Sample Questions for Chapter 3 : Stoker correct

Transcription

Sample Questions for Chapter 3 : Stoker
1. Which of the following statements concerning subatomic particles is correct?
A) Four fundamental types exist, all of which are charged.
B) Four fundamental types exist, two of which are charged.
C) Three fundamental types exist, none of which are charged.
D) Three fundamental types exist, two of which are charged.
2. Which of the following statements correctly characterizes the subatomic particle called
a neutron?
A) its mass is less than that of an electron
B) its charge is twice that of a proton
C) it is found in the nucleus
D) it contributes 75% of the mass of an atom
3. The nucleus of an atom
A) contains only protons
B) has no charge because of the presence of neutrons
C) attracts the neutral neutrons in an atom
D) is positively charged overall because of the presence of protons
4. Atoms are neutral because
A) all atoms contain neutrons.
B) all subatomic particles lose their charges once they enter an atom.
C) equal numbers of protons and electrons are present.
D) the number of subatomic particles in the nucleus is always an even number.
5. An atom contains 46 protons, 48 neutrons and 46 electrons. The atomic number and
mass number for this atom are, respectively,
A) 48 and 46
B) 46 and 48
C) 46 and 94
D) 48 and 94
6. Which of the following statements is correct for 27
14 Si ?
A) contains more electrons than neutrons
B) contains more electrons than protons
C) contains an equal number of protons and neutrons
D) contains more electrons than protons
Page 1
7. The quantity "A + Z" gives the number of
A) protons in an atom
B) electrons in an atomic nucleus
C) nuclear particles in an atomic nucleus
D) possible subatomic particles in an atom
8. Isotopes of a given element
A) have the same mass number but different numbers of protons.
B) have different mass numbers but identical numbers of protons.
C) have the same atomic number but different chemical properties.
D) have the same mass number but different chemical properties.
9. Chlorine, which exists in nature in two isotopic forms, has an atomic mass of 35.5 amu.
This means that
A) most chlorine atoms have a mass greater than 35.5 amu
B) more than half of all chlorine atoms have masses of 35.5
C) 35.5 amu is the upper limit for the mass of a chlorine atom
D) the mass of one isotope must be lighter than 35.5 amu while the mass of the other
isotope is heavier than 35.5 amu
10. Two naturally occurring isotopes exist for the hypothetical element dippium. 25.0% of
dippium atoms have a relative mass of 19.0 amu and 75.0% a relative mass of 23.8 amu.
What is the atomic mass of dippium?
A) 21.4 amu
B) 25.6 amu
C) 22.6 amu
D) 42.8 amu
11. The modern periodic table arranges the elements in order of
A) year of discovery.
B) decreasing size of the nucleus.
C) increasing reactivity with oxygen.
D) increasing number of protons.
12. In which of the following pairs of elements are both members of the pair in the same
period in the periodic table?
A) Ne and Mg
B) Cu and Ag
C) K and Se
D) Na and K
Page 2
13. In which of the following pairs of elements are both members of the pair metals?
A) Sb and S
B) In and I
C) Ti and Kr
D) Ni and Bi
14. The correct electron configuration for 17Cl is
A) 1s22s22p5.
B) 1s22s22p63s2.
C) 1s22s22p63s23p5.
D) 1s22s22p63s23p64s23d5.
15. Which of the following statements is consistent with the electron configuration
1s22s22p63s23p6?
A) there are 12 electrons present in a p orbital
B) there are 6 electrons present in a 2p subshell
C) there are 2 electrons present in a 2s shell
D) there are 6 electrons present in the third shell
16. After the 4s subshell of an atom is filled with electrons, the next electron added will
enter the
A) 3d subshell
B) 4p subshell
C) 4d subshell
D) 5s subshell
17. How many unpaired electrons are present in the orbital diagram for an atom whose
electron configuration is 1s22s22p4?
A) 0
B) 1
C) 2
D) 4
18. Which of the following statements about a d subshell is correct?
A) it contains 5 obitals
B) it contains 3 orbitals
C) it is found only in shells 4 and 5
D) it is found in all shells greater than 1
Page 3
19. The elements in group IVA of the periodic table all have electron configurations ending
in
A) p2.
B) p4.
C) d4.
D) s2.
20. Which of the following element-classification pairings is incorrect?
A) C - representative element
B) Rn - noble gas element
C) Cr - transition element
D) Ta - inner-transition element
21. Which of the following statements correctly describes the subatomic particle called a
neutron?
A) has a mass slightly less than that of a proton
