Download Chemistry 1- Final Exam Review

Chemistry 1- Final Exam Review
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1. All
a.
b.
c.
d.
e.
____
2. What is the correct answer to the following expression: (49.1 – 42.61) ! 13.1?
a. 9 ! 102
d. 85.02
b. 85
e. 85.019
c. 85.0
____
3. Read the length of the bar off the magnified ruler below. Report the correct number of digits.
a.
b.
c.
of the following are examples of chemical change EXCEPT
the condensation of steam.
the rusting of iron.
the combustion of propane gas.
the tarnishing of silver.
the decomposition of water to hydrogen gas and oxygen gas.
1.1 cm
1.10 cm
1.13 cm
d.
e.
1.130 cm
1.25 cm
____
4. Which of the following measurements contains two significant figures?
a. 0.00400 L
c. 0.00044 L
b. 0.00404 L
d. 0.00440 L
____
5. What volume would be occupied by a piece of aluminum (density 2.70 g/mL) weighing 85 g?
a. 229.5 mL
d. 3.2 mL
b. 3.2 x 10-2 mL
e. none of these
c. 31 mL
____
6. Which statement concerning NaCl is true?
a. NaCl has properties similar to sodium metal and chlorine gas.
b. NaCl is a homogeneous mixture.
c. NaCl is a heterogeneous mixture.
d. The percentage of Na in NaCl is dependent on where the sample is obtained.
e. NaCl is composed of ions, which are electrically charged atoms.
____
7. Which of the following is a homogeneous mixture?
a. italian salad dressing
d. a rock, such as granite or marble
b. chocolate chip ice cream
e. a jar of chunky peanut butter
c. gasoline
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8.
Given the particle diagram representing four molecules of a
substance:
Which particle diagram best represents this same substance after a physical change has taken place?
9. In the panels above, which represent(s) a pure compound?
10. In the panels above, which represent(s) a mixture of elements?
____ 11. The correct name for LiCl is
a. lithium monochloride
b. lithium(I) chloride
c. monolithium chloride
d.
e.
lithium chloride
monolithium monochloride
____ 12. The formula for the compound formed from the polyatomic ions NH4 + and PO4 3- is
a. NH4 (PO4 )3
c. (NH4 )3 PO4
b. NH4 PO4
d. (NH4 )2 (PO4 )2
____ 13. The correct name for Cu2 O is
a. copper oxide
b. copper(I) oxide
c. copper(II) oxide
d.
e.
dicopper oxide
dicopper monoxide
____ 14. The correct name for P2 O5 is
a. phosphorus(II) oxide
b. phosphorus(V) oxide
c. diphosphorus oxide
d.
e.
diphosphorus pentoxide
phosphorus pentoxide
____ 15. Titanium(IV) oxide has the formula
a. Ti4 O
b. TiO4
c. Ti(IV)O
d.
e.
TiO2
Ti4 O2
2
____ 16. The
a.
b.
c.
total number of oxygen atoms indicated by the formula Fe2 (CO3 ) 3 is
3
d. 12
6
e. 18
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When the following equations are balanced using the smallest possible integers, what is the number in
front of the underlined substance in each case?
____ 17. FeCl2 (aq) + Ag3 PO4 (aq) " Fe3 (PO4 )2 (aq) + AgCl(s)
a.
b.
e.
12
____ 19. Which of the following elements is an alkaline earth metal?
a. Ca
b. Cu
c. Fe
d. Na
e.
Sc
____ 20. Which of the following is a noble gas?
a. Ar
b. N2
c.
e.
CO2
e.
Br
1
2
c.
d.
4
____ 18. Which of the following is a nonmetal?
a. cerium
b. cesium
c. carbon
d.
e.
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calcium
copper
H2
d.
O2
____ 21. Which of the following elements is in the same period as phosphorus?
a. carbon
c. nitrogen
b. magnesium
d. oxygen
____ 22. Which atomic particle determines the chemical behavior of an atom?
a. proton
d. nucleus
b. electron
e. none of these
c. neutron
____ 23. Which of the following elements is most similar to chlorine?
a. H
b. He
c. Na
d. Hg
____ 24. Which of the following contains the largest number of oxygen atoms?
a. 4 H2 O
d. H2 SO4
b. 3 CO2
e. Al(NO3 ) 3
c. O3
____ 25. How many moles of silver atoms are in 1.8 ! 10
20
atoms of silver?
a.
3.0 ! 10
#4
c.
3.0 ! 10
2
b.
3.3 ! 10
#3
d.
1.1 ! 10
44
c.
d.
96 g
78 g
____ 26. What is the molar mass of (NH 4 ) 2 CO 3 ?
a.
b.
144 g
138 g
3
____ 27. What is the mass in grams of 5.90 mol C 8 H 18 ?
a.
b.
0.0512 g
19.4 g
c.
d.
