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

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(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

Vedclass · Accepted Answer

$Mg$

Vedclass · Answer

(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.

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

$B$	$801$
$Al$	$577$
$Ga$	$579$
$In$	$558$
$Tl$	$589$

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

Similar Questions

Explain why there is a phenomenal decrease in ionisation enthalpy from carbon to silicon.

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

Which element having the following electronic configurations has the minimum ionization potential?

In which of the following pairs does the molecule have a higher $IE_1$ value compared to its corresponding atom?

The first ionization enthalpy values (in $kJ\,mol^{-1}$) of group $13$ elements are :

$B$ $801$

$Al$ $577$

$Ga$ $579$

$In$ $558$

$Tl$ $589$

How would you explain this deviation from the general trend?

Vedclass Test Series

Exam Paper Generator

Online Exam Module

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$