Home
Class 12
CHEMISTRY
What are t(2g) and e(g) orbitals?...

What are `t_(2g)` and `e_(g)` orbitals?

Text Solution

Verified by Experts

In a free transition metal ion, the d-orbitals are degenerate. When it form complex, the degeneracy is split and d-orbitals split into `t_(2g)` and `e_(g)` orbitals.
Promotional Banner

Topper's Solved these Questions

  • COORDINATION COMPOUNDS

    CBSE COMPLEMENTARY MATERIAL|Exercise SHORT ANSWER-II TYPE QUESTIONS|8 Videos

  • COORDINATION COMPOUNDS

    CBSE COMPLEMENTARY MATERIAL|Exercise LONG ANSWER TYPE QUESTIONS|3 Videos

  • COORDINATION COMPOUNDS

    CBSE COMPLEMENTARY MATERIAL|Exercise VERY SHORT ANSWER TYPE QUESTIONS|11 Videos

  • CHEMISTRY IN EVERYDAY LIFE

    CBSE COMPLEMENTARY MATERIAL|Exercise LONG ANSWER TYPE QUESTIONS|2 Videos

  • ELECTROCHEMISTRY

    CBSE COMPLEMENTARY MATERIAL|Exercise LONG ANSWER TYPE QUESTIONS (5 Marks)|7 Videos

Similar Questions

Explore conceptually related problems

Which of the following complex ions has electrons that are symmetrically filled in both t_(2g) and e_(g) orbitals ?

A 5g orbital has

Which of the following statements is incorrect? (i) In octahedral complexes, t_(2g) orbitals posses low energy as compared to e_(g) orbitals (ii) In octahedral complexes, e_(g) orbitals possess low energy as compared to t_(2g) orbitals (iii) In tetrahedral complexes, t_(2g) orbitals posses high energy as compared to e_(g) orbitals

When a transition metal ion (usually) is involved in octahedral complex formation, the five degenerate d-orbitals split into two set of degenerate orbitals (3+2) . Three degenerate orbitals of lower energy (d_(xy),d_(yz),d_(zx)) and a set of degenerate orbitals of higher energy (d_(x^(2)-y^(2)" and "d_(z^(2)) . The orbitals with lower energy are called t_(2g) orbitals and those with higher energy are called e_(g) orbitals. In octahedral complexes, positive metal ion may be considered to be present at the centre and negative ligands at the corner of a regular octahedron. As lobes of d_(x^(2)-y^(2)" and "d_(z^(2) lie along the axis, i.e., along the ligands, the repulsions are more and so, high is the energy. The lobes of the remaining three d-orbitals lie between the Axis i.e., between the ligands. The repulsions between them are less, so lesser the energy. In the octahedral complexes, if metal ion has electrons more than 3, then for pairing them, the options are (i) Pairing may start with 4th electron in t_(2g) orbitals. (ii) Pairing may start normally with 6th electron when t_(2g)" and "e_(g) orbitals are singly filled. Which of the following electronic arrangement is/are possible for inner orbital octahedral complex. (P) t_(2g)^(3)e_(g)^(2)" "(Q) t_(2g)^(6)e_(g)^(1) (R ) t_(2g)^(3)e_(g)^(0)" "(S) t_(2g)^(4)e_(g)^(2) Select the correct code :

Give the total number of t_(2g) and e_(g) electrons in [NiF_(6)]^(2-) .