B) is not found in the nucleus
C) has a positive charge
D) more than one correct response
E) no correct response
22. Which of the following statements concerning the nucleus of an atom is correct?
A) It accounts for almost all of the mass of an atom.
B) It is always positively charged.
C) It contains only neutrons.
23. Which of the following collections of subatomic particles possesses a net charge of +2?
A) two neutrons and two electrons
B) three protons and one electron
C) three electrons and one proton
Page 4
27
24. Which of the following statements is correct for 14 Si?
A) atomic number = 27 and mass number = 14
B) contains 14 protons and 27 neutrons
C) contains an equal number of protons and electrons
25. Tin is element number 50. This means that all tin atoms have
A) an atomic number of 50.
B) 50 neutrons in the nucleus.
C) a total of 50 subatomic particles in the nucleus.
26. Which of the following pairs of atoms, specified in terms of subatomic particle
composition, are isotopes?
A) (24p, 24e, 24n) and (25p, 25e, 25n)
B) (24p, 24e, 24n) and (24p, 24e, 28n)
C) (24p, 24e, 28n) and (25p, 25e, 28n)
27. Element A exists in three isotopic forms with masses of 21.0, 25.0 and 26.0 amu,
respectively. Element Q also exists in three isotopic forms with masses of 20, 24.0 and
25.0 amu, respectively. It is true that
A) element A has a lower atomic mass than element Q since it has the lightest isotope.
B) elements A and Q have identical atomic masses since the sums of their isotopic
masses are equal.
C) element Q has a higher atomic mass than element A since its atomic masses are
closer together.
28. Period number and group number in the periodic table are numerically equal for which
of the following elements?
A) 13Al
B) 33As
C) 51Sb
Page 5
29. Which of the following periodic table groups contains three or more nonmetallic
elements?
A) IIIA
B) IVA
C) VA
30. Both a number and a letter are used in designating an electron subshell. The letter
A) indicates the shell to which the subshell belongs.
B) may be s, p, d, or f.
C) gives information about the maximum number of electrons the subshell can contain.
31. Which of the following electron configurations corresponds to an element in the same
group of the periodic table as the element whose electron configuration is 1s22s22p5?
A) 1s22s22p4
B) 1s22s22p6
C) 1s22s22p63s23p64s23d5
32. Two unpaired electrons are present in the orbital diagram of which of the following
elements?
A) 6C
B) 10Ne
C) 12Mg
33. Which of the following characterizations for the element 23V is correct?
A) a period 4 element
B) electron configuration ends in d3
C) an inner-transition element
Page 6
34. Which of the following characterizations for the element 52Te is correct?
A) both a representative element and a metal
B) electron configuration involves a partially filled s subshell
C) electron configuration involves a total of 52 electrons
35. Which of the following statements concerning types of elements is correct?
A) There are more noble gas elements than transition elements.
B) There are more s-block elements than d-block elements.
C) There are more nonmetals than metals.
Use the following to answer questions 36-45:
In each of the following multiple-choice questions, characterize EACH of the three given
statements as being TRUE or FALSE and then indicate the collective true-false status of the
statements using the choices
a) All three statements are true.
b) Two of the three statements are true.
c) Only one of the statements is true.
d) None of the statements is true.
36. Statements:
(1) The number of elements that are metals and nonmetals is approximately equal.
(2) The number of orbitals present in an electron subshell is always six.
(3) An atom as a whole is electrically neutral because all charged subatomic particles
reside in the nucleus.
A) All three statements are true.
B) Two of the three statements are true.
C) Only one of the statements is true.
D) None of the statements is true.
Page 7
37. Statements:
(1) The shape of an s orbital is always spherical.
(2) All naturally occurring atoms of an element must be identical to each other in terms
of subatomic particle makeup.
(3) The alkaline earth metals are the elements in group IA of the periodic table.
38. Statements:
(1) The mass of an atom and the mass of its nucleus are essentially the same.
(2) Two of the six electrons present in an atom of carbon are unpaired.
(3) The element aluminum is located in the d area of the periodic table.
39. Statements:
(1) The sum of the mass number and the atomic number for an atom corresponds to the
total number of subatomic particles present in the atom.
