Question:
Chlorides of which metal are soluble in organic solvents:
Chlorides of which metal are soluble in organic solvents:
Updated On: Mar 19, 2025
- $Mg$
- $Ca$
- $K$
- $Be$
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The Correct Option is D
Solution and Explanation
We are asked to find the metal whose chloride is soluble in organic solvents.
The solubility of metal chlorides in organic solvents varies depending on the metal. Typically, metal chlorides like those of alkali and alkaline earth metals have different solubility behaviors in organic solvents. Among the options:
- CaCl2: Calcium chloride is not soluble in most organic solvents.
- MgCl2: Magnesium chloride is also insoluble in most organic solvents.
- KCl: Potassium chloride is insoluble in organic solvents.
- BeCl2: Beryllium chloride is unique in that it is soluble in organic solvents such as ether.
Therefore, the correct answer is: BeCl2.
The chloride of Beryllium (BeCl2) is soluble in organic solvents.
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Concepts Used:
Properties of D Block Elements
- Multiple oxidation states- The oxidation states of d block elements show very few energy gaps; therefore, they exhibit many oxidation states. Also, the energy difference between s and d orbital is very less. Therefore both the electrons are involved in ionic and covalent bond formation, which ultimately leads to multiple oxidation states.
- Formation of complex compounds- Ligands show a binding behavior and can form so many stable complexes with the help of transition metals. This property is mainly due to:
- Availability of vacant d orbitals.
- Comparatively small sizes of metals.
- Hardness- Transition elements are tough and have high densities because of the presence of unpaired electrons.
- Melting and boiling points- Melting and boiling points of transition are very high because of the presence of unpaired electrons and partially filled d orbitals. They form strong bonds and have high melting and boiling points.
- Atomic radii- The atomic and ionic radius of the transition elements decreases as we move from Group 3 to group 6. However, it remains the same between group 7 and group 10, and from group 11 to group 12 increases.
- Ionization enthalpy- The ionization enthalpies of the transition elements are generally on the greater side as compared to the S block elements