Case Based Questions Test: d & f-Block Elements


20 Questions MCQ Test Chemistry Class 12 | Case Based Questions Test: d & f-Block Elements


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Attempt Case Based Questions Test: d & f-Block Elements | 20 questions in 40 minutes | Mock test for NEET preparation | Free important questions MCQ to study Chemistry Class 12 for NEET Exam | Download free PDF with solutions
QUESTION: 1

Read the passage given below and answer the following questions:

Within the 3d series, manganese exhibits oxidation states in aqueous solution from +2 to +7, ranging from Mn2+(aq) to MnO4 (aq). Likewise, iron forms both Fe2+(aq) and Fe3+(aq) as well as the FeO2−4 ion. Cr and Mn form oxyions CrO2−4, MnO4, owing to their willingness to form multiple bonds. The pattern with the early transition metals—in the 3d series up to Mn, and for the 4d, 5d metals up to Ru and Os—is that the maximum oxidation state corresponds to the number of ‘‘outer shell’’ electrons. The highest oxidation states of the 3d metals may depend upon complex formation (e.g., the stabilization of Co3+ by ammonia) or upon the pH (thus MnO42− (aq) is prone to disproportionation in acidic solution). Within the 3d series, there is considerable variation in relative stability of oxidation states, sometimes on moving from one metal to a neighbour; thus, for iron, Fe3+ is more stable than Fe2+, especially in alkaline conditions, while the reverse is true for cobalt. The ability of transition metals to exhibit a wide range of oxidation states is marked with metals such as vanadium, where the standard potentials can be rather small, making a switch between states relatively easy.

In the following questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices on the basis of the above passage.

Assertion (A): Highest oxidation state is exhibited by transition metal lying in the middle of the series.

Reason (R): The highest oxidation state exhibited corresponds to number of (n−1)d electrons.

Solution: Higher oxidation states are usually exhibited by the members in the middle of a series of transition elements due to greater number of unpaired electrons in (n−1)d and ns orbitals at the middle of the series.
QUESTION: 2

Read the passage given below and answer the following questions:

Within the 3d series, manganese exhibits oxidation states in aqueous solution from +2 to +7, ranging from Mn2+(aq) to MnO4 (aq). Likewise, iron forms both Fe2+(aq) and Fe3+(aq) as well as the FeO2−4 ion. Cr and Mn form oxyions CrO2−4, MnO4, owing to their willingness to form multiple bonds. The pattern with the early transition metals—in the 3d series up to Mn, and for the 4d, 5d metals up to Ru and Os—is that the maximum oxidation state corresponds to the number of ‘‘outer shell’’ electrons. The highest oxidation states of the 3d metals may depend upon complex formation (e.g., the stabilization of Co3+ by ammonia) or upon the pH (thus MnO42− (aq) is prone to disproportionation in acidic solution). Within the 3d series, there is considerable variation in relative stability of oxidation states, sometimes on moving from one metal to a neighbour; thus, for iron, Fe3+ is more stable than Fe2+, especially in alkaline conditions, while the reverse is true for cobalt. The ability of transition metals to exhibit a wide range of oxidation states is marked with metals such as vanadium, where the standard potentials can be rather small, making a switch between states relatively easy.

In the following questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices on the basis of the above passage.

Assertion (A): Vanadium had the ability to exhibit a wide range of oxidation states.

Reason (R): The standard potentials Vanadium are rather small, making a switch between oxidation states relatively easy.

Solution:
QUESTION: 3

Read the passage given below and answer the following questions:

Within the 3d series, manganese exhibits oxidation states in aqueous solution from +2 to +7, ranging from Mn2+(aq) to MnO4 (aq). Likewise, iron forms both Fe2+(aq) and Fe3+(aq) as well as the FeO2−4 ion. Cr and Mn form oxyions CrO2−4, MnO4, owing to their willingness to form multiple bonds. The pattern with the early transition metals—in the 3d series up to Mn, and for the 4d, 5d metals up to Ru and Os—is that the maximum oxidation state corresponds to the number of ‘‘outer shell’’ electrons. The highest oxidation states of the 3d metals may depend upon complex formation (e.g., the stabilization of Co3+ by ammonia) or upon the pH (thus MnO42− (aq) is prone to disproportionation in acidic solution). Within the 3d series, there is considerable variation in relative stability of oxidation states, sometimes on moving from one metal to a neighbour; thus, for iron, Fe3+ is more stable than Fe2+, especially in alkaline conditions, while the reverse is true for cobalt. The ability of transition metals to exhibit a wide range of oxidation states is marked with metals such as vanadium, where the standard potentials can be rather small, making a switch between states relatively easy.

