What is the structure of Aluminium tetrahydridoborate (Al(BH4)3) ?

Al(BH₄)₃ is a volatile liquid and covalent compound and does not contain any ion but it contain (B-H-Al) hydrogen bridge structure in which each boron atom attach to aluminium by hydrogen bridge.

Related Questions: 

(1) Why aqueous solution of AlCl3 is acidic in nature ?

(2) What happen when aq AlCl3 react with Acid or Base?

(3) Although anhydrous aluminium chloride is covalent but its aqueous solution is ionic in nature. Why?

(4) Why BF3 do not exist as dimer?. Explain.

(5) Why B-F bond length in BF3 is shorter (130 pm) than B-F bond Iength in BF4- (143 pm)?. Explain.

(6) B-F bond length in BF3 is shorter than B-F bond length in (BF4)- why?

(7) When B2H6 is allowed to react with following Lewis bases, then how may given Lewis base form adduct through symmetrical Cleavage of B2H6.

(8) What is product of reaction between diborane (B2H6) and ammmonia (NH3)?

(9) Why methylation of Diborane (B2H6) replace four hydrogen only ?

(10) What is Use of Boric Acid?

(11) What is use of Orthoboric acids?

(12) What is basicity of "Boric acid" ?

(13) Why Boric acid exist in solid state ?

(14) What is structure of solid Ortho Boric acid ?

(15) What is effect of heat on Borax?

(16) What is the structure of trimetaboric acid and trimetaborate ion?

(17) What is the Sodium per borate ,give the structure and its uses?

(18) Why aqueous solution of borax reacts with two moles of acids ?

(19) What is the molecular formula of Borax ?

(20) Why Boric acid become strong acid in the presence of cis 1,2-diol or 1,3-diol ?

(21) Why Borazine is more reactive than benzene towards Electrophic Aromatic substitution reactions ?

(22) Why Borazine (B3N3H6) is also known as inorganic benzene ?.

(23) Four-center two-electron bond (4C-2e Bond): Structure of AlCl3:

(24) What is the difference between the structure of AlCl3 and diborane?

Why Sulphide ion (S2-) is less basic than oxide ion ( O2-)?

SOLUTION: Sulphide ion (S^2-) is less basic than oxide ion (O^2-) due  to its larger size. the oxide ion has a higher charge density than the sulphide ion hence the small H⁺ more attracted toward smaller ion (O^2-) .

Which is more basic oxide ion (O-2 ) or hydroxide ion( OH- ) and why ?

SOLUTION: The basic strength of base primarily depends on the ability of a species to attract H⁺, which is also depends upon electrostatic interactions. The smaller and more highly charged a negative species is, the stronger the attraction for the small, positive H⁺ ion. For example, O^2- has a higher negative charge than OH^-, and as a result it is a stronger base. One does not normally expect reactions that take place in aqueous solutions to produce oxides as a result of the basicity of O^2-. Ionic oxides normally react with water to produce hydroxides:

                                           CaO + H₂O → Ca(OH)₂

Structure of "Borazon" (Cubic boron nitride):

(1) In contrast to graphite, layered boron nitride is stable in air up to 1000°C, making it a useful refractory material. Layered boron nitride changes into a denser cubic phase at high pressures and temperatures (60 kbar and 3000 degree centigrade). And the denser and cubic form of this boron nitride is known as “Borazon”  and its structure is similar to diamond.

(2) The of “Borazon” is similar to that of diamond and it is stable at high temperature.

(3)The extreme hardness of Borazon is due to fact that the B-N bond. The B-N bond possess covalent character comparable to C-C bond of diamond and more important that B-N bond also some ionic stabilization due to electronegativity difference  boron and nitrogen atom.

Structure of "Inorganic Gaphite";

Structure of “Borazine/Borazole”/inorganic Benzene:

 Related Questions: 

Why aqueous solution of AlCl3 is acidic in nature ?

What happen when aq AlCl3 react with Acid or Base?

Although anhydrous aluminium chloride is covalent but its aqueous solution is ionic in nature. Why?

Why BF3 do not exist as dimer?. Explain.

Why B-F bond length in BF3 is shorter (130 pm) than B-F bond Iength in BF4- (143 pm)?. Explain.

B-F bond length in BF3 is shorter than B-F bond length in (BF4)- why?

When B2H6 is allowed to react with following Lewis bases, then how may given Lewis base form adduct through symmetrical Cleavage of B2H6.

What is product of reaction between diborane (B2H6) and ammmonia (NH3)?

Why methylation of Diborane (B2H6) replace four hydrogen only ?

What is Use of Boric Acid?

What is use of Orthoboric acids?

What is basicity of "Boric acid" ?

Why Boric acid exist in solid state ?

What is structure of solid Ortho Boric acid ?

What is effect of heat on Borax?

What is the structure of trimetaboric acid and trimetaborate ion?

What is the Sodium per borate ,give the structure and its uses?

Why aqueous solution of borax reacts with two moles of acids ?

What is the molecular formula of Borax ?

Why Boric acid become strong acid in the presence of cis 1,2-diol or 1,3-diol ?

Why Borazine is more reactive than benzene towards Electrophic Aromatic substitution reactions ?

Why Borazine (B3N3H6) is also known as inorganic benzene ?.

Four-center two-electron bond (4C-2e Bond): Structure of AlCl3:

Why N-N bond length of H2N-NH2 is greater than N-N bond length of F2N-NF2 molecules?

Electronegativity of F is much more than hydrogen and also hybridization of nitrogen atoms in of H₂N-NH₂ and F₂N-NF₂ both have (sp3) same . According bent’s rule those hybrid orbitals containing flourine atom have less % s-characterand more p-character while other orbitals have more % s-character and less % s-character hence N-N bond length in F₂N-NF₂ is shorter than H₂N-NH₂

Related Questions:

What is Bent’s rule of hybridization?

Which of the following compound have longest (S=O)bond length , O=SF2, O=SCl2, O=SBr2.

Why Bond length of O-O is greater in H2O2 than O2F2?

How to arrange increasing (C-H) bond length in increasing order and H-C-F bond angle in the given compounds, CH4, CH3F, CH2F2 and CHF3 ?