Explain the directional properties of bonds using $VB$ theory.
(N/A) The covalent bond is formed by the overlapping of atomic orbitals.
The molecule of hydrogen is formed due to the overlap of $1s$ orbitals of two $H$ atoms.
In the case of polyatomic molecules like $CH_4$,$NH_3$,and $H_2O$,the geometry of the molecules is also important in addition to the bond formation.
In $CH_4$,the shape is tetrahedral and the $H-C-H$ bond angle is $109.5^{\circ}$. $NH_3$ has a pyramidal shape.
To explain these directional properties,the concept of hybridization of atomic orbitals is required.
The molecule of hydrogen is formed due to the overlap of $1s$ orbitals of two $H$ atoms.
In the case of polyatomic molecules like $CH_4$,$NH_3$,and $H_2O$,the geometry of the molecules is also important in addition to the bond formation.
In $CH_4$,the shape is tetrahedral and the $H-C-H$ bond angle is $109.5^{\circ}$. $NH_3$ has a pyramidal shape.
To explain these directional properties,the concept of hybridization of atomic orbitals is required.
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View SolutionMatch the following:
| List-$I$ (Molecule/ion) | List-$II$ (Hybridisation) |
| :--- | :--- |
| $(A)$ $ICl_4^-$ | $(P)$ $sp^3$ |
| $(B)$ $NO_3^-$ | $(Q)$ $sp^3d$ |
| $(C)$ $PCl_4^+$ | $(R)$ $sp^3d^2$ |
| $(D)$ $SiF_6^{2-}$ | $(S)$ $sp^2$ |
| | $(T)$ $sp$ |
| List-$I$ (Molecule/ion) | List-$II$ (Hybridisation) |
| :--- | :--- |
| $(A)$ $ICl_4^-$ | $(P)$ $sp^3$ |
| $(B)$ $NO_3^-$ | $(Q)$ $sp^3d$ |
| $(C)$ $PCl_4^+$ | $(R)$ $sp^3d^2$ |
| $(D)$ $SiF_6^{2-}$ | $(S)$ $sp^2$ |
| | $(T)$ $sp$ |
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