2.54 cm (exact) 1000 mm = 1 m 1 mole (NA) = x dm=lm 1000 m = 1 km 1000mL= 1 L 100 cm = 1 m 10rnm= 1 cm Lithium 1 Bcrylltum Boron I Carbon 1 Nirmgen I Oxygen I Fluorine,I Neon Potassium I Calcium VII IIIB IVB VB VIB V W t 1 1B IIB Ti V Cr Mn Sc Scandlum Trtan~um Vanadium Chramtum Manganese Iran Cobalt Nickel Copper Zinc ie Co Ni Cu Zn 1 Ga Aluminum Silicon Phosphoms Sulfur Chlorine Argon I Se Ge 1 As Br Kr Gallium Germanium Anenic Selenium Bmmine Krypton Rb Rubidium Sr Strontium Y Yurium Zr Zirconium Nb Niobium Mo Molybdenum Tc Techneuum Ru Ruthenium Rh Rhodium Pd Palladium Ag Silver Cd Cadmium In Indium Sn Tin Sb Antimony Te Tellurium I Iodine Xe Xenon Cs Cesium Fr Francium (223) 56 Ba Barium Ra Radium *Rare earths t~ctinidcs Rutherfordium Hf Hafnium Rf (261) 73 Ta Tantalum Ha Hahnium (262) 74 W (263) 75 Re l'ungften Rhenium Osmium Iridium : Sg 107 Ns 108 Hs 109 Mt Seaborgium Ncilsbohrium Hassium Meiknerium (262) 76 0s (265) 77 Ir (266) 78 Pt Platinum I0 % (269) 79 Au Gold % 80 Hg Mercury 8 1.T1 Thallium Pb Lead 2M Bi Bismuth Po Polonium (209) 85 At Astatine (210),Stable region? 86 Rn &on (222) 57 La mthanium Ac - 58 Ce Cerium Th 59 Pr Pa 60 Nd 144.M 92 U 61 Pm Praseodymium Neodymium Romethium Sm Samarium Np Aclinium I Dorium I htacunium Uranium Neptunium I Plutonium I Am:2km Berkelium 1 Californium Einsteinium Fermium lmcndclcvium Nobelium I Law;ium (2MI 1' Oil) 1,254, 1,757, c7511) 1, Pu 63 Eu Europium Am 64 Gd Gadolinium Cm 65 Tb Terbium Bk 66 Dy Dysprosium Cf 67 Ho Holmium Es 68 Er Erbium M) Fm 69 Tm Thulium Md 70 Yb Ytlerbium No Lu Lutetium Lr

2 1. A student measures the length of a green crystal to be 0.09l470-m. There are seven significant figures in this measured quantity. There are three significant figures in this measured quantity. 3,.,, #,+ \cu"'""'""'2 yrracr +. M-. ri3%a ~ C G s; 3 re (&., Lt-C ~<PPc+cA a5 MC&$*eCd) 2. A student combines 12.1 g of iron chloride and g of nickel oxalate. The mass of the mixture (with the proper number of significant figures) is: I x 1 o4 g 1.64~10~~ 3. Which of the following statements is FALSE? e. A neutral atom has an equal number of protons and electrons. An electron is roughly ' the mass of a neutron. 4. Which of these pairs of elements would most likely combine to form a molecule? He and Li Pae and F Mg and Sr K and Br ~zg-=

3 Which of these pairs of elements would be most likely to form an ionic compound? P and Br Cr and K C and 0 6. Which of the following figures best represents stable isotopes? protons (A> protons protons

4 A student measures the volume of a Potassium Trioxalatoferrate (111) crystal to be inches3. Expressed in rnm3, this volume is: 1.351x10"mm mm x10-~mm~ in3(, 5 jc 1:; \ :ri 3 87 I,B M M 8. The two stable isotopes of beaverium are Bv-28 1 (mass = amu and a percent abundance of 23.55%) and Bv-283 (mass = amu and a percent abundance of 76.45%). What is the average mass of beaverium? '-',+, amu (26, $,.3 am*)(0.235~)+ (2Q3,i91An.X~.?h~i~) ' 35.7amu amu amu 281.9arnu 9. Consider (NH4)3PO4. Each unit contains: a (El One nitrogen ion, four hydrogen ions, one phosphorous ion, and four oxide ions Twelve ammonium ions, one phosphorous ion, and four oxide ions horus ion, and four oxide ions

