regents chemistry Flashcards

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1. Which statement describes the charge of an electron and the charge of a proton? A. An electron and a proton both have a charge of +1. B. An electron and a proton both have a charge of −1. C. An electron has a charge of +1, and a proton has a charge of −1. D. An electron has a charge of −1, and a proton has a charge of +1.
2. Which subatomic particles are found in the nucleus of an atom of beryllium? A. electrons and protons B. electrons and positrons C. neutrons and protons D. neutrons and electrons
3. The elements in Period 4 on the Periodic Table are arranged in order of increasing A. atomic radius B. atomic number C. number of valence electrons D. number of occupied shells of electrons
4. Which phrase describes two forms of solid carbon, diamond and graphite, at STP? A. the same crystal structure and the same properties B. the same crystal structure and different properties C. different crystal structures and the same properties D. different crystal structures and different properties
5. Which element has six valence electrons in each of its atoms in the ground state? A. Se B. As C. Kr D. Ga
6. What is the chemical name for H2SO3(aq)? A. sulfuric acid B. sulfurous acid C. hydrosulfuric acid D. hydrosulfurous acid
7. Which substance is most soluble in water? A. (NH4)3PO4 B. Cu(OH)2 C. Ag2SO4 D. CaCO3
8. Which type of bonding is present in a sample of an element that is malleable? A. ionic B. metallic C. nonpolar covalent D. polar covalent
9. Which atom has the greatest attraction for the electrons in a chemical bond? A. hydrogen B. oxygen C. silicon D. sulfur
10. Which type of reaction involves the transfer of electrons? A. alpha decay B. double replacement C. neutralization D. oxidation-reduction
11. A 10.0-gram sample of nitrogen is at STP. Which property will increase when the sample is cooled to 72 K at standard pressure? A. mass B. volume C. density D. temperature
12. Which element is a gas at STP? A. sulfur B. xenon C. potassium D. phosphorus
13. A 5.0-gram sample of Fe(s) is to be placed in 100. milliliters of HCl(aq). Which changes will result in the fastest rate of reaction? A. increasing the surface area of Fe(s) and increasing the concentration of HCl(aq) B. increasing the surface area of Fe(s) and decreasing the concentration of HCl(aq) C. decreasing the surface area of Fe(s) and increasing the concentration of HCl(aq) D. decreasing the surface area of Fe(s) and decreasing the concentration of HCl(aq)
14. Which process is commonly used to separate a mixture of ethanol and water? A. distillation B. ionization C. filtration D. titration
15. A sample of hydrogen gas will behave most like an ideal gas under the conditions of A. low pressure and low temperature B. low pressure and high temperature C. high pressure and low temperature D. high pressure and high temperature
16. The collision theory states that a reaction is most likely to occur when the reactant particles collide with the proper A. formula masses B. molecular masses C. density and volume D. energy and orientation
17. At STP, which sample contains the same number of molecules as 3.0 liters of H2(g)? A. 1.5 L of NH3(g) B. 2.0 L of CO2(g) C. 3.0 L of CH4(g) D. 6.0 L of N2(g)
18. The addition of a catalyst to a chemical reaction provides an alternate pathway that A. increases the potential energy of reactants B. decreases the potential energy of reactants C. increases the activation energy D. decreases the activation energy
19. A sample of water is boiling as heat is added at a constant rate. Which statement describes the potential energy and the average kinetic energy of the water molecules in this sample? A. The potential energy decreases and the average kinetic energy remains the same. B. The potential energy decreases and the average kinetic energy increases. C. The potential energy increases and the average kinetic energy remains the same. D. The potential energy increases and the average kinetic energy increases.
