[Bush] Chemistry Exam #1 - Fall 2007

[Bush] Chemistry Exam #1 - Fall 2007 - NAME Chemistry 1301...

Info iconThis preview shows pages 1–12. Sign up to view the full content.

View Full Document Right Arrow Icon
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 2
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 4
Background image of page 5

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 6
Background image of page 7

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 8
Background image of page 9

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 10
Background image of page 11

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 12
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: NAME Chemistry 1301 Fall 2007 (M. A. Busch) Exam #1 PLEASE READ THESE INSTRUCTIONS CAREFULLY BEFORE BEGINNING THIS EXAMINATION. Select the single best response to each question. There is only one best response to each question unless otherwise indicated in the question. There are 40 questions on this examination. The first 30 are worth 3.0 points each, and the last 10 are worth 1.0 point each. (Total of 100 points.) Check your test booklet to be sure you have a complete exam with all 40 questions. Write your NAME and SECTION NUMBER on your Scantron answer sheet. Write your name on the first page of the test booklet also. Work each problem carefully on the test booklet or on the scratch paper provided. Then select the answer that you feel is the best response. ALL ANSWERS MUST APPEAR ON THE ANSWER SHEET. Your grade will be determined only by what appears on the answer sheet, not by work on the test booklet. Look over your exam and work the easiest problems first, saving the more difficult ones for last. Be sure that you have correctly indicated your final choices on the answer sheet before turning in your paper. If a question is incorrectly marked on the answer sheet, it will be counted wrong even if it was correctly marked on the test booklet. If you have any questions about any of the problems on this exam, it is your responsibility to ask for a clarification from the instructor during the examination. You should have plenty of time to do this exam, so please check your answers carefully before turning in your paper. 1. A student obtains the number 1200.04674 on her calculator. If this number actually has only four (4) significant figures and is correctly rounded off, how should it be written using scientific notation? _ a) 1.2 x 103 ‘ , 5.5; ‘1) db“ wgamwmi b) 1.20 x 103 3 (::)1.200 x 103 \0 IO ‘13wa 0(41 . ‘15 d) 1 2000 x 103 m Pun wad; “flu—“’5‘ ' Acct.me m e) none of the above 2. A compound consists only of two elements, carbon and oxygen. If a pure sample of this compound contains 12.011 grams of carbon and 15.9994 grams of oxygen, what is the percent oxygen by mass? Express your answer to 4 significant figures. a) 27.29% oxygen Wm:— \’Z..©\\ ‘53 C- b 42.88% oxygen ‘b'qoflq 9 O @57.12% oxygen 28'0‘94 0 o . d) 72.71% oxygen /OO>.L‘S;LL: [53901457400 .: 57.‘2/b e) none of the above 2%.m04 ' ‘an’kOZtSX'. 3. The atomic masses in the periodic table are not whole numbers because a) we can't measure the masses closely enough to express the results as whole numbers b) atoms gain and lose electrons easily, thus changing the mass significantly 0) real samples are always contaminated with other elements d) atoms of the same element have different numbers of protons the masses are weighted averages of the naturally occurring isotopes 4. Which one of the following sets of compounds could be used to illustrate the Law of Multiple Proportions? a) C02, H20 and 802 NO, N02 and N20 Sam 2 c) NBr3, NH3 and NCl3 nan—hos d) CaClz, CaBrz and CaI2 e) C2H4, N2H4, and Si2H4 5. The accuracy of a data set is considered to be poor, if _ a) the data vary widely from the average value. pom mm b) the data are a set of closely spaced numbers. 3m W'\ C the average of the data is close to the actual value. CLMC‘LCLMS the average of the data is far from the actual value. mmU-mcfl e) the precision of the data is poor. WW w‘ {301-46) WW3 <14 01¢ij ' 6. What is the volume, in mL, of 1000. g of ethanol if the density of 7. 8. ethanol is 0.789 g/mL? Cfl_:‘gi (:rIQAJ nnL ‘Tzfilmna b) 789 mL 3 c) 7.89 x 103mL V ,_ C3, .900. 