Understanding Hund's Rule | Chemistry for EmSAT Achieve PDF Download

Chemistry

• Structure of Atom
• Hund's Rule

Introduction to Hund's Rule

The Aufbau principle states that electrons fill the lowest energy orbitals before moving to higher ones. However, it does not specify the order in which the three 2p orbitals are filled.

Hund's Rule dictates that before any orbital is doubly occupied, each orbital in the sublevel must be singly occupied. Moreover, to maximize total spin, all electrons in a singly occupied orbital must have the same spin.

• Before the double occupation of any orbital, every orbital in the sublevel is singly occupied.
• For maximizing total spin, all electrons in a singly occupied orbital have the same spin.

In atoms at ground state, many unpaired electrons exist due to electrons' tendency to minimize repulsion. Electrons exhibit behavior similar to magnets, attempting to maximize distance between one another before pairing up.

Hund's Rule of Maximum Multiplicity

Explaining Hund's Rule

Key Points about Hund's Rule:

Understanding with an Example:

Understanding Electron Configuration and Its Significance

• The interaction between the valence shells of atoms plays a crucial role in determining stability. Atoms with incomplete valence shells are less stable, making them more likely to engage in chemical reactions.
• The chemical behavior of an element is primarily influenced by its valence electrons. Elements with similar valence electron numbers exhibit comparable chemical properties.
• Electron configuration serves as a predictor of stability. An atom is most stable when all its orbitals are filled. Noble gases, with completely filled energy levels, exemplify this stability by not readily reacting with other elements.
• Elements with full energy levels, such as noble gases, are considered the most stable due to their lack of reactivity with other elements.

Hund’s Rule of Maximum Multiplicity

• Hund's rule, formulated by Friedrich Hund in 1925, determines the electron configuration of atoms based on the spin multiplicity principle.
• According to this rule, when orbitals with the same energy level are available, electrons will fill them individually before pairing up.
• Observations of atomic spectra support this rule, aiding in predicting the ground state of atoms or molecules with open electronic shells.

Applications of Hund’s Rule

• Hund’s Rule finds extensive use in various fields, including atomic chemistry, quantum chemistry, and spectroscopy.

Frequently Asked Questions

• Violations of Hund’s Rule

  When filling orbitals of the same energy, ensure each orbital has at least one electron with the same spin before pairing them up.

• Explanation of Hund’s Rule

  According to Hund’s rule, electrons prefer to occupy empty orbitals before pairing up. This behavior minimizes repulsion since electrons carry negative charges and repel each other.

• Aufbau Principle

  The Aufbau principle dictates that electrons first fill the lowest energy orbital in an atom's ground state before moving on to higher energy orbitals.

Explore more:

• Aufbau's principle, Hund's rule, and Pauli's exclusion principle
• Pauli's exclusion principle

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