Name

CHEM 115 EXAM #3 Practice Exam Fall 2013

Circle the correct answer. (numbers 1-9, 3 points each) 1. Choose the correct statement about the compound SO2. a. the S—O bonds are ionic in character b. the molecule cannot exit since the bonding does not obey the octet rule c. the S atom has a lone pair of electrons d. the S—O bonds are different lengths since one is a single and the other a double bond e. none of the above 2. An expanded octet may occur: a. in the first and second period only b. in groups 1A, 2A, and 3A c. in periods 3 and greater d. in all groups except 1A e. none of the above 3. Which chloride should exhibit the most covalent (least ionic) type of bond? a. NaCl b. KCl c. BaCl2 d. BeCl2 e. CaCl2 4. Which of the following bonds should be the most polar? a. N—Cl b. N—F c. F—F d. H—I e. N—Br 5. Which of the following species has a central atom with sp2 hybridization?

a. CO2 b. NO3- c. CH4 d. PCl5 e. none of the above 6. Which of the following bonds should be the shortest and strongest?

a. C=C b. C≡C c. O=O d. C≡O e. C_C 7. Which of the following sets contains the greatest number of bent molecules? a. CO2, HCN, O2 b. H2S, HCN, CO2 c. H2O, CO, H2S d. H2S, CO, CO2 8. Which of the following is a tetrahedral molecule (or ion)?

a. CO2 b. NO3- c. CH4 d. PCl5 e. none of the above 9. Which of the following is a molecule (or ion) that contains at least one π bond?

a. CO2 b. NO3- c. CH4 d. PCl5 e. none of the above

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Complete the following as directed (point values as indicated). (16 points) 10. For the following two species complete the tasks specified below in a - d.

i. CH3COOH ii. C2H2 a. Draw the best Lewis structures.

b. Specify the hybridization of both the C atoms and the O atom specified in (i) and the C atoms in (ii)?

C in CH3 C in CO O between CO and H

C in CH

c. Show the energy level diagram for both the C atoms and the O atom in (i) and the C atoms in (ii), fill the diagrams with the correct number of valence electrons, and identify the types of electrons present (i.e. σ, π, lone pair)

C in CH3 C in CO O between CO and H

C in CH

d. What are the bond angles around both the C atoms and the O atom in (i) and each of the C atoms in (ii)?

C in CH3 C in CO O [the COH angle]

C in CH

(10 points) 11. (a) Draw Lewis structures for CN-, CO, N2, and NO+. Label all atoms with their formal charges. (b) Select the species from part (a) that you would expect to have the shortest, strongest bond. In

order to receive credit you must EXPLAIN the reasoning for your selection.

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(15 points) 12. Fill in the MO energy diagrams for the species listed below using valence electrons ONLY. The

answer the questions that appear under the MO energy diagram of each species.

Oxygen Ο2 Peroxide Ο2−2

σ∗2p

σ∗2p

π∗2p

π∗2p

π∗2p

π∗2p

π2p

π2p

π2p

π2p

σ2p

σ2p

σ∗2s

σ∗2s

σ2s

σ2s

Show the calculation of the bond order for oxygen.

Show the calculation of the bond order for the peroxide ion.

Is oxygen diamagnetic or paramagnetic? Explain your answer.

Is the peroxide ion diamagnetic or paramagnetic? Explain your answer.

Draw the Lewis structure of oxygen.

Draw the Lewis structure for the peroxide ion.

Does the bond order for oxygen from the Lewis structure match the bond order from the MO diagram?

Does the bond order for the peroxide ion from the Lewis structure match the bond order from the MO diagram?

Which should have the longer, weaker bond; oxygen or the peroxide ion? Explain your choice!

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Answer the following. Provide as much information as required to answer the question clearly. 13. Balance the following reactions AND draw Lewis symbol structures for part (e): (a) C6H14 (l) + O2 (g) CO2 (g) + H2O (l) (b) O2 (g) + NH3 (g) NO (g) + H2O (l) (c) NO2 (g) + H2O (l) HNO3 (aq) + NO (g) (d) Fe2O3 (s) + Al (s) Fe (l) + Al2O3 (s) Don’t forget to draw the Lewis symbols for each of the compounds in this next reaction! (e) CaC2 (s) + H2O → C2H2 + Ca(OH)2 14. Write balanced chemical equations for each of the following “word descriptions” of a

chemical process.

(a) Solid magnesium metal reacts with carbon dioxide to produce magnesium oxide and carbon monoxide.

(b) Solid magnesium oxide reacts with water to form aqueous magnesium hydroxide.

(c) Liquid bromine reacts (quite violently) with aluminum metal to form aluminum bromide.

(d) Butane gas combusts completely with oxygen gas to form the expected products.

(e) Aqueous hydrochloric acid reacts with solid zinc to form zinc chloride and hydrogen.

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(f) BONUS (for up to 10 points) Place the correct atomic symbols into the correct blocks for elements 1 through 30. Label the following correctly on the table as well:

(a) noble gases, (b) alkali metals, (c) halogens, (d) alkali metals, (e) transition metals, (f) lanthanides, (g) actinides, (h) the coinage metals, and (i) the chalcogens.

See the next page for a chart of shape and name info you should also study. In addition to knowing the names, bond angles, etc. you should also know the hybridization type for each category. Below you will find a quick listing. #RHED hybridization 2 sp 3 sp2 4 sp3 5 sp3d 6 sp3d2 RHED = region of high electron density

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Note: other options exist beyond those in this table . . . but we’ll not be testing all the way up to a 16 coordinate system that employs all of the s, p, d and f orbitals from a single atom!