Subjective Type

State and explain the 'Hund's rule of maximum multiplicity'.

Solution

Hund's rule of maximum multiplicity states that for a given electronic configuration, the electron pairing in $$p, d$$ and $$f$$ orbitals cannot occur until each orbital of a given subshell is filled with one electron each or is singly occupied.

The $$s$$-orbital contains only one orbital, so it is excluded form the Hund's rule of maximum multiplicity. It can accomodate two electrons only, in opposite spins.

Thus, the Hund's rule of maximum multiplicity states that:

$$1.$$ In a sublevel, each orbital is singly occupied before it is doubly occupied.

$$2.$$ The electrons present in singly occupied orbitals possess identical spin, i.e., clock-wise spin.

SIMILAR QUESTIONS

Atomic Structure

Which rule explains the electronic configuration of chromium is [Ar] $$3d^{5} 4s^{1}$$ instead of [Ar]$$3d^{4}4s^{2}$$?

Atomic Structure

The largest number of unpaired electrons: $$ F,\ N, \ S^{2-},\ Mg^{2+},\ Sc^{3+}, \ Ti^{3+}$$

Atomic Structure

If Hund's rule is not followed, magnetic moment if Fe$$^{2+}$$, Mn$$^\oplus$$ and Cr all having 24 electrons will be in order :

Atomic Structure

According to Hund's rule, the distribution of electron within the various orbitals of a given sub-shell is one which is associated with :

Atomic Structure

State Hund's rule of maximum multiplicity.

Atomic Structure

Using the Hund rules, find the basic term of the atom whose partially filled subshell contains (a) three p electrons; (b) four p electrons.

Atomic Structure

Why Hund's rule is called rule of maximum multiplicity ?

Atomic Structure

Which of the following statements is correct?

Atomic Structure

In which of the following orbital diagrams are both Pauli's exclusion principle and Hund's rule violated?

Atomic Structure

In a set of degenerate orbitals, the electrons distribute themselves to retain similar spins as far as possible. This statement is attributed to :

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