Two electrons can occupy the 2s subshell, and 8 electrons can occupy the 3d subshell.
Cobalt (Co) has 7 electrons in its 3d subshell.
The electron configuration Ar4s²3d⁷ corresponds to the element cobalt (Co), which has an atomic number of 27. In this configuration, "Ar" represents the noble gas argon, which accounts for the first 18 electrons. The 4s² indicates two electrons in the 4s subshell and the 3d⁷ indicates seven electrons in the 3d subshell, totaling 27 electrons for cobalt.
A subshell that contains eight electrons is the 3d subshell. The d subshell can hold a maximum of 10 electrons, but in this case, with eight electrons, it is likely filled with a combination of spin-up and spin-down electrons. Other subshells, such as p (which can hold a maximum of 6 electrons) or s (which can hold a maximum of 2 electrons), cannot contain eight electrons.
The element that contains five electrons in its 3d orbital is manganese (Mn). Manganese has an atomic number of 25, and its electron configuration is [Ar] 4s² 3d⁵. This means it has five electrons in the 3d subshell.
Two electrons can occupy the 2s subshell, and 8 electrons can occupy the 3d subshell.
One Mn atom contains 5 electrons in it's 3d subshell, all of which are unpaired.
Cobalt (Co) has 7 electrons in its 3d subshell.
On the periodic chart, the element with 5 electrons in its 3d orbital can be quickly identified. Elements with partially filled d-orbitals are located in the middle section, the "transitional metals." 3d is the first d-orbital, so we look in the first row of the middle section. This section fills the orbital by one more electron per element, so the one with 5 electrons is the fifth from the left.... Manganese! Atomic number 25.
The electron configuration Ar4s²3d⁷ corresponds to the element cobalt (Co), which has an atomic number of 27. In this configuration, "Ar" represents the noble gas argon, which accounts for the first 18 electrons. The 4s² indicates two electrons in the 4s subshell and the 3d⁷ indicates seven electrons in the 3d subshell, totaling 27 electrons for cobalt.
A subshell that contains eight electrons is the 3d subshell. The d subshell can hold a maximum of 10 electrons, but in this case, with eight electrons, it is likely filled with a combination of spin-up and spin-down electrons. Other subshells, such as p (which can hold a maximum of 6 electrons) or s (which can hold a maximum of 2 electrons), cannot contain eight electrons.
Scandium has 1 3d electron.
In theory all elements have all the orbitals. Zinc has electrons in four of them.
Neutral arsenic has 33 protons and 33 electrons. The first 33 electron orbitals are filled as 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3. The superscripts above these subshells is the number of electrons in them.
There are 3d^10 electrons in arsenic, as it is located in the 4th period of the periodic table.
It's chromium. The element would have lost 2 electrons from the 4s subshell, leaving 3d4 as your valence.
The element that contains five electrons in its 3d orbital is manganese (Mn). Manganese has an atomic number of 25, and its electron configuration is [Ar] 4s² 3d⁵. This means it has five electrons in the 3d subshell.