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MEASUREMENTS
1.. What are the five steps of the scientific method? Give an example of each component.
2. Define precision and accuracy. Give an example of precise measurements and accurate measurements.
3. What is a significant figure? Give an example of a significant figure.
4. How many significant figures are in the following measured values:
204.7040 cm 6.12 x 1010 cm 70030 m 6.0210 x 102 cm
0.00710050 kg 1432010 kg 0.107020 g 4010 nm
5. Complete the following calculations and report your answer to the correct number of significant figures.
4.41 x 1021 m + 6.02 x 1023 m
0.06015 g + 14.2 g
10 g + 15 g
32.3 m x 1.4 x 10-2 m
18.603 g / 2
6. How many significant figures are in a counted number?
7. Convert the following measurements:
1.75 g to mg 4.7 nm to m 0.57 mg to cg
8. Round the following measurements to 3 significant figures.
57.0485 m 12.17 deg C 1764.9 mL 0.0007631 cg
9. The density of the element manganese is 7.21 g/cm3. If you have a piece of manganese with of mass of 25.3 g, what is the volume of this piece of
metal?
Energy and Matter
10. Describe, in your own words, the law of the conservation of matter. Discuss how this law is used in chemistry.
11. What is energy? Give examples of at least three forms of energy.
12. What is matter? Describe some of the properties of matter. What are the four states of matter?
13. Describe the difference between a physical and chemical change.
14. Describe the following and give examples of each: an element, a compound, a substance, a heterogeneous mixture, a homogeneous mixture
Atomic Structure
15. Discuss each of the atomic models that you studied, Dalton's model, Thomson's model, Bohr's model, the modern atomic model.
16. Describe the fundamental particles of the atom.
17. The atomic number is 42. What is the element?
18. What fundamental atomic particle uniquely determines every element?
19. Complete the following table for neutral atoms.
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Atomic Number
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Atomic Mass
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No. of Protons
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No. of Neutrons
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No. of Electrons
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Element Symbol
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8
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8
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14
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7
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7
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21
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20
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56
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26
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11
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23
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20. The atomic number is 19. The number of electrons in the atom is 18. What is the element and what is the charge on the atom?
The Periodic Table
21. How did Mendeleev arrange his periodic table? What is the modern periodic law?
22. Why do the elements in a group have similar properties?
23. Where are the metals, nonmetals and metalloids located in the table? What are the alkali metals, alkaline earth metals, halogens and noble gases?
24. Describe the general differences between elements on the right side of the table and elements on the left side of the table.
25. Do metals gain or lose electrons? Do nonmetals gain or lose electrons?
Chemical Formulas and Bonding
26. What is an ionic bond? What is a covalent bond?
27. Determine the valence electrons and draw the electron dot structure for: Mg, Al, S, Ba, Rb
28. Give the formulas for the following compounds
Copper (II) sulfate Calcium sulfide Potassium nitrate Ammonium nitrate
Silver chloride Sodium phosphate Lithium bromide potassium sulfate
Iron (III) phosphate dinitrogen trioxide sulfur hexachloride
29. Name the following compounds:
NaClO3 NiCl2 MgBr2 Ag2CO3 FeCl3 NH4Cl SO2 PCl5
Chemical Reactions and Equations
30. What is a chemical reaction? Give an example of a reaction.
31. What is a reactant and a product? Give an example of each.
32. Write a balanced chemical equation for the reaction in which sodium and oxygen combine to form sodium oxide.
33. Describe each of the four types of chemical reactions. Give an example of each.
34. Given two chemical equations, how can you determine which equation describes a single-replacement reaction and which describes a double-replacement reaction?
35. Classify the type of reaction that occurs given the following reactants:
a) Element + Element =
b) Element + Ionic Compound =
c) Ionic Compound + Ionic Compound =
d) Compound =
36. What are 3 evidences for chemical change?
The Mole Concept
37. Explain why the mole concept is important in chemistry. What exactly is one mole?
38. What is the molar mass of a substance? What is the molar mass of ammonium carbonate?
39. You have 15.5 g of ammonium carbonate. How many moles of ammonium carbonate do you have?
40. You have 0.35 moles of ammonium carbonate. How many grams of ammonium carbonate do you have?
41. You have 1.2 x 1024 atoms of platinum. How many moles of platinum do you have? How many grams of platinum do you have?
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