In the following questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices on the basis of the above passage.

Assertion (A): The highest oxidation states of the 3d metals depends only on electronic configuration of the metal.

Reason (R): The number of electrons in the (n-1) d and ns subshells determine the oxidation states exhibited by the metal.

Solution:
QUESTION: 4

Read the passage given below and answer the following questions:

Within the 3d series, manganese exhibits oxidation states in aqueous solution from +2 to +7, ranging from Mn2+(aq) to MnO4 (aq). Likewise, iron forms both Fe2+(aq) and Fe3+(aq) as well as the FeO2−4 ion. Cr and Mn form oxyions CrO2−4, MnO4, owing to their willingness to form multiple bonds. The pattern with the early transition metals—in the 3d series up to Mn, and for the 4d, 5d metals up to Ru and Os—is that the maximum oxidation state corresponds to the number of ‘‘outer shell’’ electrons. The highest oxidation states of the 3d metals may depend upon complex formation (e.g., the stabilization of Co3+ by ammonia) or upon the pH (thus MnO42− (aq) is prone to disproportionation in acidic solution). Within the 3d series, there is considerable variation in relative stability of oxidation states, sometimes on moving from one metal to a neighbour; thus, for iron, Fe3+ is more stable than Fe2+, especially in alkaline conditions, while the reverse is true for cobalt. The ability of transition metals to exhibit a wide range of oxidation states is marked with metals such as vanadium, where the standard potentials can be rather small, making a switch between states relatively easy.

In the following questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices on the basis of the above passage.

Assertion (A): Fe3+ is more stable than Fe2+.

Reason (R): Fe3+ has 3d5 configuration while Fe2+ has 3d6 configuration.

Solution: This can be understood as follows

Fe3+ has 3d5 , half filled configuration , whereas Fe2+ has 3d6 configuration.

Due to half filled , 3d5 stable configuration , the Fe3+ is more stable than the Fe2+.

Due to the same reason, the

B: Core of Fe3+ is more stable,

and C: IInd and IIIrd IP difference is less than 11.0 ev.

QUESTION: 5

Read the passage given below and answer the following questions:

Within the 3d series, manganese exhibits oxidation states in aqueous solution from +2 to +7, ranging from Mn2+(aq) to MnO4 (aq). Likewise, iron forms both Fe2+(aq) and Fe3+(aq) as well as the FeO2−4 ion. Cr and Mn form oxyanions CrO2−4, MnO4, owing to their willingness to form multiple bonds. The pattern with the early transition metals—in the 3d series up to Mn, and for the 4d, 5d metals up to Ru and Os—is that the maximum oxidation state corresponds to the number of ‘‘outer shell’’ electrons. The highest oxidation states of the 3d metals may depend upon complex formation (e.g., the stabilization of Co3+ by ammonia) or upon the pH (thus MnO42− (aq) is prone to disproportionation in acidic solution). Within the 3d series, there is considerable variation in relative stability of oxidation states, sometimes on moving from one metal to a neighbour; thus, for iron, Fe3+ is more stable than Fe2+, especially in alkaline conditions, while the reverse is true for cobalt. The ability of transition metals to exhibit a wide range of oxidation states is marked with metals such as vanadium, where the standard potentials can be rather small, making a switch between states relatively easy.

In the following questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices on the basis of the above passage.

Assertion (A): Transition metals like Fe, Cr and Mn form oxyions.

Reason (R): Oxygen is highly electronegative and has a tendency to form multiple bonds.

