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प्रश्न
Why are halogens strong oxidising agents?
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उत्तर १
The general electronic configuration of halogens is np5, where n = 2-6. Thus, halogens need only one more electron to complete their octet and to attain the stable noble gas configuration. Also, halogens are highly electronegative with low dissociation energies and high negative electron gain enthalpies. Therefore, they have a high tendency to gain an electron. Hence, they act as strong oxidizing agents.
उत्तर २
Halogens are strong oxidising agents because:
- They have a strong tendency to gain one electron to achieve a noble gas configuration.
- This is due to their high electronegativity and high negative electron gain enthalpy.
- Halogens readily gain electrons, undergoing reduction, which makes them strong oxidisers.
- The oxidising power decreases from fluorine to iodine due to decreasing standard reduction potential.
- Halogens with lower atomic numbers can displace halide ions of halogens with higher atomic numbers from their salts.
संबंधित प्रश्न
Account for the following: Oxygen shows catenation behavior less than sulphur.
Give reasons for the following : H2Te is the strongest reducing agent amongst all the hydrides of Group 16 elements.
List the important sources of sulphur.
Write the order of thermal stability of the hydrides of Group 16 elements.
Why is H2O a liquid and H2S a gas?
Why does NH3 form hydrogen bond but PH3 does not?
Give reasons Thermal stability decreases from H2O to H2Te.
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.
Arrange the following in order of the property indicated set.
HF, HCl, HBr, HI - decreasing bond enthalpy.
The boiling points of hydrides of group 16 are in the order:
Which of the following statement is incorrect?
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:
Strong reducing behaviour of \[\ce{H3PO2}\] is due to ______.
Out of \[\ce{H2O}\] and \[\ce{H2S}\], which one has higher bond angle and why?
The correct order of ΔiHs among the following elements is
______ is a radioactive element in group 16 elements.
