Name:
GHS STAAR Chemistry Review Worksheet
(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 energy of one photon of light is 4.9X10-19J. What is the frequency of this light?
4. The frequency of a wave is 4.0X1014Hz. Calculate the energy.
5. Electrons travel as waves within the atom. Calculate the wavelength of a wave if the energy is 6.9X10-19J.
6. Determine the energy associated with a wave if the wavelength is 9.1X10-7m.
Behavior of Gases
7. The total pressure of a homogenous gaseous mixture is 780mmHg. If the gas mixture contains helium at a
pressure of 190mmHg, oxygen at a pressure of 200mmHg, and neon what is the partial pressure of the neon
gas?
8. 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?
9. What is the volume, in L, of 4.0 moles of carbon dioxide gas at 10.0ºC and 867mmHg?
10. How many moles of hydrogen gas are present in a5.0L sample at 25.0ºC and 1.20atm?
11. 4.50 moles of a certain gas occupies a volume of 550.mL at 5.00C and 1.00 atm. What would the volume be if
10.5 moles were present at 27.0C and 1.25 atm?
12. A given sample of gas has a volume of 4.20 L at 60.0C and 1.00 atm. Calculate its pressure if the volume is
changed to 5.00 L and the temperature to 27C.
13. A gas sample contained in a cylinder equipped with a moveable piston occupied 300. mL at a pressure of 2.00
atm. What would be the final pressure if the volume were increased to 500. mL at constant temperature?
14. A balloon that contains 1.50 L of air at 1.00 atm is taken underwater to a depth at which the pressure is 3.00
atm. Calculate the new volume of the balloon. Assume that the temperature remains constant.
15. A fixed quantity of gas at 23.0C exhibits a pressure of 748 torr and occupies a volume of 10.3 L. Calculate the
volume the gas will occupy if the temperature is increased to 145C while the pressure is held constant.
16. A sample of gas occupies a volume of 7.50 L at 0.988 atm and 28.0C. At what temperature is the volume of the
gas 4.00 L if the pressure is kept constant?
17. A 5.50 mole sample of gas has a volume of 2.50L. What would be the volume if the amount increased to 11.0
moles?
18. 7.50 moles of nitrogen occupies 4.25 L. How many moles of nitrogen would be present if the volume were 12.5 L,
assuming pressure and temperature remain constant?
Solutions
19. Calculate the amount in moles of hydrochloric acid needed to make 2000.mL of a 1.5M solution.
20. Find the volume of a solution if 5.00 moles of solute are present and the molarity is 2.25M.
21. If 88.0 grams of NaOH are dissolved in water and the volume of the solution is 3000.mL what is the molarity of
the solution?
22. Calculate the [OH-] in a 0.004M HCl solution.
23. Calculate the [H+] in a 0.09M NaOH solution.
24. 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.
25. 1.5L of a 3.0M solution was diluted to a concentration of 1.8M. What is the volume of the dilute solution?
26. HCl is a strong acid. If the concentration of HCl is 0.0001M what is the pH of the solution?
27. During a titration the concentration of an acidic solution is found to be 0.10M. What is the pH of the solution?
Thermochemistry
28. The reaction of zinc with nitric acid was carried out in a calorimeter. This reaction caused the temperature of 72.0
grams of liquid water, within the calorimeter, to raise from 25.0C to 100.C. If the specific heat of water is 4.18
J/(g•K) calculate the energy associated with this reaction.
29. A 4.00 gram sample of solid gold was heated from 274K to 314K. If the specific heat of gold is 0.129 J/(g•K) how
much energy was involved in this change?
30. Calculate the change in enthalpy for the following reaction given that the standard enthalpy of formation for water
is -285.4kJ/mol, 0.0 kJ/mol for oxygen, and -187.8kJ/mol for hydrogen peroxide.
2H2O(l) + O2(g) → 2H2O(l)
31. Calculate the H value for the following reaction:
CaSO4(s)  CaO(s) + SO3(g) H = ? kJ/mol
Substance
Substance
SO3(g)
CaSO4(s)
CaO(s)
32. Each graph represents the enthalpy diagram for the reaction:
Calculate the H value for each graph.
Hf (kJ/mol)
Hf (kJ/mol)
-395.7
-1434.5
-634.9
A2(g) + X2(g) → 2AX(g)
Other Formulas
33. A 10.0mL sample of water has a mass of 10.0g. Calculate the density of water. (Memorize the density of water.)
34. The density of aluminum is 2.70g/cm3. Calculate the volume of a 25.0g sample of aluminum.
35. During a laboratory investigation a group of students determined the melting point of an unknown substance to be
40.0ºC. The accepted melting point value for this substance was 48.0°C. Calculate percent error.
36. An electronic balance used to mass a 10.0g weight reported the mass to be 20.0g. Determine percent error.
37. During a reaction 15.0g of magnesium reacted with excess oxygen.
2Mg(s) + O2(g) → 2MgO(s)
After the reaction students collected 20.2g of magnesium oxide powder. Determine the percent yield for this reaction.
