The orbital picture of an electron in an atom is just another representation of the solutions of the Schrodinger equation describing the states of an electron inside an atom. The Schrodinger equation gives you different possible energy states of the electron in an atom along with their wavefunctions.
If you are familiar with the basics of quantum mechanics, we know that the wave function gives a complete description of the properties of electrons. One such property is the probability to find an electron at a given position in space. The popular drawings of the orbitals like $s, p, d$, and $f$ are the probability distributions and do not represent any potential in the space, and therefore do not correspond to its potential energy. The plots also do not give us any information about the kinetic energy of the electron either.
Coming to the commonly used phrase "energy of orbital", it only means the energy of the electron which is in the state represented by the s-orbital. For example, if one says that s-orbital energy of a Hydrogen atom is -13.6 eV, it means that an electron that has the wave function of an s-orbital has an energy of -13.6 eV.
Do remember that the "shapes of the orbitals" is a wrong term to use. Rather, the orbitals have a positional probability distribution in those shapes, and they represent, more accurately, the wavefunction of the electron in the atom.
Edit: Do note that I am only talking about a single electron in an atom. If there are more than 1 electrons, then the description in the other answer makes complete sense. I was only explaining the terms used, what energy means and clear any confusion.