The main reason for the actinoids exhibiting | vedclass

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(B) The electronic configuration of lanthanoids is $[Xe] 4f^{1-14} 5d^{0-1} 6s^2$,while for actinoids it is $[Rn] 5f^{1-14} 6d^{0-1} 7s^2$. In actinoi

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The energy difference between $5f$ and $6d$ orbitals is less than that between $4f$ and $5d$ orbitals.

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(B) The electronic configuration of lanthanoids is $[Xe] 4f^{1-14} 5d^{0-1} 6s^2$,while for actinoids it is $[Rn] 5f^{1-14} 6d^{0-1} 7s^2$. In actinoids,the energy difference between the $5f$ and $6d$ orbitals is much smaller than the energy difference between the $4f$ and $5d$ orbitals in lanthanoids. Additionally,because the $5f$ orbitals are further from the nucleus,they are less tightly held,allowing for greater participation in bonding and the exhibition of a wider range of oxidation states.

The main reason for the actinoids exhibiting a larger number of oxidation states than the lanthanoids is:

Similar Questions

The most common oxidation state of Lanthanoid elements is $+3$. Which of the following is likely to deviate easily from $+3$ oxidation state?

The electronic configurations of bivalent europium and trivalent cerium are
(atomic number : $Xe=54, Ce=58, Eu=63$ )

Determine whether the following statements are True $(T)$ or False $(F)$:
$(a)$ All actinoid elements have a $7s^1$ configuration.
$(b)$ All actinoid elements have a $7s^0$ configuration.
$(c)$ There are no electrons in the $7s$ orbital of actinoids.

Which lanthanoid from the following may exhibit $+4$ oxidation state with $f^{0}$ configuration?

The most basic hydroxide among the following is-

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