A) atomic mass B) atomic number C) molar mass D) oxidation number
1. The elements on the Periodic Table are arranged in order of increasing
A) Li, Na, Rb B) Cr, Mo, W C) Sn, Si, C D) O, S, Te
2. Which list of elements consists of a metal, a metalloid, and a nonmetal?
A) Br, Ga, Hg B) Cr, Pb, Xe C) O, S, Se D) N, O, F
3. Which list includes elements with the most similar chemical properties?
A) Ba B) Cd C) In D) Na
4. If an element, X, can form an oxide that has the formula X2O3, then element X would most likely be located on the Periodic Table in the same group as
A) tungsten B) antimony
C) krypton D) methane
5. Which substance can be decomposed by chemical means?
A) 1 B) 2 C) 15 D) 16
6. Element X is a solid that is brittle, lacks luster,and has six valence electrons. In which group on the Periodic Table would element X be found?
A) hydrogen B) calcium
C) sodium D) zinc
7. Which element is an alkali metal?
A) calcium B) cesium
C) potassium D) sodium
8. Which element has properties most like those of magnesium?
A) upper right corner B) lower right corner C) upper left corner D) lower left corner 9. In which section of the Periodic Table are the most
active metals located?
A) H B) He C) S D) Sn
10. A sample of an element is malleable and can conduct electricity. This element could be
A) the solid phase, only B) the liquid phase, only
C) both the solid and the liquid phase D) neither the solid nor the liquid phase 11. Metallic substances will conduct electricity in
A) S B) Si C) Ge D) Au
12. Which element is malleable and ductile?
A) metal B) metalloid
C) nonmetal D) noble gas
13. An element that has a low first ionization energy and good conductivity of heat and electricity is classified as a
A) iodine B) phosphorus
C) sulfur D) tin
14. Which element is malleable and can conduct electricity in the solid phase?
A) nitrogen B) phosphorus
C) antimony D) bismuth
15. Which of the following Group 15 elements has the greatest metallic character?
A) Group 1 metal B) Group 2 metal C) Group 1 nonmetal D) Group 2 nonmetal 16. In the formula XF2, the element represented by X can
be classified as a
A) low electrical conductivity B) high heat conductivity C) existence as brittle solids D) existence as molecular solids
17. Which property is generally characteristic of metallic elements?
A) They tend to gain electrons easily when bonding.
B) They tend to lose electrons easily when bonding.
C) They are poor conductors of heat.
D) They are poor conductors of electricity.
18. What is a property of most metals?
A) methane B) propanal
C) tungsten D) water
19. Which substance can not be broken down by a chemical change?
A) S B) N C) Br D) Ni
20. Which of these elements is the best conductor of electricity?
A) carbon B) germanium
C) silicon D) tin
21. Which Group 14 element is classified as a metal?
A) low first ionization energy and low electronegativity
B) low first ionization energy and high electronegativity
C) high first ionization energy and low electronegativity
D) high first ionization energy and high electronegativity
22. Which two characteristics are associated with metals?
A) Si, As, and Te B) N2, O2, and F2
C) Mg, Sr, and Ba D) Ca, Cs, and Cu 23. Which elements have the most similar chemical
properties?
A) silver B) mercury
C) barium D) bromine
24. Which element is a liquid at STP and has low electrical conductivity?
A) the same molecular structures and the same properties
B) the same molecular structures and different properties
C) different molecular structures and the same properties
D) different molecular structures and different properties
25. Which phrase describes the molecular structure and properties of two solid forms of carbon, diamond and graphite?
A) B)
C) D)
26. Which particle diagram represents the arrangement of F
2 molecules in a sample of fluorine at 95 K and standard pressure?