Solution:
QUESTION: 6

Read the passage given below and answer the following questions:

The transition metals when exposed to oxygen at low and intermediate temperatures form thin, protective oxide films of up to some thousands of Angstroms in thickness. Transition metal oxides lie between the extremes of ionic and covalent binary compounds formed by elements from the left or right side of the periodic table. They range from metallic to semiconducting and deviate by both large and small degrees from stoichiometry. Since d-electron bonding levels are involved, the cations-exist in various valence states and hence give rise to a large number of oxides. The crystal structures are often classified by considering a cubic or hexagonal close-packed lattice of one set of ions with the other set of ions filling the octahedral or tetrahedral interstices. The actual oxide structures, however, generally show departures from such regular arrays due in part to distortions caused by packing of ions of different size and to ligand field effects. These distortions depend not only on the number of d-electrons but also on the valence and the position of the transition metal in a period or group.

In the following questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices on the basis of the above passage.

Assertion (A): Cations of transition elements occur in various valence states

Reason (R): Large number of oxides of transition elements are possible.

Solution: The lowest oxide of transition metal is basic because of some valence electron are not involved in bonding thus act as a base due to the availability of free electrons. The highest oxide of transition metal electrons of metal is involved in the bonding. Therefore, these electrons are not available for donation. Hence, they are acidic in nature.
QUESTION: 7

Read the passage given below and answer the following questions:

The transition metals when exposed to oxygen at low and intermediate temperatures form thin, protective oxide films of up to some thousands of Angstroms in thickness. Transition metal oxides lie between the extremes of ionic and covalent binary compounds formed by elements from the left or right side of the periodic table. They range from metallic to semiconducting and deviate by both large and small degrees from stoichiometry. Since d-electron bonding levels are involved, the cations-exist in various valence states and hence give rise to a large number of oxides. The crystal structures are often classified by considering a cubic or hexagonal close-packed lattice of one set of ions with the other set of ions filling the octahedral or tetrahedral interstices. The actual oxide structures, however, generally show departures from such regular arrays due in part to distortions caused by packing of ions of different size and to ligand field effects. These distortions depend not only on the number of d-electrons but also on the valence and the position of the transition metal in a period or group.

In the following questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices on the basis of the above passage.

Assertion (A): Transition metals form protective oxide films.

Reason (R): Oxides of transition metals are always stoichiometric.

Solution:
QUESTION: 8

Read the passage given below and answer the following questions:

The transition metals when exposed to oxygen at low and intermediate temperatures form thin, protective oxide films of up to some thousands of Angstroms in thickness. Transition metal oxides lie between the extremes of ionic and covalent binary compounds formed by elements from the left or right side of the periodic table. They range from metallic to semiconducting and deviate by both large and small degrees from stoichiometry. Since d-electron bonding levels are involved, the cations-exist in various valence states and hence give rise to a large number of oxides. The crystal structures are often classified by considering a cubic or hexagonal close-packed lattice of one set of ions with the other set of ions filling the octahedral or tetrahedral interstices. The actual oxide structures, however, generally show departures from such regular arrays due in part to distortions caused by packing of ions of different size and to ligand field effects. These distortions depend not only on the number of d-electrons but also on the valence and the position of the transition metal in a period or group.

In the following questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices on the basis of the above passage.

Assertion (A): Crystal structure of oxides of transition metals often show defects.

Reason (R): Ligand field effect cause distortions in crystal structures.

Solution:
QUESTION: 9

Read the passage given below and answer the following questions:

The transition metals when exposed to oxygen at low and intermediate temperatures form thin, protective oxide films of up to some thousands of Angstroms in thickness. Transition metal oxides lie between the extremes of ionic and covalent binary compounds formed by elements from the left or right side of the periodic table. They range from metallic to semiconducting and deviate by both large and small degrees from stoichiometry. Since d-electron bonding levels are involved, the cations-exist in various valence states and hence give rise to a large number of oxides. The crystal structures are often classified by considering a cubic or hexagonal close-packed lattice of one set of ions with the other set of ions filling the octahedral or tetrahedral interstices. The actual oxide structures, however, generally show departures from such regular arrays due in part to distortions caused by packing of ions of different size and to ligand field effects. These distortions depend not only on the number of d-electrons but also on the valence and the position of the transition metal in a period or group.

