Ne2 does not exist but Ne2+ exists.
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It can be explained by means of molecular orbital diagrams.
Ne2
10Ne = 2,8 = 1s2, 2s22p6
10Ne = 2,8 = 1s2, 2s22p6
Molecular Orbital Configuration
(σ1s)2 , (σ*1s)2 , (σ2s)2 , (σ*2s)2 , (σ2p)2 , (π2px)2
= (π2py)2(π*2px)2 = (π*2py)2(σ*2pz)2
Molecular Orbital Diagram
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Bond order = \(\frac{n_b-n_a}{2}\) = \(\frac{6-6}{2}\) = \(\frac{0}{2}\) = 0
Since the bond order no Ne2 is zero it does not exist as a molecule.
However, in case of Ne2+ ,
Bond order = \(\frac{n_b-n_a}{2}\) = \(\frac{6-5}{2}\) = \(\frac{1}{2}\) = 0.5
(Due to positive charge, one election is lost from σ*p antibonding orbital.)
Thus, it is clear that noble gas Ne2 does not exist but Ne2+ exists.
These are the key concepts you need to understand to accurately answer the question.
Understanding the orbital electron configurations of atoms is a foundational concept in chemistry, essential for predicting how atoms will interact and bond with each other. Atoms contain electrons that are arranged in various energy levels or orbitals, following a specific order defined by quantum mechanics.
For noble gases like helium (He) and neon (Ne), their electron configurations are what make them exceptionally stable. Helium possesses a filled 1s orbital, denoted as 1s², meaning it has two electrons in its first and only energy level. Neon, on the other hand, has a configuration of 1s² 2s² 2p', indicating that besides a filled 1s orbital, it also has filled 2s and 2p orbitals. Stability arises from the fact that these orbitals are completely filled, following the octet rule for neon and the 'duet' rule for helium, which is the completion of its only energy shell.
When considering diatomic noble gas molecules, however, a hypothetical combination of their electron configurations might look like 1s' for \(\mathrm{He}_{2}\) or 1s' 2s' 2p¹² for \(\mathrm{Ne}_{2}\), theoretically doubling their electron counts. Nevertheless, nature favors stability, and because these noble gases are already stable as individual atoms, their drive to share or transfer electrons to form molecules is significantly reduced, leading to the non-existence of these diatomic molecules under normal conditions.
The molecular stability of a compound is determined by several factors, including the nature of bond interactions, electron configurations, and the resultant molecular structure. When we consider noble gases, their molecular stability is naturally high when they are in their monoatomic form due to their complete valence electron shells. This characteristic is primarily why they are called 'noble' ' they do not readily react.
For most elements, forming covalent bonds by sharing electrons can lead to a lower energy state, which is more stable. However, for noble gases, their filled valence shells mean they already have low potential energy and are in a preferred stable state. Attempting to form diatomic molecules like \(\mathrm{He}_{2}\) or \(\mathrm{Ne}_{2}\) seems counterintuitive to their inherent stability and is unfavorable due to the introduction of electron-electron repulsion without any energy benefit.
Even when an electron is removed to form positive ions such as \(\mathrm{He}_{2}^{+}\) or \(\mathrm{Ne}_{2}^{+}\), these ions are less stable than the separate atoms themselves. Although the removal of an electron creates an unpaired electron situation, possibly allowing for bonding, it also creates partial shells, which increase the energy of the system. The resultant molecular ions are not favored energetically and hence, less stable than their individual gaseous counterparts.
The noble gas electron configuration is the end goal for many elements undergoing chemical reactions ' to achieve a filled valence shell akin to that of a noble gas. The noble gases possess a unique electron configuration that is highly stable, often referred to as the 'noble gas configuration'. As mentioned previously, helium has a full 1s shell (1s²), and neon has a complete second shell with 1s² 2s² 2p'.
Elements strive to reach this level of stability through chemical bonding, either by shedding electrons, gaining them, or sharing them to complete their outermost electron shells. In contrast, noble gases, including helium and neon, rarely participate in such bonding since they already exhibit this prized electron configuration. The inert nature of noble gases leads to a significant lack of chemical reactivity and thus provides a benchmark for understanding chemical stability. In essence, the noble gas electron configuration epitomizes the chemical stability that other elements are so often seeking to achieve through their reactions.
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