Chemistry Final Exam
Study Guide
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What is chemistry?
What is mass?
What is volume?
How does the composition of a pure compound differ from that of a mixture?
What is the difference between extensive properties and intensive properties?
Define chemical property and list two examples.
Define physical property and list two examples.
Distinguish between a physical and chemical change.
What is meant by a change in state?
Be EXTREMELY familiar with all aspects of the periodic table and the elements.
Explain the law of conservation of mass, law of definite proportions, and the law of multiple
proportions.
12. What is an atom?
13. What two regions make up the atom? What particles are located in each region? What are their
charges?
14. What number uniquely identifies an element?
15. What are isotopes? How are they similar? Different?
16. How many moles of atoms are there in:
6.022 x10^23 atoms Ne
3.011 x 10^23 atoms Mg
3.25 x 10^5 g Pb
4.50 x 10^-12 g O
17. How many atoms are there in:
1.50 mol Na
6.755 mol Pb
7.02 g Si
18. Describe the Bohr model of the atom.
19. Characterize each of the following as absorption or emission: an electron moves from E2 to E1; an
electron moves from E1 to E3; and an electron moves from E6 to E3.
20. How many electrons could be contained in the following main energy levels with n equal to the
number provided: a. 1 b. 3 c. 4 d. 6 e. 7
21. State the Aufbau principle.
22. What is Hund’s rule?
23. Write the orbital notation for the following elements: 1. P; 2. B; 3. Na; 4. O
24. Write the electron-configuration notation for the element whose atoms contain the following
number of electrons: 1. 3; 2. 6; 3. 8; 4. 13
25. What are the noble gases? Where are they located? Why are they so stable?
26. Who discovered the periodic law?
27. State the periodic law.
28. Name three sets of elements that have been added to the periodic table after Mendeleev’s time.
29. What name is given to each of the following groups of elements in the periodic table:
a. Group 1; b. Group 2; c. Groups 3-12; d. Group 17; e. Group 18
30. What is the main distinction between ionic and covalent bonding?
31. What type of bonding would be expected between the following atoms:
a. Li and F; b. Cu and S; c. I and Br
32. Draw the Lewis structure of NH3, H2S, SiH4, PF3
33. Now the difference in single, double, and triple bonds.
34. Name the three types of bonding and the category of elements that are involved.
35. What is the significance of a chemical formula?
36. Write formulas for the compounds formed between the following:
a. aluminum and bromine
d. Pb2+ and O2b. sodium and oxygen
e. Sn2+ and Ic. magnesium and iodine
f. Cu2+ and NO₃37. Write formulas for each of the following compounds:
a. sodium hydroxide
b. lead (II) nitrate
c. diphosphrous trioxide
d. sulfurous acid
38. Assign oxidation #’s to the following:
a. HF; b. CI₄; c. H2O; d. H2CO3
39. Describe the differences between word equations, formula equations, and chemical equations.
40. List the five types of chemical reactions. Provide the general equation for each.
41. What is stoichiometry?
42. For each equation write all possible mole ratios:
a. 2HgO  2Hg + O₂
b. 4NH₃ + 6NO  5N₂ + 6H₂O
43. Balance the following equation. Then, given the moles of reactant or product below, determine the
corresponding amount in moles of each of the other reactants and products.
NH₃ + O₂  N₂ + H₂O
44. Be familiar with the kinetic molecular theory.
45. Describe the gas, liquid, and solid phase in terms of particle arrangement and properties.
46. What is sublimation? Give one example.
47. Name the two types of solids.
48. Define pressure.
49. What units are used for pressure?
50. Convert the following pressures to pressures in standard atmospheres:
a. 151.98 kPa
b. 456 torr
51. Be familiar with Dalton’s Law of Partial Pressure.
52. A sample of oxygen gas has a volume of 150.0 mL when its pressure is 0.947 atm. What will the
volume of the gas be at a pressure of 0.987 atm if the temperature remains constant?
53. Compare diffusion and effusion.
54. Classify the following as either a heterogeneous or homogeneous mixture and explain:
a. orange juice
b. tap water
55. What are substance called whose waeter solutions conduct electricity? Name the solute and solvent
in the following:
a. 14 karat gold b. corn syrup c. carbonated, or sparkling, water
56. What is the term used to describe the ability of something to be dissolved?
57. How could you increase the rate of dissolution?
58. What is the solute to solvent combination of sugar in tea?
59. You have 3.50 L of a solution that contains 90.0 g of NaCl. What is the molarity of the solution?
60. What quantity, in grams, of methanol, CH3OH, is required to prepare a 0.244 m solution in 400.0 g of
water?
61. What are the five properties of acids? Bases?
62. What is a binary acid? Oxyacid? Give two examples of each.
63. Why are strong acids also strong electrolytes?
64. What are the three types of acids? List the characteristics of each.
65. Name three kinds of common industrial acids and list two uses, properties, etc.
66. What is the relationship between the strength of an acid and the strength of its conjugate base?
67. Distinguish between a monoprotic, diprotic, and triprotic acid and provide one example of each.
68. Be able to balance equations.
69. What is the pH of a 1.0 x 10^-3 M NaOH solution?
70.Be familiar with pH values, pH scale, and how to calculate the pH of a solution.