The ground state electronic configurations of some elements, P, Q, R, S, and T (these symbols represent the some of the known elements given in the periodic table) are as follows.
P : 1s 2 2s 2 2p 6 3s 2 3p 2
Q : 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1
R : 1s 2 2s 2 2p 6 3s 2 3p 1
S : 1s 2 2s 2 2p 6 3s 2 3p 6 3d 5 4s 1 T : 1s
2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 .
Match the electronic configurations of the elements with the properties given below and select the correct sequence by choosing the correct codes given.
(i) Element forms a cation which is isoelectronic with P 3– .
(ii) Element which in its compounds can show a maximum oxidation state of +6 and that is coloured too.
(iii) Element has largest atomic radius and highest first ionisation energy in the respective period.
(iv) Element which has intermediate value of electronegativity and its oxide forms salts with strong acids and bases.
Text Solution
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(i) Alkali metal, potassium forms K + (number of electrons = 18) which is isoelectronic with P 3– (number of electrons = 18) → Q.
(ii) Transition element, chromium show maximum oxidation state of +6 in Cr 2 O 7 2– and CrO 4 2– and they are coloured → S.
(iii) Noble gas, Kr has largest atomic radius because radius is expressed as vander Waal's radius and there is interelectronic repulsions due to completely filled outer most shell. Inert gas has highest first ionisation energy in the respective period because of stable valence shell electron configuration → T.
(iv) Element (Z = 13), aluminium has intermediate value of electronegativity and therefore its oxide is amphoteric in nature → R.
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