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chem midterm 1.pdf

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Gillian Goward

Name: ____________________ Student number: ______________ Chemistry 1A03 Test 1 October 10, 2008 McMaster University VERSION 1 Instructors: Drs. P.,, Dura1i0n: minutes This test contains 20 numbered pages printed on both sides. There are 25 multiple-choice questions appearing on pa ges numbered 3 to 17. Page 18 is extra sp ace for rough work. Page 19 includes some useful data and equations, and there is a periodic table on page 20. You may tear off the last page to view the periodic table and the data provided. You must enter your name and student number on this question sheet, as well as on the answer sheet. Your invigilator will be checking your student card for identification. You are responsible for ensuring that your copy of the question paper is complete. Bring any discrepancy to the attention of your invigilator. Questions 1 to 19 are each worth 2 marks, que stions 20 – 25 are each worth 3 marks; the total marks available are 56. There is no additional penalty for incorrect answers. BE SURE TO ENTER THE CORRECT VERSION OF YOUR TEST (shown near the top of page 1), IN THE SPACE PROVIDED ON THE ANSWER SHEET. ANSWER ALL QUESTIONS ON THE ANSWER SHEET, IN PENCIL. Instructions for entering multiple-choice answers are given on page 2. SELECT ONE AND ONLY ONE ANSWER FOR EACH QUESTION from the answers (A) through (E). No work written on the question sheets will be marked. The question sheets may be collected and re viewed in cases of suspected academic dishonesty. Academic dishonesty may include, among other actions, communication of any kind (verbal, visual, etc.) between students, sharing of mate rials between students, copying or looking at other students’ work. If you have a problem please ask the invigilator to deal with it for you. Do not make contact with othe r students directly. Try to keep your eyes on your own paper – looking around the room may be interpreted as an attempt to copy. Only Casio FX 991 electronic calculators may be used; but they must NOT be transferred between students. Use of peri odic tables or any aids, other than those provided, is not allowed. Page 1 of 20 Version # 1 Continued on next page Name: ____________________ Student number: ______________ OMR EXAMINATION – STUDENT INSTRUCTIONS NOTE: IT IS YOUR RESPONSIBILITY TO ENSURE THAT THE ANSWER SHEET IS PROPERLY COMPLETED: YOUT EXAMINIATION RESULT DEPENDS UPON PROPER ATTENTION TO THESE INSTRUCTIONS. The scanner, which reads the sheets, senses the bubble shaded areas by their non-reflection of light. A heavy mark must be made, completely filling the circular bubble, with an HB pencil. Marks made with a pen will NOT be sensed. Erasures must be thorough or the scanner will still sense a mark. Do NOT use correction fluid on the sheets. Do NOT put any unnecessary marks or writing on the sheet. 1. On SIDE 1 (red side) of the form, in the top box, in pen, print your student number, name, course name, (section number, instructor name) and the date in the spaces provided. Then you MUST write your signature, in the space marked SIGNATURE. 2. In the second box, with a pencil, mark your student number, exam version number (mark “1”, “2”, “3” or “4” and do not use the “0” bubble) (and course section number) in the space provided and fill in the corresponding bubble numbers underneath. 3. Answers: mark only ONE choice from the alternatives (,2,3,4,5 or A,B,C,D,E) provided for each question. If there is a True/False question, enter response o 1 (or A) as True, and 2 (or B) as False. The question number is to the left of the bubbles. Make sure that the number of the question on the scan sheet is the same as the number on the test paper. 4. Pay particular attention to the Marking+ Directions on the form. 5. Begin answering the question using the first set of bubbles, marked “1”. Page 2 of 20 Version # 1 Continued on next page Name: ____________________ Student number: ______________ See page 2 of the test for instructions. Questions 1-19 are worth two (2) marks each. 1. The element oxygen consists of more than one isotope. One naturally occurring isotope of oxygen is16O . Which of the following could also be an isotope of 8 oxygen? 