Quizzes :Electronic Configuration of First Transition Series
Introduction
In this lesson, we delve into the electronic configuration of the first transition series, shedding light on general principles and key exceptions. Uncover the reasons behind the unique electron configurations of chromium and copper, and understand the stability factors associated with d sublevels. From the ordering of subshells to the impact of ion charges on electron distribution, this lesson provides a comprehensive exploration of the electronic intricacies of transition metals.
Quiz on Electronic Configuration of First Transition Series:
1-What is the general electron configuration for d-block elements?
a) ns1-2(n-1)d1-10
b) ns2(n-1)d1-10
c) ns1-2(nd)1-10
d) ns2(nd)1-10
2-What is the typical valence configuration for first series transition metals
(Groups 3 – 12)?
a) 3dn 4s1
b) 3dn 4s2
c) 3dn 4s3
d) 3dn 4s4
3-Which of the following statements about the exceptions in the electronic configurations of chromium and copper is true?
a) Chromium and copper have the same electron configuration.
b) The 3d5 4s1 configuration is of higher energy for both chromium and copper.
c) The 3d10 4s1 configuration is of lower energy for both chromium and copper.
d) The energy of 3d orbitals increases going across the row.
4-Why do chromium and copper exhibit exceptions in their electron configurations?
a) 3d and 4s orbitals have significantly different energies.
b) The energy of 3d orbitals drops across the row.
c) The 4s subshell is of higher energy than the 3d subshell.
d) The 3d5 4s1 configuration has the maximum number of unpaired electrons.
5-What is the relationship between the total number of valence electrons and the group number for transition metal atoms?
a) They are unrelated.
b) The total number of valence electrons equals the group number.
c) The total number of valence electrons is half of the group number.
d) The total number of valence electrons is double the group number.
6-For transition metal ions with a charge ≥ +2, how can you determine the number of d electrons?
a) Number of d electrons = group number.
b) Number of d electrons = total valence electrons + charge of the ion.
c) Number of d electrons = total valence electrons – charge of the ion.
d) Number of d electrons = charge of the ion.
7-Which of the following is a stable electronic configuration for a transition metal atom?
a) d5
b) d7
c) d12
d) d15
8-For the element with the electronic configuration [54Xe]6S2, 5d5, determine:
a) The transition series order.
b) The period number.
c) The column number.
9-What is the atomic number of Rhenium (Re) based on its electronic configuration?
a) 65
b) 70
c) 75
d) 80
10-For the electronic configuration of Vanadium, choose the correct answer:
The outer electron configuration of the first transition series is:
a) ns1-2
b) (n-1)d1-10
c) ns2(n-1)d1-10
d) (n-1)d1-10 ns1-2
11-What is the order of the third transition series based on the electronic configuration [54Xe]6S2, 5d5?
a) First transition series
b) Second transition series
c) Third transition series
d) Fourth transition series
12-In the electronic configuration [75]1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p6 4f14 5d5 6s2, identify the period number.
a) 4
b) 5
c) 6
d) 7
13-For the electronic configuration [75]1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p6 4f14 5d5 6s2, determine the column number of Rhenium (Re).
a) 5
b) 6
c) 7
d) 8
14-What is the value of ‘n’ in the outer electron configuration (n-1)d1-10 ns1-2?
a) 2
b) 3
c) 4
d) 5
15-Why does the 3d5 4s1 configuration have lower energy for chromium?
a) 3d and 4s orbitals have significantly different energies.
b) The energy of 3d orbitals increases going across the row.
c) The difference in 3d and 4s orbital energies is similar to the pairing energy.
d) The 4s subshell is of higher energy than the 3d subshell.
16-Which of the following statements is true regarding the stability of electronic configurations in the d sublevel?
a) A half-filled d sublevel (d5) is more stable.
b) A completely filled d sublevel (d10) is less stable.
c) An empty d sublevel (d0) is less stable.
d) All of the above.
17-What is the relationship between the electron configuration and stability for transition metal ions with a charge ≥ +2?
a) 3d is of higher energy than 4s.
b) 4s is of higher energy than 3d.
c) 3d is empty in transition metal ions.
d) 4s is empty in transition metal ions.
