Consider the reaction \(Cu^{2+} + X^- → Cu_2X_2 + X_2\).
X2 will be predominantly?
X2 will be predominantly?
- Cl2
- Br2
- I2
- All halogens are possible.
The Correct Option is C
Solution and Explanation
Top JEE Main Chemistry Questions
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Top JEE Main d -and f -Block Elements Questions
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(a) \([Cr(H_2O)_6]^{+3}\) (i) \(t^2_{2g}eg^0\) (b) \([Fe(H_2O)_6]^{+3}\) (ii) \(t^3_{2g}eg^0\) \((c) [Ni(H_2O)_6]^{+2}\) (iii) \(t^3_{2g}eg^2\) (d) \([V(H_2O)_6]^{+3}\) (iv) \(t^6_{2g}eg^2\) - The compound that is white in color is
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Top JEE Main Questions
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Concepts Used:
d block elements
The elements, in the columns of the periodic table in which d subshells are being occupied are known as d block elements.
These are the elements that have the capability of forming stable cations with incompletely filled d orbitals. Elements like mercury and Zinc are not considered transition metals because they have electronic configurations: (n-1)d10 ns2. These elements have filled d-orbitals in their ground state and, therefore, even in some of their oxidation states.
General 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 behaviour 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. This is because of the presence of unpaired electrons and partially filled d orbitals. Because of these two things, they form strong bonds and therefore 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