KEY Exam2 1311 F16 v D - the full version of exam 2 for F16. Grading policy and test-taking policy are PDF

Preview

Summary

the full version of exam 2 for F16. Grading policy and test-taking policy are provided...

Description

CHEM 1311: General Chemistry 1, Fall 2016 Exam #2, October 15, 2016 Class section: Instructor Taylor Sibert Dieckmann Dieckmann Taylor Wijenayake

Section # 001 002 003 004 005 501

Class time 9:00 to 9:50 am 10:00 to 10:50 am 11:00 to 11:50 am 1:00 to 1:50 pm 2:00 to 2:50 pm 5:30 to 6:45 pm

EXAM TYPE: D You have 80 minutes to answer 34 questions AND bubble the scantron. No additional time to bubble will be given. _________________________________________________________________________________ Scantron Use In general: 1. For this exam, you are allowed to use ONLY a TI-30X IIS, TI-30X IIB or TI-30Xa that you have at your desk. You MAY NOT borrow another person’s calculator. You MAY NOT use your cell phone, PDA, or other non-calculator device as a calculator. 2. Your cell phone should be turned OFF and stored in your bag or on the floor, under your seat. NO wristwatches will be permitted to be worn during this exam. 3. Use ONLY a #2 pencil to fill out the scantron sheet. Do not use a pen or marker. 4. When filling in the bubbles on the scantron, be sure to fill in bubble completely, and only one bubble for each entry. Pay attention to line numbers on the scantron so that you put the answer in the correct spot. 5. When you first get the exam, check to make sure you have all pages of the exam and one periodic table. You should also have one scantron sheet. If you don’t have any of these, contact us immediately. 6. We will announce periodically how much time has elapsed/is remaining. 7. If you have a question, ASK (if taking the exam at the Office of Student AccessAbility or the Testing Center, let your proctor know and they can call immediately to get an answer to your question) FILLING IN SCANTRON PERSONAL INFO: Bubble info: 1. I.D. NUMBER:

4-digit exam number (left justified)

2. NAME:

LAST NAME

3. TEST FORM:

exam type (A, B, C or D)

4. SUBJECT SCORE:

your section number (see above for list)

Vertical lines: 1. NAME:

“Exam 2” GOOD LUCK!

space

FIRST NAME

space

MI (left justified)

CHEM 1311: Exam #2

October 15, 2016

Page 2 of 6

1. Which of the following is the correct name for CuSO3? A. copper(II) sulfate, cupric sulfate B. copper(I) sulfate, cuprous sulfate C. copper(II) sulfite, cupric sulfite D. copper(I) sulfite, cuprous sulfite E. copper sulfur trioxide __________________________________________________________________________________ 2. How many equivalent resonance structures are possible for the tellurite ion (TeO32–)? A. 1 B. 2 C. 3 D. 4 E. 5 __________________________________________________________________________________ 3. What is the Br–O bond order in the “best” Lewis structure of the perbromate ion (BrO4– )? A. 1 B. 1.75 C. 1.33 D. 1.5 E. 1 and 2 __________________________________________________________________________________ 4. The radii of the species, Y,Y+, and Y– decrease in the following order: A. Y+ > Y >Y– B. Y+ > Y– >Y C. Y > Y– >Y+ D. Y > Y+ > Y– E. Y– > Y > Y+ __________________________________________________________________________________ 5. Predict the ideal bond angle(s) in the nitrite ion: A. 90° B. 109.5° C. 120° D. 180° E. more than one of the other answers is correct __________________________________________________________________________________ 6. How many individual ions are in 18.2 grams of Al2O3? A. 1.07 × 1023 ions B. 5.37 × 1023 ions C. 2.55 × 1023 ions D. 5.10 × 1023 ions E. 1.46 × 1023 ions __________________________________________________________________________________ 7. How many lone pairs of electrons are on the tellurium atom in the Lewis structure of TeF4? A. 0 B. 1 C. 2 D. 3 E. 4 __________________________________________________________________________________ 8. Which of the following elements has the lowest first ionization energy? A. Rb B. Mg C. Na D. Cl E. Br __________________________________________________________________________________ 9. Select the correct Lewis structure for nitrogen trifluoride. B.

A. F

N

F

F

N

F

F

F

C.

D. F

N

F

F

F

N

F

F

E. F

N

F

F

__________________________________________________________________________________

CHEM 1311: Exam #2

October 15, 2016

Page 3 of 6

10. How many resonance structures are possible for nitrate, NO3– ? A. 0 B. 4 C. 3 D. 1 E. 2 __________________________________________________________________________________ 11. Xanthophyll, the yellow pigment that occurs widely in nature, has a molecular formula of C40H56O2. What is its empirical formula? A. C0.71HO0.036 B. CH1.4O0.05 C. C20H28O D. C10H14O0.5 E. C40H56O2 __________________________________________________________________________________ 12. Select the element whose Lewis symbol is incorrect: A. Mg

B.

C. Na

Si

D. C

E. Be

__________________________________________________________________________________ 13. Arrange the following in order of increasing boiling point: CsF, CH3Br, CH3OH, CH4 A. CH4 < CH3Br < CH3OH < CsF B. CH3OH < CH4 < CH3Br < CsF C. CsF < CH3Br < CH3OH < CH4 D. CH4 < CH3OH < CH3Br < CsF E. CH3OH < CH3Br < CsF < CH4 __________________________________________________________________________________ 14. Which of the following Lewis structures is the BEST description of the bonding in ozone, O3? O O O a. O c. O O O O O b.

d.

2O

O

O

e.

