NOTE: The first ~4 pages of this document are …learnfaster.ca/wp-content/uploads/chem201/TT1/TT1---Concise... · Chem 201 – Term Test 1 – 2015 Winter *These are the summarized

NOTE:

The first ~4 pages of this document are summarized solutions so you can quickly check your answers and get a grade.

The later pages contain all the steps involved and any explanations needed to answer the questions given – this is why this document is ~30 pages.

If, after looking over the worked solutions in the later pages you still do not understand the questions, feel free to email me at [email protected] and I can point you in the right direction.

All the best!

(C) Pavel Sedach/Learnfaster.ca and Prep 101 1


mailto:[email protected]

Chem 201 – Term Test 1 – 2016 Winter

*These are the summarized solutions. There are worked solutions for each question in the later pages.

Multiple Choice

1. A

2. B

3. E

4. A

5. C

6. B

7. D

8. B

9. B

10. D

11. E

Written – see worked solutions in later pages





Multiple Choice

1. A

2. D

3. NO CORRECT ANSWER

4. E

5. A

6. B

7. C

8. A

9. C

10. D

11. C

12. C and B




Chem 201 – Term Test 1 – 2015 Fall


Multiple Choice

1. D

2. C

3. A

4. B

5. D

6. A

7. E

8. E

9. A

10. C

11. B






Multiple Choice

1. A

2. D

3. C

4. E

5. C

6. C

7. D

8. A

9. E

10. D

11. A

12. C

13. A

14. E

15. B

16. E






Multiple Choice

13. C

14. B

15. D

16. A

17. E

18. B

19. C

20. C

21. D

22. B

23. E

24. D

25. D

26. C

27. A

28. E






Multiple Choice

1. C

2. B

3. B

4. A

5. C

6. B

7. D

8. B

9. A

10. E

11. B

12. D

13. D

14. C

15. C

16. B – core electrons usually do not emit/aren’t excited so this is the most incorrect.




Chem 201 – Term Test 1 – 2012 Fall


Multiple Choice

1. B

2. A

3. C

4. E

5. A

6. A

7. D

8. D

9. D

10. B

11. E

12. B

13. C

14. B

15. E

16. C












































Chem 201 Page 1 of 13

UNIVERSITY OF CALGARY

FACULTY OF SCIENCE

TERM TEST 1 – VERSION A

CHEMISTRY 201, Winter 2014

DATE: Monday February 10th, 2014 TIME: 7:00 pm – 9:00 pm

FIRST NAME: ______________ LAST NAME: ____________________ Lab Section: ______ Lecture Section: Please check one, then fill in ID # on next page! � L01 MWF 11:00 am Dr. F. Jalilehvand

� L02 MWF 12:00 pm Dr. J. Lefebvre

� L03 TR 8:00am Dr. F. Jalilehvand

Statement about the use of electronic devices / examination aids: This is a closed-book examination. The use of camera devices, MP3 Players and headphones, or wireless access devices such as cell phones, Blackberries, etc., during the examination will not be allowed. Only non-programmable calculators are permitted for this examination. A Chemical Data Sheet is provided.

Instructions: This test consists of 16 multiple choice questions worth 1 marks each (total 16 marks) and 3 long answer questions (total 24 marks). The total value for the test is 40 marks. The exam has 13 pages make sure you have all 13 pages.

All questions must be answered to obtain full marks. The answers to the multiple choice section must be entered on the optical score sheet. The time limit includes the time necessary to fill in the answers on the optical score sheet. The answers to the long answer questions must be written in the space provided on the question sheets AND written in non-erasable ink to be eligible for re-grading.

AT THE END OF THE EXAMINATION, HAND IN THE OPTICAL SCORE SHEET AND

THE ENTIRE EXAM PAPER

Failing to encode this Exam Booklet or your Optical Score Sheet correctly, for your name, ID and lecture section, will result in the loss of two marks


ID………………….

Q17…… Q18……. Q19……. DO NOT WRITE IN THIS BOX, FOR GRADING

PURPOSES ONLY!

SECTION I - Machine graded section (Total value 16) To be answered on provided Optical Score Sheet

1) Ozone formation in the upper atmosphere starts when oxygen molecules absorb UV-radiation.