38. During a reaction 30.0L of nitrogen gas reacted with excess oxygen.
N2(g) + 2O2(g) → 2NO2(g)
If 59.0L of NO2 were collected what is the percent yield for this reaction?
Constants and Conversions
39. How many particles are in 5.0 moles of any substance?
40. How many particles are in 10.0 moles of CaCO3?
How many particles are in 10.0 moles of Cu?
How many particles are in 10.0 moles of K2SO4?
41. How many atoms are in 10.0 moles of CaCO3?
How many oxygen atoms are in 10.0 moles of CaCO3?
How many atoms are in 10.0 moles of Cu?
How many atoms are in 10.0 moles of K2SO4?
How many oxygen atoms are in 10.0 moles of K2SO4?
42. How many ions are in 10.0 moles of CaCO3?
How many carbonate ions are in 10.0 moles of CaCO3?
How many ions are in 10.0 moles of K2SO4?
How many potassium ions are in 10.0 moles of K2SO4?
43. If a certain substance contains 1.204X1025 particles, how many moles of particles are present?
44. How many moles of particles are in 3.01X1024 CaCO3 particles?
How many moles of atoms are in 3.01X1024 CaCO3 particles?
How many moles of ions are in 3.01X1024 CaCO3 particles?
45. How many moles of particles are in 3.01X1024 K2SO4 particles?
How many moles of atoms are in 3.01X1024 K2SO4 particles?
How many moles of ions are in 3.01X1024 K2SO4 particles?
46. Which particle is more massive: alpha, beta , or a neutron?
47. What can be used to shield (or protect) someone from alpha radiation?
48. What can be used to shield (or protect) someone from beta radiation?
49. What can be used to shield (or protect) someone from gamma radiation?
50. Complete the following nuclear radioactive decay equations:
210
206
Po →
Pb
+
84
82
________________
239
U →
92
239
Np
93
+
259
Md →
101
258
Md
101
+
________________
________________
51. If CO2 gas is at STP how many moles of CO2 molecules would be equivalent to 112L?
52. If CO2 gas is at STP what mass, in grams, of CO2 molecules would be equivalent to 112L?
53. If neon gas is at STP how many moles of neon atoms would be equivalent to 67.2L?
54. If neon gas is at STP what mass, in grams, of neon atoms would be equivalent to 67.2L?
55.
3F2(g) + 2AlCl3(s) → 3Cl2(g) + 2AlF3(s)
When 60.0L of F2 react how many L of Cl2 are produced?
When 60.0L of F2 react how many grams of AlF3 are produced?
56. Convert 500.mL of water into cm3.
57. Convert 5L of water into cm3.
58. Convert 5.00 cal to J.
59. Convert 5000. cal to Cal.
60. Convert 5.00kcal to J.
61. Determine the number of significant figures in each of the following quantities:
a. 100.0mL
b. 450mL
c. 8.00X10-19J
d. 0.000540kg
62. Write the formulas for the following compounds:
a. Sodium sulfate
b. Sodium sulfite
c. Lithium phosphate
d. Ammonium nitrate
e. Aluminum hypochlorite
63. Determine if the following ionic compounds are soluble or insoluble in water:
a. Ba(CN)2
b. BaSO4
c. Al(OH)3
d. Sr(OH)2
e. CaCO3
f. Na2CO3
64. Place the following metals in order from most reactive to least reactive: zinc, gold, sodium, silver, iron, lithium
65. Which of the following combinations will cause a redox reaction?
Zn + HCl
or
Cu + HCl
66. Identify the groups and periods on the above periodic table.
67. Label the common charges (or oxidation states) of the elements in following groups: 1, 2, 13, 15, 16, 17
68. On the periodic table show the order electrons fill energy levels starting at 1s and ending at 7s.
69. Label the following groups: alkali metals, alkaline earth metals, halogens, and noble gases. Also label the transition
metals. List a few properties of each.
70. 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
71. Write the electron configuration for the following atoms:
a. Bromine
b. Zirconium
c. Strontium
72. Draw the Lewis valence electron dot structures for the following atoms and compounds:
a. Bromine
b. Strontium
c. Hydrogen
d. CO2
e. H2O
f. F2
g. CH4
h. MgCl2 (IONIC!!!!!!!!)
i. CaO (IONIC!!!!!!!!!!)
73. 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
74. Classify the following as either pure substances or mixtures. Define each term.
a. Element
b. Compound
c. Solution
d. Heterogeneous Mixture
75. Balance the following chemical equations:
a. ___CH4 + ___O2 → ___H2O + ___CO2
b. ___LiOH → ___Li2O + ___H2O
c. ___Mg + ___Al2(CO3)2 → ___Al + ___MgCO3
76. Define the following terms:
a. Electrolytes
b. Nonelectrolyte
c. Unsaturated Solution
d. Saturated Solution
e. Supersaturated Solution
77.
Predict the products and balance the equations for the following reactions. Identify the type of reaction as
either acid-base reaction, precipitation reaction, or redox reaction.
Reaction Type
__________________ LiOH + H2SO4 →
__________________
KOH +
AlCl3 →
__________________
HCl +
Zn →