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Hybridisation - (Concept)
When atoms are bound together in a molecule, the individual atomic orbitals combine to produce new forms of orbitals that are same in energy and have same size and shape. This process of combining of atomic orbitals is called hybridization and is mathematically accomplished by the linear combination of atomic orbitals, LCAO. The new orbitals that result are called hybrid orbitals.
For example, the valence orbitals in an isolated oxygen atom are a 2s orbital and three 2p orbitals. But the valence orbitals in an oxygen atom in a water molecule differ; they consist of four equivalent hybrid orbitals that point approximately toward the corners of a tetrahedron as shown in the figure given below. Consequently, the overlap of the O and H orbitals should result in a tetrahedral bond angle (109.5°) but the real bond angle in water molecule is 104.5°, this is because of the presence of the lone pairs of electrons in two of the hybrid orbitals.
The salient features and conditions for hybridization:
-
Hybrid orbitals do not exist in isolated atoms. They are formed only in covalently bonded atoms.
-
Hybrid orbitals have shapes and orientations that are very different from those of the atomic orbitals in isolated atoms.
-
A set of hybrid orbitals is generated by combining atomic orbitals. The number of hybrid orbitals in a set is equal to the number of atomic orbitals that were combined to produce the set.
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All orbitals in a set of hybrid orbitals are equivalent in shape and energy.
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The type of hybrid orbitals formed in a bonded atom depends on its electron-pair geometry as predicted by the VSEPR theory.
-
Hybrid orbitals overlap to form σ bonds. Unhybridized orbitals overlap to form π bonds.
Types of Hybridisation
The hybridisation can be of several types depending on the number of hybrid orbitals involved in the formation of molecules. The table given below describes all types of hybridisation and their geometries.
| Exam | Chapter |
| JEE MAIN | Chemical Bonding and Molecular Structure |
The type of hybridisation and number of lone pair (s) of electrons of Xe in $\mathrm{XeOF}_4$ respectively, are :
| A. |
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| B. |
|
| C. |
|
| D. |
|
The correct statement about $\mathrm{ICl}_5$ and $\mathrm{ICl}_4^{-}$is:
| A. |
|
| B. |
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| C. |
|
| D. |
|
The orbitals undergoing Hybridisation involve
| A. |
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| B. |
|
| C. |
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| D. |
|
In which pair of species, both species do have the similar geometry ?
| A. |
|
| B. |
|
| C. |
|
| D. |
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The hybrid orbitals obtained after hybridization of pure atomic orbitals have
| A. |
|
| B. |
|
| C. |
|
| D. |
|
In the hybridisation of one $s$ and one $p$ orbitals, we get
| A. |
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| B. |
|
| C. |
|
| D. |
|
The number of $s p^2$ hybrid orbitals in a molecule of benzene is :
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Which of the following are isostructural pairs?
A. $\mathrm{SO}_4^{2-}$ and $\mathrm{CrO} \mathrm{O}_4^{2-}$
B. $\mathrm{SiCl}_4$ and $\mathrm{TiCl}_4$
C. $\mathrm{NH}_3$ and $\mathrm{NO}_3$
D. $\mathrm{BCl}_3$ and $\mathrm{BrCl}_3$
| A. |
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| B. |
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| C. |
|
| D. |
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Which of the following statement is not correct?
| A. |
|
| B. |
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| C. |
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| D. |
|
Hybridisation involves
| A. |
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| B. |
|
| C. |
|
| D. |
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As the p - character increases, the bond angle in hybrid orbitals formed by s and atomic orbitals
| A. |
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| B. |
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| C. |
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| D. |
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Match List - I with List - II :
| List-I | List-II | ||
| (A) | (I) | ||
| (B) | (II) | ||
| (C) | (III) | ||
| (D) | (IV) |
Choose the most appropriate answer trom the options given below :
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Number of lone pair(s) of electrons on central atom and the shape of $\mathrm{BrF}_3$ molecule respectively, are
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Structure and Hybridisation of $\mathrm{XeO}_2 \mathrm{~F}_2$ is
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The structure of $\mathrm{XeOF}_4$ is
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The hybridisation of B in B2H6 is
| A. |
|
| B. |
|
| C. |
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| D. |
|
The total number of $p \pi-d \pi$ bond in $\mathrm{SO}_3$ is
| A. |
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| B. |
|
| C. |
|
| D. |
|
Which of the following does not form a p - d
bond with another element using its d orbital in the formation of the
bond?
| A. |
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| B. |
|
| C. |
|
| D. |
|
The hybridisation and geometry of SO42- respectively are:
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The hybrid orbitals used by central atoms in molecules are respectively.
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The total number of $\mathrm{Mn}=\mathrm{O}$ bonds in $\mathrm{Mn}_2 \mathrm{O}_7$ is_________.
