Electrons in atoms are described by different types of orbitals, which are characterized by their shape, energy, and orientation. The different types of orbitals are named after the subshells they belong to. The main types of orbitals are:
s Orbitals: The s orbitals are spherical in shape and have no angular nodes. They are denoted by the letter "s" and can hold a maximum of 2 electrons. The s subshell consists of only one s orbital. Examples include the 1s, 2s, 3s orbitals, and so on.
p Orbitals: The p orbitals are dumbbell-shaped and have two lobes with a node at the center. They come in sets of three perpendicular orbitals labeled as px, py, and pz. Each p orbital can hold a maximum of 2 electrons. The p subshell consists of three p orbitals, allowing for a total of 6 electrons. Examples include the 2p, 3p, 4p orbitals, and so on.
d Orbitals: The d orbitals are more complex in shape and have four lobes with donut-shaped regions in between. There are five d orbitals: dxy, dxz, dyz, dx²-y², and dz². Each d orbital can hold a maximum of 2 electrons, allowing for a total of 10 electrons in the d subshell. Examples include the 3d, 4d, 5d orbitals, and so on.
f Orbitals: The f orbitals have intricate shapes and are composed of eight lobes with complex nodal patterns. There are seven f orbitals: fy(3x²-y²), fz(x²-y²), fxz, fyz, fxy, fxyz, and fz³. Each f orbital can hold a maximum of 2 electrons, accommodating a total of 14 electrons in the f subshell. Examples include the 4f, 5f, 6f orbitals, and so on.
It's important to note that each orbital can hold a maximum of 2 electrons, and the energy levels increase as you move further from the nucleus (e.g., 1s < 2s < 2p < 3s < 3p, and so on). The arrangement and occupation of electrons in these orbitals follow specific rules outlined in the principles of quantum mechanics and electron configuration.