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प्रश्न
Give reactions for the following:
O – O single bond is weaker than S – S single bond.
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उत्तर
Due to smaller size of ‘O’ as compared to ‘S’. Smaller size of O leads to smaller O–O bond length. As a result, the lone pair of electrons on the both O atoms repel each other leading to instability or weakening of O–O bond. S is relatively larger so an repulsion between lone pair electrons.
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संबंधित प्रश्न
a. Explain the trends in the following properties with reference to group 16:
1 Atomic radii and ionic radii
2 Density
3 ionisation enthalpy
4 Electronegativity
b. In the electolysis of AgNO3 solution 0.7g of Ag is deposited after a certain period of time. Calulate the quantity of electricity required in coulomb. (Molar mass of Ag is 107.9g mol-1)
Give reasons for the following : Oxygen has less electron gain enthalpy with negative sign than sulphur.
Why does NH3 form hydrogen bond but PH3 does not?
Knowing the electron gain enthalpy values for \[\ce{O -> O-}\] and \[\ce{O -> O^{2-}}\] 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).
Why are halogens strong oxidising agents?
Explain why inspite of nearly the same electronegativity, oxygen forms hydrogen bonding while chlorine does not.
Arrange the following in the order of the property indicated against set :
H2O, H2S, H2Se, H2Te − increasing acidic character.
The boiling points of hydrides of group 16 are in the order:
In forming (i) \[\ce{N2 -> N^{+}2}\] and (ii) \[\ce{O2 -> O^{+}2}\]; the electrons respectively are removed from:
______ is a radioactive element in group 16 elements.