In the following questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices on the basis of the above passage.

Assertion (A): CrO crystallises in a hexagonal closepacked array of oxide ions with two out of every three octahedral holes occupied by chromium ions.

Reason (R): Transition metal oxide may be hexagonal close-packed lattice of oxide ions with metal ions filling the octahedral voids.

Solution:
QUESTION: 10

Read the passage given below and answer the following questions:

The d block elements are the 40 elements contained in the four rows of ten columns (3-12) in the periodic table. As all the d block elements are metallic, the term d-block metals is synonymous. This set of d-block elements is also often identified as the transition metals, but sometimes the group 12 elements (zinc, cadmium, mercury) are excluded from the transition metals as the transition elements are defined as those with partly filled d or f shells in their compounds. Inclusion of the elements zinc, cadmium and mercury is necessary as some properties of the group 12 elements are appropriate logically to include with a discussion of transition metal chemistry. The term transition element or transition metal appeared to derive from early studies of periodicity such as the Mendeleev periodic table of the elements. His horizontal table of the elements was an attempt to group the elements together so that the chemistry of elements might be explained and predicted. In this table there are eight groups labeled I-VIII with each subdivided into A and B subgroups. Mendeleev recognized that certain properties of elements in Group VIII are related to those of some of the elements in Group VII and those at the start of the next row Group I. In that sense, these elements might be described as possessing properties transitional from one row of the table to the next.

In the following questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices on the basis of the above passage.

Assertion (A): Group 12 elements are not considered as transition metals.

Reason (R): Transition metals are those which have incompletely filled d shell in their compounds.

Solution: Transition metals are those metals who have partially filled d-orbital means not fully filled. But In group 12 elements zn,Cd and Hg have fully filled d-orbital. That's why they are not considered as transition metals.
QUESTION: 11

Read the passage given below and answer the following questions:

The d block elements are the 40 elements contained in the four rows of ten columns (3-12) in the periodic table. As all the d block elements are metallic, the term d-block metals is synonymous. This set of d-block elements is also often identified as the transition metals, but sometimes the group 12 elements (zinc, cadmium, mercury) are excluded from the transition metals as the transition elements are defined as those with partly filled d or f shells in their compounds. Inclusion of the elements zinc, cadmium and mercury is necessary as some properties of the group 12 elements are appropriate logically to include with a discussion of transition metal chemistry. The term transition element or transition metal appeared to derive from early studies of periodicity such as the Mendeleev periodic table of the elements. His horizontal table of the elements was an attempt to group the elements together so that the chemistry of elements might be explained and predicted. In this table there are eight groups labeled I-VIII with each subdivided into A and B subgroups. Mendeleev recognized that certain properties of elements in Group VIII are related to those of some of the elements in Group VII and those at the start of the next row Group I. In that sense, these elements might be described as possessing properties transitional from one row of the table to the next.

In the following questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices on the basis of the above passage.

Assertion (A): Group VII elements of Mendeleev periodic table are transition elements.

Reason (R): Group I –VIII in Mendeleev periodic table is divided into two subgroups, A and B.

Solution: In Mendeleev's periodic table, the groups were divided into two subgroups. Groups from I to VII are meant for normal elements and group VIII is for transition elements. Groups from I to VII have been divided into two subgroups, while group VIII is meant for three elements.
QUESTION: 12

Read the passage given below and answer the following questions:

The d block elements are the 40 elements contained in the four rows of ten columns (3-12) in the periodic table. As all the d block elements are metallic, the term d-block metals is synonymous. This set of d-block elements is also often identified as the transition metals, but sometimes the group 12 elements (zinc, cadmium, mercury) are excluded from the transition metals as the transition elements are defined as those with partly filled d or f shells in their compounds. Inclusion of the elements zinc, cadmium and mercury is necessary as some properties of the group 12 elements are appropriate logically to include with a discussion of transition metal chemistry. The term transition element or transition metal appeared to derive from early studies of periodicity such as the Mendeleev periodic table of the elements. His horizontal table of the elements was an attempt to group the elements together so that the chemistry of elements might be explained and predicted. In this table there are eight groups labeled I-VIII with each subdivided into A and B subgroups. Mendeleev recognized that certain properties of elements in Group VIII are related to those of some of the elements in Group VII and those at the start of the next row Group I. In that sense, these elements might be described as possessing properties transitional from one row of the table to the next.

