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प्रश्न
Nitrogen does not form pentahalide.
Why does nitrogen not form pentahalides?
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उत्तर १
Nitrogen does not form a pentahalide because of the non-availability of the d orbitals in its valence shell.
उत्तर २
- Nitrogen lacks d-orbitals in its valence shell, which are needed to expand its octet.
- Without available d-orbitals, nitrogen cannot accommodate the five covalent bonds required for pentahalides.
- Hence, unlike phosphorus and other group 15 elements, nitrogen cannot form compounds like (PCl5).
- Phosphorus pentachloride forms through (sp3d)-hybridisation and has a trigonal bipyramidal geometry, which nitrogen cannot achieve.
- This is why nitrogen pentahalides are not known in chemistry.
Notes
Students can refer to the provided solutions based on their preferred marks.
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संबंधित प्रश्न
Write four points of differences between properties of nitrogen and other elements of group 15.
Write main differences between the properties of white phosphorus and red phosphorus.
Arrange the following in the increasing order of property mentioned:
NH3, PH3, AsH3, SbH3, BiH3 (Base strength)
The oxidation state of nitrogen in dinitrogen trioxide is ____
(a) + 1
(b) + 2
(c) + 3
(d) + 4
Which of the following has the highest pπ–pπ bonding tendency?
The correct decreasing order of basic strength is:
The correct order of increasing oxidising power is:
H2S is more acidic than H2O because ____________.
Which of the following statements is true?
Which of the following options are not in accordance with the property mentioned against them?
| (i) | \[\ce{F2 > Cl2 > Br2 > I2}\] | Oxidising power. |
| (ii) | \[\ce{MI > MBr > MC1 > MF}\] | Ionic character of metal halide. |
| (iii) | \[\ce{F2 > Cl2 > Br2 > I2}\] | Bond dissociation enthalpy. |
| (iv) | \[\ce{HI < HBr < HCI < HF}\] | Hydrogen-halogen bond strength. |
