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Solution - Justify the placement of O, S, Se, Te and Po in the same group in terms of electronic configuration, oxidation state and hydride formation - CBSE (Science) Class 12 - Chemistry

Question

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.

Solution

The elements of group 16 are collectively called chalcogens.

(i) Elements of group 16 have six valence electrons each. The general electronic configuration of these elements is ns2 np4, where n varies from 2 to 6.

(ii) Oxidation state:

As these elements have six valence electrons (ns2 np4), they should display an oxidation state of −2. However, only oxygen predominantly shows the oxidation state of −2 owing to its high electronegativity. It also exhibits the oxidation state of −1 (H2O2), zero (O2), and +2 (OF2). However, 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 of the group show an oxidation state of +2, +4, and +6 due to the availability of d-orbitals.

(iii) Formation of hydrides:

These elements form hydrides of formula H2E, where E = O, S, Se, Te, PO. Oxygen and sulphur also form hydrides of type H2E2. These hydrides are quite volatile in nature.

Is there an error in this question or solution?

APPEARS IN

 NCERT Chemistry Textbook for Class 12 Part 1 (with solutions)
Chapter 7: The p-block Elements
Q: 17 | Page no. 207

Reference Material

Solution for question: Justify the placement of O, S, Se, Te and Po in the same group in terms of electronic configuration, oxidation state and hydride formation concept: Concept of Group 16 Elements. For the courses CBSE (Science), CBSE (Arts), PUC Karnataka Science, CBSE (Commerce)
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