Chemistry 1 Final Exam Review: Chem. 1B Portion:

Remember that your final will be an ACS Chemistry 1 Exam! This will include concepts from Chemistry 1A as well as Chemistry 1B. Our review today will only cover concepts that we learned during this semester. Please be sure to review your Chem 1A material.

This is my review for what I think will be on the exam. Do not use only this to study. I have not

seen the exam, so I cannot say for sure what will be on it. Some questions may have errors so be

sure to double check your answers with baseline. Continue to use your notes, textbook,

PowerPoints, homework, etc. to study. You got this!!!

Chapter 5:

1. A sample of gas has an initial volume of 5.6 L at a pressure of 735 mmHg. If the volume of the gas is increased to 9.4 L, what is its pressure in mmHg?

2. A balloon contains 0.158 mol of gas and has a volume of 2.46 L. If an additional 0.113 mol of gas is added to the balloon (at the same temperature and pressure), what is its final volume?

3. Which gas sample representation has the greatest pressure? Assume that all the samples are at the same temperature. Explain.

4. What is the pressure in a 10.0 L cylinder filled with 0.448 mol of nitrogen gas at a temperature of 315 K?

Sample A: Sample C:Sample B:

5. A piece of dry ice (solid carbon dioxide) with a mass of 28.8 g sublimes (converts from solid to gas) into a large balloon. Assuming that all of the carbon dioxide ends up in the balloon, what is the volume of the balloon at a temperature of 22oC and a pressure of 742 mmHg?

6. Use the molar volume of a gas at STP to determine the volume (in L) occupied by 33.6 g of neon at STP.

7. A sample of gas has a mass of 38.8 mg. Its volume is 224 mL at a temperature of 55oC and a pressure of 886 torr. Find the molar mass of the gas.

8. A gas mixture contains 1.25 g N2 and 0.85 g O2 in a 1.55 L container at 18oC. Calculate the mole fraction and partial pressure of each component in the gas mixture.

9. The graph shows the distribution of molecular velocities for two different molecules at the same temperature. Which molecule has the higher molar mass? Which molecule has the higher rate of effusion?

10.Methanol can be synthesized by the reaction:

CO (g) + 2 H2 (g) CH3OH (g)

500 1000 1500 2000 2500

Molecular velocity (ms-1)

Relative number of molecules

A

B

What volume of H2 gas (in L), at 748 mmHg and 86oC, is required to synthesize 25.8 g CH3OH? How many liters of CO gas, measured to the same conditions, are required?

11.Ammonium carbonate decomposes upon heating according to the balanced equation:

(NH4)2CO3 (g) 2 NH3 (g) + CO2 (g) + H2O (g)

Calculate the total volume of gas produced at 22oC and 1.02 atm by the complete decomposition of 11.83 g of ammonium to the balanced equation.

Chapter 7:

12. The distance from the sun to Earth is 1.496 x 108 km. How long does it take light to travel from the sun to Earth?

13. List these types of electromagnetic radiation in order of increasing wavelength and increasing energy per photon:

a. Radio wavesb. Microwavesc. Infrared radiationd. Ultraviolet radiation

14. A laser pulse with wavelength 532 nm contains 3.85 mJ of energy. How many photons are in the laser pulse?

15. What are the possible values of l for each value of n? a. 1b. 2c. 3d. 4

16. Which set of quantum numbers cannot occur together to specify an orbital? a. n = 2, l = 1, ml = -1b. n = 3, l = 2, ml = 0c. n = 3, l = 3, ml = 2d. n = 4, l = 3, ml = 0

17.Calculate the wavelength of light emitted when an electron in a hydrogen atom makes the transitions below. Indicate the region of the electromagnetic spectrum (infrared, visible, ultraviolet, etc.) where the light is found. *see back of review for light spectrum chart*

a. n = 2 n = 1b. n = 5 n = 2

Chapter 8:

18. Write the full orbital diagram for each element:a. Nb. Fc. Mgd. Al

19. Arrange these elements in order of increasing atomic radius: Ca, Rb, S, Si, Ge, F.

20.Write the electron configuration for each ion: a. O2-

b. Br-

c. Sr2+

d. Co3+

e. Cu2+

21. Arrange these elements in order of increasing first ionization energy: Si, F, In, N.

22. Write orbital diagrams for each ion and determine if the ion is diamagnetic or paramagnetic

a. Cr3+

b. Ni2+

c. Fe3+

23. Arrange this isoelectronic series in order of decreasing radius: F-, Ne, O2-, Mg2+, Na+.

24. Arrange these elements in order of increasing metallic character: Fr, Sb, In, Ba, Se.

25.Choose the element with the more negative (more exothermic) electron affinity for each pair.