A) boron and carbon B) oxygen and sulfur C) aluminum and bromine D) argon and silicon
27. Which elements have the most similar chemical properties?
A) Cu B) S C) Mg D) Fe
28. Which element at STP is a poor conductor of electricity and has a relatively high electronegativity?
A) 15 B) 16 C) 17 D) 18
29. Which group in the Periodic Table contains elements that are all monatomic gases at STP?
A) N B) O C) Cl D) Ne
30. Which element at STP exists as monatomic molecules?
A) W B) Ar C) N D) Er
31. Which element is a noble gas?
A) B B) Ba C) K D) Kr
32. Which element exhibits both metallic and nonmetallic properties?
A) 24Mg and 12 protons B) 28Si and 14 protons C) 75As and 75 protons D) 80Br and 80 protons
33. Which isotopic notation identifies a metalloid that is matched with the corresponding number of protons in each of its atoms?
A) metals, only B) nonmetals, only
C) both metals and nonmetals D) neither metals nor nonmetals
34. The element arsenic (As) has the properties of
A) C-12 and N-14 B) C-12 and N-16 C) C-14 and N-14 D) C-14 and N-16
35. According to Reference Table N, which pair of isotopes spontaneously decays?
A) Rn B) Xe C) Ag D) Kr
36. Given the particle diagram:
At 101.3 kPa and 298 K, which element could this diagram represent?
A) Br B) S C) Al D) Bi
37. Which element is a brittle, nonconducting solid at 25°C?
A) K B) I2 C) Hg D) Mg
38. Which element is a liquid at room temperature?
A) Ta B) Tc C) Te D) Ti
39. At STP, a 7.49-gram sample of an element has a volume of 1.65 cubic centimeters. The sample is most likely
A) Group 2 B) Group 6
C) Group 15 D) Group 17
40. Which group contains elements in three phases of matter at STP?
A) Po B) Te C) Se D) S
41. Which Group 16 element has only unstable isotopes?
A) They are formed from different elements.
B) They have different molecular structures.
C) They have different oxidation numbers.
D) They have different electronegativities.
42. Which statement explains why ozone gas, O3, and oxygen gas, O2, have different properties?
A) different molecular structures and identical properties
B) different molecular structures and different properties
C) identical molecular structures and identical properties
D) identical molecular structures and different properties
43. The two forms of oxygen, O2(g) and O3(g), have
A) aluminum B) magnesium
C) titanium D) zinc
44. A 10.0-gram sample of which element has the smallest volume at STP?
A) B)
C) D)
45. Which Lewis electron-dot diagram is correct for CO2?
A) B) C) D)
46. Which is the correct electron-dot symbol for an aluminum atom in the ground state?
A) B)
C) D)
47. Which Lewis electron-dot diagram is correct for a S2–
ion?
A) 1 B) 2 C) 3 D) 5
48. What is the total number of electrons in the outermost shell of a phosphorus atom in the ground state?
A) protons B) neutrons
C) valence electrons
D) occupied principal energy levels
49. The elements in Period 3 all contain the same number of
A) 8 B) 2 C) 3 D) 10
50. What is the total number of electrons in the valence shell of an atom of aluminum in the ground state?
A) They are the same because each has the same atomic number.
B) They are the same because each has the same electron configuration.
C) They are different because each has a different atomic number.
D) They are different because each has a different electron configuration.
51. How do the chemical properties of the Na atom and the Na+ ion compare?
A) mass
B) electronegativity C) total number of protons
D) total number of valence electrons
52. An atom of aluminum in the ground state and an atom of gallium in the ground state have the same
A) Fe B) Cu C) Cr D) Mg
53. Which element will lose only valence electrons every time its atoms enter into a chemical reaction?
A) K B) I C) Ag D) Mg
54. Which element would most likely be found uncombined in nature?
A) IA B) VIIA C) VIII D) O
55. A metallic element whose aqueous ions produce colorless solutions would be found in Period 4 and Group
A) Fe B) Mg C) Al D) Zn
56. Which element can form a chloride with a general formula of MCl2 or MCl3?
57. After a neutral sulfur atom gains two electrons, what is the resulting charge of the ion?
A) more protons B) fewer protons C) more electrons D) fewer electrons 58. Compared to a Be2+ ion, a Be0 atom has
A) The ion is positively charged and its radius is smaller than the radius of the atom.
B) The ion is positively charged and its radius is larger than the radius of the atom.
C) The ion is negatively charged and its radius is smaller than the radius of the atom.
D) The ion is negatively charged and its radius is larger than the radius of the atom.