389 g
673 g
____ 28. The equation 2C 3 H 7 OH + 9O 2 " 6CO 2 + 8H 2 O is an example of which type of reaction?
a.
b.
combustion reaction
single-replacement reaction
c.
d.
double-replacement reaction
decomposition reaction
____ 29. The reaction 2Fe + 3Cl 2 " 2FeCl 3 is an example of which type of reaction?
a.
b.
combustion reaction
single-replacement reaction
c.
d.
combination reaction
decomposition reaction
____ 30. In the reaction
a.
0
Al2 S3 (s) + 6HCl(aq) " 2AlCl3 (aq) + 3H2 S(g)
how many moles of HCl are used for each mole of AlCl3 formed?
b. 1
c. 1.5
d. 2
e.
3
____ 31. In a combustion reaction, one of the reactants is ____.
a. hydrogen
c. oxygen
b. nitrogen
d. a metal
____ 32. When potassium hydroxide and barium chloride react, potassium chloride and barium hydroxide are
formed. The balanced equation for this reaction is ____.
a. KH + BaCl " KCl + BaH
c. 2KOH + BaCl 2 " 2KCl + Ba(OH) 2
b.
KOH + BaCl " KCl + BaOH
d.
KOH + BaCl 2 " KCl 2 + BaOH
____ 33. In the reaction represented by the equation N2 + 3H2 " 2NH3 , what is the mole ratio of nitrogen to
ammonia?
a. 1:1
c. 1:3
b. 1:2
d. 2:3
____ 34. In the equation 2KClO3 " 2KCl + 3O2 , how many moles of oxygen are produced when 3.0 mol of
KClO3 decompose completely?
a. 1.0 mol
c. 3.0 mol
b. 2.5 mol
d. 4.5 mol
____ 35. For the reaction represented by the equation 2Na + 2H2 O " 2NaOH + H2 , how many grams of hydrogen
are produced if 120. g of sodium and 80. g of water are available?
a. 4.4 g
c. 80. g
b. 44 g
d. 200 g
____ 36. What is the percent by mass of carbon in acetone, C 3 H 6 O?
a.
b.
20.7%
62.1%
c.
d.
4
1.61%
30.0%
____ 37. Which of the following compounds have the same empirical formula?
a. CO 2 and SO 2
c. C 4 H 10 and C 10 H 4
b.
C 7 H 14 and C 10 H 20
d.
C 6 H 12 and C 6 H 14
____ 38. What is the empirical formula of a substance that is 53.5% C, 15.5% H, and 31.1% N by weight?
a. C 3 HN 2
c. C 2 H7 N
b.
C 4 H 14 N 2
d.
CH 4 N 7
____ 39. Atoms of the same element having the same atomic number but different mass numbers are called
a. isomers
d. isotopes
b. orbitals
e. nuclei
c. neutrons
____ 40. How many protons, electrons, and neutrons respectively does
a.
b.
c.
53, 127, 74
53, 74, 53
53, 53, 127
____ 41. Which particle has the smallest mass?
a. neutron
b. proton
____ 42. The number of neutrons in one atom of
a.
b.
c.
82
206
124
I have?
d.
e.
74, 53, 127
53, 53, 74
c.
d.
electron
helium nucleus
Pb is
d.
e.
288
none of these
____ 43. Each period in the periodic table corresponds to ____.
a. a principal energy level
c. an orbital
b. an energy sublevel
d. a suborbital
2
2
6
2
2
____ 44. What element has the electron configuration 1s 2s 2p 3s 3p ?
a. nitrogen
c. silicon
b. selenium
d. silver
____ 45. What is the energy required to remove an electron from an atom in the gaseous state called?
a. nuclear energy
c. shielding energy
b. ionization energy
d. electronegative energy
____ 46. How does atomic radius change from top to bottom in a group in the periodic table?
a. It tends to decrease.
c. It first increases, then decreases.
b. It tends to increase.
d. It first decreases, then increases.
____ 47. How does atomic radius change from left to right across a period in the periodic table?
a. It tends to decrease.
c. It first increases, then decreases.
b. It tends to increase.
d. It first decreases, then increases.
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____ 48. In which of the following sets are the charges given correctly for all the ions?
+
+
+
2#
3+
a. Na , Mg , Al
c. Rb # , Ba , P
+
2+
2#
2#
3#
b. K , Sr , O
d. N # , O , F
____ 49. What is the element with the lowest electronegativity value?
a. cesium
c. calcium
b. carbon
d. fluorine
____ 50. Which of the following elements has the smallest first ionization energy?
a. sodium
c. potassium
b. calcium
d. magnesium
____ 51. What is the amount of heat required to raise the temperature of 200.0 g of aluminum by 10°C? (specific
cal
heat of aluminum = 0.21
)
g°C
a. 420 cal
c. 42,000 cal
b. 4200 cal
d. 420,000 cal
____ 52. The specific heat of silver is 0.24
from 25.0°C to 27.5°C?
a. 2.62 J
b. 0.14 J
J
. How many joules of energy are needed to warm 4.37 g of silver
g°C
c.
d.
45.5 J
0.022 J
Figure 1
____ 53. Are the forward reaction and the reverse reaction in Figure 1 exothermic or endothermic?
a. Both reactions are exothermic.
b. The forward reaction is endothermic, the reverse reaction is exothermic.
c. The forward reaction is exothermic, the reverse reaction is endothermic.
d. Both reactions are endothermic.