20. Entropy is a measure of the A. acidity of a sample B. disorder of a system C. concentration of a solution D. chemical activity of an element
21. Which element has atoms that can bond with each other to form ring, chain, and network structures? A. aluminum B. calcium C. carbon D. argon
22. What is the number of electrons shared in the multiple carbon-carbon bond in one molecule of 1-pentyne? A. 6 B. 2 C. 3 D. 8
23. Butanal, butanone, and diethyl ether have different properties because the molecules of each compound differ in their A. numbers of carbon atoms B. numbers of oxygen atoms C. types of functional groups D. types of radioactive isotopes
24. What occurs when a magnesium atom becomes a magnesium ion? A. Electrons are gained and the oxidation number increases. B. Electrons are gained and the oxidation number decreases. C. Electrons are lost and the oxidation number increases. D. Electrons are lost and the oxidation number decreases.
25. Energy is required to produce a chemical change during A. chromatography B. electrolysis C. boiling D. melting
26. The reaction of an Arrhenius acid with an Arrhenius base produces water and A. a salt B. an ester C. an aldehyde D. a halocarbon
27. One acid-base theory defines an acid as an A. H⁻ acceptor B. H⁻ donor C. H⁺ acceptor D. H⁺ donor
28. Which phrase describes the decay modes and the half-lives of K-37 and K-42? A. the same decay mode but different half-lives B. the same decay mode and the same half-life C. different decay modes and different half-lives D. different decay modes but the same half-life
29. Which particle has a mass that is approximately equal to the mass of a proton? A. an alpha particle B. a beta particle C. a neutron D. a positron
30. Which change occurs during a nuclear fission reaction? A. Covalent bonds are converted to ionic bonds. B. Isotopes are converted to isomers. C. Temperature is converted to mass. D. Matter is converted to energy.
31. Compared to an electron, which particle has a charge that is equal in magnitude but opposite in sign? A. an alpha particle B. a beta particle C. a neutron D. a proton
32. The mass of a proton is approximately equal to A. 1 atomic mass unit B. 12 atomic mass units C. the mass of 1 mole of carbon atoms D. the mass of 12 moles of electrons
33. Which property decreases when the elements in Group 17 are considered in order of increasing atomic number? A. atomic mass B. atomic radius C. melting point D. electronegativity
34. Any substance composed of two or more elements that are chemically combined in a fixed proportion is A. an isomer B. an isotope C. a solution D. a compound
35. Which term refers to how strongly an atom of an element attracts electrons in a chemical bond with an atom of a different element? A. entropy B. electronegativity C. activation energy D. first ionization energy
36. At STP, which substance has metallic bonding? A. ammonium chloride B. barium oxide C. iodine D. silver
37. What is the number of electrons shared between the carbon atoms in a molecule of ethyne? A. 6 B. 2 C. 8 D. 4
38. Which atom in the ground state has a stable valence electron configuration? A. Ar B. Al C. Si D. Na
39. What occurs when two fluorine atoms react to produce a fluorine molecule? A. Energy is absorbed as a bond is broken. B. Energy is absorbed as a bond is formed. C. Energy is released as a bond is broken. D. Energy is released as a bond is formed.
40. Which gas sample at STP has the same number of molecules as a 2.0-liter sample of Cl2(g) at STP? A. 1.0 L of NH3(g) B. 2.0 L of CH4(g) C. 3.0 L of CO2(g) D. 4.0 L of NO(g)
41. All atoms of uranium have the same A. mass number B. atomic number C. number of neutrons plus protons D. number of neutrons plus electrons
42. The concentration of a solution can be expressed in A. kelvins B. milliliters C. joules per kilogram D. moles per liter
43. Compared to the boiling point and the freezing point of water at 1 atmosphere, a 1.0 M CaCl2(aq) solution at 1 atmosphere has a A. lower boiling point and a lower freezing point B. lower boiling point and a higher freezing point C. higher boiling point and a lower freezing point D. higher boiling point and higher freezing point
44. According to the kinetic molecular theory, which statement describes an ideal gas? A. The gas particles are diatomic. B. Energy is created when the gas particles collide. C. There are no attractive forces between the gas particles. D. The distance between the gas particles is small, compared to their size.