16 (A) 9 O (B) 18O (C) 1O 2− 8 (D) Both (A) and (B) (E) Both (B) and (C) 2. To increase the volume of a fixed amount of gas from 0.100 L to 0.200 L, you would need to: (A) increase the temperature from 25.0°C to 50.0°C at constant pressure. (B) increase the pressure from 1.00 atm to 2.00 atm at constant temperature. (C) reduce the pressure from 0.80 atm to 0.40 atm at constant temperature. (D) reduce the temperature from 400 K to 200 K at constant pressure. (E) decrease the temperature from 600 K to 400 K. Page 3 of 20 Version # 1 Continued on next page Name: ____________________ Student number: ______________ 3. The Haber-Bosch process is one of the most important chemical reactions to produce large-scale amounts of ammonia (NH ). Ammonia is used in the fertilizer industry for 3 increased food production. Determine the temperature required to generate 20.0 kg of NH3 when the reaction is performed in a vessel that has a volume of 250.0 L with external pressure of 200. atm? N2(g) + 3H 2g) 2NH 3g) (A) -450 K (B) 5.12 K (C) 519 K (D) 220 K (E) 25,000ºC 4. A solution of HCl was made by pipeting 10.00 mL of 0.2945 M HCl and diluting with distilled water to a final volume of 45.00 mL. The resulting solution was titrated to equivalence with 21.45 mL of NaOH. What is the [NaOH] (M)? (A) 0.1373 M (B) 0.6458 M (C) 0.09871 M (D) 0.1893 M (E) 0.3489 M Page 4 of 20 Version # 1 Continued on next page Name: ____________________ Student number: ______________ 5. In which of the following circumstances would it be most appropriate to hit the panic button in the laboratory? (A) In the event a large volume of concentrated acid was spilled (B) If your lab partner cut themselves severly and are in need of immediate medical attention (C) To see what it does (D) In the event of a fire (E) If an empty beaker fell and broke on the ground 6. Which of the followingstatements regardingquantum mechanicsareFALSE? (i) The energy of a photon is prportional to its frequency. (ii) In a hydrogen atom, the electron has a fixed distance from the nucleus. (iii) As the velocity of a given particle getsbigger, its wavelength gets shorter. (iv) The size of atomic orbitals is mainly determinedby the magnetic quantum number. (v) For a given shell of a many-electron ao tm, d orbitals have higher energy than s orbitals. (A) i, ii, v (B) i, iii, v (C) ii, iii, v (D) iii, iv (E) ii, iv Page 5 of 20 Version # 1 Continued on next page Name: ____________________ Student number: ______________ 7. It takes 492 kJ of energy to remove one mole of electrons from the atoms on the surface of solid gold. What is the minimum frequency (in s ) of light capable of doing this? 14 −1 (A) 9.45 × 10 s -19 −1 (B) 6.64 × 10 s 15 −1 (C) 2.82 × 10 s (D) 1.23 × 10 s5 −1 (E) 5.56 ×10 −20s−1 8. Which one of the following is NOT a consequence of, or evidence for, ‘quantization of energy’? (A) The Bohr model for the hydrogen atom. (B) The frequency and wavelength of light are inversely related. (C) Atoms can only emit and absorb light of particular frequencies. (D) Bright red light is not able to eject an electron from a sheet of gold metal. (E) Neon signs have a distinct color, determined by the electronic transitions available to the gas. Page 6 of 20 Version # 1 Continued on next page Name: ____________________ Student number: ______________ 9. Which electron configuration represents an excited state of a neutral Si atom? (A) [Ar]4p 1 (B) [Ne]3s 3p 5 (C) [Ar]4s 4p 1 2 2 (D) [Ne]3s 3p 2 1 1 (E) [Ne]3s 3p 4s 10. A simplified version of a solar cell can be understood in terms of solid silicon (Si), responding to incoming electromagnetic radiation, and undergoing the photoelectric effect. If the binding energy of Si is 7.24 ×109J, what wavelength(s) (nm) of incident light will cause electrons will be emitted from Si? (A) λ = 277 nm (B) λ > 200 nm (C) λ ≤ 274 nm (D) λ ≥ 484 nm (E) λ ≠ 393 nm Page 7 of 20 Version # 1 Continued on next page Name: ____________________ Student number: ______________ 11. Which one of the following statements below is FALSE about the series of ions below: Cl Na + O 2− Rb Se 2- 2− + (A) O and Na are isoelectronic. 2− (B) Se has the largest ionic radius. + (C) Na has the smallest ionic radius. + − (D) Rb and Cl are isoelectronic. + + (E) Rb has a l
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