Download Thursday, March 27, 2008

Third Quarter Cumulative Review Questions
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Thursday, March 27, 2008
1.
Which factor distinguishes a metallic bond from an ionic bond or a covalent bond?
1. the mobility of electrons
2. the mobility of protons
3. the equal sharing of electrons
4. the unequal sharing of electrons
2.
A 100.00-gram sample of naturally occurring boron contains 19.78 grams of boron-10 (atomic mass = 10.01 atomic
mass units) and 80.22 grams of boron-11 (atomic mass = 11.01 atomic mass units). Which numerical setup can be
used to determine the atomic mass of naturally occurring boron?
1. (0.1978)(10.01) + (0.8022)(11.01)
2. (0.8022)(10.01) + (0.1978)(11.01)
3.
4.
3.
Which atom contains exactly 15 protons?
1. phosphorus-32
2. sulfur-32
3. oxygen-15
4. nitrogen-15
4.
What is the total number of electrons present in an atom of
1. 27
2. 32
3. 39
4. 86
?
Third Quarter Cumulative Review Questions
5.
The number of atoms in a molecule of helium is
1. 1
2. 2
3. 3
4. 4
6.
The concept of an ideal gas is used to explain
1. the mass of a gas sample
2. the behavior of a gas sample
3. why some gases are monatomic
4. why some gases are diatomic
7.
When metals form ions, they tend to do so by
1. losing electrons and forming positive ions
2. losing electrons and forming negative ions
3. gaining electrons and forming positive ions
4. gaining electrons and forming negative ions
8.
What is the formula for sodium oxalate?
1. NaClO
2. Na2O
3. Na2C2O4
4. NaC2H3O2
9.
Which element forms an ion that is larger than its atom?
1. aluminum
2. chlorine
3. magnesium
4. sodium
Third Quarter Cumulative Review Questions
10.
Given the reaction: Ca + 2H 2O
Ca(OH)2 + H2
What is the total number of moles of Ca needed to react completely with 4.0 moles of H2O?
1. 1.0
2. 2.0
3. 0.50
4. 4.0
11.
As the elements in Period 3 are considered from left to right, they tend to
1. lose electrons more readily and increase in metallic
character
2. lose electrons more readily and increase in
nonmetallic character
3. gain electrons more readily and increase in metallic
character
4. gain electrons more readily and increase in
nonmetallic character
12.
What is the chemical formula for copper (II) hydroxide?
1. CuOH
2. CuOH2
3. Cu2(OH)
4. Cu(OH)2
13.
How many moles of solute are contained in 200 milliliters of a 1 M solution?
1. 1
2. 0.2
3. 0.8
4. 200
14.
A mixture of crystals of salt and sugar is added to water and stirred until all solids have dissolved. Which statement
best describes the resulting mixture?
1. The mixture is homogeneous and can be separated by
3. The mixture is heterogeneous and can be separated by
filtration.
filtration.
2. The mixture is homogeneous and cannot be separated
4. The mixture is heterogeneous and cannot be separated
by filtration.
by filtration.
Third Quarter Cumulative Review Questions
15.
Which substance has the same molecular and empirical formulas?
1. C6H4
2. C2H4
3. CH4
4. C6H12O6
16.
When a lithium atom forms an Li+ ion, the lithium atom
1. gains a proton
2. gains an electron
3. loses a proton
4. loses an electron
17.
Which substance has a definite shape, a crystalline structure, and a definite volume at STP?
1. F2
2. Cl2
3. Br2
4. I2
18.
Which kind of energy is stored in a chemical bond?
1. potential energy
2. kinetic energy
3. activation energy
4. ionization energy
19.
The temperature at which the solid and liquid phases of matter exist in equilibrium is called its
1. melting point
2. boiling point
3. heat of fusion
4. heat of vaporization
Third Quarter Cumulative Review Questions
20.
The temperature of a sample of a substance changes from 10°C to 20°C. By how many Kelvins does the temperature
change?
1. 10
2. 20
3. 283
4. 293
21.
Base your answer to the question on the information below.
An atom has an atomic number of 9, a mass number of 19, and an electron configuration of 2-6-1.
Figure 1
What is the total number of neutrons in this atom?
Answer:
neutrons
22.
Given the reaction: CH4 + 2O2
CO2 + 2H2O
What amount of oxygen is needed to completely react with 1 mole of CH4?
1. 2 moles
2. 2 atoms
3. 2 grams
4. 2 molecules
23.
An atom of carbon-14 contains
1. 8 protons, 6 neutrons and 6 electrons
2. 6 protons, 6 neutrons and 8 electrons
3. 6 protons, 8 neutrons and 8 electrons
4. 6 protons, 8 neutrons and 6 electrons
Third Quarter Cumulative Review Questions
24.
Which statement is true about the properties of the elements in any one period of the Periodic Table?
1. They are determined by the number of neutrons.
2. They are determined by the number of electrons in the first
shell.
3. They change in a generally systematic manner.
4. They change in a random, unpredictable
manner.
25.
What is the total number of hydrogen atoms required to form one molecule of C3H5(OH)3?
1. 1
2. 5
3. 3
4. 8
26.
Which electron-dot structure represents a non-polar molecule?
1.
3.
2.
4.
27.
Which substance is composed of atoms that all have the same atomic number?
1. magnesium
2. methane
3. ethane
4. ethene
28.
Which statement is true about a proton and an electron?
1. They have the same masses and the same charges.
2. They have the same masses and different charges.
3. They have different masses and the same charges.
4. They have different masses and different charges.
Third Quarter Cumulative Review Questions
29.
