Download Midterm 3 NY Regents Practice Questions

Name_______________________________________ Date:_______________ Period_______
Midterm 3 NY Regents Practice Questions
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1. An atom is electrically neutral because the
a. number of protons equals the number of electrons
b. number of protons equals the number of neutrons
c. ratio of the number of neutrons to the number of electrons is 1:1
d. ratio of the number of neutrons to the number of protons is 2:1
____
2. Which element is a solid at STP and a good conductor of electricity?
a. iodine
b. mercury
c. nickel
d. sulfur
3. Which element has both metallic and nonmetallic properties?
a. Rb
b. Rn
c. Si
d. Sr
____
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4. Matter that is composed of two or more different elements chemically combined in a fixed
proportion is classified as
a. a compound
b. an isotope
c. a mixture
d. a solution
____
5. Given the balanced equation representing a reaction: 2CO(g) + O2(g) 2CO2(g). What is the mole
ratio of CO(g) to CO2(g) in this reaction?
a. 1:1
b. 1:2
c. 2:1
d. 3:2
____
6. Given the balanced equation representing a reaction: H+(aq) + OH–(aq) H2O(l) + 55.8 kJ
In this reaction there is conservation of
a. mass, only
c. mass and energy, only
b. mass and charge, only
d. mass, charge, and energy
____
7. Which formula represents an ionic compound?
a. H2
b. CH4
c. CH4
d. NH4Cl
8. What is the total number of different elements present in NH4NO3?
a. 7
b. 9
c. 3
d. 4
9. Which sample of matter is a single substance?
a. air
b. ammonia gas
c. salt water
d. hydrochloric acid
____
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____ 10. At STP, which sample contains the same number of molecules as 11.2 liters of CO2(g) at STP?
a. 5.6 L of NO2(g)
b. 7.5 L of H2(g)
c. 11.2 L of N2(g)
d. 22.4 L of CO(g)
____ 11. A sample of gas is held at constant pressure. Increasing the kelvin temperature of this gas sample causes the
average kinetic energy of its molecules to
a. decrease and the volume of the gas sample to decrease
b. decrease and the volume of the gas sample to increase
c. increase and the volume of the gas sample to decrease
d. increase and the volume of the gas sample to increase
____ 12. Which formula represents a hydronium ion?
a. H3O+
b. NH4+
c. OH-
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d.
HCO3-
____ 13. Which compound is an Arrhenius acid?
a. H2SO4
b. KCl
c. NaOH
d. NH3
____ 14. A compound has a molar mass of 90.0 grams per mole and the empirical formula CH2O. What is the molecular
formula of this compound?
a. CH2O
b. C2H4O2
c. C3H6O3
d. C4H8O4
____ 15. The table below shows mass and volume data for four samples of substances at 298 K and
1 atmosphere.
Masses and Volumes of Four Samples
Sample
Mass (g)
Volume (mL)
A
30
60
B
40
50
C
45
90
D
90
120
Which two samples could consist of the same substance?
a. A and B
b. A and C
c. B and C
____ 16. Which kelvin temperature is equal to 56oC?
a. -329 K
b. -217 K
c. 217 K
d. C and D
d. 329 K
____ 17. Given the unbalanced ionic equation: 3Mg + ____Fe3+ 3Mg2+ + ____Fe
When this equation is balanced, both Fe3+ and Fe have a coefficient of
a. 1, because a total of 6 electrons is transferred
b. 2, because a total of 6 electrons is transferred
c. 1, because a total of 3 electrons is transferred
d. 2, because a total of 3 electrons is transferred
____ 18. What is the pH of a solution that has a hydronium ion concentration 100 times greater than a
solution with a pH of 4?
a. 5
b. 2
c. 3
d. 6
____ 19. What is the chemical formula for iron (III) oxide?
a. FeO
b. Fe2O3
c. Fe3O
d. Fe3O2
____ 20. Which phrase describes the molarity of a solution?
a. liters of solute per mole of solution
c. moles of solute per liter of solution
b. liters of solution per mole of solution
d. moles of solution per liter of solution
____ 21. Tetrachloromethane, CCl4, is classified as a
a. compound because the atoms of the elements are combined in a fixed proportion
b. compound because the atoms of the elements are combined in a proportion that varies
c. mixture because the atoms of the elements are combined in a fixed proportion
d. mixture because the atoms of the elements are combined in a proportion that varies
____ 22. Which formulas represent two polar molecules?
a. CO2 and HCl
b. CO2 and CH4
c. H2O and HCl
2
d. H2O and CH4
____ 23. Hydrocarbons are compounds that contain
a. carbon, only
b. carbon and hydrogen, only
c. carbon, hydrogen, and oxygen, only
d. carbon, hydrogen, oxygen, and nitrogen,
only
____ 24. The Arrhenius theory explains the behavior of
a. acids and bases
c. isomers and isotopes
b. alcohols and amines
d. metals and nonmetals
____ 25. In which laboratory process could a student use 0.10 M NaOH(aq) to determine the concentration of an aqueous
solution of HBr?