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Which process will affect the hybridisation of the underlined C atom in the given compounds?
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The molecules having lowest and highest S-character amongst the following options are:
| A. |
|
| B. |
|
| C. |
|
| D. |
|
In compound $\mathrm{O}_2 \mathrm{SC}-\left(\mathrm{NH}_2\right)_2$, the toll number of electrons and geometry around S and N respectively are:
| A. |
|
| B. |
|
| C. |
|
| D. |
|
A square planar complex is formed by the hybridisation of which atomic orbitals?
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Directions: In the following questions, a statement if Assertion (A) is followed by a statement of reason (R).
Assertion: All the bond lengths are equal in PCl5 molecule.
Reason: 'P' atom is sp3d2 hybridized.
Mark the correct choice as:
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Which type of bonds form while hybridization
| A. |
|
| B. |
|
| C. |
|
| D. |
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What is/ are the condition for hybridisation
| A. |
|
| B. |
|
| C. |
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| D. |
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Which of the following has hybridized orbitals
| A. |
|
| B. |
|
| C. |
|
| D. |
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How many d-orbitals are vacant in IF7 after promotion of electrons (if required) _____
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Correct order of electronegativity character of Hybridization.
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Which of the following shape is not possible in $\mathrm{Sp}^3 \mathrm{~d}^3$ hybridisation
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Hybridisation state of ' P ' in the product obtained when $P C l_5$ is heated strongly.
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The hybridisation state of 'P' in cyclotrimetaphosphoric acid is :
| A. |
|
| B. |
|
| C. |
|
| D. |
|
A molecule has 7 sigma bonds around the central atom X (with no lone pair). The d orbitals of X involved in hybridisation are
| A. |
|
| B. |
|
| C. |
|
| D. |
|
In sp3 hybridisation .there are four hybrid orbitals form
| A. |
|
| B. |
|
| C. |
|
| D. |
|
$\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_6\right]^{3+}$ and $\left[\mathrm{CoF}_6\right]^{3-}$ are respectively known as :
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Trigonal bipyramidal geometry is shown by :
| A. |
|
| B. |
|
| C. |
|
| D. |
|
What is the type of hybridisation of each carbon the following compounds?
$$
\text { (1) } \mathrm{CH}_3 \mathrm{Cl},(2)\left(\mathrm{CH}_3\right)_2 \mathrm{CO},(3) \mathrm{CH}_3 \mathrm{CN} \text {, (4) } \mathrm{HCONH}_2
$$
| A. |
|
| B. |
|
| C. |
|
| D. |
|
$X e F_6$ hydrolyses to give an oxide. The structures of $X e F_6$ and the oxide, respectively, are
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Which of the following conversions involves change in both shape and hybridisation ?
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Among the following species, the $H-X-H$ angle $(X=B, N$ or $P)$ follows the order
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Hybridization and geometry of $\left(\left[N i(C N)_4\right]^{2-}\right)$ are
| A. |
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| B. |
|
| C. |
|
| D. |
|
The correct structure of PCl3F2 is
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Which of the following statements is correct for $\mathrm{ClF}_3$ ?
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Which one of the following has the regular tetrahedral structure?
(Atomic no. B = 5, S = 16, Ni = 28, Xe = 54)
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Which one of the following is the correct bond angle between atoms adopting a trigonal planar geometry ____°
| A. |
|
| B. |
|
| C. |
|
| D. |
|
$-\mathrm{CONH}_2 \xrightarrow{\text { reduction }}-\mathrm{CH}_2 \mathrm{NH}_2$
Hybridisation state of carbon changes from
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Which of the following statement is true with respect to $\mathrm{H}_2 \mathrm{O}, \mathrm{NH}_3$ and $\mathrm{CH}_4$ ?
A. The central atoms of all the molecules are $\mathrm{sp}^3$ hybridized.
B. The $\mathrm{H}-\mathrm{O}-\mathrm{H}, \mathrm{H}-\mathrm{N}-\mathrm{H}$ and $\mathrm{H}-\mathrm{C}-\mathrm{H}$ angles in the above molecules are $104.5^{\circ}, 107.5^{\circ}$ and $109.5^{\circ}$ respectively.
C. The increasing order of dipole moment is $\mathrm{CH}_4<\mathrm{NH}_3<\mathrm{H}_2 \mathrm{O}$.
D. Both $\mathrm{H}_2 \mathrm{O}$ and $\mathrm{NH}_3$ are Lewis acids and $\mathrm{CH}_4$ is a Lewis base
E. A solution of $\mathrm{NH}_3$ in $\mathrm{H}_2 \mathrm{O}$ is basic. In this solution $\mathrm{NH}_3$ and $\mathrm{H}_2 \mathrm{O}$ act as Lowry-Bronsted acid and base respectively.
