Name

Chemistry 121 Final Examination

June16, 2010

General Examination Directions

  • If you need to use the restroom, then please do it now. No potty breaks today!
  • Please be sure to write your name above
  • Please turn off and put away all electronic devices, such as cell phones
  • Be sure to show all work for the problems
  • Answer the questions and problems that will take you the least about of time first
  • Place square boxes around your answers
  • A periodic chart is located on the last page
  • Before handing in your paper check to be sure that you have the correct number of significant figures

General Information

For Lewis Structures of molecules P = 8(n-q) + 2q -2(n-1) – v
0.0821 L-atm/mole-K is the ideal gas constant

PV/T = P’V’/T´ Combined Gas Law

C1V1 = C2V2 The dilution equation

Facts and Constants

2.54 cm = in, 12 in = ft, 5280 ft = mi

946 mL = qt, 4 qt = gal, mL = cm3

14.7 psi = atm, 101.3 kPa = atm

4.184 j = cal

Freezing Point Depression Constant = -1.86°C/M

Boiling Point Elevation Constant = 0.512°C/M

  1. Classify the following as heterogeneous, solution, compound, or element.
  2. Grass
  3. Wine
  4. Air is this room
  5. Tap water
  6. Sea water
  7. Steel
  8. Wood
  1. Record the volume to the correct number of significant figures from the picture below.
  1. Classify each of the following properties as physical or chemical.
  2. Iron melts at 1535°C
  3. Alcohol is flammable.
  4. The metal used in artificial hip-joint implants is not corroded by body fluids.
  5. Air is less dense that water.
  6. The recommended daily caloric intake for a 22 year old woman is 2000. How many calories should her breakfast contain if she wants to be 45% of her recommended daily total?
  1. A 3.22 g sample of rock displaces 1.05 mL of water. Calculate its density.
  1. The density of aluminum is 2.69 g/mL. Find the thickness of a piece of aluminum that measures 2.00 cm by 6.2 cm, if the mass of the aluminum is 1.01 g.
  1. Find the percent by weight of carbon in glucose (C6H12O6)
  1. Arrange the following elements in order of decreasing size.

In, Be, F, C, Na

  1. How many orbitals are found in a 4f subshell? What is the maximum number o electrons that can be located in this subshell?
  1. Give the abbreviated electron configuration, valence configuration and the number of valence electrons in Bi.
  1. Which element on the periodic chart has the highest ionization energy?
  1. What type of bond is formed between two ions of opposite charge?
  1. Give Lewis structures for the following.
  2. O
  3. O2-
  4. NaCl
  5. N2
  1. O3
  1. What are the intermolecular forces between two water molecules called?
  1. Give names for the following substances:
  2. CaCl2
  3. MnO4
  4. HClO3
  5. H2S (aq)
  6. HMnO4
  7. H2O
  8. FeSO4
  9. P2O5
  10. Give a formula for the following:
  11. Zinc acetate
  12. Hydrobromic acid
  13. Sulfurous acid
  14. Aluminum oxide
  15. Calcium hydroxide
  16. Sulfur trioxide
  17. Ammonium phosphate
  18. Iron(III) hydroxide
  19. Assign oxidation numbers to the following chlorine compounds below.
  20. HClO4
  21. HClO3
  22. HClO2
  23. HClO
  24. HCl
  25. Cl2
  26. An important metabolic process of the body is the oxidation of glucose to water and carbon dioxide. The equation for the reaction is

C6H12O6 + 6 O2 → 6 CO2 + 6 H2O

  1. What mass of water in grams is produced when the body oxidizes 567 g of glucose?
  1. How many grams of oxygen are needed to oxidize 567 g of glucose?
  1. Upon heating, mercury(II) oxide undergoes a decomposition reaction:

2 HgO → 2 Hg + O2

A sample of HgO weighing 7.22 g was heated. The collected mercury weighed 5.95 g

what was the percentage yield of the reaction?

  1. A student combines 25.0 mL of 0.100M HCl with 15.0 grams of zinc.
  2. Write a balanced equation.
  1. Identify the type of this equation.
  1. Is this equation a REDOX reaction?
  1. Find the mass of hydrogen gas produced.
  1. Identify the excess reactant.
  1. Find the density of carbon dioxide gas at STP.
  1. A car tire has a pressure of 32.0 psi at 25°C. Find the temperature of the tire in °C when the pressure increases to 41 psi.
  1. What is equal when a reaction is at equilibrium?
  1. For the following reaction identify the acid, base, the conjugate base and the conjugate acid.

NaNH2 + HOH → NH3 + NaOH

  1. Find the pH of 0.10 M Ca(OH)2
  1. A student adds 10.0 mL of water to a 25.00 mL sample of 18.0 M H2SO4 . Find the diluted acid concentration.
  1. Classify the following solutions as acidic, basic, or neutral. Also, give the pOH, [OH-], pHand the [H+] if they are not given.
  2. pH = 4.2
  1. pOH = 8.3
  1. [H+] = 6.2 X 10-3
  1. [OH-] = 3.2 X 10-4
  1. Give the acid and base required to make the following salts. Label the salts as acidic, basic, or neutral salts.
  2. Ca(C2H3O2)2
  1. KNO3
  1. A student titrates 25.00 mL H2SO4 with 0.3000 M NaOH. Give the following, if 38.00 mL of NaOH is required to reach a phenolphthalein end point.
  2. Write and balance the neutralization equation.
  1. Calculate the molarity of the acid.
  1. Find the % w/w of acid if the acid solution has a density of 1.45 g/mL
  1. A buffer solution is made by adding 1.0 mole of HF and 1.0 mole of NaF to one liter of water. The salt (NaF) ionizes completely into Na+(aq) and F-(aq), while the weak acid HF does not really ionize.
  2. Which species of this buffer solution will react with the strong acid HCl?
  1. Which species of this buffer solution will react with the strong base NaOH?