GHS Spring Chemistry Final Review 2014 (Use the STAAR Chemistry Reference Materials) Atomic Structure Problems
1. If the wavelength of a certain light is 6.5X10-7m what is the frequency?
2. The frequency of a wave is found to be 9.0X1014Hz. What is the wavelength?
3. The frequency of a wave is 4.0X1014Hz. Calculate the energy.
4. Electrons travel as waves within the atom. Calculate the wavelength of a wave if the energy is 6.9X10 -19J.
5. What happens to the wavelength and energy of the photons of light when the frequency becomes lower?
Behavior of Gases
6. Four gases are placed into the same container. Each gas has a partial pressure of 1.0atm what is the total pressure of the gases within the container?
7. A gas with an initial pressure of 3060 mm Hg and an initial volume of 0.520 L expands to a volume of 2.03 L. What is the final pressure of the gas after the expansion?
8. What is the volume of 2.00 moles of chlorine gas (Cl2) at STP, to the nearest tenth of a liter?
9. Explain why doubling the temperature of a gas in a closed vessel doubles the pressure.
10. Describe the kinetic molecular theory. How does it affect the structure of different states of matter?
Solutions 11. What volume of 1.0 M sodium phosphate must be used to produce 4.0L of 0.80 M sodium phosphate?
12. To prepare a dilute solution a student used 500.mL of a 12.0M HCl solution. The final volume of the dilute solution was 1750.mL. Calculate the molarity of the dilute solution.
13. Find the volume of a solution if 5.00 moles of solute are present and the molarity is 2.25M.
14. What is the pH of a substance that has a hydrogen ion concentration [H+] of 1.2 x 10-2? 15. Calculate the [OH-] in a 0.004M HCl solution.
16. Calculate the [H+] in a 0.09M NaOH solution.
Other Formulas 17. A 10.0mL sample of water has a mass of 10.0g. Calculate the density of water.
18. The density of aluminum is 2.70g/cm3. Calculate the volume of a 25.0g sample of aluminum.
19. An electronic balance used to mass a 10.0g weight reported the mass to be 20.0g. Determine percent error.
20. During a reaction 15.0g of magnesium reacted with excess oxygen. After the reaction students collected 20.2g of magnesium oxide powder. Determine the percent yield for this reaction.
2Mg(s) + O2(g) → 2MgO(s)
21. During a reaction 30.0L of nitrogen gas reacted with excess oxygen. If 59.0L of NO2 were collected what is the percent yield for this reaction?
N2(g) + 2O2(g) → 2NO2(g)
Constants and Conversions 22. How many particles are in 5.0 moles of any substance?
23. How many particles are in 10.0 moles of CaCO3?
24. How many atoms are in 10.0 moles of CaCO3? 25. How many oxygen atoms are in 10.0 moles of CaCO3?
24 26. How many moles of particles are in 3.01X10 CaCO3 particles?
24 27. How many moles of atoms are in 3.01X10 CaCO3 particles?
Conversions and Significant Figures
28. Convert 500.mL of water into L.
29. Determine the number of significant figures in each of the following quantities:
a. 100.0mL
b. 450mL
c. 8.00X10-19J
d. 0.000540kg
30. Write the formulas for the following compounds:
a. Sodium sulfate
b. Sodium sulfite
c. Disulfur decafluoride
31. Write the name of the compound for the following names
a. H3PO4
b. CO2
c. FeCl3 Periodic Table
32. Identify and label the groups and periods on the above periodic table.
33. Label the following groups: alkali metals, alkaline earth metals, halogens, transition metals, and noble gases. List a few properties of each.
34. Label the charges of the elements in following groups: 1, 2, (skip transition metals) 13, 14, 15, 16, 17
35. On the periodic table show the order electrons fill energy levels starting at 1s and ending at 7s.
36. Use the periodic table to identify and explain periodic trends, including atomic and ionic radii, electronegativity, and ionization energy.
a. Which has the larger atomic radii? Mg or Cl
b. Which has the greater electronegativity? P or O
c. Which has the lower ionization energy? K or Br
37. Write the electron configuration for the following atoms:
a. Bromine
b. Germanium
c. Strontium
38. Draw the Lewis valence electron dot structures for the following atoms and compounds:
a. Bromine (Br2)
b. Nitrogen (N) c. MgCl2 (IONIC!!!!!!!!)
39. Draw and identify the molecular geometric shape for the following atoms and compounds:
a. Water (H2O)
b. Carbon Dioxide (CO2)
c. Methane (CH4)
40. Which of the following are physical changes and which are chemical changes:
a. Salt dissolving in water
b. Magnesium reacting with hydrochloric acid
c. Milk turning sour
d. Dry ice changing to a gas
41. Classify the following as either pure substances or mixtures. Define each term.
a. Element
b. Compound
c. Heterogeneous Mixture
c.i. Colloid
c.ii. Suspension
d. Homogenous Mixture d.i. Solution 42. Balance the following chemical equations: a. ___C3H8 + ___O2 → ___H2O + ___CO2
b. ___LiOH → ___Li2O + ___H2O
c. ___Mg + ___Al2(CO3)2 → ___Al + ___MgCO3
43. Define the following terms: a. Intensive Property
b. Extensive Property