Download 1. The first scientist to show that atoms emit any negative particles

1.
The first scientist to show that atoms emit any negative particles was
a) J. J. Thomson
b) Lord Kelvin
c) Ernest Rutherford
d) William Thomson
e) John Dalton
2.
The scientist whose alpha-particle scattering experiment led him to conclude that the nucleus of an atom
contains a dense center of positive charge is
a) J. J. Thomson
b) Lord Kelvin
c) Ernest Rutherford
d) William Thomson
e) John Dalton
3.
Which one of the following statements about atomic structure is false?
a) An atom is mostly empty space.
b) Almost all of the mass of the atom is concentrated in the nucleus.
c) The protons and neutrons in the nucleus are very tightly packed.
d) The number of protons and neutrons is always the same in the neutral atom.
e) All of the above statements (A-D) are true.
4.
Which of the following atomic symbols is incorrect?
14
a)
6C
37
b)
17 Cl
32
c)
15 P
39
d)
19 K
14
e)
8N
5.
Which of the following statements is true?
a) Ions are formed by adding or removing protons or electrons.
b) Scientists believe that solids are mostly open space.
c) Heating water with a Bunsen burner results in a 2:1 mixture of hydrogen and oxygen gases.
d) At least two of the above statements (A-C) are true.
e) All of the statements (A-C) are false.
6.
The formula of water, H2O, suggests:
a) There is twice as much mass of hydrogen as oxygen in each molecule.
b) There are two hydrogen atoms and one oxygen atom per water molecule.
c) There is twice as much mass of oxygen as hydrogen in each molecule.
d) There are two oxygen atoms and one hydrogen atom per water molecule.
e) None of these.
7.
All of the following are characteristics of nonmetals except:
a) poor conductors of electricity
b) often bond to each other by forming covalent bonds
c) tend to form negative ions in chemical reactions with metals
d) appear in the upper left-hand corner of the periodic table
e) do not have a shiny (lustrous) appearance
8.
How many protons and electrons does the most stable ion for magnesium have?
# protons # electrons
a)
10 p
12 e
b)
12 p
14 e
c)
14 p
12 e
d)
12 p
12 e
e)
12 p
10 e
9.
The correct name for Ca2+ is
a) calcium
b) calcium(II) ion
c) calcium ion
d) calcium(I) ion
e) monocalcium ion
10. Which form of electromagnetic radiation has the longest wavelengths?
a) gamma rays
b) microwaves
c) radio waves
d) infrared radiation
e) x-rays
11. In an investigation of the electronic absorption spectrum of a particular element, it is found that a photon
to the third. From this information, we can deduce
a) the energy of the n = 2 level
b) the energy of the n = 3 level
c) the sum of the energies of n = 2 and n = 3
d) the difference in energies between n = 2 and n = 3
e) all of these
12. What is the wavelength of light that is emitted when an excited electron in the hydrogen atom falls from
n = 5 to n = 1?
7
a)
m
–8
b)
m
–18
c)
m
–8
d)
m
e) none of these
13. How many d orbitals have n = 4?
a) 2
b) 5
c) 10
d) 7
e) 18
14. Which of the following was not an elemental property usually predicted by Mendeleev for as-yetunknown elements?
a) electron configuration
b) atomic mass
c) density
d) boiling point
e) hydride formula
15. Of the following elements, which needs three electrons to complete its valence shell?
a) Ba
b) Ca
c) Si
d) P
e) Cl
16. Which of the following processes represents the ionization energy of bromine?
 Br+(g) + e–
a) Br(s) 
b)
c)
d)
e)
 Br+(g) + e–
Br(l) 
 Br+(g) + e–
Br(g) 
 Br+(s) + e–
Br(s) 
 Br2+(g) + e–
Br2(g) 
17. Order the elements S, Cl, and F in terms of increasing ionization energy.
a) S, Cl, F
b) Cl, F, S
c) F, S, Cl
d) F, Cl, S
e) S, F, Cl
18. Order the elements S, Cl, and F in terms of increasing atomic radii.
a) S, Cl, F
b) Cl, F, S
c) F, S, Cl
d) F, Cl, S
e) S, F, Cl
19. Which of the following atoms would have the largest second ionization energy?
a) Mg
b) Cl
c) S
d) Ca
e) Na
20. The first ionization energy of Mg is 735 kJ/mol. The second ionization energy is
a) 735 kJ/mol
b) less than 735 kJ/mol
c) greater than 735 kJ/mol
d) More information is needed to answer this question.
e) None of these.
