The molecule NE2+ is not stable. Ne2+ is an ion formed by removing one electron from the neon molecule (Ne2).
Regarding its stability, Ne2+ is unstable because neon is a noble gas, meaning it has a full electron configuration and is not prone to gaining or losing electrons. Removing an electron from the stable neon molecule disrupts its electron configuration, making it highly unstable.
Since Ne2+ is an ion formed by removing one electron, it has an odd number of electrons (9). Therefore, it is paramagnetic because it possesses unpaired electrons.
The bond order of Ne2+ can be calculated using the formula:
Bond Order = (Number of bonding electrons - Number of antibonding electrons) / 2
In the case of Ne2+, all 9 electrons are bonding electrons since there are no antibonding orbitals. Therefore, the bond order would be:
Bond Order = (9 - 0) / 2 = 4.5
However, since Ne2+ is an unstable ion, the concept of bond order may not be applicable.
Is Ne2 + stable? Is it diamagnetic or paramagnetic? What is it’s bond order?
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