What then do we call #1?chemisttree said:#2 is the winner!
Why then is the filling of subshell much more important for chemical properties?Borek said:I don't think it has a special name. Yes, it is a correct number of electrons on each shell, but it is filling of subshells that is much more important for chemical properties. That's why we prefer #2, as it tells as much more.
And yes, thanks to Aufbau principle they are to some degree equivalent.
Because it tells you which orbitals the valence electrons are in, and they are the most important electrons to understand things like the spectrum of atoms and chemical reactivity.Chijioke said:Why then is the filling of subshell much more important for chemical properties?
Chijioke said:Why then is the filling of subshell much more important for chemical properties?
Electronic configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals. It describes the arrangement of electrons around the nucleus of an atom in its different energy levels or shells.
The electronic configuration of an element can be determined using the Aufbau principle, Hund's rule, and the Pauli exclusion principle. Electrons fill orbitals starting from the lowest energy level to the highest, with each orbital holding a maximum of two electrons with opposite spins.
Electronic configuration is crucial in chemistry as it determines an element's chemical properties, reactivity, and placement in the periodic table. It helps predict how an element will interact with others, its ionization energy, electronegativity, and other chemical behaviors.
Some elements have irregular electronic configurations due to electron-electron interactions and the relative energies of orbitals. For example, copper and chromium have configurations that differ from the expected pattern to achieve a more stable, lower-energy state by having half-filled or fully filled d-orbitals.
Notable exceptions to the Aufbau principle include elements like chromium (Cr) and copper (Cu). Instead of following the expected pattern, chromium has an electronic configuration of [Ar] 3d5 4s1, and copper has [Ar] 3d10 4s1. These configurations provide extra stability due to half-filled or fully filled d-subshells.