21. Which of the following concerning second ionization energies is true?
a) That of Al is higher than that of Mg because Mg wants to lose the second electron, so it is easier to
take the second electron away.
b) That of Al is higher than that of Mg because the electrons are taken from the same energy level,
but the Al atom has one more proton.
c) That of Al is lower than that of Mg because Mg wants to lose the second electron, thus the energy
change is greater.
d) That of Al is lower than that of Mg because the second electron taken from Al is in a p orbital, thus
it is easier to take.
e) The second ionization energies are equal for Al and Mg.
22. Consider the following orderings.
+
2+
3+
I.
II.
III.
Na < Mg < Al < Si
Be < Mg < Ca < Sr
I < Br < Cl < F
IV.
Al < Si < P < Cl
4+
Which of these give(s) a correct trend in ionization energy?
a)
b)
c)
d)
e)
III
II, IV
I, IV
I, III, IV
none of them
23. Of the following elements, which is most likely to form a negative ion with charge 1–?
a) Ba
b) Ca
c) Si
d) P
e) Cl
24. Which of the following atoms has the largest ionization energy?
a) O
b) Li
c) Ne
d) Be
e) K
25. Which of the following statements is true?
a) The first ionization potential of H is greater than that of He.
b) The ionic radius of Fe+ is larger than that of Fe3+.
c) The ionization energy of S2– is greater than that of Cl–.
d) The atomic radius of Li is larger than that of Cs.
e) All are false.
26. Which of the following statements are false?
I. It takes less energy to add an electron to nitrogen than to carbon because nitrogen
will be closer to achieving a noble gas configuration.
II. It takes more energy to add an electron to fluorine than to oxygen because the radius
of fluorine is smaller and more repulsion would occur in the p-orbitals.
III. It takes more energy to add an electron to nitrogen than to carbon because of the
extra repulsions that would occur in the 2p orbitals.
IV. Less energy is released in adding an electron to iodine than to chlorine because
the radius of iodine is larger and the electron is added at a distance further
from the nucleus.
a)
b)
c)
d)
e)
II, III
I, II, IV
III only
I, II
All of the above are false statements.
27. T
F The second ionization energy for calcium is smaller than the first ionization energy.
28. T
F When a metal reacts with a nonmetal a covalent bond is formed.
29. For the elements Cs, F, and P, the order of increasing electronegativity is:
a) Cs < F < P
b) Cs < P < F
c) P < F < Cs
d) F < Cs < P
e) none of these
30. Metals typically have _______ electronegativity values.
a) high
b) low
c) negative
d) no
e) two of these
31. Which of the following has the smallest radius?
a) Br–
b) S2–
c) Xe
d) Ca2+
e) Kr
32. Which of these is an isoelectronic series?
a) Na+, K+, Rb+, Cs+
b) K+, Ca2+, Ar, S2–
c) Na+, Mg2+, S2–, Cl–
d) Li, Be, B, C
e) none of these (A-D)
33. Which of the following has the smallest radius?
a) K+
b) Cl–
c) Rb+
d) S2–
e) Ar
34. Which of the following has the smallest radius?
a) F–
b) Ne
c) O2–
d) Mg2+
e) Na+
35. Which of the following pairs is isoelectronic?
a) Li+ and K+
b) Na+ and Ne
c) I– and Cl–
d) S2– and Ne
e) Al3+ and B3+
36. Which of the following arrangements is in order of increasing size?
a) Ga3+ > Ca2+ > K+ > Cl– > S2–
b) S2– > Cl– > K+ > Ca2+ > Ga3+
c) Ga3+ > S2– > Ca2+ > Cl– > K+
d) Ga3+ > Ca2+ > S2– > Cl– > K+
e)
37. T
Ga3+ > Ca2+ > S2– > K+ > Cl–
F The size in a series of isoelectronic ions increases as the nuclear charge increases.
38. The first electron affinity value for oxygen is _______ and the second electron affinity value is
________.
a) unfavorable (endothermic), favorable (exothermic)
b) unfavorable (endothermic), unfavorable (endothermic)
c) favorable (exothermic), favorable (exothermic)
d) favorable (exothermic), unfavorable (endothermic)
e) More information is needed.
39. In the reaction between magnesium and sulfur, the magnesium atoms
a) become anions
b) become cations
c) become part of polyatomic ions
d) share electrons with sulfur
e) crystallize
40.
The effective nuclear charge experienced by the outermost electron of Na is different than the
effective nuclear charge experienced by the outermost electron of Ne. This difference best accounts
for which of the following?
(A) Na has a greater density at standard conditions than Ne.
(B) Na has a lower first ionization energy than Ne.
(C) Na has a higher melting point than Ne.
(D) Na has a higher neutron-to-proton ratio than Ne.
(E) Na has fewer naturally occurring isotopes than Ne.