Ozone absorbs radiation of wavelengths 220 – 290 nm, thus protecting organisms from this

radiation. What is the energy of the most energetic of these photons?

a) 9.03 x 10-19 J

b) 9.03 x 10-28 J

c) 6.85 x 10-19 J

d) 6.85 x 10-28 J

e) None of the above

2) A nitrogen gas laser emits photons with a frequency of 8.9 x 1014 Hz. If a nitrogen laser pulse

gives off 3.83 x 10-3 J of energy, how many photons does the pulse contain?

a) 34.09 x 1011 photons

b) 2.32 x 1011 photons

c) 2.32 x 1017 photons

d) 6.49 x 1015 photons



3) When comparing the 3p orbitals in aluminium with 3p orbitals in phosphorus:

i) They have the same quantum number sets.

ii) They have the same size.

iii) They have the same shape.

Which of the above statements is true?

a) i only

b) i and ii only

c) i and iii only

d) ii and iii only

e) All the above statements (i – iii) are true.

4) Which of the following describes a correct set of quantum number for an orbital?

a) n = 3, l = 0, ml = -1

b) n = 3, l = 3, ml = 1

c) n = 4, l = 1, ml = -2

d) n = 2, l = 1, ml = -2

e) n = 2, l = 1, ml = -1


5) Which of the following statements about quantum numbers and orbitals is correct?

a) It is not possible to have two electrons with the quantum numbers (1,0,0,+ ½) and (2,0,0,+½) in the same atom at the same time.

b) The secondary quantum number l provides information about the size of an orbital.

c) The magnetic quantum number ml provides information about the orientation of an orbital.

d) A complete description of an electron in an atom requires three quantum numbers.

e) All of the above statements are incorrect.

6) Which of the following diagrams represents a 3dz2 orbital?

7) Which of the following statements is correct for a non-hydrogen atom?

i. An electron in a 3d orbital is on average closer to the nucleus than an electron in a 4s orbital.

ii. The probability of finding an electron in a 1s orbital is the same everywhere within this orbital.

iii. An electron in a 4s orbital has less energy than an electron in a 3d orbital.

a) i and ii

b) iii only

c) ii and iii

d) i and iii

e) All of them are correct

a) b) c) d) e)


8) Among the following species:

i) As3+ ii) Ca iii) Ti2+

which species are diamagnetic?

a) i and ii only

b) i and iii only

c) ii and iii only

d) All the species (i – iii) are diamagnetic.

e) None of the species are diamagnetic.

9) Which of the following is the correct electronic configuration for the Co2+ ion in its ground state?

a) [Ar] 4s2 3d7

b) [Ar]4s2 3d5

c) [Ar] 4s1 3d7

d) [Ar] 3d6

e) [Ar] 3d7

10) Which of the following species have six valence electrons?

i) O2- ii) Cr iii) S

a) i only

b) iii only

c) i and iii only

d) ii and iii only

e) All above species (i – iii) have six valence electrons


11) The electronic configuration of an atom in an excited state is [Ne] 3s1 3p4. This element is:

a) P

b) Si

c) Al

d) S

e) N

12) Consider these consecutive ionization energies:

IE1 = 578 kJ/mol

IE2 = 1820 kJ/mol

IE3 = 2750 kJ/mol

IE4 = 11600 kJ/mol

To which third period (row) element do these ionization values belong?

a) Na

b) Mg

c) Al

d) Si


13) Which of the following represents the correct order of atomic size from largest to smallest?

a) P3- > S2- > Ca2+ > Sc3+

b) Sc3+ > Ca2+ > S2- > P3-

c) P3- > S2- > Sc3+ > Ca2+

d) Sc3+ > Ca2+ > P3- > S2-

e) All these ions have similar size.


14) Which of the following statements is correct about chlorine and phosphorus atoms?

a) The electron affinity of a chlorine atom is smaller than that of a phosphorus atom due to its smaller radius.

b) A chloride anion has higher electron affinity than a neutral chlorine atom.

c) A chlorine atom can easily gain and/or lose an electron since it has both a large electron affinity and a large ionization energy.

d) The effective nuclear charge experienced by the valence electrons in a chlorine atom is smaller than in a phosphorus atom.

e) All of the above statements are false.