(2) The element sulfur is both a nonmetal and a representative element.
(3) Elements with electron configurations that end in p4 would be found in group VIA of
the periodic table.
40. Statements:
(1) Electrons occupy the orbitals of a subshell such that each orbital acquires one
electron before any orbital acquires a second electron.
(2) The nucleus of an atom is always positively charged.
(3) Both electrons and protons are massive particles when compared with neutrons.
Page 8
41. Statements:
(1) The maximum number of electrons that can occupy an electron shell is the same as
the shell number.
(2) A nucleus is the very small dense uncharged center of an atom.
(3) The number of inner transition elements is greater than the number of transition
elements.
42. Statements:
(1) Most of the mass of an atom is concentrated in its nucleus.
(2) Sufficient information is present on a “standard” periodic table to determine the
number of neutrons present in atoms of an element.
(3) An atom whose electron configuration is 1s22s22p63s1 contains twelve electrons.
43. Statements:
(1) All naturally occurring atoms of an element must have the same mass number.
(2) Protons and electrons carry the same amount of charge.
(3) An isotope of chlorine with A = 35 and Z = 17 contains more neutrons than protons.
44. Statements:
(1) An electron configuration specifies subshell occupancy for electrons.
(2) The atomic number is double the mass number for atoms that contain an equal
number of protons and neutrons.
(3) All occupied orbitals are completely filled in atoms of the element neon, which
contains a total of 12 electrons.
Page 9
45. Statements:
(1) An atom is in an excited state when one or more of its electrons is in higher energy,
normally unoccupied orbitals.
(2) Most, but not all, of the trace elements needed for the proper functioning of the
human body are metals.
(3) Deuterium is an isotope of hydrogen in which two protons are present.
For each characterization, choose the correct atom from the response. Responses on the right
may be used more than once or need not be used at all.
a)
b)
c)
d)
25
12 Mg
40
20 Ca
17
9F
37
17 Cl
46. Has an atomic number of 17
47. Has a mass number of 17
48. Has a nuclear charge of +17
49. Has an equal number of protons, neutrons, and electrons
50. Has fewer neutrons than electrons
Page 10
For each characterization, choose an appropriate pair of atoms from the response. Responses on
the right may be used more than once or need not be used at all.
a)
b)
c)
d)
13
13
6 C and 7 N
37
36
17 Cl and 18 Ar
18
19
8 O and 9 F
6
7
3 Li and 3 Li
51. Atoms that contain the same number of protons
52. Atoms that contain the same number of electrons
53. Atoms that contain the same number of neutrons
54. Atoms that contain the same number of nucleons
55. Atoms that contain the same number of subatomic particles
For each characterization, choose an appropriate electron configuration from the response.
Responses on the right may be used more than once or need not be used at all.
a) 1s22s22p63s23p6
b) 1s22s22p63s23p4
c) 1s22s22p63s1
d) 1s22s22p5
56. Element that has five completely filled subshells
57. Element whose third shell contains six electrons
58. Element that has electrons in six orbitals
59. Element that has two unpaired electrons
Page 11
60. Element with no unpaired electrons
For each characterization, choose an appropriate pair of elements from the response. Responses
on the right may be used more than once or need not be used at all.
a) 37Rb and 38Sr
b) 7N and 82Pb
c) 9F and 17Cl
d) 42Mo and 75Re
61. Elements are in the same period of the periodic table.
62. Elements are in the same group of the periodic table.
63. Elements have similar chemical properties.
64. Elements are in the d area of the periodic table.
65. Elements have electron configurations ending in p5.
For each characterization, choose an appropriate element from the response. Responses on the
right may be used more than once or need not be used at all.
a) 9F
b) 50Sn
c) 79Au
d) 92U
66. A transition element
67. An inner-transition element
68. A halogen
69. Both a metal and a representative element
Page 12
70. Both a nonmetal and a representative element
Page 13
Answer Key
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
41.
42.
43.
44.
D
C
D
C
C
A
D
B
D
C
D
C
D
C
B
A
C
A
A
D
E
D
B
C
A
B
E
D
C
D
E
A
D
C
E
D
C
B
A
B
D
C
B
C
Page 14
45.
46.
47.
48.
49.
50.
51.
52.
53.
54.
55.
56.
57.
58.
59.
60.
61.
62.
63.
64.
65.
66.
67.
68.
69.
70.
B
d
c
d
b
c
d
d
c
a
b
a
b
c
b
a
a
c
c
d
c
c
d
a
b
a
Page 15

Sample Questions for Chapter 3 : Stoker correct

Transcription

Similar documents