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
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)
Give reasons for the following : H2Te is the strongest reducing agent amongst all the hydrides of Group 16 elements.
Write the order of thermal stability of the hydrides of Group 16 elements.
Which of the following does not react with oxygen directly?
Zn, Ti, Pt, Fe
Why does NH3 form hydrogen bond but PH3 does not?
The HNH angle value is higher than HPH, HAsH and HSbH angles. Why? [Hint: Can be explained on the basis of sp3 hybridisation in NH3 and only s−p bonding between hydrogen and other elements of the group].
Justify the placement of O, S, Se, Te and Po in the same group of the periodic table in terms of electronic configuration, oxidation state and hydride formation.
Arrange the following in the order of property indicated for the given set:
F2, Cl2, Br2, I2 - increasing bond dissociation enthalpy.
Arrange the following in the order of the property indicated against set :
H2O, H2S, H2Se, H2Te − increasing acidic character.
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 ____________.
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:
Strong reducing behaviour of \[\ce{H3PO2}\] is due to ______.
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)