a. Na or Rbb. B or Sc. C or Nd. Li or F

Chapter 9:

26.Write the Lewis structure for each molecule. a. PH3

b. SCl2

c. HId. CH4

27.Write the Lewis symbols that represent the ions in each ionic compound. e. NaFf. CaOg. SrBr2

h. K2O

28.Explain the trend in the lattice energies of the alkaline earth metal oxides.

Metal Oxide Lattice Energy (kJ/mol)MgO -3795CaO -3414SrO -3217BaO -3029

29. Determine whether a bond between each pair of atoms would be pure covalent, polar covalent, or ionic.

i. Br and Brj. C and Clk. C and Sl. Sr and O

30.Write the Lewis structure that obeys the octet rule for each molecule or ion. Include resonance structures if necessary and assign formal charges to each atom.

m. SeO2

n. CO32-

o. ClO-

p. NO2-

31.What are the formal charges of the atoms of the following molecule?

32.Write Lewis structures for each molecule or ion. Use expanded octets as necessary.

q. BCl3

r. NO2

s. PF5

t. I3-

u. SF4

v. GeF4

33.Order these compounds in order of increasing carbon-carbon bond strength and in order of decreasing carbon-carbon bond length: HCCH, H2CCH2, H3CCH3.

34.Hydrogenation reactions are used to add hydrogen across double bonds in hydrocarbons and other organic compounds. Use average bond energies to calculate ∆ H rxn for the hydrogenation reaction. (Energies given at back of review)

C2H4 (g) + H2 (g) C2H6

35. Hydrogen, a potential future fuel, can be produced from carbon (from coal) and steam by this reaction:

C2 (s) + 2 H2O (g) 2 H2 (g) + CO2 (g)

Use the average bond energies to calculate the ∆ H rxn for this reaction. (Energies given at back of review)

36.Carbon ring structures are a common in organic chemistry. Draw a Lewis structure for each carbon ring structure, including any necessary resonance structures.

a. C4H8

b. C4H4

c. C6H12

d. C6H6

Chapter 10:

37. Fill out the electron and molecular geometry chart below:

Electron Regions and Bonding Lone Pairs Electron Molecular Geometry Bond

Hybridization Regions Geometry Angle (o)

2, sp 2 0 Linear Linear 180

1 1 Linear 180

3, sp2 3 0 Trigonal planar Trigonal planar 120

2 1 Bent <120

4, sp3 4 0 Tetrahedral Tetrahedral 109.5

3 1 Trigonal pyramidal ~107

2 2 Bent ~104.5

5,sp3d 5 0 Trigonal

bipyramidal

Trigonal bipyramidal 90 axial

120 equi.

4 1 Seesaw <90 axial

<120 equi.

3 2 T-shaped <90

2 3 Linear ~180

6, sp3d2 6 0 Octahedral Octahedral 90

5 1 Square pyramidal <90

4 2 Square planar 90

T-shaped

Linear

38. Determine the electron geometry, molecular geometry, and idealized bond angles for each molecule. In which cases do you expect deviations from the idealized bond angle?

a. PF3

b. CHCl3

c. SBr2

d. CS2

39. Determine whether the given molecules above are polar or nonpolar bonds.

40.Determine whether each molecule is polar or nonpolar.

a. SCl2

b. SCl4

c. BrCl5

41.How many bonds can each of these atoms make without hybridization? a. Beb. Pc. F

42.Write orbital diagrams (boxes with arrows in them) to represent the electron configuration of carbon before and after sp3 hybridization.

43.Which hybridization scheme allows the formation of at least one pi bond? a. sp3

b. sp2

c. sp3d2

44.Consider the structure of the amion acid alanine. Indicate the hybridization about each interior atom.

45. According to Molecular Orbital theory, which molecule or ion has the highest bond order? Highest bond energy? Shortest bond length?

C2, C2+, C2

-

46.

To be used for 36 and 37:

This is all that you will be given on the final exam: