What is indicated by Hund's Rule in relation to electron distribution?

What is indicated by Hund's Rule in relation to electron distribution?

• A. All orbitals must be fully occupied before any are singly occupied
• B. Every orbital in a subshell is singly occupied before any orbital is doubly occupied
• C. Electrons will not occupy the same orbital
• D. Electrons fill orbitals from highest to lowest energy

Answer: (B)

Hund's Rule states that within a subshell, every orbital is singly occupied before any orbital is doubly occupied. This means that when electrons are added to orbitals of the same energy level (degenerate orbitals), each orbital receives one electron first, which all have the same spin direction, before any orbital is filled with a second electron. This arrangement minimizes electron-electron repulsions and stabilizes the atom. This principle is crucial for understanding how electrons are distributed in an atom and helps to explain the ground state electron configurations of many elements. By ensuring that each orbital is occupied singly first, atoms can maintain a lower energy state, which is critical in chemistry and bonding behavior.

Hund's Rule states that within a subshell, every orbital is singly occupied before any orbital is doubly occupied. This means that when electrons are added to orbitals of the same energy level (degenerate orbitals), each orbital receives one electron first, which all have the same spin direction, before any orbital is filled with a second electron. This arrangement minimizes electron-electron repulsions and stabilizes the atom.

This principle is crucial for understanding how electrons are distributed in an atom and helps to explain the ground state electron configurations of many elements. By ensuring that each orbital is occupied singly first, atoms can maintain a lower energy state, which is critical in chemistry and bonding behavior.