In the following questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices on the basis of the above passage.

Assertion (A): All d block elements are metallic in nature.

Reason (R): The d –block elements belong to Group 3 -12 of the periodic table.

Solution: Transition Elements are so named, indicating their positioning and transition of properties between, s and p block elements. So, all the transition metals are d block elements but all d block elements are not transition elements.
QUESTION: 13

Read the passage given below and answer the following questions:

The d block elements are the 40 elements contained in the four rows of ten columns (3-12) in the periodic table. As all the d block elements are metallic, the term d-block metals is synonymous. This set of d-block elements is also often identified as the transition metals, but sometimes the group 12 elements (zinc, cadmium, mercury) are excluded from the transition metals as the transition elements are defined as those with partly filled d or f shells in their compounds. Inclusion of the elements zinc, cadmium and mercury is necessary as some properties of the group 12 elements are appropriate logically to include with a discussion of transition metal chemistry. The term transition element or transition metal appeared to derive from early studies of periodicity such as the Mendeleev periodic table of the elements. His horizontal table of the elements was an attempt to group the elements together so that the chemistry of elements might be explained and predicted. In this table there are eight groups labeled I-VIII with each subdivided into A and B subgroups. Mendeleev recognized that certain properties of elements in Group VIII are related to those of some of the elements in Group VII and those at the start of the next row Group I. In that sense, these elements might be described as possessing properties transitional from one row of the table to the next.

In the following questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices on the basis of the above passage.

Assertion (A): Nickel is a transition element that belongs to group 10 and period 4 of the modern periodic table.

Reason (R): Electronic configuration of Nickel is [Ar]183d84s2

Solution:
QUESTION: 14

Read the passage given below and answer the following questions:

In transition elements, generally, ions of the same charge in a given series show progressive decrease in radius with increasing atomic number. This is because the new electron enters a d orbital each time the nuclear charge increases by unity. But the radii of the third (5d) series are virtually the same as those of the corresponding members of the second series. This phenomenon is associated with the intervention of the 4f orbitals which must be filled before the 5d series of elements begin. The filling of 4f before 5d orbital results in a regular decrease in atomic radii called Lanthanoid contraction. In these questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.

Following are the transition metal ions of 3d series: Ti4+, V2+, Mn3+, Cr3+ (Atomic number: Ti = 22, V = 23, Mn = 25, Cr = 24)

Assertion (A): Among the given ions, Cr3+ is the most stable in an aqueous environment.

Reason (R): Cr3+ has half filled t32g.

Solution: Cr3+, half filled t32g.
QUESTION: 15

Read the passage given below and answer the following questions: In transition elements, generally, ions of the same charge in a given series show progressive decrease in radius with increasing atomic number. This is because the new electron enters a d orbital each time the nuclear charge increases by unity. But the radii of the third (5d) series are virtually the same as those of the corresponding members of the second series. This phenomenon is associated with the intervention of the 4f orbitals which must be filled before the 5d series of elements begin. The filling of 4f before 5d orbital results in a regular decrease in atomic radii called Lanthanoid contraction. In these questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.

Following are the transition metal ions of 3d series: Ti4+, V2+, Mn3+, Cr3+ (Atomic number: Ti = 22, V = 23, Mn = 25, Cr = 24)

Assertion (A): Among the given ions, Mn3+ is the most strong oxidizing agent.

Reason (R): Mn3+ has an unstable configuration.