59. An atom of an element has a total of 12 electrons. An ion of the same element has a total of 10 electrons.
Which statement describes the charge and radius of the ion?
A) an increase in radius and an increase in ionization energy
B) an increase in radius and a decrease ionization energy
C) a decrease in radius and an increase in ionization energy
D) a decrease in radius and a decrease in ionization energy
60. As the atoms in Period 3 of the Periodic Table are considered from left to right, the atoms generally show
A) decreases B) increases C) remains the same
61. Within Period 2 of the Periodic Table, as the atomic number increases, the atomic radius generally
A) The ion is smaller because it has fewer electrons.
B) The ion is smaller because it has more electrons.
C) The ion is larger because it has fewer electrons.
D) The ion is larger because it has more electrons.
62. How does the size of a barium ion compare to the size of a barium atom?
A) Ba2+ B) Ca2+ C) Mg2+ D) Sr2+
63. Which ion would have the smallest radius?
A) Na+ B) K+ C) Mg2+ D) Ca2+
64. Which of the following ions has the smallest radius?
A) have higher electronegativities B) have lower first ionization energies C) conduct electricity more readily D) lose electrons more readily
65. Compared to atoms of metals, atoms of nonmetals generally
A) Electronegativity increases, and first ionization energy decreases.
B) Electronegativity decreases, and first ionization energy increases.
C) Electronegativity and first ionization energy both increase.
D) Electronegativity and first ionization energy both decrease.
66. Which statement describes the general trends in electronegativity and first ionization energy as the elements in Period 3 are considered in order from Na to Cl?
A) 2372 kJ B) 2081 kJ
C) 1313 kJ D) 10 kJ
67. What is the first ionization energy of an element that has the electron configuration 2-8?
A) nuclear charge is decreasing B) number of neutrons is increasing
C) number of principal energy levels is decreasing D) distance between the valence electron and the
nucleus is increasing
68. As the Group 1 elements of the Periodic Table are considered from top to bottom, the first ionization energy of each successive element decreases. One reason for this is that the
A) Ge B) Ca C) Ga D) K
69. Which atom requires the least energy to form a positive ion?
A) nitrogen B) phosphorus
C) antimony D) bismuth
70. Which element in Group 15 has the greatest metallic character?
A) decreases B) increases C) remains the same
71. As the elements in Group 17 are considered in order of increasing atomic number, the chemical reactivity of each successive element
A) Mg B) H C) He D) Cl
72. Which element has the highest electrical conductivity?
A) compound B) element
C) mixture D) solution
73. Two solid samples each contain sulfur, oxygen, and sodium, only. These samples have the same color, melting point, density, and reaction with an aqueous barium chloride solution. It can be concluded that the two samples are the same
A) Co B) CO C) Cr D) Cu
74. Which substance can be decomposed by a chemical change?
A)
B)
C)
D)
75. Which diagram represents a physical change, only?
A) sodium B) argon
C) sulfur D) ammonia
76. Which substance can be decomposed by a chemical change?
A) N2 B) NH4+
C) Na D) NaHCO3
77. Which species represents a chemical compound?
A) 7 B) 9 C) 3 D) 4
78. What is the total number of different elements present
in ?
A) Na2SO3 B) Na2SO4
C) NaSO3 D) NaSO4
79. What is the chemical formula for sodium sulfate?
A) XO B) X2O C) XO2 D) X2O3
80. If X represents an element of Group 1, the formula of its oxide would be
A) 1 (IA) B) 2 (IIA)
C) 13 (IIIA) D) 14 (IVA)
81. Element X forms the compounds XCl3 and X2O3. In the Periodic Table, element X would most likely be found in Group
A) 1 B) 2 C) 13 D) 14
82. In which Group do the elements usually form oxides which have the general formula M2O3?
A) hydroxide B) oxalate
C) oxide D) peroxide
83. What is the name of the polyatomic ion in the compound Na2O2?
A) PbO B) Pb2O
C) PbO2 D) Pb2O2
84. The correct formula for lead (IV) oxide is
A) mercury B) ethanol
C) sodium D) ammonia
85. An example of a compound containing only two elements is
