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Valence Bond Theory - (Concept)
According to this theory, the metal atom or ion under the influence of ligands can use its (n-1)d or nd orbitals along with its ns and np for hybridisation to yield a set of equivalent orbitals of definite geometry such as octahedral, tetrahedral, square planar and so on. These hybridised orbitals are allowed to overlap with ligand orbitals that can donate electron pairs for bonding. The different types of hybridisation and their respective shapes are given below
| Coordination Number | Type of Hybridisation | Shape |
| 4 | sp3 | Tetrahedral |
| 4 | dsp2 | Square Planar |
| 5 | sp3d | Trigonal Bipyramidal |
| 6 | sp3d2 | Octahedral |
| 6 | d2sp3 | Octahedral |
| Exam | Chapter |
| JEE MAIN | Co-ordination Compounds |
Complete removal of both the axial ligands (along the z-axis) from an octahedral complex leads to which of the following splitting patterns? ( relative orbital energies not on scale).
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The molecule in which hybrid molecular orbitals involve only one d-orbital of the central atom is:
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According to the valence bond theory, the hybridization of the central metal atom is dsp2 for which one of the following compounds?
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3 moles of metal complex with formula gives 3 moles of silver chloride on treatment with excess of silver nitrate. The secondary valency of CO in the complex is_______.
(Round off to the nearest integer)
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The sum of oxidation states of two silver ions in complex is ___________.
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In Wilkinson’s catalyst, the hybridization of central metal ion and its shape are respectively :
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Identify the pair in which the geometry of the species is T-shape and square pyramidal, respectively :
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The geometry of and
are respectively :
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In the complex hybridisation is present. Geometry of the complex is.
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An octahedral complex is formed, when hybrid orbitals of the following type are involved
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Which complex has square planar structure?
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$\left[\mathrm{Pt}\left(\mathrm{NH}_3\right)_4\right] \mathrm{Cl}_2$ is is
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hybridisation leads to
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$$
\text { The hybridisation of the complex }\left[\mathrm{CoF}_6\right]^{3-} \text { is }
$$
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In the species $\left[\mathrm{Ni}(\mathrm{CO})_4\right],\left[\mathrm{Ni}(\mathrm{CN})_4\right]^{2-},\left[\mathrm{NiCl}_4\right]^{2-}$, the hybiridisation of Ni are respectively
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One mole of the complex compound gives 3 moles of ions on dissolution in water. One mole of the same complex reacts with two moles of
solution to yield two moles of
. The structure of the complex is
| A. |
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The coordination geometry around the manganese in decacarbonyldimanganese ( 0 ) is
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$\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_6\right]^{3+}$ and $\left[\mathrm{CoF}_6\right]^{3-}$ are respectively known as :
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Which is inner sphere complex ?
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Which of the following is diamagnetic ?
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$\left[\mathrm{Cu}\left(\mathrm{NH}_3\right)_4\right]^{2+}$ has hybridisation and magnetic moment of
| A. |
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Given below are two statements:
Statement I: $\left[\mathrm{Ni}(\mathrm{CN})_4\right]^{2-}$ is square planar and diamagnetic complex, with $\mathrm{dsp}^2$ hybridization for Ni but $\left[\mathrm{Ni}(\mathrm{CO})_4\right]$ is tetrahedral, paramagnetic and with sp3 hybridization for Ni.
Statement II: $\left[\mathrm{NiCl}_4\right]^{2-}$ and $\left[\mathrm{Ni}(\mathrm{CO})_4\right]$ both have same d-electron configuration, have same geometry and are paramagnetic.
