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Question:
\(K_2Cr_2O_7\) paper acidified with dil. \(H_2SO_4\) turns green when exposed to :
\(K_2Cr_2O_7\) paper acidified with dil. \(H_2SO_4\) turns green when exposed to :
Updated On: Sep 30, 2024
\(SO_2\)
\(SO_3\)
\(CO_2\)
\(H_2S\)
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The Correct Option is A
Solution and Explanation
\(SO_2 \text{ } \text{ } \text{ } \underset{H^+}{\underset{\longrightarrow}{K_2Cr_2O_7}} \text{ } \text{ } \text{ }\underset{(green)}{Cr^{3+}} + SO_4^{2-}\)
The correct option is (A): \(SO_2\)
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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
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