Consider atoms of the following elements. Assume that the atoms are in the ground state
(A) S
(B) Ca
(C) Ga
(D) Sb
(E) Br
41.
The atom that contains exactly two unpaired electrons.
42.
The atom that contains only one electron in the highest occupied energy sublevel.
43.
In which of the following groups are the three species isoelectronic; i.e., have the same number of
electrons?
(A) S2–, K+, Ca2+
(B) Sc, Ti, V2+
(C) O2–, S2–, Cl–
(D) Mg2+, Ca2+ Sr2+
(E) Cs, Ba2+, La3+
44.
Which of the following properties generally decreases across the periodic table from sodium to
chlorine?
(A) First ionization energyAtomic Theory and Periodicity
(B) Atomic mass
(C) Electronegativity
(D) Maximum value of oxidation number
(E) Atomic radius
45.
Chose Answer C
____ 46. Of the elements Fe, Hg, U, and Te, which is a representative element?
a. Fe
c. U
b. Hg
d. Te
____ 47. Which of the following factors contributes to the increase in atomic size within a group in the periodic table
as the atomic number increases?
a. more shielding of the electrons by the highest occupied energy level
b. an increase in size of the nucleus
c. an increase in number of protons
d. fewer electrons in the highest occupied energy level
____ 48. Which of the following elements has the smallest atomic radius?
a. sulfur
c. selenium
b. chlorine
d. bromine
____ 49. In which of the following sets are the charges given correctly for all the ions?
a. Na , Mg , Al
b. K , Sr , O
c. Rb , Ba , P
d. N , O , F
____ 50. In which of the following groups of ions are the charges all shown correctly?
a. Li , O , S
c. K , F , Mg
b. Ca , Al , Br
d. Na , I , Rb
____ 51. Which of the following factors contributes to the increase in ionization energy from left to right across a
period?
a. an increase in the shielding effect
b. an increase in the size of the nucleus
c. an increase in the number of protons
d. fewer electrons in the highest occupied energy level
____ 52. As you move from left to right across the second period of the periodic table ____.
a. ionization energy increases
c. electronegativity decreases
b. atomic radii increase
d. atomic mass decreases
____ 53. Of the following elements, which one has the smallest first ionization energy?
a. boron
c. aluminum
b. carbon
d. silicon
____ 54. Of the elements Pt, V, Li, and Kr, which is a nonmetal?
a. Pt
c. Li
b. V
d. Kr
____ 55. The atomic number of an element is the total number of which particles in the nucleus?
a. neutrons
c. electrons
b. protons
d. protons and electrons
____ 56. What element has the electron configuration 1s 2s 2p 3s 3p ?
a. nitrogen
c. silicon
b. selenium
d. silver
____ 57. Which of the following is true about the electron configurations of the noble gases?
a. The highest occupied s and p sublevels are completely filled.
b. The highest occupied s and p sublevels are partially filled.
c. The electrons with the highest energy are in a d sublevel.
d. The electrons with the highest energy are in an f sublevel.
____ 58. Which of the following electron configurations is most likely to result in an element that is relatively
inactive?
a. a half-filled energy sublevel
b. a filled energy sublevel
c. one empty and one filled energy sublevel
d. a filled highest occupied principal energy level
____ 59. Which subatomic particle plays the greatest part in determining the properties of an element?
a. proton
c. neutron
b. electron
d. none of the above
____ 60. Which of the following is true about the electron configurations of the representative elements?
a. The highest occupied s and p sublevels are completely filled.
b. The highest occupied s and p sublevels are partially filled.
c. The electrons with the highest energy are in a d sublevel.
d. The electrons with the highest energy are in an f sublevel.
____ 61. What are the Group 1A and Group 7A elements examples of?
a. representative elements
c. noble gases
b. transition elements
d. nonmetallic elements
____ 62. 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.
____ 63. What causes the shielding effect to remain constant across a period?
a. Electrons are added to the same principal energy level.
b. Electrons are added to different principal energy levels.
c. The charge on the nucleus is constant.
d. The atomic radius increases.
____ 64. Atomic size generally ____.
a. increases as you move from left to right across a period
b. decreases as you move from top to bottom within a group
c. remains constant within a period
d. decreases as you move from left to right across a period
____ 65. What element in the second period has the largest atomic radius?
a. carbon
c. potassium
b. lithium
d. neon
____ 66. Which of the following statements is true about ions?
a. Cations form when an atom gains electrons.
b. Cations form when an atom loses electrons.
c. Anions form when an atom gains protons.
d. Anions form when an atom loses protons.