In light the above statements, choose the correct answer from the options given below:
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The complex $\left[\mathrm{Pt}\left(\mathrm{NH}_3\right)_4\right]^{2+}$ has $\qquad$ ________structure :
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On addition of $\mathrm{AgNO}_3$, which of the following compounds doesn't give a white precipitate of AgCl
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The primary valency of the central metal ion in the complex $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_5 \mathrm{Cl}\right] \mathrm{Cl}_2$ is
| A. |
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$\mathrm{Ni}(\mathrm{CO})_4$ is
| A. |
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Among the following the square planer geometry is exiited by:
(A) $\mathrm{CdCl}_4^{2-}$
(B) $Z n(C N)_4^{2-}$
(C) $\mathrm{PdCl}_4^{2-}$
$(D) C u(C N)_4^{3-}$
| A. |
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| B. |
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| D. |
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In aqueous solution. $\left[\mathrm{Co}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{2+}$ (X) reacts with molecular oxygen in the presence of excess liquor $\mathrm{NH}_3$ to give a new complex Y. The number of unpaired electrons in X are
| A. |
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| B. |
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| C. |
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| D. |
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List-I |
List-II |
| (A) | $\left[\mathrm{MnBr}_4\right]^{2-}$ | (I) | $\mathrm{d}^2 \mathrm{sp}^3 \&$ diamagnetic |
| (B) | $\left[\mathrm{FeF}_6\right]^{3-}$ | (II) | $\mathrm{sp}^3 \mathrm{~d}^2 \&$ paramagnetic |
| (C) | $\left[\mathrm{Co}\left(\mathrm{C}_2 \mathrm{O}_4\right)_3\right]^{3-}$ | (III) | $\mathrm{sp}^3 \&$ diamagnetic |
| (D) | $\left[\mathrm{Ni}(\mathrm{CO})_4\right]$ | (IV) | $\mathrm{sp}^3 \&$ paramagnetic |
Choose the correct answer from the options given below :
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| C. |
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| D. |
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In a borax bead test under hot condition, a metal salt (one from the given) is heated at point B of the flame, resulted in green colour salt bead. The spin-only magnetic moment value of the salt is $\qquad$ BM (Nearest integer)
[Given atomic number of $\mathrm{Cu}=29, \mathrm{Ni}=28$, $\mathrm{Mn}=25, \mathrm{Fe}=26]$
| A. |
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| B. |
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| C. |
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| D. |
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In which of the following molecule/ion, all the bonds are not equal?
| A. |
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Match List I with List II
| List-I | List - II | ||
| A. | $\mathrm{K}_2\left[\mathrm{Ni}(\mathrm{CN})_4\right]$ | I. | $\mathrm{sp}^3$ |
| B. | $\left[\mathrm{Ni}(\mathrm{CO})_4\right]$ | II. | $\mathrm{sp}^3 \mathrm{~d}^2$ |
| C. | $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_6\right] \mathrm{Cl}_3$ | III. | $\mathrm{dsp}^2$ |
| D. | $\mathrm{Na}_3\left[\mathrm{CoF}_6\right]$ | IV. | $\mathrm{d}^2 \mathrm{sp}^3$ |
Choose the correct answer from the options given below:
| A. |
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| B. |
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| C. |
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| D. |
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Nickel ( $Z=28$ ) combines with a uninegative monodentate ligand $X^{-}$to form a paramagnetic complex $\left[\mathrm{Ni} \mathrm{X}_4\right]^{2-}$. The number of unpaired electron(s) in the nickel and geometry of this complex ion are, respectively
| A. |
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| B. |
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| C. |
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| D. |
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The correct statements from following are:
A. The strength of anionic ligands can be explained by crystal field theory.
B. Valence bond theory does not give a quantitative interpretation of kinetic stability of coordination compounds.
C. The hybridization involved in formation of $\left[\mathrm{Ni}(\mathrm{CN})_4\right]^{2-}$ complex is $\mathrm{dsp}^2$.
D. The number of possible isomer(s) of cis- $\left[\mathrm{PtCl}_2(\mathrm{en})_2\right]^{2+}$ is one
Choose the correct answer from the options given below:
| A. |
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| B. |
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| C. |
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| D. |
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The octahedral diamagnetic low spin complex among the following is
| A. |
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| B. |
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| C. |
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| D. |
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The type of hybridization and the magnetic property of $\left[\mathrm{MnCl}_6\right]^{3-}$ are :
| A. |
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| B. |
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| C. |
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| D. |
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According to this theory, the metal atom or ion under the influence of ligands can use its (n-1)d, ns, np or ns, np, nd orbitals for hybridisation to yield a set of equivalent orbitals of definite geometry such as octahedral, tetrahedral, square planar and so on (Table 9.2).
