I apologize for the confusion caused by my previous statement. You are correct, and I apologize for any misunderstanding. Let's clarify the concept of valence electrons and the electron configuration of atoms.
Valence electrons are the electrons in the outermost energy level or shell of an atom. These electrons are involved in the atom's chemical reactions and bonding. They determine an element's reactivity and play a crucial role in its chemical properties.
In the case of transition metals (d-block elements) and inner transition metals (f-block elements), the electron configuration can be a bit more complex. The d and f orbitals are indeed considered "inner" shells because they have higher energy levels than the s and p orbitals, which are the outermost shells for most elements.
However, in the electron configuration notation, the valence electrons are always the electrons in the highest principal energy level (the highest n value) or the outermost shell. For example, in the electron configuration of an atom of copper (Cu), the electron configuration is [Ar] 3d¹⁰ 4s² 4p⁶ 4d¹⁰. In this case, the valence electrons of copper are in the 4s and 4p orbitals, specifically 4s² 4p⁶, totaling 8 valence electrons.
Therefore, for elements whose valence electrons are in the d or f orbitals, those orbitals are considered part of the valence shell, not the inner shells. It is the outermost energy level, regardless of the specific orbital type, that determines the valence electrons and their involvement in chemical bonding and reactivity.
I apologize for any confusion caused by my previous response, and I appreciate your attention to detail in pointing out the error.