in paramagnetic ions all the bonds formed between Mn and O are covalent,why?
There may be a number of reasons. One is that the electrons in Mn and O are shared and not transferred but this may not be the answer you are looking for.
To understand why the bonds formed between manganese (Mn) and oxygen (O) in paramagnetic ions are covalent, we need to consider a few key factors.
1. Electronic configuration: Manganese typically has an electronic configuration of [Ar] 3d⁵ 4s². This means that it has five unpaired electrons in its d-orbital, making it highly reactive and likely to form covalent bonds.
2. Oxygen's electron affinity: Oxygen has a high electronegativity and strong electron affinity. It readily accepts electrons, making it capable of forming covalent bonds.
3. Octet rule: Both manganese and oxygen strive to achieve a stable electronic configuration by either gaining or losing electrons to achieve a full valence shell. In this case, Mn could lose electrons or gain electrons from O, but gaining electrons would be more favorable due to its lower ionization energy.
When manganese and oxygen come together to form a compound, such as manganese oxide (MnO), they share electrons in a covalent bond. In this bonding arrangement, oxygen primarily gains two electrons from manganese, resulting in an ionic-like interaction. However, due to the covalent nature of the bond, there is also electron density overlapping between the manganese and oxygen atoms.
It's important to note that while the majority of the bonding between Mn and O is covalent, there can be some degree of ionic character as well. The strength and extent of this covalent-ionic character can vary depending on factors such as the oxidation state of manganese and the specific compound being formed.