The ionization potential (IP) values for an e | vedclass

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(A) To identify the element,we look for a large jump in the successive ionization potential values,which indicates the removal of an electron from a s

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$Mg$

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(A) To identify the element,we look for a large jump in the successive ionization potential values,which indicates the removal of an electron from a stable noble gas core.$1$. The given values are: $(IP)_1 = 7.1 \ eV$,$(IP)_2 = 10.3 \ eV$,$(IP)_3 = 36.2 \ eV$,and $(IP)_4 = 39.1 \ eV$.$2$. The jump from $(IP)_2$ to $(IP)_3$ is very large $(36.2 - 10.3 = 25.9 \ eV)$,suggesting that the element has $2$ valence electrons.$3$. An element with $2$ valence electrons belongs to Group $2$ (alkaline earth metals).$4$. Among the given options,$Mg$ (Magnesium) is in Group $2$ with the electronic configuration $[Ne] 3s^2$. Therefore,it has $2$ valence electrons.

$(IP)_1$	$7.1 \ eV$
$(IP)_2$	$10.3 \ eV$
$(IP)_3$	$36.2 \ eV$
$(IP)_4$	$39.1 \ eV$

The ionization potential $(IP)$ values for an element are given below. Identify the element:
$(IP)_1$ $7.1 \ eV$
$(IP)_2$ $10.3 \ eV$
$(IP)_3$ $36.2 \ eV$
$(IP)_4$ $39.1 \ eV$

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The ionization potential $(IP)$ values for an element are given below. Identify the element:$(IP)_1$$7.1 \ eV$$(IP)_2$$10.3 \ eV$$(IP)_3$$36.2 \ eV$$(IP)_4$$39.1 \ eV$