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Aluminium chloride exists as dimer, Al(...

Aluminium chloride exists as dimer, `Al_(2)Cl_(6)` in solid state as well as in solution of non-polar solvents such as benzene. When dissolved in water, it gives :

A

`Al^(3+) + 3Cl^(Ө)`

B

`Al_(2)O_(3) + 6HCl`

C

`[Al(H_(2)O)_(6)]^(3+) + 3Cl^(Ө)`

D

`[Al(OH)_(6)]^(3-) + 3HCl`.

Text Solution

Verified by Experts

The correct Answer is:
C
The dimeric form `Al_(2)Cl_(6)` is retained in non-polar solvent but is broken into `[Al(H_(2)O)_(6)]Cl_(3)` on dissolution in water due to high heat of hydration.
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Aluminium chloride exists as a dimer, Al_(2)Cl_(6) in solid state as well as in solution of non-polar solvents such as benzene. When dissolved in water, it gives :

Anhydrous aluminium chloride (Al_(2)Cl_(6)) is covalent compound and soluble in water giving:

Why boron halides do not exists as a dimer. While AlCl_(3) exists as Al_(2)Cl_(6) ?

The small size and high charge of Al^(3+) ion gives it a high charge density which is responsible for its tendency to show (a) covalency in its compounds in the gaseous state (b) high hydration energy which stabilizes its compounds in solution, and (c) high lattice energy of its compounds in the solid state. Thus aluminium can forms both covalent and ionic bond. Like halides of boron, halides of aluminium do not show back bonding because of increase in size of aluminium. Actually aluminium atoms complete their octets by forming dimers. Thus chloride and bromide of aluminium exist as dimers, both in the vapour state and in polar-solvents like benzene while the corresponding boron halides exists as monomer. In boron trihalides the extent of back bonding decreases with increases with increase in size of halogens and thus lewis acid character increases. All BX_(3) are hydrolysed by water but BF_(3) shows a different behaviour. Which of the following statements about anhydrous aluminium chloride is correct ?

The small size and high charge of Al^(3+) ion gives it a high charge density which is responsible for its tendency to show (a) covalency in its compounds in the gaseous state (b) high hydration energy which stabilizes its compounds in solution, and (c) high lattice energy of its compounds in the solid state. Thus aluminium can forms both covalent and ionic bond. Like halides of boron, halides of aluminium do not show back bonding because of increase in size of aluminium. Actually aluminium atoms complete their octets by forming dimers. Thus chloride and bromide of aluminium exist as dimers, both in the vapour state and in polar-solvents like benzene while the corresponding boron halides exists as monomer. In boron trihalides the extent of back bonding decreases with increases with increase in size of halogens and thus lewis acid character increases. All BX_(3) are hydrolysed by water but BF_(3) shows a different behaviour. Which of the following reaction is incorrect ?

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Ionic bond is defined as the electrostatic force of attraction holding the oppositely charged ions. Ionic compounds are mostly crystalline solid having high melting and boiling points, electrical conductivity in moleten state, solubility in water etc. Covalent bond is defined as the force which binds atoms of same or different elements by mutual sharing of electrons in a covalent bond. Covalent compounds are solids, liquids or gases. They have low melting and boiling points compounds. They are more soluble in non-polar solvents. The valence electrons are involved in formation of covalent bonds is /are called :

Explain the following: (a) Sodium chloride is an ionic compound which does not conduct electricity in solid state whereas it does conduct electricity in molten state as well as in aqueous solution. (b) Reactivity of aluminium decrease if it is dipped in nitric acid. (c) Metals like calcium and magnesium are never found in their free state in nature.

A white solid P, on strong heating, decomposes to give reddish brown gas R and a residue Q. The residue R is yellow when hot and white when cold. The solution of white solid P in water gives white precipitate S, with concentrated sodium hydroxide. The white precipitate S dissolves in excess of sodium hydroxide solution to form colourless solution. Another sample of the solid P in water is mixed with ferrous sulphate solution and then to this solution are added a few drops of conc. sulphuric acid. A brown ring is formed at the junction of liquids. Answer the following questions: Name the salt formed when S dissolves in excess of sodium hydroxide.

CENGAGE CHEMISTRY ENGLISH-P-BLOCK GROUP 13 - BORON FAMILY-Exercise (Single Correct)
  1. Al(2)O(3) can be converted into anhydrous AlCl(3) by heating

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  2. Boric acid is used in carrom boards for smooth gliding of pawns becaus...

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  3. Aluminium chloride exists as dimer, Al(2)Cl(6) in solid state as wel...

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  4. In which of the following molecules is hydrogen bridge bond present ?

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  5. Which one of the following molecular hydrides acts as a Lewis acid ?

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  6. The stability of +1 oxidation state among Al,Ga,In and Tl increases in...

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  7. Na(2)B(4)O(7).10H(2)O is correctly represented as

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  8. AlCl(3) is an electron-deficient compound but AlF(3) is not, due to

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  9. Bauxite ore is generally contaminated with impurity of oxides of two...

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  10. Explain, why does boron not form B^(3+) ions.

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  11. Borazine is converted into a disubstituted product B(3)N(3)H(4)X(2)....

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  12. Aqueus solution of borax acts as a buffer because

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  13. Correct match is :

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  14. When aluminium is heated in atomosphere of nitrogen it forms :

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  15. Which one of the following is more abundant in the earth's crust ?

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  16. Which of the following is acidic in nature ?

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  17. alums are used for :

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  18. The liquified metal expanding on solidification is :

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  19. How can the following reaction be made to proceed in forward direction...

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  20. Borax-bead test is responded by

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