When is an electron considered to be at ground state?
when it is paired with another electron with an opposite spin
when it moves around the nucleus in a circular motion
when it is at its lowest possible energy state
when it has undergone a change in energy
An electron is considered to be at its ground state when it is at its lowest possible energy level. This means that it is in the most stable configuration and has not undergone any changes in energy. One way to determine the electron's ground state is by considering its placement in an atom. In atoms, electrons occupy specific energy levels or shells around the nucleus. The closest energy level to the nucleus is called the 1s orbital, followed by the 2s, 2p, 3s, and so on.
In each energy level, there are sublevels or orbitals where electrons can be found. A single orbital can hold a maximum of two electrons, and when two electrons occupy the same orbital, they must have opposite spins. This is known as Hund's rule. Therefore, when an electron is paired with another electron in the same orbital with opposite spins, it is considered to be in its ground state. This ensures that the electrons are in the most stable arrangement, minimizing their electrostatic repulsion.