3(mL L. .LQB-74..Mo d) 0.789 mL 3— 037892; f; 5.5:, e) 1.27 mL fag; Md? % \-27$(DmL The following calculation was performed on a calculator. After performing all calculations, round off the final answer to the correct number of significant figures, and express the answer in scientific notation 4 (264.7 + 102) / 0.010 = 36670 3.7 x 10 e .7 (ED 4 +¥o§ 3bé-7 . + b) 3.67 x 10 4 666,? __,,_.___i -; agave), 2 3.7‘510 c) 3.667 x 10 _' 0.0!9 1x 4 sxr (5.) 3.6670 x 10 t5sF. 7‘25? mtfw¢up e) none of the above nmxkpq\ I . In theAperiodic table, elements are arranged in a) alphabetical order b) order of increasing atomic mass (9 d) order of increasing neutron count order of increasing atomic number e) something else Complete the following sentence: (99‘91xfiko are pure substances with constant composition and made up of more than one element. a) alloys b) homogeneous mixtures c) elements compounds e) heterogeneous mixtures 10. Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? @ Ca, Sr b) Cs, Ba c) H3 Li d) Ga, Ge e) C, 0 Lb! 3 3 11. Supply the missing number: ; g/cm = kg/m 7 a) 1.61 x 104 k5; fb 3 1 q , b) 1.61 x 102 “5L1 __ £9.23 - IQIMO 5 ma "~ng \m m3 0) 1.61 x 161 d) 1.61 none of the above 12. Which one of the following represents a chemical property? a) a block of wood floats on water b) a slab of marble feels cold to the touch wfiLCQJ c) lead is more dense than water M d) an iron nail is attracted to a magnet none of the above represents a chemical property 13. Which one of the following is an intensive property? a) volume cnUanme density W04 2 $64515 I'D" W on C) mass 9A2»;th db .erum «smut d) length P! ‘ e) none of the above is intensive 14. A 0.455-g sample of magnesium is allowed to burn in 2.315 g of oxygen gas. The only product is magnesium oxide. After the reaction, no magnesium remains and the mass of unreacted oxygen W (oxygen left over) is 2.015 g. What mass of magnesium oxide was produced? 0.4539 on H9 #5 cub-‘QQ ope. @ 0.755 g magnesium oxide (2.55 _ 2'0l55>0 (3.5211 0.3003 b) 2.77 g magnesium oxide 3 O .7559 c) 2.47 g magnesium oxide pwadbck d) 0.300 g magnesium oxide e) none of the above 15. Which one of the following statements about atomic structure is false? Choose response (e) only if (a)—(d) are all correct. a) The number of protons determines the identity of the atom. b) Almost all of the mass of the atom is found in the nucleus. c) The electrons are spread out in a much larger volume of space compared to the nucleus. d) The number of protons equals the number of electrons in a neutral atom. & of the above are true. (Choose only if a—d are all correct.) 16. John Dalton proposed the atomic theory in 1803 a) after careful reading of ancient Greek and Latin manuscripts. GE» on the basis of the laws of conservation of mass, constant composition, and multiple proportions. c) based on the predictions of Noiradamus. d) while conducting experiments on changing lead into gold. e) after attending a lecture by Antoine Lavoisier in Paris. 17. A column in the periodic table is often referred to as a) a period a c) a series a n group d) 9) quantum one of the above 18. An element is designated as “Rx. Element Xnmst be: a) Zn . . b) Ru X Wm Mr W C) S A moer he, 3' Si e) none of the above 19. A neutral atom of Hg-201 has a) 201 neutrons Vka L11” 5&3 Prc¢uyLb 121 neutrons 10‘ ‘94.“ C) 80 neutrons - '80 p d) 281 neutrons |2| rvuufitxxb e) none of the above 20. In a recent accident some drums of uranium hexafluoride were lost in the English Channel. The melting point of uranium hexafluoride is 64°C. What is the melting point of uranium hexafluoride on the Kelvin scale? Absolute zero is —273%L a) —209 K K; DC, + 937?) b’ “3 K = Juan : am K c_ 32 K d) 337 K e) none of the above 21. From its position in the periodic table, the element selenium- would best be considered as a) a metalloid b) a transition element 0) a metal (j) a non—metal e) a lanthanide (an inner transition element) 22. From its position in the periodic table, the element antimony would best be a considered as a metalloid b) a transition element c) a metal d) a non-metal e) a lanthanide (an inner transition element) 23. From its position in the periodic table, the element bismuth woulc best be considered as a) a metalloid b) a transition element (E? a metal d) a non—metal e) a lanthanide (an inner transition element) 24. Atoms with the same atomic number but different mass numbers are called a) positrons b) isomers c) elements isotopes e) none of the above 25. According to the Law of Constant Composition a) if the same two elements form two different compounds, they dc so in the ratio of small whole numbers. b) it is not possible for the same two elements to form more than one compound. (::> the ratio of the masses of the elements in the same pure compound is always the same. d) the total mass after a chemical change is the same as before the change. e) elements under one another in the Periodic Table tend to behav in a similar manner. 