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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
Give reasons Thermal stability decreases from H2O to H2Te.
Explain the following properties of group 16 elements :
1) Electro negativity
2) Melting and boiling points
3) Metallic character
4) Allotropy
Give a reason for the following:
Fluorine gives only one oxide but chlorine gives a series of oxides.
Arrange the following in order of the property indicated set.
HF, HCl, HBr, HI - decreasing bond enthalpy.
The formation of \[\ce{O^+_2[PtF6]^-}\] is the basis for the formation of first xenon compound. This is because ____________.
Which of the following statement is incorrect?
The correct order of ΔiHs among the following elements is
These are physical properties of an elements.
- Sublimation enthalpy
- Ionisation enthalpy
- Hydration enthalpy
- Electron gain enthalpy
The total number of above properties that affect the reduction potential is ______. (Integer answer)