5 10. A student places grams of an irregularly shaped piece of metal into ml of water in a graduated cylinder. The water level rises to ml. The metal is: A1 (d = 2.72 g/ml) Au (d = g/ml) Pt (d = g/ml) Vm 73\,79 g 8% -q-" = 1 \ \3CI ~ / M L \b.7-smk - Sb.Za*h ~m2+ has: 95 protons, 24.1 neutrons, 95 electrons +\.w 146 protons, 146 neutrons, 97 electrons 95 protons, 146 neutrons, 97 electrons 9s %+ -. e 12. Which of the following sets of elements are expected to have similar properties? Sulfur and chlorine Sulfur and argon 13. Which of the following chemical formulae is incorrect? Ba3(P04)2

6 14. The name of Ca(N03)2 is: calcium nitri e calcium dinitrate calcium dinitride monocalcium dinitride 15. Two elements that will form 2+ ions in ionic compounds are: IV and P 0 and S LJ Grasp The mass percent compositions of the elements in dimethyl ether, C2H60, are: C=12.011% H = % 0 = % C = % H = % 0 = % 4# G(\a\ar M*rs 4 b.a7 Ybb, 17. Which of the following pairs are isotopes? 12c and 12c. Sane r\=wmt (~nc nrnbcr og 14c and 14~. pr6t.n~) br+ d;fcirm+ nu-b~r (Dl O& n+\.-h~-o* a, (El

7 18. Provide the coefficients needed to balance the following combustion equation:., -rh -*- a=7 b = 22 c= 14 d= 16 a= 1 b = 22 c=7 d=8 a=2 b= 11 c= 14 d=8 19. Consider the following reaction: 2 Na (s) + 2 H20 (1) -+ 2 NaOH (aq) + H2 (g) In a given experiment, the theoretical yield of H2 (g) for the above reaction is 7.00g. If the reaction actually produces 2.50 g hydrogen gas, what is the percent yield for the reaction? 0.50 % a 2.80 % 17.7% 5.7% 7.a0 20. Consider the following reaction: 4 P (s) (g) -+ P4010 (s) How many moles of P4Ol0 (s) are produced from Bi moles of P (s) in an excess amount of O2 (g)? 1 mol P4010 (s) 16 mol P4010 (s)

8 21. The mass of a single carbon atom is: grams x 1 grams 12.0 (Dl (El \\ Q/,,,ol \ wo( -23 qi -\,9elSxre, - 6, o ~ z 23 ~ ia o f DM$ a+on 22. A student places grams of sodium chloride into a liter volumetric flask and fills to the mark with water. What is the molarity (a unit of concentration) of the solution? 1.350M ~7i5zGi-J M M M 6, \ \S 5 mo\ M= - = = o. a23\u bq 5,000 L 23. A student obtains grams of H20 (1). How many water molecules are present? x 1 o~~ H20 molecules x 10" '20 molecules x 10" H20 molecules

9 24. A student combusts grams of propane, C3H8 (g), in an excess amount of oxygen. How many grams of H20 (g)are produced? grams of H20 (g) are produced grams of H20 (g) are produced 25. Because of Chemistry I get lots of dates by using pick-up lines that include the words charge, centimeters, molecules, charge, neutrons, metalloids, ions, and combustion. My appreciation for art has increased. I have laughed more times in the past three weeks than I have in the previous three years. n about Lindsay Lohan -at least until 3 seconds ago!

10 [Any response will receive full credit; even no response.]

This resource contains three different versions of the periodic table, including a blank one for colouring!

Teaching notes This resource contains three different versions of the periodic table, including a blank one for colouring! It also contains tables of the Group 0, 1 and 7 elements with a few columns for