In H_2B(mu_2-H)_2BH_2 the terminal hydride bonds are also shorter than the bridging bonds. The four - terminal hydrogen atoms and the two boron atoms are lying in one plane. The momentum distributions of valence orbital shown in Fig.

B 4 H 10 + H 2 → 2B 2 H 6. For example, diborane has 10 valence orbitals (four from each boron atom and one from each hydrogen) but 12 valence electrons. BF 3 + R-O-R F 3BOR 2 The Structure of B 2H 6 (diborane) – multicentre bonds Contains a 3-centre-2-electron bond (called a banana bond) B H H H H 2-center-2 electron bond 3-center-2 electron bond B B B sp3 hybridized The structure of the three-centre, two-electron bond in a B-H-B fragment of a diborane molecule.

Diborane(4) has been produced by abstraction of two hydrogen atoms from diborane(6) using atomic fluorine and detected by photoionization mass spectrometry.

Which one of the following statements about diborane is not true (a) The B atoms in it are SP 3 hybridised (b) It contains two 3-centre-2-electron bonds (c) All B-H bond lengths in it are equal due to resonance (d) The molecule contains 12 valence electrons Diborane is more easily prepared in high yield by reaction of iodine (I 2) with sodium tetrahydroborate (NaBH 4, commonly called sodium borohydride) in diglyme as a solvent, 2NaBH 4 + I 2 → B 2 H 6 (g) + 2NaI + H 2 (g), or by reaction of a solid borohydride (i.e., a salt containing the BH 4 − ion) with an anhydrous acid, 2NaBH 4 + 2H 3 PO 4 → B 2 H 6 (g) + 2NaH 2 PO 4 + 2H 2 (g).

Answer. Select the correct option.

Jump to navigation Jump to search ... A 2-centre-2-electron bond is a ordinary, every-day bond, the simplest example being H 2.

A priori, would we not expect the latter to be stronger? For the eight atoms of B 2 H 6, this would require a minimum of seven bonds and therefore fourteen valence electrons (as in ethane, C 2 H 6), but B 2 H 6 has only twelve valence electrons.

2Mg 3 B 2 + 12HCl → 6MgCl 2 + B 4 H 10 + H 2.
Three-center two-electron bonds are seen in many boron compounds, such as diborane (B 2 H 6).The monomer BH 3 is unstable since the boron atom is only surrounded by six valence electrons.A B−H−B 3-center-2-electron bond is formed when a boron atom shares electrons with a B−H bond on another boron atom. According to structure , There are four 2 - centre - 2 - electron bonds and two 3 - centre - 2 - electron bonds in B2H6 .Hence, the correct option is D .

Three-Center, Two Electron Bonds Explained: Molecules that have lower than two valence electrons per bond are said to be electron deficient. They regard diborane as three atoms held together by a pair of electrons delocalized over three atoms but are aware that this semilocalized picture is only a part of the true picture.

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