Question:
Which one of the following is correct for all elements from $Sc$ to $Cu$ ?
Which one of the following is correct for all elements from $Sc$ to $Cu$ ?
Updated On: Nov 14, 2025
- The lowest oxidation state shown by them is +2
- 4 S orbital is completely filled in the ground state
- 3 d orbital is not completely filled in the ground state
- The ions in +2 oxidation states are paramagnetic
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The Correct Option is D
Solution and Explanation
To address the question regarding the properties of elements from \(Sc\) (Scandium) to \(Cu\) (Copper) in the periodic table, we need to analyze the electronic configuration and typical oxidation states of these transition metals.
The elements from Sc to Cu are transition elements and hence, follow typical behavior such as incomplete \(d\) subshells in their ground state.
- Analyzing the options:
- Option 1: The lowest oxidation state shown by them is +2.
- Option 2: 4 S orbital is completely filled in the ground state.
- Option 3: 3 d orbital is not completely filled in the ground state.
- Option 4: The ions in +2 oxidation states are paramagnetic.
- Explanation:
- Consider Option 1: While several of the elements do show a +2 oxidation state, it is not always the lowest possible oxidation state for each element. For example, Copper (Cu) can show a +1 oxidation state.
- Consider Option 2: Not all elements from Sc to Cu have a completely filled 4s orbital in their elemental state. For instance, in the case of Scandium (Sc), its configuration is \([\text{Ar}] 3d^1 4s^2\), but it changes when ions are formed.
- Consider Option 3: The statement "3d orbital is not completely filled in the ground state" is true for elements from Sc to Ni. However, Copper (Cu) has a configuration of \([\text{Ar}] 3d^{10} 4s^1\), implying a completely filled 3d subshell.
- Verification of Option 4:
- In the +2 oxidation state, all these elements have electrons removed from their outermost energy level, the 4s orbital, and partially from the 3d subshell. This typically results in unpaired electrons, especially because \(3d\) is not fully filled in ions. Therefore, they are usually paramagnetic due to the presence of unpaired electrons.
- Conclusion:
- Option 4, "The ions in +2 oxidation states are paramagnetic," is the correct statement for this group of transition elements, as they all tend to have unpaired electrons in the \(3d\) subshell making them paramagnetic.
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Concepts Used:
d block elements
The elements, in the columns of the periodic table in which d subshells are being occupied are known as d block elements.
These are the elements that have the capability of forming stable cations with incompletely filled d orbitals. Elements like mercury and Zinc are not considered transition metals because they have electronic configurations: (n-1)d10 ns2. These elements have filled d-orbitals in their ground state and, therefore, even in some of their oxidation states.
General Properties Of d-Block Elements
- Multiple oxidation states- The oxidation states of d block elements show very few energy gaps; therefore, they exhibit many oxidation states. Also, the energy difference between s and d orbital is very less. Therefore both the electrons are involved in ionic and covalent bond formation, which ultimately leads to multiple oxidation states.
- Formation of complex compounds- Ligands show a binding behaviour and can form so many stable complexes with the help of transition metals. This property is mainly due to:
- Availability of vacant d orbitals.
- Comparatively small sizes of metals.
- Hardness- Transition elements are tough and have high densities because of the presence of unpaired electrons.
- Melting and boiling points- Melting and boiling points of transition are very high. This is because of the presence of unpaired electrons and partially filled d orbitals. Because of these two things, they form strong bonds and therefore have high melting and boiling points.
- Atomic radii- The atomic and ionic radius of the transition elements decreases as we move from Group 3 to group 6. However, it remains the same between group 7 and group 10, and from group 11 to group 12 increases.
- Ionization enthalpy- The ionization enthalpies of the transition elements are generally on the greater side as compared to the S block elements