Download Ch 1-4 Final Review - Iowa State University

Lilli Howard
Chem 177 (BC)
Dr. Irmi
12/08/13
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Ch. 1-4 Review
Supplemental Instruction
Iowa State University
1. Match the following characteristics to one or more of the three states of matter:
1. Has no shape of its own
2. Has a definite shape
3. Occupies the total volume of a container
4. Partially takes on the shape of a container
5. Does not take shape of container
6. Readily compressible
7. Slightly compressible
8. Essentially non-compressible
2. Are the following changes physical or chemical?
1. The vaporization of solid carbon dioxide
2. The explosion of solid TNT
3. The aging of an egg with a resultant unpleasant smell
4. The formation of a solid when honey is cooled
3. Fill in the following table concerning physical quantities and units:
Physical Quantity
Metric Unit Name
SI unit name
Length
Volume
gram
Time
calorie
Newton per square meter
4. How many significant figures does each number possess:
1. 225
2. 10,004
3. 0.0025
4. 1.0025
5. 0.002500
6. 14,100
7. 14,100.0
5. Which has the greater mass, 2.0 cm3 of iron (d = 7.9 g/cm3) or 1.0 cm3 of gold (d = 19.32
g/cm3)?
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6. Write the isotopic symbols for the four isotopes of sulfur with 16, 17, 18, and 20
neutrons, respectively.
7. Write the expected formula when the following elements combine to form compounds:
1. Al and O
2. B and Cl
3. S and O
4. H and Ca
8. Name the following compounds:
1. ZnS
2. (NH4)2SO4
3. FeCl2
4. KClO4
5. SnCl2
6. SF6
7. CO
9. Name the following acids:
1. HCN
2. H2S
3. H2CO3
4. H3PO4
10. Name the following anions and cations:
1. Na+
2. Al3+
3. Co3+
4. S25. PO436. H2PO411. Write the chemical formulas for:
1. ethane
2. propane
3. butanol
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12. Combustion Reactions:_____________________________________________________
13. Combination Reactions:____________________________________________________
14. Decomposition Reactions:__________________________________________________
15. Write the balanced chemical equation for the combustion of butane in air.
16. Calculate the molecular formula weights for (a) NO3- and (b) C21H30O2
17. A sample of Na2B4O7 contains 0.3478 g of sodium. What is the mass of this sample?
18. A compound contains only the elements Al and O. Its elemental composition is
determined to be 53.0% aluminum and 47.0% oxygen. The mass of one mole of a
compound is 102 g. What is the empirical formula of the compound? What is the
molecular formula?
19. How many grams of HI are required to form 1.20 moles of H2 when HI reacts according
to the balanced chemical equation: 2 HI (g) → H2 (g) + I2 (g)
20. What is the limiting reactant when 10.0 g of C2H6 reacts with 50.0 g of O2 according to
the equation: 2 C2H6 (g) + 7 O2 (g) → 4 CO2 (g) + 6 H2O (l)
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Define the following, give examples:
21. Solvent:________________________________________________________________
22. Solute:_________________________________________________________________
23. Acids: _________________________________________________________________
24. Bases: _________________________________________________________________
28. Classify each of the following as a strong, weak, or non-electrolyte in water:
1. HBr
2. H2S
3. NH3
4. Ba(OH)2
29. Identify the following salts as soluble or insoluble in water:
1. Fe(NO3)3
2. PbCl2
3. CaBr2
4. BaSO4
5. Na2SO4
30. Complete the following reactions and write net ionic equations for them:
1. Pb(NO3)2 (aq) + KBr (aq) →
2. NiCl2 (aq) + Na3PO4 (aq) →
31. What is the molarity of a solution of NaOH formed by diluting 125 ml of 3.0 M NaOH
solution to exactly 500 mL?
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32. Determine the oxidation state of nitrogen in each of the following:
1. NH3
2. N2O4
3. NaNO3
33. What volume of 0.250 M HCl is required to react completely with 25.00 mL of 0.500 M
NaOH?
34. Use the activity series of metals to predict if a reaction occurs:
1. Hg (l) + MnSO4 (aq)  HgSO4 (s) + Mn (s)
2. 2 Ag (s) + H2SO4 (aq)  Ag2SO4 (aq) + H2 (g)
3. Ca (s) + 2H2O (l)  Ca(OH)2 (aq) + H2 (g)
35. How many grams of HCl are contained in exactly 500 mL of a 0.25 M HCl solution?
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