Question

According to Hund's rule of maximum spin multiplicity, how many singly-occupied orbitals are there in the valence shells of the following elements in their ground states? Enter your answer as the sum of all the orbitals (for example 15). A) calcium B) gallium C) silicon D) vanadium E) carbon F) neon

Answer 1

Answer:

A) calcium-0 B) gallium-1 C) silicon-2 D) vanadium-3 E) carbon-2 F) neon-0

Explanation:

Hund's rule of maximum multiplicity:-

Firstly, every orbital which is present in the sublevel is singly occupied and then the orbital is doubly occupied.  

(A) Calcium.

The electronic configuration is -  

$1s^22s^22p^63s^23p^64s^2$

Thus, 4s orbital is fully filled and thus there is no singly filled orbital in calcium.

(B) Gallium.

The electronic configuration is -  

$1s^22s^22p^63s^23p^63d^{10}4s^24p^1$

Thus, 4s orbital is fully filled and p orbital can singly filled 3 electrons. Thus, no electrons will be paired and thus, 1 orbital will be singly filled in gallium.

(C) Silicon.

The electronic configuration is -  

$1s^22s^22p^63s^23p^2$

Thus, 3s orbital is fully filled and p orbital can singly filled 3 electrons. Thus, no electrons will be paired and thus, 2 orbitals will be singly filled in silicon.

D) Vanadium

The electronic configuration is -  

$1s^22s^22p^63s^23p^63d^{3}4s^2$

Thus, 4s orbital is fully filled and d orbital can singly filled 5 electrons. Thus, 3 orbitals will be singly filled in vanadium.  

(E) Carbon.

The electronic configuration is -  

$1s^22s^22p^2$

Thus, 2s orbital is fully filled and p orbital can singly filled 3 electrons. Thus, Carbon has 2 singly occupied orbitals.

F) Neon

The electronic configuration is -  

$1s^22s^22p^6$

Thus, 2s orbital is fully filled and p orbital can singly filled 3 electrons which is also fully filled. So, there is no singly filled orbital in neon.