45. Which physical change is endothermic? A. CO2(s) → CO2(g) B. CO2(ℓ) → CO2(s) C. CO2(g) → CO2(ℓ) D. CO2(g) → CO2(s)
46. Which Group 16 element combines with hydrogen to form a compound that has the strongest hydrogen bonding between its molecules? A. oxygen B. selenium C. sulfur D. tellurium
47. Hydrocarbons are composed of the elements A. carbon and hydrogen, only B. carbon and oxygen, only C. carbon, hydrogen, and oxygen D. carbon, nitrogen, and oxygen
48. Which atom is bonded to the carbon atom in the functional group of a ketone? A. fluorine B. hydrogen C. nitrogen D. oxygen
49. Two types of organic reactions are A. addition and sublimation B. deposition and saponification C. decomposition and evaporation D. esterification and polymerization
50. The isomers butane and methylpropane have A. the same molecular formula and the same properties B. the same molecular formula and different properties C. different molecular formulas and the same properties D. different molecular formulas and different properties
51. In a redox reaction, which particles are lost and gained in equal numbers? A. electrons B. neutrons C. hydroxide ions D. hydronium ions
52. What is the oxidation state for a Mn atom? A. 0 B. +7 C. +3 D. +4
53. Which compounds are classified as electrolytes? A. KNO3 and H2SO4 B. KNO3 and CH3OH C. CH3OCH3 and H2SO4 D. CH3OCH3 and CH3OH
54. Which compound is an Arrhenius base? A. CO2 B. CaSO4 C. Ca(OH)2 D. C2H5OH
55. According to one acid-base theory, a water molecule acts as a base when it accepts A. an H⁺ ion B. an OH⁻ ion C. a neutron D. an electron
56. Given the equation representing a system at equilibrium: N2(g) + 3H2(g) ⇌ 2NH3(g) Which statement describes this reaction at equilibrium? A. The concentration of N2(g) decreases. B. The concentration of N2(g) is constant. C. The rate of the reverse reaction decreases. D. The rate of the reverse reaction increases.
57. The acidity or alkalinity of an unknown aqueous solution is indicated by its A. pH value B. electronegativity value C. percent by mass concentration D. percent by volume concentration
58. The laboratory process in which the volume of a solution of known concentration is used to determine the concentration of another solution is called A. distillation B. fermentation C. titration D. transmutation
59. Which list of nuclear emissions is arranged in order from the greatest penetrating power to the least penetrating power? A. alpha particle, beta particle, gamma ray B. alpha particle, gamma ray, beta particle C. gamma ray, alpha particle, beta particle D. gamma ray, beta particle, alpha particle
60. Which electron shell contains the valence electrons of a radium atom in the ground state? A. the sixth shell B. the second shell C. the seventh shell D. the eighteenth shell
61. Which list of symbols represents nonmetals, only? A. B, Al, Ga B. Li, Be, B C. C, Si, Ge D. P, S, Cl
62. In the formula XSO4, the symbol X could represent the element A. Al B. Ar C. Mg D. Na
63. What is the chemical formula for lead(IV) oxide? A. PbO2 B. PbO4 C. Pb2O D. Pb4O
64. Which statement describes the general trends in electronegativity and atomic radius as the elements in Period 2 are considered in order from left to right? A. Both electronegativity and atomic radius increase. B. Both electronegativity and atomic radius decrease. C. Electronegativity increases and atomic radius decreases. D. Electronegativity decreases and atomic radius increases.