a. chromatography
c. evaporation of the solvent
b. decomposiiton of the solute
d. titration
____ 26. What is the percent composition by mass of hydrogen in NH4HCO3 (gram-formula mass 
79 g/mol)?
a. 5.1%
b. 6.3%
c. 10.%
d. 50.%
____ 27. A temperature of 37oC is equivalent to a temperature of
a. 98.6 K
b. 236 K
c. 310 K
d. 371 K
____ 28. Given the balanced equation representing a reaction:
NH3(g) + H2O(l) NH4+(aq) + OH-(aq)
According to one acid-base theory, the NH3(g) molecules act as
a. an acid because they accept H+ ions
c. a base because they accept H+ ions
+
b. an acid because they donate H ions
d. a base because they donate H+ ions
____ 29. What volume of 0.120 M HNO3(aq) is needed to completely neutralize 150.0 milliliters of
0.100 M NaOH(aq)?
a. 62.5 mL
b. 125 mL
c. 180 mL
d. 360 mL
____ 30. Which isotopic notation represents an atom of carbon-14?
a. C
b. C
c.
C
d.
C
____ 31. The elements on the Periodic Table are arranged in order of increasing
a. boiling point
c. atomic number
b. electronegativity
d. atomic mas
____ 32. Given the balanced equation representing the reaction between propane and oxygen:
C3H8 + 5O2 3CO2 + 4H2O
According to this equation, which ratio of oxygen to propane is correct?
a.
b.
c.
d.
____ 33. Which substance, when dissolved in water, forms a solution that conducts an electric current?
a. C2H5OH
b. C6H12O6
c. C12H22O11
d. CH3COOH
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____ 34. The balanced equation below represents a molecule of bromine separating into two bromine atoms.
Br2 Br + Br
What occurs during this change?
a. Energy is absorbed and a bond is formed.
b. Energy is absorbed and a bond is broken.
c. Energy is released and a bond is formed.
d. Energy is released and a bond is broken
____ 35. Bronze contains 90 to 95 percent copper and 5 to 10 percent tin. Because these percentages can vary, bronze is
classified as
a. a compound
b. an element
c. a mixture
d. a substance
____ 36. The molar mass of Ba(OH)2 is
a. 154.3 g
b. 155.3 g
c. 171.3 g
d. 308.6 g
____ 37. Given the balanced equation representing a reaction:
4NH3 + 5O2 4NO + 6H2O
What is the minimum number of moles of O2 that are needed to completely react with 16 moles of NH3?
a. 16 mol
b. 20 mol
c. 64 mol
d. 80 mol
____ 38. Which Lewis electron-dot diagram correctly represents a hydroxide ion?
a. 1
b. 2
c. 3
d. 4
____ 39. A 10.0-gram sample of which element has the smallest volume at STP?
a. aluminum
b. magnesium
c. titanium
d. zinc
____ 40. At which temperature would atoms of a He(g) sample have the greatest average kinetic energy?
a. 25oC
b. 37oC
c. 273K
d. 298K
____ 41. At room temperature, a mixture of sand and water can be separated by
a. ionization
b. combustion
c. filtration
d. sublimation
____ 42. As the pH of a solution is changed from 3 to 6, the concentration of hydronium ions
a. increases by a factor of 3
c. decreases by a factor of 3
b. increases by a factor of 1000
d. decreases by a factor of 1000
____ 43. Which value of an element is calculated using both the mass and the relative abundance of
each of the naturally occurring isotopes of this element?
a. atomic number
b. atomic mass
c. half-life
d. molar volume
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____ 44. Sodium atoms, potassium atoms, and cesium atoms have the same
a. atomic radius
c. total number of protons
b. first ionization energy
d. oxidation state
____ 45. Which element has the greatest density at STP?
a. calcium
b. carbon
c. chlorine
d. copper
____ 46. Which unit can be used to express solution concentration?
a. J/mol
b. L/mol
c. mol/L
d. mol/s
____ 47. Under which conditions of temperature and pressure is a gas most soluble in water?
a. high temperature and low pressure
c. low temperature and low pressure
b. high temperature and high pressure
d. low temperature and high pressure
____ 48. Given the equation representing a system at equilibrium:
At which temperature does this equilibrium exist at 101.3 kilopascals?
a. 0 K
b. 0oC
c. 32 K
d. 273oC
____ 49. Which substance is an Arrhenius acid?
a. Ba(OH)2
b. CH3COOCH3
c. H3PO4
d. NaCl
____ 50. Which compound releases hydroxide ions in an aqueous solution?
a. CH3COOH
b. CH3OH
c. HCl
d. KOH
____ 51. What is the gram-formula mass of Ca3(PO4)2?
a. 248g/mol
b. 263 g/mol
c. 279 g/mol
d. 310 g/mol
____ 52. What is the concentration of O2(g), in parts per million, in a solution that contains 0.008 gram of O2(g) dissolved
in 1000.0 grams of H2O(l)?