Under which conditions does a real gas behave most like an ideal gas?
1. at low temperatures and high pressures
2. at low temperatures and low pressures
3. at high temperatures and high pressures
4. at high temperatures and low pressures
30.
Which process is a chemical change?
1. melting of ice
3. subliming of ice
2. boiling of water
4. decomposing of water
31.
Which Lewis electron-dot diagram properly shows a sulfur atom in the ground state?
1.
2.
3.
4.
32.
At STP, solid carbon can exist as graphite or as diamond. These two forms of carbon have
1. the same properties and the same crystal structures
2. the same properties and different crystal structures
3. different properties and the same crystal structures
4. different properties and different crystal structures
33.
The temperature of 100 grams of water changes from 16°C to 20°C. What is the total number of joules of heat energy
absorbed by the water?
1. 210J
2. 168J
3. 42000J
4. 1680J
Third Quarter Cumulative Review Questions
34.
The modern model of the atom is based on the work of
1. one scientist over a short period of time
2. one scientist over a long period of time
3. many scientists over a short period of time
4. many scientists over a long period of time
35.
What is the total number of electrons in a S 2- ion?
1. 10
3. 16
2. 14
4. 18
36.
Which group contains elements that are monatomic gases at STP?
1. 1
2. 2
3. 17
4. 18
37.
Which nonmetal is a liquid at STP?
1. oxygen
2. bromine
3. chlorine
4. mercury
38.
The compound CO2(s) sublimes readily at 25°C. Which properties are usually associated with a compound that
undergoes this kind of change?
1. high vapor pressure and high intermolecular
attractions
2. high vapor pressure and low intermolecular attractions
3. low vapor pressure and high intermolecular
attractions
4. low vapor pressure and low intermolecular attractions
Third Quarter Cumulative Review Questions
39.
In which sample are the particles arranged in a regular geometric pattern?
1. HCL(l)
2. NaCl(aq)
3. N2(g)
4. I2(s)
40.
Which sample of water has the lowest vapor pressure?
1. 100 mL at 50°C
2. 200 mL at 30°C
3. 300 mL at 40°C
4. 400 mL at 20°C
41.
Based on the nature of the reactants in each of the equations below, which reaction at 25°C will occur at the fastest
rate?
1. C(s) + O2(g) → CO2 (g)
2. NaOH(aq) + HCl(aq) → NaCl(aq) + H2O( )
3. CH3OH( ) + CH3COOH( ) → CH3COOCH3 (aq) + H2O( )
4. CaCO3(s) → CaO(s) + CO2 (g)
42.
What effect does the addition of a catalyst have on a chemical reaction at equilibrium?
1. It increases the rate of the forward reaction,
only.
2. It increases the rate of the reverse reaction,
only.
3. It increases the rate of both the forward and reverse
reactions.
4. It decreases the rate of both the forward and reverse
reactions.
43.
Which statement best describes the production of a chlorine molecule according to the reaction
Cl + Cl
Cl2 + 58 kcal?
1. A bond is broken, and the reaction is exothermic.
2. A bond is broken, and the reaction is endothermic.
3. A bond is formed, and the reaction is exothermic.
4. A bond is formed, and the reaction is endothermic.
Third Quarter Cumulative Review Questions
44.
Given the balanced equation: 4Fe(s) + 3O 2(g)
2Fe2O3(s) + 1640 kJ
Which phrase best describes this reaction?
1. endothermic with H = +1640 kJ
2. endothermic with H = -1640 kJ
3. exothermic with H = +1640 kJ
4. exothermic with H = -1640 kJ
45.
Which reaction results in an increase in the entropy of a system?
1. H2O(g)
H2O(l)
2. H2O(l)
H2O(s)
3. 2H2O(l)
2H2(g) + O2(g)
4. 2H2(g) + O2(g)
2H2O(l)
46.
Given the change of phase: CO2(g)
CO2(s)
As CO2(g) changes to CO2(s), the entropy of the system
1. decreases
2. increases
3. remains the same
47.
What is the safest method for diluting concentrated sulfuric acid with water?
1. add the acid to the water quickly
2. add the water to the acid quickly
3. add the acid to the water slowly while stirring
4. add the water to the acid slowly while stirring
Third Quarter Cumulative Review Questions
48.
Which piece of laboratory equipment should be used to remove a heated crucible from a ringstand?
1.
3.
2.
4.
49.
Given the reaction: 4Na + O 2
2Na2O
How many grams of oxygen are completely consumed in the production of 1.00 mole of Na2O?
1. 16.0
2. 32.0
3. 62.0
4. 124
50.
Which expression defines the molality (m) of a solution?
1. grams of solute/kg of solution
2. moles of solute/kg of solution
3. grams of solute/kg of solvent
4. moles of solute/kg of solvent
Third Quarter Cumulative Review Questions
Answer Key for Third Quarter Cumulative Review Questions
1. 1
2. 1
3. 1
4. 1
5. 1
6. 2
7. 1
8. 3
9. 2
10. 2
11. 4
12. 4
13. 2
14. 2
15. 3
16. 4
17. 4
18. 1
19. 1
20. 1
21. 10
22. 1
23. 4
24. 3
25. 4
26. 2
27. 1
28. 4
29. 4
30. 4
31. 3
32. 4
33. 4
34. 4
35. 4
36. 4
37. 2
38. 2
39. 4
40. 4
41. 2
42. 3
43. 3
44. 4
45. 3
46. 1
Third Quarter Cumulative Review Questions
47. 3
48. 1
49. 1
50. 4