18-For Ni (Group 10), how many valence electrons does it have, and what is the electron configuration for Ni2+?
a) 8 valence electrons, d5
b) 10 valence electrons, d8
c) 10 valence electrons, d5
d) 8 valence electrons, d8
19-For Fe (Group 8), how many valence electrons does it have, and what is the electron configuration for Fe3+?
a) 8 valence electrons, d5
b) 10 valence electrons, d8
c) 8 valence electrons, d8
d) 10 valence electrons, d5
20-For Ti (Group 4), how many valence electrons does it have, and what is the electron configuration for Ti3+?
a) 4 valence electrons, d1
b) 6 valence electrons, d2
c) 4 valence electrons, d3
d) 6 valence electrons, d1
21-What is the significance of the exceptions in the electronic configurations of chromium and copper in relation to the energy levels of 3d and 4s orbitals?
a) 3d and 4s orbitals have significantly different energies.
b) The energy of 3d orbitals increases going across the row.
c) The energy of 4s orbitals drops going across the row.
d) 4s subshell is of higher energy than the 3d subshell.
22-Why does the 3d10 4s1 configuration have lower energy for copper?
a) The 3d orbitals are of lower energy than 4s orbitals.
b) The energy of 4s orbitals drops going across the row.
c) The difference in 3d and 4s orbital energies is similar to the pairing energy.
d) 3d orbitals are half-filled in the 3d10 4s1 configuration.
23-In the electronic configuration [54Xe]6S2, 5d5, what is the transition series order, period number, and column number?
a) First transition series, period 4, column 5
b) Second transition series, period 5, column 6
c) Third transition series, period 6, column 7
d) Fourth transition series, period 7, column 8
24-What is the atomic number of Vanadium (V) based on its electronic configuration?
a) 20
b) 23
c) 40
d) 50
25-Choose the correct statement about the electronic configuration of Vanadium:
a) ns1-2
b) (n-1)d1-10 ns1-2
c) ns2(n-1)d1-10
d) (n-1)d1-10 ns2
26-In the electronic configuration [75]1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p6 4f14 5d5 6s2, which subshell contains the valence electrons?
a) 4d
b) 5s
c) 5d
d) 6s
27-What is the significance of having a half-filled or completely filled d sublevel in terms of stability?
a) Half-filled d sublevel (d5) is more stable.
b) Completely filled d sublevel (d10) is more stable.
c) Both are equally stable.
d) Neither is stable.
28-In the electron configuration [54Xe]6S2, 5d5, which orbital contains the outermost electrons?
a) 5s
b) 5d
c) 6s
d) 6p
29-For the electronic configuration [75]1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p6 4f14 5d5 6s2, what is the period number?
a) 4
b) 5
c) 6
d) 7
30-What is the electron configuration of Ni2+?
a) 3d10
b) 3d8
c) 4s2
d) 4p6
31-For Fe3+, how many valence electrons are there, and what is its electron configuration?
a) 6 valence electrons, d2
b) 7 valence electrons, d6
c) 5 valence electrons, d5
d) 8 valence electrons, d5
32-In the electron configuration [54Xe]6S2, 5d5, what is the group number of the element?
a) 4
b) 5
c) 6
d) 7
33-For Ti3+, how many valence electrons are there, and what is its electron configuration?
a) 2 valence electrons, d1
b) 3 valence electrons, d2
c) 1 valence electron, d1
d) 4 valence electrons, d1
34-What is the significance of having a half-filled or completely filled d sublevel in terms of stability?
a) Half-filled d sublevel (d5) is more stable.
b) Completely filled d sublevel (d10) is more stable.
c) Both are equally stable.
d) Neither is stable.
35-For the electronic configuration
[75]1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p6 4f14 5d5 6s2, what is the atomic number of the element?
a) 75
b) 80
c) 85
d) 90
36-What is the electron configuration of chromium?
a) 3d6 4s2
b) 3d7 4s1
c) 3d5 4s2
d) 3d4 4s3
37-What is the electron configuration of copper?
a) 3d8 4s2
b) 3d9 4s1
c) 3d10 4s1
d) 3d7 4s2
38-In the electron configuration [54Xe]6S2, 5d5, which subshell has the maximum number of electrons?
a) 6s
b) 5d
c) 4p
d) 3d
39-Why does the electron configuration of chromium deviate from the expected pattern?
a) Energy of 4s is higher than 3d.
b) Energy of 3d drops across the row.
c) Energy of 3d is higher than 4s.
d) 4s is empty in chromium.
