Answer:
a) Mo the electron configuration: 42Mo: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d4
Mo3+ - is Paramagnetic
b) Au - [Xe] 4f14 5d10 6s1
For Au+ is not paramagnetic
c) Mn - [Ar] 3d5 4s2
Mn2+ is paramagnetic
d)Hf -[Xe] 4f¹⁴ 5d² 6s²
Hf2+ is not paramagnetic
Explanation:
An atom becomes positively charged when it looses an electron.
Diamagnetism in atom occurs whenever two electrons in an orbital paired equalises with a total spin of 0.
Paramagnetism in atom occurs whenever at least one orbital of an atom has a net spin of electron. That is a paramagnetic electron is just an unpaired electron in the atom.
Here is a twist even if an atom have ten diamagnetic electrons, the presence of at least one paramagnetic electron, makes it to be considered as a paramagnetic atom.
Simply put paramagnetic elements are one that have unpaired electrons, whereas diamagnetic elements do have paired electron.
Paramagnetic species are species that contain unpaired electrons.
The ground state is the lowest energy state of an atom. Electron configuration refers to the arrangement of electrons in an atom into energy levels and orbitals. A chemical specie is paramagnetic if it contains unpaired electrons.
The electron configuration of Mo³⁺ is [Kr]4d3. The ion is paramagnetic because it has three unpaired electrons.
The electron configuration of Au⁺ is [Xe] 4f14 5d10. The ion is diamagnetic because there all electrons are paired.
The electron configuration of Mn²⁺ is [Ar] 3d5. There are five unpaired electrons in the ion hence the ion is paramagnetic.
The electron configuration of Hf²⁺ is [Xe] 4f^14 5d^2. The ion is paramagnetic because there are two unpaired electrons present.
Learn more: https://brainly.com/question/5624100
