Question:
The free gaseous Cr atom has six unpaired electrons.
Half-filled s-orbital has greater stability.
The free gaseous Cr atom has six unpaired electrons.
Half-filled s-orbital has greater stability.
Updated On: Jul 28, 2022
- Both Assertion and Reason are true and Reason is the correct explanation of Assertion
- Both Assertion and Reason are true but Reason is not the correct explanation of Assertion
- Assertion is true but Reason is false
- Both Assertion and Reason are false
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The Correct Option is C
Solution and Explanation
The free gaseous $Cr$ atom has six unpaired electrons due to following electronic configuration $($ atomic number $=24)$ $=[ Ar ] 3 d^{5} 4 s^{1}$. This is because half-filled $d$ -orbital is more stable as compared to incompletely filled $d$ -orbital. So, one electron jumps from $4 s^{2}$ -orbital to $3 d$ - orbital.
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Concepts Used:
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 behavior 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 because of the presence of unpaired electrons and partially filled d orbitals. They form strong bonds and 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