Advertisements
Advertisements
प्रश्न
Explain why inspite of nearly the same electronegativity, oxygen forms hydrogen bonding while chlorine does not.
Advertisements
उत्तर १
- Both nitrogen (N) and chlorine (Cl) have an electronegativity of 3.0.
- However, only nitrogen is involved in the hydrogen bonds (e.g., NH3) and not chlorine.
- This is due to the smaller atomic size of nitrogen (atomic radius = 70 pm) as compared to chlorine (atomic radius = 99 pm), therefore, N can cause greater polarisation of N-H bond than Cl in the case of Cl-H bond.
- Consequently, the N atom is involved in hydrogen bonding and not chlorine.
उत्तर २
Despite having almost identical electronegativity values, O and Cl have very different atomic sizes (O = 66 pm, Cl = 99 pm). Because of this, the electron density of the O atom is significantly higher than that of the Cl atom. As a result, although chlorine cannot form hydrogen bonds, oxygen can.
संबंधित प्रश्न
Account for the following : There is large difference between the melting and boiling points of oxygen and sulphur.
Give reasons for the following : H2Te is the strongest reducing agent amongst all the hydrides of Group 16 elements.
Give reasons for the following : Oxygen has less electron gain enthalpy with negative sign than 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?
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).
Arrange the following in the order of property indicated for the given set:
F2, Cl2, Br2, I2 - increasing bond dissociation enthalpy.
Give reasons Thermal stability decreases from H2O to H2Te.
Arrange the following in the order of the property indicated against set :
H2O, H2S, H2Se, H2Te − increasing acidic character.
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:
The formation of \[\ce{O^+_2[PtF6]^-}\] is the basis for the formation of first xenon compound. This is because ____________.
Strong reducing behaviour of \[\ce{H3PO2}\] is due to ______.
Out of \[\ce{H2O}\] and \[\ce{H2S}\], which one has higher bond angle and why?
In forming (i) \[\ce{N2 -> N^{+}2}\] and (ii) \[\ce{O2 -> O^{+}2}\]; the electrons respectively are removed from:
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)
______ is a gaseous element of group 16.
