The successive 5 ionisation energies of an el | vedclass

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Question

(B) The successive ionization energies are $IE_1 = 800 \ kJ/mol$,$IE_2 = 2427 \ kJ/mol$,$IE_3 = 3658 \ kJ/mol$,$IE_4 = 25024 \ kJ/mol$,and $IE_5 = 328

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Group $13$

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(B) The successive ionization energies are $IE_1 = 800 \ kJ/mol$,$IE_2 = 2427 \ kJ/mol$,$IE_3 = 3658 \ kJ/mol$,$IE_4 = 25024 \ kJ/mol$,and $IE_5 = 32824 \ kJ/mol$. There is a large jump in energy between the $3^{rd}$ and $4^{th}$ ionization energy $(IE_4 - IE_3 = 25024 - 3658 = 21366 \ kJ/mol)$. This indicates that the $4^{th}$ electron is being removed from a stable noble gas core. Therefore,the element has $3$ valence electrons,which places it in Group $13$.

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

The successive $5$ ionisation energies of an element are $800, 2427, 3658, 25024$ and $32824 \ kJ/mol$,respectively. By using the above values,predict the group in which the above element is present:

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The atomic numbers of elements $X, Y$,and $Z$ are $19, 37$,and $55$ respectively. Which of the following statements is correct?

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

The increasing order of the first ionization enthalpies of the elements $B$,$P$,$S$ and $F$ (lowest first) is:

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