Final answer:
A 3d orbital can have various shapes like clover or a 'doughnut' with electron density, with two nodal surfaces and similar energies; while a 4d orbital shares these shapes but is larger due to a higher principal quantum number (n=4), reflecting an increased electron distance probability from the nucleus.
Step-by-step explanation:
The student's question involves drawing a typical 3d orbital and a typical 4d orbital, as well as explaining the differences between them. Due to the constraints of the response format, I cannot physically draw these orbitals, but I can explain their characteristics and differences.
All 3d orbitals contain two nodal surfaces, with shapes varying from clover-shaped in the 3dxy, 3dxz, and 3dyz orbitals, to the more complex 3dz² orbital which resembles a 2pz orbital with a doughnut-shaped electron density in the xy plane. All these orbitals share the same energy levels. In contrast, 4d orbitals are similar in shape to 3d orbitals, but are larger in size due to the higher principal quantum number (n=4). This means that the radial probability distribution extends further from the nucleus, indicating that there's a higher probability of finding an electron at greater distances from the nucleus.
While it's important to recognize that the size of the orbital increases with higher principal quantum numbers, the overall shapes remain consistent with their respective types. For instance, the 4dxy would have the same orientation as the 3dxy, just with a larger radial extent. Similarly, illustrations often depict 3d and 4d orbitals as 'balloon' or 'plump' shapes to more easily visualize their geometry, though actual electron probability distributions might be more complex.