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प्रश्न
Why does NH3 form hydrogen bond but PH3 does not?
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उत्तर १
Nitrogen is highly electronegative as compared to phosphorus. This causes a greater attraction of electrons towards nitrogen in NH3 than towards phosphorus in PH3. Hence, the extent of hydrogen bonding in PH3 is very less as compared to NH3.
उत्तर २
Nitrogen has an electronegativity value of 3.0, which is much higher than that of H (2.1). As a result, N-H bond is quite polar and hence NH3 undergoes intermolecular H-bonding.
Phosphorus has an electronegativity value of 2.1. Thus, the P–H bond is not polar, and hence PH3 does not undergo H-bonding.
संबंधित प्रश्न
Account for the following: Oxygen shows catenation behavior less than sulphur.
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
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Give reasons: SO2 is reducing while TeO2 is an oxidising agent.
Give reasons for the following : Oxygen has less electron gain enthalpy with negative sign than sulphur.
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?
Which of the following does not react with oxygen directly?
Zn, Ti, Pt, Fe
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.
Draw the structures of `H_3PO_2`
Explain the following properties of group 16 elements :
1) Electro negativity
2) Melting and boiling points
3) Metallic character
4) Allotropy
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Fluorine gives only one oxide but chlorine gives a series of oxides.
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:
Which of the following statements are correct?
(i) \[\ce{CaF2 + H2SO4 -> CaSO4 + 2HF}\]
(ii) \[\ce{2HI + H2SO4 -> I2 + SO2 + 2H2O}\]
(iii) \[\ce{Cu + 2H2SO4 -> CuSO4 + SO2 + 2H2O}\]
(iv) \[\ce{Nacl + H2SO4 -> NaHSO4 + HCl}\]
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______ is a gaseous element of group 16.
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Statement I: The boiling point of hydrides of Group 16 elements follows the order:
H2O > H2Te > H2Se > H2S
Statement II: On the basis of molecular mass, H2O is expected to have a lower boiling point than the other members of the group but due to the presence of extensive H-bonding in H2O, it has a higher boiling point.
In the light of the above statements, choose the correct answer from the options given below:
