So, I assumed a pair of electron and proton to behave as a dipole

Classicaly, this is correct. It would behave as a dipole.

But in quantum mechanics we don't talk about a localised electron  ,but about orbitals. This is because particles have an associated wavefunction $\psi(t)$, which tells you the probability of finding your particle at a particular place.

In the case of an electron and a proton (hydrogen atom), the orbital has spherical symmetry. This means that the will be no net charge.

So, I assumed a pair of electron and proton to behave as a dipole

Classically, this is correct. It would behave as a dipole.

But in quantum mechanics we don't talk about a localized electron, but about orbitals. This is because particles have an associated wavefunction $\psi(t)$, which tells you the probability of finding your particle at a particular place.

In the case of an electron and a proton (hydrogen atom), the orbital has spherical symmetry. This means that the will be no net charge.

So, I assumed a pair of electron and proton to behave as a dipole

Classicaly, this is correct.

But in quantum mechanics we don't talk about a localised electron ,but a wavefunction.

In the case of an electron and proton (hydrogen), the orbital has spherical symmetry. This means that the will be no net charge.

So, I assumed a pair of electron and proton to behave as a dipole

Classicaly, this is correct. It would behave as a dipole.

But in quantum mechanics we don't talk about a localised electron ,but about orbitals. This is because particles have an associated wavefunction $\psi(t)$, which tells you the probability of finding your particle at a particular place.

In the case of an electron and a proton (hydrogen atom), the orbital has spherical symmetry. This means that the will be no net charge.