26. The Periodic Table is one of the great intellectual achievements in chemistry and represents the great systematizing principal in chemistry. The scientist most closely associated with the development of the periodic table, and pictured in cartoon form 0 the last page of this exam, is a) John Dalton b) Antoine Lavoisier c) Svante Arrhenius d) Joseph Proust (::>someone else tJmufidggstV 27. Which one of the following compounds is ionic ? a) CCl4 b) PCl3 c) NCl3 @ CaClz metal + nonmdzal e) none of the above 28. Naturally occurring element X consists of the two isotopes: Xle and X—12. The atomic mass of X is approximately 10.4. What is the best estimate of the relative percentages of X—lO and X—12, respectively? 90% x—10 d 10% x—12 V _ an (we) =mmcd 0Lth ‘7 x ‘2' 80% x—10 and 20% x—12 n) 70% x—10 and 30% x—12 IDOL} + “1.4%: 10.4— d) 60% x-10 and 40% x-12 ,Ox+,2_.2x = {OH-P 8‘.) 50% x—10 and 50% x—12 Mo = 29. Whose name is associated with the invention of an analytical balance and is sometimes called the "Father of Modern Chemistry"? (:9 Antoine Lavoisier b) John Dalton c) Dmitri Mendeleev d) Albert Einstein e) Joseph Proust 30. Which one of the following is classified as an acid? a) Ba(OH)2 b) NaCl (9 H2C03 d) NH3 e) none of the above- THE FOLLOWING NOMENCLATURE QUESTIONS ARE WORTH ONE POINT EACH. 31. Which one of the following names is incorrectly paired with its symbol? Choose (e) if all are correctly paired. a) gallium = Ga b) germanium = Ge c) platinum = Pt d) rhodium = Rh all of the above are correctly paired. 9 32. Which one of the following names is incorrectly paired with its symbol? a) bismuth = Bi ‘ . @ iridium = I I:pCLL~(\o_ It; vnckwnm c) mercury = Hg d) cerium = Ce e) all of the above are correctly paired. 33. Which one of the following names is incorrectly paired with its symbol? Q thallium = Th “E: thomw b) cesium = Cs tkafl‘m: TL c) lanthanum = La d) sodium = Na e) all of the above are correctly paired. 34. Which one of the following names is incorrectly paired with its symbol? a) manganese = Mn b) mercury = Hg c) osmium = Os d magnesium = Mg all of the above are correctly paired 35. Which one of the following symbols is incorrectly paired with its name? '; (DJ—1m \‘Ca (E) Ar = arsenic lx‘ cmkfiéd\ S“: b) Fe = iron pk 0) Au = gold d) Zn = zinc e) all of the above are correctly paired 10 36. Which one of the following symbols is incorrectly paired with its name? a) Mo = molybdenum ® Re = rubidium C) Pd = palladium d) Cu 9) all of the above are correctly paired YQQ: w Yau::~rufiiui\LNY\ H copper 37. Which one of the following symbols is incorrectly paired with it name? a) Ag = silver b) Ti = titanium c) Cd = cadmium 3n:+~‘,\ 5k, :anhmmmi Sn = antimony e) all of the above are correctly paired 38. Which one of the following symbols is incorrectly paired with it name? @ A = argon AV :msm WM no QLMMJ megawatt) A b) B = boron c) C = carbon d) F = fluorine e) all of the above are correctly paired 39. Which one of the following symbols is incorrectly paired with it name? a) Sr = strontium b) Ru = ruthenium c) Zr = zirconium d) S = sulfur all of the above are correctly paired 11 40. which one of the following symbols is _i_r_100rrectly paired with its name? a) AC : actinium b) Fr = francium c) Pu = plutonium ) Rn = radon all of the above are correctly paired P J?“ r: ..- ' “Hf, l2 ...
View Full Document

This note was uploaded on 04/08/2008 for the course CHE 1301 taught by Professor Klausmeyer during the Fall '08 term at Baylor.

Page1 / 12

[Bush] Chemistry Exam #1 - Fall 2007 - NAME Chemistry 1301...

This preview shows document pages 1 - 12. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online