Choose the correct answer from the options given below :
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The molecule in which the central atom is sp3d2 hybridised is :
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Given below are two statements:
Statement I: $\mathrm{PF}_5$ and $\mathrm{BrF}_5$ both exhibit $\mathrm{sp}^3 \mathrm{~d}$ hybridisation.
Statement II: Both $\mathrm{SF}_6$ and $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_6\right]^{3+}$ exhibit $\mathrm{sp}^3 \mathrm{~d}^2$ hybridisation.
In the light of the above statements, choose the correct answer from the options given below:
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Hybridisation of phosphorus in $\mathrm{PCl}_3$ is
| A. |
|
| B. |
|
| C. |
|
| D. |
|
If AB4 molecules is a polar molecule, a possible geometry of AB4 is :
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Which of the following angle corresponds to sp2 hybridization?
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Nitrogen in the amines is :
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Number of lone pairs of electrons in the central atom of $\mathrm{SCl}_{2^{\prime}} \mathrm{O}_3, \mathrm{ClF}_3$ and SF6 respectively, are:
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Number of molecules/ions from the following in which the central atom is involved in $\mathrm{sp}^3$ hybridization is __________
$\mathrm{NO}_3^{-}, \mathrm{BCl}_3, \mathrm{ClO}_2^{-}, \mathrm{ClO}_3$
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The electronic geometry of the ion formed by the combination of $\mathrm{H}^{+}$and $\mathrm{H}_2 \mathrm{O}$
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The hybridization of P exhibited in$\mathrm{PF}_5$ is $\mathrm{sp}^{\mathrm{x}} \mathrm{d}^{\mathrm{y}}$..
The value of is _____________
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The incorrect statement regarding ethyne is
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The maximum number of $90^{\circ}$ angles between bond- pair, bond pair of electrons is observed in
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The number of $\mathrm{Sp}^3$ hybridised carbons in an acyclic neutral compound with molecular formula $\mathrm{C}_4 \mathrm{H}_5 \mathrm{~N}$ is $\qquad$
"Only - $\mathrm{C} \equiv \mathrm{N}$ contain compound"
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The number of species below that have lone pairs of electrons in their central atom is ____________ (Rounded off to the nearest integer)
$\mathrm{SF}_4, \mathrm{BF}_4^{-}, \mathrm{CIF}_3, \mathrm{AsF}_3, \mathrm{PCl}_5, \mathrm{BrF}_5, \mathrm{XeF}_4, \mathrm{SF}_6$
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The species in which the N atom is in a state of sp hybridization is
| A. |
|
| B. |
|
| C. |
|
| D. |
|
In how many of the given compound the central atom uses all their three p orbitals in hybridisation
$\mathrm{IF}_5, \mathrm{BCl}_3, \mathrm{BeCl}_2, \mathrm{AsCl}_4^{-}, \mathrm{XeO}_2 \mathrm{~F}_2$ $\mathrm{H}_3 \mathrm{BO}_3, \mathrm{SnO}_2, \mathrm{ClO}_2^{+}, \mathrm{SeF}_4, \mathrm{I}_3^{+}$
| A. |
|
| B. |
|
| C. |
|
| D. |
|
There is no change in the type of hybridisation when
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The $F-B r-F$ bond angles in $B r F_5$ and the $C l-P-C l$ bond angles in $P C l_5$ respectively, are
| A. |
|
| B. |
|
| C. |
|
| D. |
|
oxidation state and hybridisation of sulphur in sulphuric acid molecule are respectively
| A. |
|
| B. |
|
| C. |
|
| D. |
|
$B F_3$ reacts with water to give $H B F_4$ what is the change in hybridization
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Among $\mathrm{SO}_2, \mathrm{NF}_3, \mathrm{NH}_3, \mathrm{XeF}_2, \mathrm{ClF}_3$ and $\mathrm{SF}_4$, the hybridization of the molecule with non-zero dipole moment and highest number of lone-pairs of electrons on the central atom is
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Match the LIST-I with LIST-II
| LIST-I (Molecules/ion) |
LIST-II (Hybridisation of central atom) |
||
| A. | $\mathrm{PF}_5$ | I. | $\mathrm{dsp}^2$ |
| B. | $\mathrm{SF}_6$ | II. | $\mathrm{sp}^3 \mathrm{~d}$ |
| C. | $\mathrm{Ni}(\mathrm{CO})_4$ | III. | $\mathrm{sp}^3 \mathrm{~d}^2 $ |
| D. | $\left[\mathrm{PtCl}_4\right]^{2-}$ | IV. | $\mathrm{sp}^3$ |
Choose the correct answer from the options given below :
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Pauling introduced the concept of hybridisation. According to him the atomic orbitals combine to form new set of equivalent orbitals known as hybrid orbitals.
