An electron moves from the 4s sublevel to produce a completely filled 3d sublevel. A completely filled sublevel is more stable. Just because it has a filled d sublevel doesn't prevent it from being a transition metal. It has variable valence (1+ and 2+).
p-block elements have partially filled p-subshell. It is not completely filled.
noble gases.
According to definition, transition elements are those which have partially filled d-subshell in there elementary state or in one of the oxidation states. silver(z=47) can exhibit 2 oxidation state in which it has incompletely filled d-subshell (4d9). hence silver is regarded as trnsition element.
Ground state electron configuration of zinc (Zn): [Ar]3d104s2.
The electron configuration of ytterbium (Yb) is [Xe] 4f14 6s2. This means it has 2 electrons in the 6s subshell and a completely filled 4f subshell.
Argon has completely filled M shell (or 3p orbital)
A transition element are those element who have a partially filled d or f subshell in any common oxidation state. It is also any set of metallic elements occupying a central block in the periodic table such as copper, iron, manganese, and chromium.
p-block elements have partially filled p-subshell. It is not completely filled.
noble gases.
According to definition, transition elements are those which have partially filled d-subshell in there elementary state or in one of the oxidation states. silver(z=47) can exhibit 2 oxidation state in which it has incompletely filled d-subshell (4d9). hence silver is regarded as trnsition element.
There are two ions formed by copper. In copper(I) ion, the 3d orbital is fully filled, and show no transitional behaviour. Whereas copper(II) ion shows transitional characteristics as it has unfilled 3d orbitals. Therefore, copper is a transitional element.
Lutetium (Lu) has no unpaired electrons because it is a transition metal and its electron configuration ends in a fully-filled d subshell.
Ground state electron configuration of zinc (Zn): [Ar]3d104s2.
The electron configurations of chromium (Cr) and copper (Cu) are exceptions to the expected order due to the stability gained from half-filled and fully filled d subshells. For chromium, having a half-filled 3d subshell (3d^5) provides extra stability, so one electron from the 4s subshell is promoted to the 3d subshell, resulting in 3d^5 4s^1. Similarly, for copper, a fully filled 3d subshell (3d^10) is more stable than having one more electron in the 4s subshell (3d^9 4s^2), leading to the configuration of 3d^10 4s^1.
The electron configuration of ytterbium (Yb) is [Xe] 4f14 6s2. This means it has 2 electrons in the 6s subshell and a completely filled 4f subshell.
An example of a situation where an orbital diagram violates the aufbau principle is in the case of chromium (Cr) and copper (Cu). For chromium, one electron is placed in the 4s orbital instead of the 3d orbital to achieve a more stable half-filled or fully filled d subshell. Similarly, for copper, one electron is placed in the 4s orbital before filling the 3d orbital to achieve a more stable fully filled d subshell.
true