____ 67. The metals in Groups 1A, 2A, and 3A ____.
a. gain electrons when they form ions
b. all form ions with a negative charge
c. all have ions with a 1 charge
d. lose electrons when they form ions
____ 68. Which of the following statements is NOT true about ions?
a. Cations are positively charged ions.
b. Anions are common among nonmetals.
c. Charges for ions are written as numbers followed by a plus or minus sign.
d. When a cation forms, more electrons are transferred to it.
____ 69. Why is the second ionization energy greater than the first ionization energy?
a. It is more difficult to remove a second electron from an atom.
b. The size of atoms increases down a group.
c. The size of anions decreases across a period.
d. The nuclear attraction from protons in the nucleus decreases.
____ 70. Which of the following elements has the smallest ionic radius?
a. Li
c. O
b. K
d. S
____ 71. 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
____ 72. For Group 2A metals, which electron is the most difficult to remove?
a. the first
b. the second
c. the third
d. All the electrons are equally difficult to remove.
____ 73. Which of the following factors contributes to the decrease in ionization energy within a group in the periodic
table as the atomic number increases?
a. increase in atomic size
b. increase in size of the nucleus
c. increase in number of protons
d. fewer electrons in the highest occupied energy level
____ 74. Which of the following elements has the smallest first ionization energy?
a. sodium
c. potassium
b. calcium
d. magnesium
____ 75. Which of the following elements has the lowest electronegativity?
a. lithium
c. bromine
b. carbon
d. fluorine
____ 76. Which statement is true about electronegativity?
a. Electronegativity is the ability of an anion to attract another anion.
b. Electronegativity generally increases as you move from top to bottom within a group.
c. Electronegativity generally is higher for metals than for nonmetals.
d. Electronegativity generally increases from left to right across a period.
____ 77. Which of the following decreases with increasing atomic number in Group 2A?
a. shielding effect
c. ionization energy
b. ionic size
d. number of electrons
____ 78. Which of the following statements correctly compares the relative size of an ion to its neutral atom?
a. The radius of an anion is greater than the radius of its neutral atom.
b. The radius of an anion is identical to the radius of its neutral atom.
c. The radius of a cation is greater than the radius of its neutral atom.
d. The radius of a cation is identical to the radius of its neutral atom.
____ 79. What is another name for the representative elements?
a. Group A elements
c. Group C elements
b. Group B elements
d. transition elements
____ 80. What is another name for the transition metals?
a. noble gases
c. Group B elements
b. Group A elements
d. Group C elements
____ 81. Which of the following elements is in the same period as phosphorus?
a. carbon
c. nitrogen
b. magnesium
d. oxygen
____ 82. Who arranged the elements according to atomic mass and used the arrangement to predict the properties of
missing elements?
a. Henry Moseley
c. John Dalton
b. Antoine Lavoisier
d. Dmitri Mendeleev
____ 83. Which of the following categories includes the majority of the elements?
a. metalloids
c. metals
b. liquids
d. nonmetals
____ 84. In which of the following sets is the symbol of the element, the number of protons, and the number of
electrons given correctly?
a. In, 49 protons, 49 electrons
c. Cs, 55 protons, 132.9 electrons
b. Zn, 30 protons, 60 electrons
d. F, 19 protons, 19 electrons
____ 85. Which of the following elements is a transition metal?
a. cesium
c. tellurium
b. copper
d. tin
____ 86. Which of the following groupings contains only representative elements?
a. Cu, Co, Cd
c. Al, Mg, Li
b. Ni, Fe, Zn
d. Hg, Cr, Ag
____ 87. 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.
____ 88. What is the charge of a cation?
a. a positive charge
b. no charge
c. a negative charge
d. The charge depends on the size of the nucleus.
____ 89. What is the element with the lowest electronegativity value?
a. cesium
c. calcium
b. helium
d. fluorine
____ 90. What is the element with the highest electronegativity value?
a. cesium
c. calcium
b. helium
d. fluorine
91. T F A nonpolar covalent bond results from the unequal sharing of a pair of electrons between
atoms in a molecule.
92. Match the ions below with the pictures that represent their relative sizes. Justify your answers.
Ions:
Se2–
K+
Ga3+
Br–
Ca2+
93. The ability of an atom in a molecule to attract shared electrons to itself is called __________.
94. Larger atomic radius, Fe2+ or Fe3+
95. In general, the ionization energy and electron affinity involve more energy from __________ (left to
right or right to left) in a period of the periodic table. Why?
96. In general, the ionization energy and electron affinity involve more energy from _________ (top to
bottom or bottom to top) in a family of the periodic table. Why?
96. For the set of elements Be, B, C, and N, which element has the smallest ionization energy? Explain
any deviation from the expected pattern.