When an electron in a certain shell absorbs energy but not enough to enable it to jump to the next shell, the energy is typically converted into kinetic energy of the electron itself. According to the Bohr model of the atom, electrons occupy discrete energy levels or shells, and each shell has a specific energy associated with it.
If an electron in a particular shell absorbs energy, it gains additional kinetic energy, causing it to move to a higher-energy state within that same shell. This higher energy state corresponds to an electron with greater velocity and a higher average distance from the nucleus. The electron remains in the same shell but moves to a higher energy level within that shell.
It's important to note that the distribution of electrons within an atom's energy levels is not solely determined by their energies but also by quantum mechanical principles and the Pauli exclusion principle, which states that no two electrons can occupy the same quantum state. This means that even though electrons in the same shell have the same energy, they have different quantum numbers and occupy different subshells and orbitals within that shell.
If the energy absorbed by an electron is significantly higher, it may have enough energy to overcome the attractive force of the nucleus and transition to a higher shell or even be ionized, causing the electron to leave the atom altogether. However, if the energy is insufficient to reach the next shell, the electron will remain in the same shell but at a higher energy level within it.