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On hybridisation of one s and three p-orbitals, we get
- a)Four orbitals with tetrahedral orientation
- b)Three orbitals with trigonal orientation
- c)Two orbitals with linear orientation
- d)Two orbitals with perpendicular orientation
Correct answer is option 'A'. Can you explain this answer?
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On hybridisation of one s and three p-orbitals, we geta)Four orbitals ...
Four sp3 hybrid orbitals are formed when one sand three p-orbitals hybridise.
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On hybridisation of one s and three p-orbitals, we geta)Four orbitals ...
**Explanation:**
When one s orbital and three p orbitals undergo hybridization, they form four sp³ hybrid orbitals. These hybrid orbitals have a tetrahedral orientation.
**Hybridization:**
Hybridization is a concept used in chemistry to describe the mixing of atomic orbitals to form new hybrid orbitals. It is used to explain the geometry of molecules and the bonding properties of atoms.
In the case of one s orbital and three p orbitals, they can hybridize to form four sp³ hybrid orbitals. The s orbital and the three p orbitals combine and rearrange to form four hybrid orbitals.
**Tetrahedral Orientation:**
The sp³ hybrid orbitals resulting from the hybridization have a tetrahedral orientation. This means that they are arranged in a three-dimensional shape resembling a tetrahedron, with the four hybrid orbitals pointing towards the four corners of the tetrahedron.
**Importance of Hybridization:**
Hybridization is important because it allows for the formation of strong sigma bonds in molecules. These sigma bonds are formed by the overlap of hybrid orbitals with other atomic orbitals or hybrid orbitals of other atoms.
In the case of sp³ hybridization, the resulting hybrid orbitals have 25% s character and 75% p character. This means that they are intermediate in shape between an s orbital and a p orbital. The hybrid orbitals have a greater directional character compared to the pure p orbitals, allowing for better overlap and stronger bonding.
**Conclusion:**
In conclusion, when one s orbital and three p orbitals undergo hybridization, they form four sp³ hybrid orbitals with a tetrahedral orientation. This is an important concept in understanding the geometry and bonding properties of molecules.
When one s orbital and three p orbitals undergo hybridization, they form four sp³ hybrid orbitals. These hybrid orbitals have a tetrahedral orientation.
**Hybridization:**
Hybridization is a concept used in chemistry to describe the mixing of atomic orbitals to form new hybrid orbitals. It is used to explain the geometry of molecules and the bonding properties of atoms.
In the case of one s orbital and three p orbitals, they can hybridize to form four sp³ hybrid orbitals. The s orbital and the three p orbitals combine and rearrange to form four hybrid orbitals.
**Tetrahedral Orientation:**
The sp³ hybrid orbitals resulting from the hybridization have a tetrahedral orientation. This means that they are arranged in a three-dimensional shape resembling a tetrahedron, with the four hybrid orbitals pointing towards the four corners of the tetrahedron.
**Importance of Hybridization:**
Hybridization is important because it allows for the formation of strong sigma bonds in molecules. These sigma bonds are formed by the overlap of hybrid orbitals with other atomic orbitals or hybrid orbitals of other atoms.
In the case of sp³ hybridization, the resulting hybrid orbitals have 25% s character and 75% p character. This means that they are intermediate in shape between an s orbital and a p orbital. The hybrid orbitals have a greater directional character compared to the pure p orbitals, allowing for better overlap and stronger bonding.
**Conclusion:**
In conclusion, when one s orbital and three p orbitals undergo hybridization, they form four sp³ hybrid orbitals with a tetrahedral orientation. This is an important concept in understanding the geometry and bonding properties of molecules.
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On hybridisation of one s and three p-orbitals, we geta)Four orbitals with tetrahedral orientationb)Three orbitals with trigonal orientationc)Two orbitals with linear orientationd)Two orbitals with perpendicular orientationCorrect answer is option 'A'. Can you explain this answer?
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