Occurrence, Electronic Configuration, Atomic and Ionic Radii, Ionisation Enthalpy, Electron Gain Enthalpy, Electronegativity, Physical Properties and Chemical Properties (Oxidation states and trends in chemical reactivity and Anomalous behaviour of oxygen)
- P Block part 28 (Reaction with hydrogen and oxygen)
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- P Block part 26 (Group 16 trends)
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- P Block part 27 (Oxygen)
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- P Block part 24 (Group 16, oxygen family introduction)
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- P Block part 29 (Reaction with halogens and numerical)
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- P Block part 25 (Group 16 trends)
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- P Block part 38 (Numericals)
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Account for the following : There is large difference between the melting and boiling points of oxygen and sulphur.
Give reasons for the following : Oxygen has less electron gain enthalpy with negative sign than sulphur.
Arrange the following in the order of property indicated for each set:
F2, Cl2, Br2, I2 - increasing bond dissociation enthalpy.
Give reasons for the following : H2Te is the strongest reducing agent amongst all the hydrides of Group 16 elements.
Explain why inspite of nearly the same electronegativity, oxygen forms hydrogen bonding while chlorine does not.
Knowing the electron gain enthalpy values for O → O− and O → O2− as −141 and 702 kJ mol−1 respectively, how can you account for the formation of a large number of oxides having O2− species and not O−? (Hint: Consider lattice energy factor in the formation of compounds).
The HNH angle value is higher than HPH, HAsH and HSbH angles. Why? [Hint: Can be explained on the basis of sp3 hybridisation in NH3 and only s−p bonding between hydrogen and other elements of the group].
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.