Chemistry Midterm Exam Review
Chemistry Midterm Exam Review
1. Determine the number of significant figures in the following numbers.
a. 0.0107690 g c. 0.010910 mm
b. 9.0100 km d. 910100 cg
2. Record your answer with the correct number of significant figures and units.
a. 65.4 g + 5.399 g c. (5.6 cm)(1.23 cm)
b. 0.00351 mL - 0.000328mL d. (3.20 kg)/(5.10 kg)
3. Convert the following numbers from scientific notation to ordinary notation.
a. 7.02 x 10-5 g b. 5.791 x 105 m
4. Convert the following numbers from ordinary notation to scientific notation.
a. 6500.0 cm b. 0.005800 g
5. How many kilograms are in 691 cg?
6. The Density of Mercury is 13.0 g/mL. If you have 52.5 mL of Mercury, how much does it weigh?
7. A cube of wood that weighs 15.5 g measures 1.42 cm by 2.5 cm by 4.73 cm. What is the density of the wood?
8. What is the volume of a cylinder with a density of 2.70 g/cm3, a height of 52.4 cm, and a diameter of 4.54 cm?
9. Classify the following as a chemical or physical property.
a. color
b. reactivity
c. solubility
10. Classify the following as a chemical or physical change.
a. Burning wood
b. Dry ice coverts to gas
c. boiling water
11. Classify the following as an element or a compound.
a. potassium
b. carbon tetrachloride
c. water
12. Classify the following as a mixture or pure substance.
a. Kool-aid
b. rocky road ice cream
c. tap water
13. Classify the following as a homogeneous or heterogeneous mixture.
a. chunky peanut butter
b. a solution of copper (II) sulfate
c. a bag of trail mix
14. Give the symbols for the following elements
a. Tin d. Bromine
b. Fluorine e. Helium
c. Beryllium f. Antimony
15. Write the formula for the compound containing
a. a two to three ratio of iron to oxygen
b. six carbon, twelve hydrogen and six oxygen
16. Name the scientist responsible for the following.
a. Gold Foil Experiment
b. Plum Pudding Model
c. Atomic Theory
17. From the following symbol determine the number of protons, neutrons, and electrons.
a. 41Ca d. 31P-3
b. 60Co+3 e. 52Cr
c. 6Li+1 f. 127I-1
18. What is the maximum number of electrons that can be in the following:
a. 3rd principle energy level c. any d sublevel
b. 2s sublevel d. 5p orbital
19. Write the complete electron configuration and the orbital diagram for cobalt, boron, krypton and sulfur.
20. Using your periodic table, write the noble gas configurations for rubidium, iron, tungsten and iodine.
21. For each of the following pairs of bonds, choose the bond that will be more polar.
a. H-Si or H-C b. O-Cl or O-I c. F-O or F-H
22. Draw the Lewis dot structure for each of the following (practice “five step math”):
a. CO c. O2 e. NO+
b. CHCl3 d. C2H4 f. NO3-
23. Draw the Lewis dot structure and give the name for the shape of each of the following molecules or ions:
a. BeCl2 c. NBr3 e. BF2I
b. SO4-2 d. H2S f. H2O
24. Identify the following elements as a metal, a nonmetal or a semi-metal
a. Strontium d. Cadmium
b. Antimony e. Silicon
c. Selenium
25. Write the name for the following compounds.
a. CoBr3 g. C2H6
b. Au(CN)3 h. Cs2SO4
c. HCN i. H2S
d. Mg3(PO4)2 j. Sr(OH)2
e. HNO2 k. SiF6
f. NH3 l. BeO
26. Write the formula for the following compounds.
a. calcium peroxide g. tricarbon hexahydride
b. tetraphosphorus decoxide h. nitric acid
c. lithium sulfite i. lead (IV) nitrate
d. manganese (II) acetate j. zinc bromide
e. sodium hypochlorite k. copper (II) hydroxide
f. hydronitric acid l. pentanitrogen octoxide
27. Balance the following equations.
a. ___ C2H5OH + ___ O2 à ___ CO2 + ___ H2O
b. ___ CaC2 + ___ H2O à ___ Ca(OH)2 + ___ C2H2
c. ___ Cl2 + ___ KI à ___ KCl + ___ I2
d. ___ NH3 + ___ Cl2 à ___ NH4Cl + ___ NCl3
e. ___ PbCl2 + ___ K2SO4 à ___ PbSO4 + ___ KCl
28. Write and balance the following equations include state symbols.
a. Solid iron (III) oxide is heated strongly with carbon monoxide gas to produce elemental iron and carbon dioxide gas.
b. Acetylene gas (C2H2) is burned in air to produce carbon dioxide gas and water vapor.
c. Calcium metal is added to water to produce hydrogen gas and the solid calcium hydroxide.
29. Write word equations for the following reactions.
a. 2H2O2 (aq) à 2H2O (l) + O2 (g)
b. 2Ag (s) + H2S (g) à Ag2S (s) + H2 (g)
c. 2FeO (s) + C (s) à 2Fe (l) + CO2 (g)
30. Determine whether the following compounds are soluble or insoluble.
a. sodium acetate
b. silver hydroxide
c. lithium sulfide
d. cobalt (II) sulfate
31. Write Molecular, Complete Ionic, and Net Ionic Equations for the following reactions.
a. lead (II) acetate + aluminum chloride
b. barium hydroxide + nitric acid
c. zinc + sulfuric acid
32. Predict the products and balance the following equations. Include physical state symbols.
a. 2 C4H10 (g) + 13 O2 (g) à ?
b. SO2 (g) + H2O (l) à ?
c. Ca (s) + H2O (l) à ?
d. MgSO3 (aq) à ?
e. AgC2H3O2 (aq) + KBr (aq) à
f. Pb(NO3)2 (aq) + K2CrO4 (aq) →
g. Zn (s) + H2CO3 (aq) →
h. 2 C5H8 (g) + O2 (g) →
i. CaCO3 (s) →
j. Fe2O3 (aq) + H2O(l) →
33. Classify the reactions from #32 as many ways as possible.