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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
Account for the following : There is large difference between the melting and boiling points of oxygen and sulphur.
List the important sources of sulphur.
Write the order of thermal stability of the hydrides of Group 16 elements.
Why are halogens strong oxidising agents?
Explain why inspite of nearly the same electronegativity, oxygen forms hydrogen bonding while chlorine does not.
Give a reason for the following:
Fluorine gives only one oxide but chlorine gives a series of oxides.
The boiling points of hydrides of group 16 are in the order:
Match the items of Columns I and II and mark the correct option.
| Column I | Column II |
| (A) \[\ce{H2SO4}\] | (1) Highest electron gain enthalpy |
| (B) \[\ce{CCl3NO2}\] | (2) Chalcogen |
| (C) \[\ce{Cl2}\] | (3) Tear gas |
| (D) Sulphur | (4) Storage batteries |
Given below are two statements labelled as Assertion (A) and Reason (R).
Assertion (A): Electron gain enthalpy of oxygen is less than that of Flourine but greater than Nitrogen.
Reason (R): Ionisation enthalpies of the elements follow the order Nitrogen > Oxygen > Fluorine.
Select the most appropriate answer from the options given below:
Out of \[\ce{H2O}\] and \[\ce{H2S}\], which one has higher bond angle and why?
