Electron Distribution in Different Orbits (Shells)

Introduction
Electrons are subatomic particles that are distributed in specific energy levels known as shells or orbits around the nucleus of an atom. These shells are represented by the letters K, L, M, N, and so on, with the K shell being the closest to the nucleus. The distribution of electrons in these shells follows certain rules and patterns.

1. Shell Capacity
Each shell has a specific capacity to hold a certain number of electrons. The capacity of each shell is given by the formula 2n², where 'n' represents the shell number. For example, the K shell can hold a maximum of 2 electrons (2 x 1²), the L shell can hold a maximum of 8 electrons (2 x 2²), and so on.

2. Aufbau Principle
The Aufbau principle states that electrons occupy the lowest energy level available before filling higher energy levels. This means that electrons will first fill the K shell before moving on to the L shell, and so on.

3. Pauli Exclusion Principle
The Pauli exclusion principle states that no two electrons in an atom can have the same set of quantum numbers. In other words, each electron in an atom must have its own unique set of quantum numbers, which include the principal quantum number (n), the azimuthal quantum number (l), the magnetic quantum number (m), and the spin quantum number (s).

4. Hund's Rule
Hund's rule states that when filling orbitals of equal energy, electrons will occupy separate orbitals before pairing up. This means that if there are multiple orbitals of the same energy level, one electron will go into each orbital before any of them pair up.

5. Electron Configuration
Electron configuration is a shorthand notation used to represent the distribution of electrons in different shells. It is written in the form of numbers and letters, where the numbers represent the shell and the letters represent the subshell. For example, the electron configuration for carbon (Z = 6) is 1s² 2s² 2p², indicating that carbon has 2 electrons in the 1s shell, 2 electrons in the 2s shell, and 2 electrons in the 2p shell.

Conclusion
In summary, electrons are distributed in different orbits or shells around the nucleus of an atom. This distribution follows specific rules such as the shell capacity, Aufbau principle, Pauli exclusion principle, and Hund's rule. Understanding the electron distribution in atoms is crucial for determining the chemical properties and behavior of elements.