Justify the placement of O, S, Se, Te and Po in the same group of the periodic table in terms of electronic configuration, oxidation state and hydride formation.

Name: Justify the placement of O, S, Se, Te and Po in the same group of the periodic table in terms of electronic configuration, oxidation state and hydride formation.
Uploaded: Fri, 2019-05-24 11:31
Description: Justify the placement of O, S, Se, Te and Po in the same group of the periodic table in terms of electronic configuration, oxidation state and hydride formation.

7.17 Justify the placement of $O$ , $S$ , $Se$ , $Te$ and $Po$ in the same group of the periodic table in terms of electronic configuration, oxidation state and hydride formation.

Answers (1)

Electronic Configuration-
$O$ , $S$ , $Se$ , $Te$ and $Po$ , all have six valance electron each. The general electronic configuration of these elements is $ns^2,\ np^4$ , where $n$ varies from 2 to 6.
Oxidation state-
As all of these elements have six valence electrons, they should display an oxidation state of -2. The stability of the -2 oxidation state decreases on moving down a group due to a decrease in the electronegativity of the elements. The heavier elements show +2, +4 and +6 oxidation state due to availability of $d$ -orbitals. It also exhibits the oxidation state of -1 ( $H_{2}O_{2}$ ), zero ( $O_{2}$ ), and +2 ( $OF_{2}$ )
Hydrides-
They all form hydrides of formula $H_{2}E$ , where $E = O, S, Se, Te, Po.$ Oxygen and sulphur also form hydrides of type $H_{2}E_{2}$ .These hydrides are volatile in nature.

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Pankaj Sanodiya

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7.17 Justify the placement of , , , and in the same group of the periodic table in terms of electronic configuration, oxidation state and hydride formation.

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Posted by

Pankaj Sanodiya

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7.17 Justify the placement of $O$ , $S$ , $Se$ , $Te$ and $Po$ in the same group of the periodic table in terms of electronic configuration, oxidation state and hydride formation.