The electronic configurations of four element | vedclass

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(B) Let us analyze the given electronic configurations:$(i) \; [Xe] \; 6s^1$: This is Cesium $(Cs)$,an alkali metal. It has a low ionization enthalpy

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$(ii)$ is a $d-$block element

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(B) Let us analyze the given electronic configurations:$(i) \; [Xe] \; 6s^1$: This is Cesium $(Cs)$,an alkali metal. It has a low ionization enthalpy and is a strong reducing agent. This statement is true.$(ii) \; [Xe] \; 4f^{14}5d^16s^2$: This is Lutetium $(Lu)$. Although it has a $5d^1$ electron,it is the last element of the lanthanoid series ($4f$ block). It is considered an $f-$block element,not a $d-$block element. This statement is false.$(iii) \; [Ne] \; 3s^23p^5$: This is Chlorine $(Cl)$,a halogen. It has a high negative electron gain enthalpy. This statement is true.$(iv) \; [Ar] \; 3d^74s^2$: This is Cobalt $(Co)$,a transition metal. Transition metals typically show variable oxidation states. This statement is true.Therefore,the incorrect statement is $(ii)$.

The electronic configurations of four elements are:
$(i) \; [Xe] \; 6s^1$
$(ii) \; [Xe] \; 4f^{14}5d^16s^2$
$(iii) \; [Ne] \; 3s^23p^5$
$(iv) \; [Ar] \; 3d^74s^2$
Which one of the following statements about these elements is not true?

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The electronic configurations of four elements are:$(i) \; [Xe] \; 6s^1$$(ii) \; [Xe] \; 4f^{14}5d^16s^2$$(iii) \; [Ne] \; 3s^23p^5$$(iv) \; [Ar] \; 3d^74s^2$Which one of the following statements about these elements is not true?