Answer
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Hint: The shape of $A{{B}_{5}}$ molecule with zero lone pair is trigonal bipyramidal and with 4 bond pairs and one lone pair is T- shape and with 3 bond pair and 2 lone pairs is T- shape .We need to know about VSEPR theory for more details.
Complete step by step answer:
- VSEPR theory is defined as the electron pairs surrounding the atom present in the centre that must be arranged in space in such a distance so as to minimize the electrostatic repulsion experienced between them.
- The most important rule of the VSEPR theory states that the bond angles about a central atom are those that minimize the overall repulsion which is experienced between the Electron pairs in the valence shell of the atom.
- As the interior angle increases, the repulsion forces decrease sharply. As the value of electronegativity of an atom forming a molecule gets increased, the influence of a bonding electron pair decreases.
- Multiple bonds behave similar to a single electron pair for the sake of VSEPR bond theory.
- Hybridization of an atom can be found out by calculating the summation of lone pairs and sigma bonds.
If a sum of sigma bonds and lone pairs is 2, we have sp hybridization
If a sum of sigma bonds and lone pairs is 3 , we have $s{{p}^{2}}$ hybridization
If a sum of sigma bonds and lone pairs is 4 , we have $s{{p}^{3}}$ hybridization
If a sum of sigma bonds and lone pairs is 5, we have $s{{p}^{3}}d$ hybridization
If a sum of sigma bonds and lone pairs is 6, we have $s{{p}^{3}}{{d}^{2}}$ hybridization.
So the given molecule has 4 sigma bonds 1 lone pair that the sum is 5. So its hybridization is $s{{p}^{3}}d$ and therefore the shape is see saw.
So, the correct answer is “Option B”.
Note:
As a result of the distortions created different types of shapes can be drawn :
Complete step by step answer:
- VSEPR theory is defined as the electron pairs surrounding the atom present in the centre that must be arranged in space in such a distance so as to minimize the electrostatic repulsion experienced between them.
- The most important rule of the VSEPR theory states that the bond angles about a central atom are those that minimize the overall repulsion which is experienced between the Electron pairs in the valence shell of the atom.
- As the interior angle increases, the repulsion forces decrease sharply. As the value of electronegativity of an atom forming a molecule gets increased, the influence of a bonding electron pair decreases.
- Multiple bonds behave similar to a single electron pair for the sake of VSEPR bond theory.
- Hybridization of an atom can be found out by calculating the summation of lone pairs and sigma bonds.
If a sum of sigma bonds and lone pairs is 2, we have sp hybridization
If a sum of sigma bonds and lone pairs is 3 , we have $s{{p}^{2}}$ hybridization
If a sum of sigma bonds and lone pairs is 4 , we have $s{{p}^{3}}$ hybridization
If a sum of sigma bonds and lone pairs is 5, we have $s{{p}^{3}}d$ hybridization
If a sum of sigma bonds and lone pairs is 6, we have $s{{p}^{3}}{{d}^{2}}$ hybridization.
![seo images](https://www.vedantu.com/question-sets/1885a2ef-5df9-497d-9e38-39aefdfe95e36296242765423091763.png)
So the given molecule has 4 sigma bonds 1 lone pair that the sum is 5. So its hybridization is $s{{p}^{3}}d$ and therefore the shape is see saw.
So, the correct answer is “Option B”.
Note:
As a result of the distortions created different types of shapes can be drawn :
Bond pair | Lone pair | Shape |
5 | 0 | Trigonal bipyramidal |
4 | 1 | See saw |
3 | 2 | T shape |
2 | 3 | Linear. |
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