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Chapter 1: Problem 9

Would you expect \(\mathrm{He}_{2} \oplus\) to be more stable than \(\mathrm{He}_{2}\) ? Than \(\mathrm{He}\) ?

Short Answer

Expert verified
In conclusion, \(\mathrm{He}_{2} \oplus\) is more stable than \(\mathrm{He}_{2}\) due to bond formation. However, it is difficult to conclusively say if it is more stable than \(\mathrm{He}\) without further details such as bond dissociation energy or other factors that contribute to their stabilities.

Step by step solution

01

Identify electronic configurations

To compare the stabilities of these species, we first need to determine their electronic configurations. Here are the electronic configurations of the ground state: - \(\mathrm{He}\): 1s\(^2\) - \(\mathrm{He}_{2}\): (1s\(_{A}$$)^2\) (1s\(_{B}$$)^2\) where A and B represent the two helium atoms. - \(\mathrm{He}_{2} \oplus\): (1s\(_{A}$$)^2\) (1s\(_{B}$$)^1\) (one electron is removed)
02

Analyze bond formation

Now, let's analyze the bond formation for \(\mathrm{He}_{2}\) and \(\mathrm{He}_{2} \oplus\): - \(\mathrm{He}_{2}\): There are four electrons, and since the 1s orbital can only accommodate two electrons, there are no available orbitals for bond formation, making \(\mathrm{He}_{2}\) unstable and less likely to exist. - \(\mathrm{He}_{2} \oplus\): There are three electrons. The two electrons from 1s\(_{A}\) and one electron from 1s\(_{B}\) can occupy molecular orbitals, promoting bond formation and making \(\mathrm{He}_{2} \oplus\) more stable than \(\mathrm{He}_{2}\).
03

Compare with \(\mathrm{He}\) stability

Finally, let's compare the stability of \(\mathrm{He}_{2} \oplus\) and \(\mathrm{He}\). Because \(\mathrm{He}\) is a noble gas and has a filled 1s orbital, it is relatively stable. However, it is necessary to consider the bond dissociation energy to compare their stability: - \(\mathrm{He}_{2} \oplus\): The bond dissociation energy (energy required to break the bond) is positive, meaning it is stable. - \(\mathrm{He}\): No bond exists, and the species is overall stable due to its full 1s orbital.
04

Conclusion

In conclusion, we would expect \(\mathrm{He}_{2} \oplus\) to be more stable than \(\mathrm{He}_{2}\) because it has a bond formation that makes it more stable. While \(\mathrm{He}_{2} \oplus\) is also stable, it is difficult to conclusively say if it is more stable than \(\mathrm{He}\) without knowing further details such as bond dissociation energy or other factors that contribute to their stabilities.

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What are the characteristics which ionic, ion-dipole, and dipole-dipole bonds have in common? How do they differ?

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