Which of the following do not exist as stable molecules?

H_{3}

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H - H e

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H e_{2}

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H_{3} O

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Solution

The correct options are
A $H_{3}$
B $H e_{2}$
C $H_{3} O$
D $H - H e$
$H_{3}$ : Hydrogen has $1$ electron in its outer layer. So $2$ Hydrogen could bond and the result is a new $H_{2}$ which has a $2$ -electron in its covalent bond. If you want to add another $H$ to this $H_{2}$ the new electron can not be stable on the same layer.
$H - H e$ : Helium is a stable atom, so the tendency to form a molecule with Hydrogen will be very less.
${H e}_{2}$ : It is unstable as a molecule as it already has a fully filled orbital as a single helium atom. So there is no need of forming a molecule.
$H_{3} O$ : Oxygen just has two unpaired electrons and needs two more to complete its octet. One hydrogen needs one electron to make itself stable. So, here a total of three electrons are required to make the molecule stable, but Oxygen just has two. So, all the hydrogen can not be stabilized.

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Question 19

Which of the following statement is not correct from the view point molecular orbital theory?

(a) $B e_{2}$ is not a stable molecule

(b) $H e_{2}$ is not stable but $H e_{2}^{+}$ is expected to exist.

(d) The order of energies of molecular orbitals in $N_{2}$ molecule is

$σ 2 s < σ^{*} 2 s < σ 2 p_{z} < (π^{*} 2 p_{x} ≃ π^{*} 2 p_{y}) < σ^{*} 2 p_{z}$

H e_{2}

H e

H e_{2}

H_{3} O^{+}

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