Solution: Mn3+ is the strong oxidising agent because it has 4 electrons in its valence shell and when it gains one electron than it forms Mn2+, it results in the half-filled (d5) configuration that provides extra stability.
QUESTION: 16

Read the passage given below and answer the following questions: In transition elements, generally, ions of the same charge in a given series show progressive decrease in radius with increasing atomic number. This is because the new electron enters a d orbital each time the nuclear charge increases by unity. But the radii of the third (5d) series are virtually the same as those of the corresponding members of the second series. This phenomenon is associated with the intervention of the 4f orbitals which must be filled before the 5d series of elements begin. The filling of 4f before 5d orbital results in a regular decrease in atomic radii called Lanthanoid contraction. In these questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.

Following are the transition metal ions of 3d series: Ti4+, V2+, Mn3+, Cr3+ (Atomic number: Ti = 22, V = 23, Mn = 25, Cr = 24)

Assertion (A): Ti4+ ion is colourless.

Reason (R): All valence electrons are unpaired in Ti4+ ion.

Solution: Ti4+, No unpaired electrons.
QUESTION: 17

Read the passage given below and answer the following questions:

Although actinoids are similar to lanthanoids in that their electrons fill the 5f orbitals in order, their chemical properties are not uniform and each element has characteristic properties. Promotion of 5f - 6d electrons does not require a large amount of energy and examples of compounds with ππacid ligands are known in which all the 5f, 6d, 7s, and 7p orbitals participate in bonding. Trivalent compounds are the most common, but other oxidation states are not uncommon. Especially thorium, protactinium, uranium, and neptunium tend to assume the +4 or higher oxidation state. The following questions are multiple choice questions. Choose the most appropriate answer:

Q. Which of the following oxidation state is common for all lanthanoids?

Solution: All of the lanthanide elements are commonly known to have the +3 oxidation state.
QUESTION: 18

Read the passage given below and answer the following questions:

Although actinoids are similar to lanthanoids in that their electrons fill the 5f orbitals in order, their chemical properties are not uniform and each element has characteristic properties. Promotion of 5f - 6d electrons does not require a large amount of energy and examples of compounds with ππacid ligands are known in which all the 5f, 6d, 7s, and 7p orbitals participate in bonding. Trivalent compounds are the most common, but other oxidation states are not uncommon. Especially thorium, protactinium, uranium, and neptunium tend to assume the +4 or higher oxidation state. The following questions are multiple choice questions. Choose the most appropriate answer:

Q. There are 14 elements in actinoid series. Which of the following element does not belong to this series?

Solution: Tm is Thulium which belongs to Lanthanoids. Uranium(U), Neptunium(Np), Fermium(Fm) belong to Actinoid series.
QUESTION: 19

Read the passage given below and answer the following questions:

Although actinoids are similar to lanthanoids in that their electrons fill the 5f orbitals in order, their chemical properties are not uniform and each element has characteristic properties. Promotion of 5f - 6d electrons does not require a large amount of energy and examples of compounds with ππacid ligands are known in which all the 5f, 6d, 7s, and 7p orbitals participate in bonding. Trivalent compounds are the most common, but other oxidation states are not uncommon. Especially thorium, protactinium, uranium, and neptunium tend to assume the +4 or higher oxidation state. The following questions are multiple choice questions. Choose the most appropriate answer:

Q. Gadolinium belongs to 4f series. Its atomic number is 64. Which of the following is the correct electronic configuration of Gadolinium?

Solution: Gadolinium has an electronic configuration of [Xe] 4f 75d16s2.
QUESTION: 20

Read the passage given below and answer the following questions:

Although actinoids are similar to lanthanoids in that their electrons fill the 5f orbitals in order, their chemical properties are not uniform and each element has characteristic properties. Promotion of 5f - 6d electrons does not require a large amount of energy and examples of compounds with ππacid ligands are known in which all the 5f, 6d, 7s, and 7p orbitals participate in bonding. Trivalent compounds are the most common, but other oxidation states are not uncommon. Especially thorium, protactinium, uranium, and neptunium tend to assume the +4 or higher oxidation state. The following questions are multiple choice questions. Choose the most appropriate answer:

Q. General electronic configuration of actinoids is (n – 2)f1–14 (n – 1)d0–2 ns2. Which of the following actinoids have one electron in 6d orbital?

Solution: Uranium has an electronic configuration of 5f3 6d1 7s2.
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