Which set of these comparisons is incorrect? (more stable means it has a more negative energy.) a. the 1s orbital in h is more stable than the 1s orbital in he+ b. the 2s orbital in he atom is less stable than the 2s orbital in he+ c. the 2s subshell in li is more stable than the 2p subshell in li?

b.The 2s orbital in He atom is less stable than 2s orbital in He+.

Explanation:

We have to find incorrect comparison

1.The 1 s orbital  in H is more stable than the 1 s orbital in He+

We know that

Atomic number of H=1

Atomic number of He+=1

Configuration of H=

Configuration of He+=

We know that neutral atom is more stable than charged atom.

He atom have two electron before losing one electron but after losing 1 electron it becomes positive ion.

Both have half filled configuration but helium atom attained this configuration after losing on electron.

So, it highly reactive to fill their outer shell.

Therefore, it is less stable.

Therefore, the 1 s orbital of H is more stable than the 1 s orbital of He+.

b.The 2s orbital in He atom is le.ss stable than 2s orbital in He+.

Configuration He=

Configuration of He+=

We know that fully filled or half filled configuration are stable configuration.

Configuration of He is full filled because s orbital can have maximum two electron .

But both cannot have 2 s orbital .

If atom have no 2s orbital then we can not compare stability of 2s orbital  of  He and He+.

So , it is false.

C.The 2s sub-shell in Li is more stable than the 2p sub-shell in Li.

Atomic number of Li=3

Configuration of Li=

We know that s orbital can have maximum 2 electron and p orbital can have maximum 6 electrons.

Half filled or fully filled configuration is more stable configuration .

2s orbital of Li is half filled .Therefore, it is more stable.

Hence, it is true.

b.The 2s orbital in He atom is less stable than 2s orbital in He+.

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.

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