a. 0.8 ppm
b. 8 ppm
c. 80 ppm
d. 800 ppm
____ 53. The table below shows data for the temperature, pressure, and volume of four gas samples.
Data for Four Gas Samples
Gas
Sample
A
Temperature
(K)
100
Pressure
(atm)
2
Volume
(mL)
400
B
200
2
200
C
100
2
400
D
200
4
200
Which two gas samples have the same total number of molecules?
a. A and B
b. A and C
c. B and C
d. B and D
____ 54. A rigid cylinder with a movable piston contains a 2.0-liter sample of neon gas at STP. What is
the volume of this sample when its temperature is increased to 30oC while its pressure is
decreased to 90 kilopascals?
a. 2.5 L
b. 2.0 L
c. 1.6 L
d. 0.22 L
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____ 55. Which volume of 0.10 M NaOH(aq) exactly neutralizes 15.0 milliliters of 0.20 M HNO3(aq)?
a. 1.5 mL
b. 7.5 mL
c. 3.0 mL
d. 30 mL
____ 56. The pH of an aqueous solution changes from 4 to 3 when the hydrogen ion concentration in
the solution is
a. decreased by a factor of 3/4
c. increased by a factor of 4/3
b. decreased by a factor of 10
d. increased by a factor of 10
____ 57. Which two particles each have a mass approximately equal to one atomic mass unit?
a. electron and neutron
c. proton and electron
b. electron and positron
d. proton and neutron
____ 58. Which element is most chemically similar to chlorine?
a. Ar
b. F
c. Fr
d. S
____ 59. When an atom loses one or more electrons, this atom becomes a
a. positive ion with a radius smaller than the radius of this atom
b. positive ion with a radius larger than the radius of this atom
c. negative ion with a radius smaller than the radius of this atom
d. negative ion with a radius larger than the radius of this atom
____ 60. Given the balanced equation: I + I I2
Which statement describes the process represented by this equation?
a. A bond is formed as energy is absorbed.
b. A bond is formed and energy is released.
c. A bond is broken as energy is absorbed.
d. A bond is broken and energy is released.
____ 61. An oxygen molecule contains a double bond because the two atoms of oxygen share a total of
a. 1 electron
b. 2 electrons
c. 3 electrons
d. 4 electrons
____ 62. Which term is defined as a measure of the average kinetic energy of the particles in a sample?
a. temperature
b. pressure
c. thermal energy
d. chemical energy
____ 63. A 3.0 M HCl(aq) solution contains a total of
a. 3.0 grams of HCl per liter of water
b. 3.0 grams of HCl per mole of solution
c. 3.0 moles of HCl per liter of solution
d. 3.0 moles of HCl per mole of water
____ 64. An Arrhenius base yields which ion as the only negative ion in an aqueous solution?
a. hydride ion
c. hydronium ion
b. hydrogen ion
d. hydroxide ion
____ 65. According to one acid-base theory, a water molecule acts as an acid when the water
molecule
a. accepts an H+
c. donates an H+
–
b. accepts an OH
d. donates an OH–
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____ 66. Which particle diagram represents a sample of one compound, only?
a. 1
b. 2
c. 3
d. 4
____ 67. Which two formulas represent Arrhenius acids?
a. CH3COOH and CH3CH2OH
c. KHCO3 and KHSO4
b. HC2H3O2 and H3PO4
d. NaSCN and Na2S2O3
____ 68. A proton has a charge that is opposite the charge of
a. a positron
b. a neutron
c. an electron
d. an alpha particle
____ 69. As a bond between a hydrogen atom and a sulfur atom is formed, electrons are
a. shared to form an ionic bond
c. transferred to form an ionic bond
b. shared to form a covalent bond
d. transferred to form a covalent bond
____ 70. In which sample is the average kinetic energy of the particles greatest?
a. 10 mL of HCl(aq) at 20oC
c. 10 mL of H2O(l) at 35oC
o
b. 15 mL of HCl(aq) at 20 C
d. 15 mL of H2O(l) at 30oC
____ 71. Which sample at STP has the same number of molecules as 5 liters of NO2(g) at STP?
a. 5 grams of H2(g)
c. 5 moles of O2(g)
b. 5 liters of CH4(g)
d. 5 x 1023 molecules of CO2(g)
____ 72. Under which conditions of temperature and pressure does oxygen gas behave least like an
ideal gas?
a. low temperature and low pressure
c. high temperature and low pressure
b. low temperature and high pressure
d. high temperature and high pressure
____ 73. Given the balanced equation representing a reaction: 2H2 + O2 2H2O
What is the total mass of water formed when 8 grams of hydrogen reacts completely with
64 grams of oxygen?
a. 18 g
b. 36 g
c. 56 g
d. 72 g
____ 74. An iron bar at 325 K is placed in a sample of water. The iron bar gains energy from the water
if the temperature of the water is
a. 65 K
b. 45 K
c. 65oC
d. 45oC
____ 75. A sample of gas occupies a volume of 50.0 milliliters in a cylinder with a movable piston. The
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pressure of the sample is 0.90 atmosphere and the temperature is 298 K. What is the volume of the sample at
STP?
a. 41 mL
b. 49 mL
c. 51 mL
d. 55 mL
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Midterm 3 NY Regents Practice Questions
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