Consider the following elements In,Tl,Al,Pb,S | vedclass

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(B) The first ionisation enthalpy $(IE_1)$ generally decreases down a group and increases across a period. Among the given elements ($Al$,$In$,$Tl$,$G

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$+4$ and $+3$

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(B) The first ionisation enthalpy $(IE_1)$ generally decreases down a group and increases across a period. Among the given elements ($Al$,$In$,$Tl$,$Ge$,$Sn$,$Pb$),$Ge$ (Germanium) has the highest $IE_1$ and $In$ (Indium) has the lowest $IE_1$. For $Ge$ (Group $14$),the most stable oxidation state is $+4$. For $In$ (Group $13$),the most stable oxidation state is $+3$. Therefore,the most stable oxidation states for the elements with the highest and lowest $IE_1$ are $+4$ and $+3$,respectively.

List-$A$	List-$B$
$(1)$ $He$	$(A)$ High electron gain enthalpy
$(2)$ $Cl$	$(B)$ Electropositive element
$(3)$ $Ca$	$(C)$ Strong reducing agent
$(4)$ $Li$	$(D)$ High ionization enthalpy

Consider the following elements $In$,$Tl$,$Al$,$Pb$,$Sn$ and $Ge$. The most stable oxidation states of elements with highest and lowest first ionisation enthalpies,respectively,are

Similar Questions

Identify the incorrect order.

Match the items in List-$A$ with the items in List-$B$.

List-$A$ List-$B$

$(1)$ $He$ $(A)$ High electron gain enthalpy

$(2)$ $Cl$ $(B)$ Electropositive element

$(3)$ $Ca$ $(C)$ Strong reducing agent

$(4)$ $Li$ $(D)$ High ionization enthalpy

Select the correct order for the elements $B, C, N, O$:

Which of the following points is never the same for $IP$ and $EA$?

The electronic configurations of $4$ atoms are given below:
$P = [Ne] \, 3s^2 3p^3$
$Q = [Ar] \, 3d^{10} 4s^2 4p^3$
$R = [He] \, 2s^2 2p^5$
$S = [Ne] \, 3s^1$
Which of the following statements is incorrect?

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