40-What is the valence electron configuration for transition metal atoms according to the periodic table?
a) ns1-2
b) (n-1)d1-10 ns1-2
c) ns2(n-1)d1-10
d) (n-1)d1-10 ns2
41-What is the significance of the statement “For transition metal ions having a charge ≥ +2, the number of d electrons equals the total number of valence electrons minus the charge on the ion”?
a) It explains the stability of transition metal ions.
b) It helps determine the electron configuration of transition metal ions.
c) It illustrates the relationship between charge and electron distribution.
d) It describes the transition metal ionization process.
42-Which of the following elements has the electronic configuration [54Xe]6S2, 5d5?
a) Molybdenum (Mo)
b) Technetium (Tc)
c) Ruthenium (Ru)
d) Rhodium (Rh)
43-What is the electron configuration of Ni (Nickel) in its ground state?
a) [Ar] 4s2 3d8
b) [Ar] 4s1 3d10
c) [Ar] 4s2 3d9
d) [Ar] 4s2 3d8 4p1
44-For the electronic configuration [75]1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p6 4f14 5d5 6s2, what is the total number of electrons?
a) 50
b) 60
c) 70
d) 75
45-What is the electron configuration of Vanadium (V)?
a) [Ar] 4s2 3d3
b) [Ar] 4s2 3d5
c) [Ar] 4s2 3d7
d) [Ar] 4s1 3d10 4p1
46-Which of the following elements is in the third transition series?
a) Copper (Cu)
b) Cobalt (Co)
c) Rhodium (Rh)
d) Silver (Ag)
47-What is the electron configuration of Fe3+?
a) [Ar] 3d5
b) [Ar] 3d6
c) [Ar] 3d7
d) [Ar] 3d8
48-In the electron configuration [54Xe]6S2, 5d5, how many unpaired electrons are there?
a) 0
b) 1
c) 3
d) 5
49-What is the electron configuration of Ti (Titanium) in its ground state?
a) [Ar] 4s2 3d2
b) [Ar] 4s2 3d5
c) [Ar] 4s2 3d7
d) [Ar] 4s2 3d10
50-For the electronic configuration
[75]1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p6 4f14 5d5 6s2,
what is the name and symbol of the element?
a) Tungsten (W)
b) Rhenium (Re)
c) Iridium (Ir)
d) Osmium (Os)
The answers of all questions
Here are the answers to the quiz:
1-a) ns1-2(n-1)d1-10
2-b) 3dn 4s2
3-c) The 3d10 4s1 configuration is of lower energy for both chromium and copper.
4-c) The energy of 3d orbitals drops going across the row.
5-b) The total number of valence electrons equals the group number.
6-c) Number of d electrons = total valence electrons – charge of the ion.
7-a) d5
8-a) The transition series order: Third transition series
b) Period No.: 6
c) Column No.: 7
9-c) 75
10-d) (n-1)d1-10 ns1-2
11-c) Third transition series
12-c) 6
13-c) 7
14-c) 4
15-c) The difference in 3d and 4s orbital energies is similar to the pairing energy.
16-a) Half-filled d sublevel (d5) is more stable.
17-b) 4s is of higher energy than 3d.
18-b) 10 valence electrons, d8
19-a) 8 valence electrons, d5
20-a) 4 valence electrons, d1
21-c) The energy of 4s orbitals drops going across the row.
22-a) The 3d orbitals are of lower energy than 4s orbitals.
23-c) Third transition series, period 6, column 7
24-b) 23
25-b) (n-1)d1-10 ns1-2
26-d) 6s
27-a) Half-filled d sublevel (d5) is more stable.
28-c) 6s
29-c) 6
30-b) 3d8
31-d) 8 valence electrons, d5
32-a) 4
33-a) 2 valence electrons, d1
34-a) Half-filled d sublevel (d5) is more stable.
35-a) 75
36-c) 3d5 4s1
37-c) 3d10 4s1
38-b) 5d
39-a) Energy of 3d is higher than 4s.
40-b) (n-1)d1-10 ns1-2
41-b) It helps determine the electron configuration of transition metal ions.
