Honors Chemistry Classroom Final Exam Review 2011
1. A 0.558 g sample of a new compound has been analyzed and found to contain the
following masses of elements: Carbon, 0.2322 g; hydrogen, 0.05848 g; oxygen,
0.3091 g. Calculate the % composition of the compound.
2. Calculate the empirical formula of the compound above.(answer: CH3O )
3. If the molar mass is 62.0 g/mole, find the molecular formula.
4. Calculate the % composition of C in dextrose C6H12O6.
5. What is the molar mass of a gas that diffuses twice as fast as O2?
6. Vapor pressure equilibrium and the effect on changing the temperature of the
system: How will the pressure be affected when the T increases and decreases?
7. What are the states of matter at each letter? What are the T (y axis) if this
substance is H2O?
Time
8. Nomenclature: Transition elements, Zn Ag Cd Pb Sn
Acids, Bases, Molecules, ions, alkanes
9. Examples of physical and chemical changes
10. Formula for density of a gas at STP
11. Effusion (diffusion) of a gas: Find the molar mass of a gas that effuses (diffuses)
twice as fast as CO2.
12. Give an example of a network solid, amorphous solid, molecular solid, ionic solid
13. Hydrogen bond, covalent bonds, ionic bonds, London dispersion forces, dipoledipole forces. Regroup these and name the groups. Give an example of each.
Relate this to the boiling point of each type. How does SiO2 (quartz) fit in?
14. How many grams of water can be vaporized by the addition of 8170 J of heat
energy? (heat of vaporization of water = 40.7 kJ/mole)
15. Write the electron configuration for niobium, 41Nb using the abbreviated noble
gas configuration.
16. Suppose 1.25 L of argon is cooled from 291 K to 78 K. What will be the new
volume of the argon sample?
17. What is the pressure on a 25 L vessel containing 1.0 kg of oxygen gas at 300.K?
18. Which elements on the periodic table are always radioactive?
19. Which elements appear on the zone of stability?
20. Give examples of where nuclear fission and fusion take place.
21. Illustrate the Dalton, Thomson, Rutherford and Bohr model of the atom.
22. What important experiments led these scientists to their models of the atom?
23. In the equation: Energy = -1312/n2 ; what energy is being calculated? What is
the difference between an atom in the ground state and the excited state? What is
an atomic emission spectrum? How can the wavelength and frequency of light be
calculated for a given atom?
24. How many sublevels when n = 4? Name the sublevels.
25. How many electrons can exist in the n = 4 level?
26. Uranium – 235. How many protons, neutrons, electron in this atom?
27. Rubidium has two common isotopes, 85Rb and 87Rb. If the abundance of
85
Rb is 72.2% and the abundance of 87Rb is 27.8%, what is the average
atomic mass of rubidium? (answer 85.56 amu)
27. Period properties: Ionization energy, atomic radius, ion radius, electronegativity,
metallic character,
28. Draw the Lewis dot structure for NO3 -1. Name the type of bonds between the
atoms. What is the hybridization of N? How many sigma and pi bonds?
Resonance?
29. What is an expanded octet? Give some examples of molecules having different
molecular geometries. What are the bond angle?
30. An experiment that led to the formation of the new field of organic chemistry
involved the synthesis of urea, CN2H4O, (MM = 60.0 g) by the controlled reaction
of ammonia and carbon dioxide
2NH3 (g) + CO2 (g)  CN2H4O (s) + H2O (l)
What is the theoretical yield of urea if 100. g of each react is combined?
(answer: limiting reagent is CO2; theoretical yield is 136 g urea)
Find the volume of the limiting reagent at STP. (answer: 50.8 L CO2) Find the
volume of the excess reagent that reacts, if at STP (answer: 102 L NH3)
31. Find the molarity of a solution made with 40.0 g of NaCl and enough water to
make 1.5 liters of solution.
32. Give an example of each of the following reactions: single replacement, double
replacement, decomposition, synthesis, neutralization, oxidation-reduction,
combustion of a hydrocarbon.
33. What are the x and y axis of a solubility graph?
34. What factors effect the solubility of a substance? What factors effect the rate of
dissolving?
35. Explain “Like dissolves like”. Give examples of solutes and solvents. Which are
soluble?
36. What factors affect the degree to which the freezing point of a solution is
depressed or a boiling point is elevated as compared to the pure solvent?
37. If H2O (s) is a molecule, what is NaCl (s)? What is SiO2 (s)? What is copper?
38. A saturated solution of silver sulfate at 25oC can be prepared by dissolving 1.2 g
of silver sulfate in water to make 250.0 mL of solution. What is Ksp for silver
sulfate? (answer: Ksp = 1.5 x 10-5)
39. Ksp of BaF2 is 1.8 x 10-7. Calculate the solubility in a) moles per liter b) grams
per liter. (answer: a) 3.6 x 10-3 mol/L b) 0.63 g/L )
40. What is the pH of a 0.1 M HNO3 solution? How would the pH of a 0.1 M
HC2H3O2 compare?
41. What is the pOH of a 0.1 M NaOH solution?
42. Give some examples of weak electrolytes, strong electrolytes and nonelectrolytes.
43. What is an Arrhenius acid? Arrhenius Base
44. Which are acids? Bases?
CH3COOH
HC2H3O2
C2H5OH Mg(OH)2 H2SO3
(weak acid, same weak acid, alcohol is neutral, weak base, weak acid)
45. Using Gibbs Free Energy Equation, describe the conditions for entropy (exo or
endothermic reactions and enthalpy (more disorder or less disorder) necessary for
a spontaneous reaction.
46. + ΔH. –ΔH, +ΔS, -ΔS What to these signs tell you about a chemical reaction?
47. Name some factors that influence the amount of entropy of a system
48. Calculate the enthalpy change (ΔH) in kJ for the following reaction.
2Al(s) + Fe2O3(s)  2Fe(s) + Al2O3(s)
Use the enthalpy changes for the combustion of aluminum and iron:
2Al(s)) + 3/2O2(g)  Al2O3(s)
ΔH = -1669.8 kJ
2Fe(s) + 3/2O2  Fe2O3(s)
ΔH = -824.2 kJ
49. What is the ΔHf? Write a chemical equation for the formation of water from its
free elements at standard conditions.
50. What is the standard heat of reaction (ΔHo) for the reaction of CO(g) with O2(g)
to form CO2(g)? ΔHfo of CO(g) = -110.5 kJ/mol; ΔHfo of CO2(g)= -393.5 kJ/mol
(hint: write a balanced equation first!) (answer: ΔHo -= -566.0 kJ
51. How are these reaction pathways changed when a catalyst if present?
52. What is equilibrium? What is Le Chatelier’s Principle?