Like the piano on the ground, the atom in its ground state means it is in its lowest energy state. All elements on the periodic table are in their ground states. In the question, the only configuration for a ground state atom is d. It follows the rules for electron configuration filling in the ground state An orbital can only hold 0,1, or 2 electrons.
The electrons must have opposite spins if there are 2 electrons in the orbital. On the other hand, above ground states are "excited states". These are states with higher energy than the one of the ground state. If you shoot the atom with a photon, then the photon may be absorbed, so the electrons of the atom will jump from the ground state to an excited state the difference between the two energies of the final and initial state is the energy of the photon that got absorbed.
In an excited state, not all electrons are in the lowest possible energy levels. For example, in the question, a carbon is not in the ground state, and it doesn't follow Hund's rule.
Jul 26, Related questions How do electron configurations in the same group compare? How do the electron configurations of transition metals differ from those of other elements? How do electron configurations affect properties and trends of a compound? What is the electron configuration for a sodium ion?
What is the electron configuration for a nitride ion? What is the electron configuration of chromium? The ground state configuration is the lowest energy, most stable arrangement.
An excited state configuration is a higher energy arrangement it requires energy input to create an excited state.
Core electrons are electrons that under 'normal' reaction conditions are chemically inert and are in the completely filled inner energy levels. Ian Hunt , Department of Chemistry.
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