15) Methanol (CH3OH) can be oxidized to methanal (CH2O) upon reaction with MnO4

− ions.

Identify which of the following chemical reactions is properly balanced.

a) CH3OH (aq) + MnO4− (aq) + 2 H+ (aq) � CH2O (aq) + MnO2 (aq) + 2 H2O (l)

b) 3 CH3OH (aq) + 2 MnO4− (aq) + 2 H+ (aq) � 3 CH2O (aq) + 2 MnO2 (aq) + 4 H2O (l)

c) CH3OH (aq) + MnO4− (aq) + 2 H+ (aq) � CH2O (aq) + MnO2 (aq) + 2 H2O (l) + 1e− (aq)

d) CH3OH (aq) + MnO4− (aq) � CH2O (aq) + MnO2 (aq) + O2 (g) + H2 (g)


16) Which of the following quantities is not equivalent to 5 mg of sodium bicarbonate, NaHCO3?

a) 6 x 10-5 mol

b) 0.005 g

c) 5000 µg

d) 0.000005 kg

e) All of the above are equivalent

*******END OF MULTIPLE CHOICE QUESTION SECTION*******


SECTION II: To be graded manually (Total value 24) Answers must be written in non-erasable ink to be considered for re-grading!

QUESTION 17 VALUE 6 MARKS Consider the generic atomic emission line spectrum and the energy diagram shown below for a species (atom or ion) with one electron.

a) Which emission line has the highest energy?

b) If the wavelength of emission line 1 (L1) is 444 µm, what is its frequency in Hz?

c) Explain how the energy levels (E1, E2 and E3) are related to the energies of the emission lines (L1, L2 and L3) in the emission spectrum.

d) Line L2 is more intense than the other two emission lines. Explain what does this mean?

increasing wavelength

L1 L2 L3

Ene

rgy E3

E2

E1

1 point

1 point

3 points

1 point


QUESTION 18 VALUE 11 MARKS

a) Use the orbital box diagram and write the short-hand electronic configuration for the ground state

of germanium (Ge) atom in the space below. Make sure to label the subshells.

b) Write the simple electronic configuration for its valence electrons:

c) Is germanium atom diamagnetic or paramagnetic?

d) Write a full set of quantum numbers for the highest energy electron.

e) Draw the electron density and radial distribution diagrams for an electron with 4s wave function.

f) Use your answer in part (a) and draw the orbital box diagram for an excited germanium atom.


g) Complete the following table about the orbitals found in germanium. Make sure to include axes with your diagrams.

Name of orbital

Boundary diagram Number of nodes

2pz

0

x

y


QUESTION 19 VALUE 7 MARKS

H2SO4 is a component of “acid rain” that is formed when air pollutant SO2(g) reacts with gaseous

oxygen O2(g) and liquid water.

a) Write a balanced equation for this “acid rain” reaction. Assume that no other product is formed by this reaction.

b) Sulfuric acid can react with marble (CaCO3), forming calcium sulfate (CaSO4), water and carbon

dioxide CO2(g), and can damage the surface of statues made from this stone:

H2SO4 (aq) + CaCO3 (s) → CaSO4 (s) + H2O (l) + CO2 (g)

Assuming that in a polluted area, the rainwater contains 0.0050 %w/w sulfuric acid, how much

rainwater (in kg) is needed to dissolve 5.000 g of a marble statue?


c) Sulfuric acid can be used to titrate a sodium hydroxide solution. The balanced reaction taking

place is:

H2SO4 (aq) + 2 NaOH (aq) → Na2SO4 (aq) + 2 H2O (l)

If 17.75 mL of 0.555 M H2SO4 solution are required to titrate 25.00 mL of NaOH solution, what was

the NaOH concentration at the beginning?

*******END OF WRITTEN ANSWER SECTION*******










Documents

NOTE: The first ~4 pages of this document are …learnfaster.ca/wp-content/uploads/chem201/TT1/TT1---Concise... · Chem 201 – Term Test 1 – 2015 Winter *These are the summarized