42-c) Ruthenium (Ru)
43-a) [Ar] 4s2 3d8
44-c) 70
45-b) [Ar] 4s2 3d5
46-c) Rhodium (Rh)
47-a) [Ar] 3d5
48-b) 1
49-a) [Ar] 4s2 3d2
50-b) Rhenium (Re)
Quiz:give reasons questions about this lesson
Here are some “give reasons” questions based on the lesson about the electronic configuration of the first transition series:
1-Give a reason for the exceptions in the electron configurations of chromium and copper.
2-Explain the significance of the statement: “For both chromium and copper, the configuration having more electrons in the 3d orbitals is of lower energy.”
3-Provide a reason for the statement: “For transition metal ions having a charge ≥ +2, the number of d electrons equals the total number of valence electrons minus the charge on the ion.”
4-Explain why the electron configuration [54Xe]6S2, 5d5 corresponds to the third transition series.
5-**Give a reason for the statement: “An element becomes more stable (less energy) when the d sublevel is half-filled (d5).”
6-Explain why the electron configuration [54Xe]6S2, 5d5 corresponds to a period number of 6.
7-Provide a reason for the statement: “In transition metal atoms, the total number of valence electrons equals the number of the column (group) in the periodic table (counting from the left).”
8-Explain the rationale behind the statement: “For transition metal ions of charge ≥ +2, all valence electrons are in the d-subshell.”
9-Give a reason for the order of stability mentioned for d sublevels: half-filled (d5), completely filled with electrons (d10), and empty (d0).
********
Here are the answers to the “give reasons” questions:
1-Give a reason for the exceptions in the electron configurations of chromium and copper.
Reason: The 3d and 4s orbitals are very close in energy, and the energy of 3d orbitals drops going across the row. The electron configurations for chromium and copper are exceptions because the 3d5 4s1 configuration has lower energy due to the similarity in 3d and 4s orbital energies.
2-Explain the significance of the statement: “For both chromium and copper, the configuration having more electrons in the 3d orbitals is of lower energy.”
Reason: This statement highlights that the 3d orbitals are of lower energy than the 4s orbitals for chromium and copper, leading to a more stable electron configuration when there are more electrons in the 3d orbitals.
3-Provide a reason for the statement: “For transition metal ions having a charge ≥ +2, the number of d electrons equals the total number of valence electrons minus the charge on the ion.”
Reason: In transition metal ions with a charge ≥ +2, electrons are removed starting from the outermost shell, and since the 4s subshell is of lower energy than the 3d subshell, the d electrons are the last to be removed, determining the number of d electrons in the ion.
4-Explain why the electron configuration [54Xe]6S2, 5d5 corresponds to the third transition series.
Reason: The presence of electrons in the 5d subshell indicates that the element is part of the third transition series. The transition series corresponds to the filling of the d orbitals, and in this case, the 5d orbitals are being filled, placing the element in the third transition series.
5-Give a reason for the statement: “An element becomes more stable (less energy) when the d sublevel is half-filled (d5).”
-Reason: A half-filled d sublevel (d5) is more stable because it maximizes the number of unpaired electrons in the d subshell, and this configuration is associated with lower energy, following the Hund’s rule of maximum multiplicity.
6-Explain why the electron configuration [54Xe]6S2, 5d5 corresponds to a period number of 6.
Reason: The presence of electrons in the 6th energy level (6S2) indicates that the element is in the 6th period of the periodic table.
7-Provide a reason for the statement: “In transition metal atoms, the total number of valence electrons equals the number of the column (group) in the periodic table (counting from the left).”
Reason: Transition metal atoms typically have a valence configuration of ns2(n-1)d, and the number of valence electrons is determined by the number of electrons in the outermost shell, corresponding to the group number in the periodic table.
8-Explain the rationale behind the statement: “For transition metal ions of charge ≥ +2, all valence electrons are in the d-subshell.”
Reason: In transition metal ions with a charge ≥ +2, electrons are removed starting from the outermost shell, and since the 4s subshell is of lower energy than the 3d subshell, the d electrons are the last to be removed, leading to all valence electrons being in the d-subshell.
9-Give a reason for the order of stability mentioned for d sublevels: half-filled (d5), completely filled with electrons (d10), and empty (d0).
Reason: Half-filled d sublevel (d5) and completely filled d sublevel (d10) are more stable because they maximize the number of unpaired electrons or achieve a completely filled sublevel, both of which result in lower energy configurations. An empty d sublevel (d0) is less stable as it lacks the stability associated with either half-filled or completely filled sublevels.