____ 54. In Figure 1, what is the value of $H for the forward reaction?
a. –20 kJ
c. –30 kJ
b. +20 kJ
d. +30 kJ
____ 55. What is the activation energy for the reverse reaction in Figure 1?
a. –50 kJ
c. –20 kJ
b. +50 kJ
d. +20 kJ
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____ 56. All of the following atoms have an octet of electrons except
a. Al3+.
c. Mg2+.
–
b. Cl .
d. O –.
____ 57. Which of the following atoms has the smallest atomic radius?
a. As
d. P
b. Sb
e. N
c. Bi
____ 58. Which of the following has the highest ionization energy?
a. K
d. N
b. Ca
e. O
c. C
____ 59. For the element whose electron configuration is [Ne] 3s2 3p 3 , how many dots would the Lewis dot
diagram have?
a. 3
c. 8
b. 5
d. 13
____ 60. Which of the following bonds is primarily covalent?
a. O–N
c. O–K
b. Na–S
d. Cl–Li
____ 61. Which of the following bonds would be considered completely nonpolar?
a. H–N
c. O–C
b. O–O
d. F–Cl
____ 62. The shape of the methane molecule is called ____.
a. tetrahedral
c. four-cornered
b. square
d. planar
____ 63. What shape does a water molecule have?
a. linear
b. pyramidal
c.
d.
trigonal planar
bent
____ 64. In a pyramidal molecule, how many unshared pairs of valence electrons does the central atom have?
a. none
c. two
b. one
d. three
____ 65. Which of the following contains the largest number of oxygen atoms?
a. 4H2 O
c. H2 SO4
b. 3CO2
d. 2Al(NO3 ) 3
____ 66. An element’s most stable ion forms an ionic compound with chlorine having the formula XCl2 . If the ion
of element X has a mass of 89 and 36 electrons, what is the identity of the element, and how many
neutrons does it have?
a. Kr, 53 neutrons
d. Sr, 51 neutrons
b. Kr, 55 neutrons
e. Rb, 52 neutrons
c. Se, 55 neutrons
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____ 67. Which of these elements does not exist as a diatomic molecule?
a. C
c. H
b. F
d. I
____ 68. At constant temperature and pressure, gas volume is directly proportional to the
a. molar mass of the gas.
c. density of the gas at STP.
b. number of moles of gas.
d. pressure of the gas
____ 69. Calculate the approximate temperature of a 0.50 mol sample of gas at 750 mm Hg and a volume of 12 L.
a. –7°C
c. 16°C
b. 11°C
d. 288°C
____ 70. What happens to the pressure of a gas inside a container if the temperature of the gas decreases?
a. The pressure increases.
c. The pressure decreases.
b. The pressure does not change.
d. The pressure cannot be predicted.
____ 71. If 4 moles of gas are added to a container that already holds 1 mole of gas, how will the pressure change
inside the container?
a. The pressure will be five times higher.
b. The pressure will double.
c. The pressure will be four times higher.
d. The pressure will not change.
____ 72. A gas occupies a volume of 2.4 L at 14.1 kPa. What volume will the gas occupy at 84.6 kPa?
a. 497 L
c. 14 L
b. 2.5 L
d. 0.40 L
____ 73. At a certain temperature and pressure, 0.20 mol of carbon dioxide has a volume of 3.1 L. A 3.1-L sample
of hydrogen at the same temperature and pressure ____.
a. has the same mass
b. contains the same number of atoms
c. has a higher density
d. contains the same number of molecules
____ 74. Which of the following usually makes a substance dissolve faster in a solvent?
a. agitating the solution
b. increasing the particle size of the solute
c. lowering the temperature
d. decreasing the number of particles
____ 75. What is the maximum amount of KCl that can dissolve in 200 g of water?
(The solubility of KCl is 34 g/100 g H2 O at 20°C.)
a. 17 g
c. 68 g
b. 34 g
d. 6800 g
____ 76. If a crystal added to an aqueous solution causes many particles to come out of the solution, the original
solution was ____.
a. unsaturated
c. an emulsion
b. saturated
d. supersaturated
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____ 77. The solubility of a gas in a liquid is ____.
a. proportional to the square root of the pressure of the gas above the liquid
b. directly proportional to the pressure of the gas above the liquid
c. inversely proportional to the pressure of the gas above the liquid
d. unrelated to the pressure of the gas above the liquid
____ 78. What is the number of moles of solute in 250 mL of a 0.4M solution?
a. 0.1 mol
c. 0.62 mol
b. 0.16 mol
d. 1.6 mol
____ 79. What is the molarity of a solution containing 56 grams of solute in 959 mL of solution? (molar mass of
solute = 26 g/mol)
a. 1.5M
c. 2.1M
b. 2.2M
d. 0.0022M
____ 80. How many mL of a 2.0M NaBr solution are needed to make 200.0 mL of 0.50M NaBr?
a. 25 mL
c. 100 mL
b. 50 mL
d. 150 mL
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Chemistry 1- Final Exam Review
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