Diborane is simplest and most familiar h...

Diborane is simplest and most familiar hydride of boton. Its chemical formula is `B_(2)H_(6)`. Comparing with ethane, diborane is regarded as electron deficient molecule. In the excited state boron of diborane undergoes `sp^(3)` hybridisation. Bonding in doborane is described as tricentric two electron bonding.
Structure of `-BH_(2)` group is

linear

planar

tetrahedral

octahedral

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The correct Answer is:

Two - `BH_2` groups present in the same palne

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Diborane is simplest and most familiar hydride of boton. Its chemical formula is B_(2)H_(6) . Comparing with ethane, diborane is regarded as electron deficient molecule. In the excited state boron of diborane undergoes sp^(3) hybridisation. Bonding in doborane is described as tricentric two electron bonding. Number of empty sp^(3) hybrid orbitals of each ''B'' atom in B_(2)H_(6) Each B contains one sp^(3) vacant hybrid orbital

The bonding in diborane (B_2H_6) can be described by

Boran forms a number of hydrides having the general formulae BnH_(n+4) and BnH_(n+6) . These are called boranes the simplest hydride of boran is diborane. Borane contains special types of bonds known as multicentric bonds. Borans have high heat of combustion. The type of hybridisation of boron in diborane is

The statements regarding Diborane are i) Diborane contains 2-centred - 3-electron bonds ii) B - H bond is formed by sp^(3)-s overlapping iii) It contains two coplanar BH_(2) groups The correct statements in above are

The statements regarding Diborane are i) Diborane contains 2-centred-3-electron bonds ii) B-H bond is formed by sp^(3)-s overlapping iii) It contains two coplanar BH_2 groups The correct statements in above are

Some statements about the structure of diborane are given below (A) Studies have confirmed that four hydrogens of diborane are one type and remaining two are of another type (B) Diborane contains two coplanar BH_(2) groups (C) Diborane is a planar molecule (D) Boron of diborane undergoes sp^(2) hybridization The correct statements above are

Covalent molecules formed by heteroatoms bound to have some ionic character. The ionic character is due to shifting of the electron pair towards A or B in the molecule AB. Hence, atoms acquire small and equal charge but opposite in sign. Such a bond which has some ionic character is described as polar covalent bond. Polar covalent molecules can exhibit dipole moment. Dipole moment is equal to the product of charge separation, q and the bond length, d for the bond. The unit of dipole moment is Debye. One Debye is equal to 10^(-18) esu cm. Dipole moment is a vector quantity. It has both magnitude and direction. Hence, dipole moment of molecules depends upon the relative orientation of the bond dipoles, but not on the polarity of bonds alone. A symmetrical structure shows zero dipole moment. Thus, dipole moments help to predict the geometry of the molecules. Dipole moment values can be used to distinguish between cis-and traps-isomers, ortho-, meta-and para-forms of a substance, etc. The percentage of ionic character of a bond can be calculated by the application of the following formula : % " ionic character " = ("Experimental value of dipole moment ")/("Theoretical value of dipole moment ") xx 100 A diatomic molecule has a dipole moment of 1.2 D. If the bond length is 1.0 xx 10^(-8) cm, what fraction of charge does exist on each atom?

The statements regarding Diborane are i) B_2 H_6 is stable in the absence of grease and moisture at low temperature ii) Diborane burns in oxygen to produce a very high temperature iii) Borazole contains ionic bonds

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