The atomic number of titanium (Ti) is 22, which means it has 22 electrons. When we refer to the "3D orbital" of titanium, we are referring to the 3d subshell, which consists of five orbitals: 3dxy, 3dyz, 3dz^2, 3dxz, and 3dx^2-y^2.
To determine whether the 3d orbital of titanium is partially filled, we need to know the electron configuration of titanium. The electron configuration of titanium can be determined by filling the orbitals in order of increasing energy, following the Pauli exclusion principle and Hund's rule.
The electron configuration of titanium is: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2.
From this electron configuration, we can see that the 3d orbital of titanium is not partially filled. It is only partially filled when it has 5, 6, or 7 electrons, but in the case of titanium, it has only 2 electrons in the 3d orbital. Therefore, we would say that the 3d orbital of titanium is not partially filled.