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प्रश्न
Give reasons for the following : Oxygen has less electron gain enthalpy with negative sign than sulphur.
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उत्तर
The elements of group 16 have two electrons less than the nearest noble gas configuration. Therefore, they have a high tendency to accept two additional electrons and hence have large negative electron gain enthalpies next only to the halogens. The electron gain enthalpy of oxygen is however least negative in this group. This is due to its small size. As a result of which, the electron – electron repulsions in the relatively small 2p-subshell are comparatively large and hence the incoming electrons are not accepted with the same ease in case of other elements of this group.
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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)
Which of the following does not react with oxygen directly?
Zn, Ti, Pt, Fe
Explain why inspite of nearly the same electronegativity, oxygen forms hydrogen bonding while chlorine does not.
Explain the following properties of group 16 elements :
1) Electro negativity
2) Melting and boiling points
3) Metallic character
4) Allotropy
Give reactions for the following:
O – O single bond is weaker than S – S single bond.
Give a reason for the following:
Fluorine gives only one oxide but chlorine gives a series of oxides.
The formation of \[\ce{O^+_2[PtF6]^-}\] is the basis for the formation of first xenon compound. This is because ____________.
The correct order of ΔiHs among the following elements is
What is the basicity of \[\ce{H3PO4}\]?
______ is a gaseous element of group 16.
