Types of orbitals in Atom explained

In atomic physics and chemistry, orbitals are regions of space around the nucleus of an atom where electrons are likely to be found. Each type of orbital has a unique shape, size, and orientation in three-dimensional space. Orbitals are described using quantum mechanics, specifically the Schrödinger equation, which provides a mathematical description of the behavior of electrons in atoms.

Types of orbitals

1. s-Orbitals: These are spherical in shape and centered on the nucleus. They are the simplest type of orbital and have only one orientation. An s-orbital can hold a maximum of 2 electrons.

2. p-Orbitals: These have a dumbbell shape with two lobes, one on each side of the nucleus. There are three p-orbitals in each energy level (designated as px, py, and pz), and they are oriented along the x, y, and z axes of a Cartesian coordinate system. Each p-orbital can hold a maximum of 2 electrons, resulting in a total of 6 electrons for the three p-orbitals.

3. d-Orbitals: These are more complex in shape and have five different orientations. They can have various shapes, including cloverleaf, double dumbbell, and even more complex shapes. There are five d-orbitals in each energy level, and they can collectively hold a maximum of 10 electrons.

4. f-Orbitals: These are even more complex than d-orbitals and have seven different orientations. They have intricate shapes and can hold a maximum of 14 electrons. f-orbitals are typically found in the f-block of the periodic table.

5. g-Orbitals: In theory, there are higher-energy g-orbitals with even more complex shapes, but they are not commonly encountered because they occur at very high energy levels and are not found in the electron configurations of elements in the known periodic table.

Electrons fill these orbitals according to the Aufbau principle, Pauli exclusion principle, and Hund's rule

• The Aufbau principle states that electrons fill the lowest energy orbitals first.
• The Pauli exclusion principle states that no two electrons in the same atom can have the same set of quantum numbers, meaning they must have opposite spins.
• Hund's rule states that electrons will fill degenerate orbitals (orbitals with the same energy level) singly before pairing up.

Understanding the various orbitals and how they are filled with electrons is crucial for predicting the chemical behavior of elements and molecules. It forms the basis of the periodic table and helps explain the properties and reactivity of different elements.