O

O

O

__________________________________________________________________________________ 15. What is the electron domain geometry around the sulfur in SF5– ? A. linear B. trigonal planar C. tetrahedral D. trigonal bipyramidal E. octahedral __________________________________________________________________________________ 16. Which of the following sets of names and their formulas is correct? B. H2CrO7 (aq), hypochromous acid A. H2SO4 (aq), sulfurous acid C. H3PO3 (aq), phosphoric acid D. HClO4 (aq), perchloric acid E. HCl (aq), chloric acid __________________________________________________________________________________ 17. What is the correct electron configuration of a calcium ion, Ca2+ ? A. [Ar] 3s1 B. [Ne] C. [Ar] D. [Ar] 3s1 E. [Ar] 3s2 __________________________________________________________________________________ 18. The best Lewis structure for sulfuric acid has zero formal charges, sulfur as the central atom, and no bonds between S and H. How many total single and double bonds, respectively, are there in this Lewis structure? A. 2 single, 4 double B. 6 single, no double C. 4 single, 2 double D. 5 single, 1 double E. 4 have 1 ½ bonds, no single, no double __________________________________________________________________________________

CHEM 1311: Exam #2

October 15, 2016

Page 4 of 6

19. Which of these ionic solids would have the smallest magnitude lattice energy? A. KF B. CsBr C. NaF D. CaO E. CsI __________________________________________________________________________________ 20. What is the electron configuration of Cd2+? A. [Kr] 5s2 4d10

B. [Kr] 5s2 4d8

C. [Kr] 4d10

D. [Kr] 5s2 4d10 5p1

E. [Kr] 5s1 4d10 __________________________________________________________________________________ 21. What is the molecular geometry for SF3–? A. Square pyramidal B. Trigonal pyramidal C. T-shaped D. Trigonal planar E. See saw __________________________________________________________________________________ 22. What is the percent composition of cobalt in cobalt(II) chloride hexahydrate? A. 29.8% B. 24.8% C. 47.9% D. 39.8% E. 45.4% __________________________________________________________________________________ 23. What is the formal charge on the oxygen atom in carbon monoxide? A. 0 B. 1 C. –2 D. 6 E. –1 __________________________________________________________________________________ 24. What types of intermolecular forces exist between hydrogen iodide molecules? I. London forces II. dipole-dipole interactions III. hydrogen bonding IV. ion-dipole interactions A. I and II only B. I only C. III only D. II and III only E. I, II, and III only __________________________________________________________________________________ 25. In neutral molecules, how many bonds are commonly formed by oxygen? A. 5 B. 4 C. 3 D. 2 E. 1 __________________________________________________________________________________ 26. Which is the LEAST polar bond? A. S–H B. Br–H C. Cl–H D. O–H E. C–H __________________________________________________________________________________ 27. Which of the following molecules has a net dipole moment (i.e. is polar)? A. XeF2 B. TeCl2 C. CO2 D. BeF2 E. SiCl4 __________________________________________________________________________________ 28. A 14.7 gram sample contains 5.66 g calcium, 3.02 g sulfur and the rest is oxygen. What is the empirical formula for this compound? A. Ca1.5SO4 B. CaSO C. Ca2SO2 D. Ca3SO3 E. Ca3S2O8 __________________________________________________________________________________

CHEM 1311: Exam #2

October 15, 2016

Page 5 of 6

29. Predict the actual bond angle(s) in chlorite (best estimate): A. 180° exactly B. < 90° C. < 109.5° D. < 120° E. < 180° __________________________________________________________________________________ 30. Which of the following sets of names and compounds is incorrect? A. NaN3 sodium azide B. KCl potassium chloride C. NO2 nitrogen oxide D. AlH3 aluminum hydride E. CO2 carbon dioxide __________________________________________________________________________________ 31.Which one of the following equations correctly represents the process involved in the third electron affinity of As? A. As(g) + e– → As–(g) B. As–(g) + e– → As2–(g) C. As(g) → As+(g) + e– D. As–(g) → As(g) + e– 2– – 3– E. As (g) + e → As (g) __________________________________________________________________________________ 32. What is the molar mass of Na2S? A. 126.05 g mol–1 B. 103.06 g mol–1 C. 87.13 g mol–1 –1 –1 D. 55.06 g mol E. 78.05 g mol __________________________________________________________________________________ 33. Select the best Lewis structure for ClCN. A. C. E.

Cl

Cl

Cl

C

C

N

D.

N

C

B.

Cl

Cl

C

C

N

N

N

__________________________________________________________________________________ 34. Which of the following is false concerning electronegativity? A. Fluorine is the most electronegative atom B. Electronegativity can be measured by observing individual atoms in the gas phase C. Electronegativity affects covalent bonds D. All electronegativity scales are relative E. Larger atoms generally have lower electronegativities than smaller atoms __________________________________________________________________________________

END OF QUESTIONS

CHEM 1311: Exam #2

October 15, 2016

Page 6 of 6

Potentially Useful Information Avogadro’s Number:

NA = 6.022 x 1023

Constant for Bohr model of H atom:

b = 2.180 x 10–18 J

Speed of light:

c = 2.998 x 108 m s–1

Planck’s constant:

h = 6.626 x 10–34 J s

1 J = 1 kg m2 s–2 electron: proton: neutron:

mass (me) = 9.1093897 x 10–28 g mass = 1.673 x 10–24 g mass = 1.675 x 10–24 g

1 in = 2.54 cm (exactly) 1 amu = 1.66054 x 10–24 g

1 ft = 12 in

charge (e) = –1.60 x 10–19 C

1 mi = 5280 ft...