65. What is the percent composition by mass of nitrogen in (NH4)2CO3 (gram-formula mass = 96.0 g/mol)? A. 14.6% B. 29.2% C. 58.4% D. 87.5%
66. Given the balanced equation 2KI + F2 → 2KF + I2, which type of chemical reaction does this equation represent? A. synthesis B. decomposition C. single replacement D. double replacement
67. Given the balanced equation representing a reaction: 2H2O + energy → 2H2 + O2. Which statement describes the changes in energy and bonding for the reactant? A. Energy is absorbed as bonds in H2O are formed. B. Energy is absorbed as bonds in H2O are broken. C. Energy is released as bonds in H2O are formed. D. Energy is released as bonds in H2O are broken.
68. Which aqueous solution has the highest boiling point at standard pressure? A. 1.0 M KCl(aq) B. 1.0 M CaCl2(aq) C. 2.0 M KCl(aq) D. 2.0 M CaCl2(aq)
69. Given the equation representing a system at equilibrium: KNO3(s) + energy ⇌ K⁺(aq) + NO3⁻(aq). Which change causes the equilibrium to shift? A. increasing pressure B. increasing temperature C. adding a noble gas D. adding a catalyst
70. Which hydrocarbon is saturated? A. C2H2 B. C3H4 C. C4H6 D. C4H10
71. Which volume of 0.600 M H2SO4(aq) exactly neutralizes 100. milliliters of 0.300 M Ba(OH)2(aq)? A. 25.0 mL B. 50.0 mL C. 100. mL D. 200. mL
72. Which substance is an electrolyte? A. O2 B. Xe C. C3H8 D. KNO3
73. Which type of organic reaction produces both water and carbon dioxide? A. addition B. combustion C. esterification D. fermentation
74. Chlorine and element X have similar chemical properties. An atom of element X could have an electron configuration of A. 2-2 B. 2-8-1 C. 2-8-8 D. 2-8-18-7
75. Which group of elements contains a metalloid? A. Group 8 B. Group 2 C. Group 16 D. Group 18
76. In the formula for the compound XCl4, the X could represent A. C B. H C. Mg D. Zn
77. The formula C2H4 can be classified as A. a structural formula, only B. a molecular formula, only C. both a structural formula and an empirical formula D. both a molecular formula and an empirical formula
78. Given the balanced equation representing a reaction: 4Al(s) + 3O2(g) → 2Al2O3(s). How many moles of Al(s) react completely with 4.50 moles of O2(g) to produce 3.00 moles of Al2O3(s)? A. 1.50 mol B. 2.00 mol C. 6.00 mol D. 4.00 mol
79. What is the percent composition by mass of oxygen in Ca(NO3)2 (gram-formula mass = 164 g/mol)? A. 9.8% B. 29% C. 48% D. 59%
80. Given the balanced equation 6Li + N2 → 2Li3N, which type of chemical reaction is represented by this equation? A. synthesis B. decomposition C. single replacement D. double replacement
81. Which elements can react to produce a molecular compound? A. calcium and chlorine B. hydrogen and sulfur C. lithium and fluorine D. magnesium and oxygen
82. Compared to a 1.0-mole sample of NaCl(s), a 1.0-mole sample of NaCl(ℓ) has a different A. number of ions B. empirical formula C. gram-formula mass D. electrical conductivity
83. Which property of an unsaturated solution of sodium chloride in water remains the same when more water is added to the solution? A. density of the solution B. boiling point of the solution C. mass of sodium chloride in the solution D. percent by mass of water in the solution
84. Which ion combines with Ba²⁺ to form a compound that is most soluble in water? A. S²⁻ B. OH⁻ C. CO3²⁻ D. SO4²⁻
85. When a sample of gas is cooled in a sealed, rigid container, the pressure the gas exerts on the walls of the container will decrease because the gas particles hit the walls of the container A. less often and with less force B. less often and with more force C. more often and with less force D. more often and with more force
86. A rigid cylinder with a movable piston contains 50.0 liters of a gas at 30.0°C with a pressure of 1.00 atmosphere. What is the volume of the gas in the cylinder at STP? A. 5.49 L B. 45.0 L C. 55.5 L D. 455 L

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