Successive ionization energies of an element ‘X’ are given below (in K Cal) IP1 IP2 IP3 IP4 165 195 556 595 Electronic configuration of the element ‘X’ is
Answers
Therefore the electronic configuration of element X is 1s², 2s², 2p⁶ , 3s².
Given : Successive ionisation energies of an element ‘X’ are given below (in KCal) ....
IP₁ , IP₂ , IP₃ , IP₄ ; 165 , 195, 556, 595
To find : Electronic configuration of the element X.
solution : we know, ionisation enthalpy is the energy required to remove an electron from an isolated gaseous atom.
it is clearly shown that there is a significance difference between 2nd and 3rd ionisation potentials (i.e., 556 - 195 = 361 > 195), it has two electrons in its valence shell. it means element belongs to alkaline earth metal.
we know, configuration of alkaline earth metal is ns²
as energy required to remove 1st electron from isolated gaseous state of element X is 165 KCal
so, element X is not other than magnesium.
we know configuration of Mg is 1s², 2s² , 2p⁶ , 3s²
Therefore the electronic configuration of element X is 1s², 2s², 2p⁶ , 3s²
Answer:
THE ANSWER IS 1S22S22P63S2 (MG)
Explanation:
THERE WAS A SUDDEN JUMP BETWEEN IP2 AND IP3
556-195=361
TO DETERMINE NO OF VALENCE ELECTRONS
THE FORMULA IS
NO OF VALENCE ELECTRONS=NO OF LOWER VALUES OF IP BEFORE 1st HIGHEST JUMP
SO THAT NO OF VALENCE ELECTRONS=2
ONLY ALKALINE EARTH METALS HAVE 2 ELECTRONS IN THE OUTERMOST SHELL.
SO THAT THE ELEMENT IS MAGNESIUM(MG)
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