Long Answer TypeWrite down the electronic configuration of elements from atomic number 21 to atomic number 30. Also name the elements.
How will you account for the electronic configuration of the elements with atomic number of 24 and 29?
Or
Account for the following:
The continuous building up of 3d subshell interpreted in chromium (At. No. 24) and copper (At No. 29).
Or
Outer electronic configuration of chromium is 3d5 4s1 and not 3d4 4s2. Explain.
Short Answer TypeWrite the electronic configurations of the following ions: (a)H- (b) Na+ (c) O2- (d) F-
Which atoms are indicated by the following configurations?
(a) [He] 2s1
(b) [Ne] 3s2 3p3
(c) [Ar] 4s2 3d1.
Which of the following are isoelectronic species, i.e. those having the same number of electrons?
Na+, K+ , Mg2+, Ca2+, S2-, Ar.
What is the cause of greater stability of exactly half-filled and completely filled configurations?
The greater stability of these configurations is due to following two reasons:
(i) Symmetry. The half-filled and completely filled configurations are more symmetrical and symmetry leads to greater stability.
(ii) Exchange energy. In an atom, the electrons present in various orbitals of the same sub-shell tend to exchange their positions. Such an exchange of electrons results in the release of energy called exchange energy. Greater the exchange energy, more is the stability associated with the orbitals. Now half filled and completely filled sub-shell configurations allow the maximum exchange of electron to take place. Therefore, such configurations have maximum stability.
An atom of an element contains 29 electrons and 35 Deutrons. Deduce (i) the number of protons and (ii) the electronic configuration of the element.
Long Answer TypeWrite the electronic configurations of the following ions/atom:
(i) Cu2+ (ii) Cr3+
(iii) Ni2+ (iv) Rubidium (Z = 37)
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