In an atom, there are five d orbitals, which are designated as dxy, dxz, dyz, dx^2-y^2, and dz^2. These d orbitals belong to the d-subshell and have different spatial orientations within the atom.
The dxy orbital is shaped like a four-leaf clover and lies in the xy-plane. It has two lobes along the x and y axes and a nodal plane along the z-axis.
The dxz and dyz orbitals are similar in shape but differ in their orientation. The dxz orbital has lobes along the x and z axes, while the dyz orbital has lobes along the y and z axes. Both orbitals have a nodal plane in the xy-plane.
The dx^2-y^2 orbital is often depicted as a four-lobed shape, similar to a double dumbbell. It lies along the x and y axes and has two lobes along the diagonals and two nodal planes along the axes.
The dz^2 orbital has a doughnut-shaped region around the z-axis and has a nodal plane in the xy-plane.
These d orbitals play a crucial role in determining the shape and geometry of chemical bonds, as well as the electronic properties of transition metals and their compounds.