Question:
The incorrect statement in respect of Chromyl chloride test is
The incorrect statement in respect of Chromyl chloride test is
Updated On: Apr 15, 2024
- formation of Chromyl chloride
- liberation of Chlorine
- formation of red vapours
- formation of lead chromate
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The Correct Option is B
Solution and Explanation
$4 NaCl + K _{2} Cr _{2} O _{7}+3 H _{2} SO _{4} \longrightarrow K _{2} SO _{4}+2 Na _{2} SO _{4}+\underset{\text{chromyl chloride(reddish brown vapour) }}{2 CrO _{2} Cl _{2} \uparrow }+3 H _{2} O$
$CrO _{2} Cl _{2}+4 NaOH \longrightarrow 2 NaCl + Na _{2} CrO _{4}+2 H _{2} O$
$Na _{2} CrO _{4}+\left( CH _{3} COO \right)_{2} Pb \longrightarrow 2 CH _{3} COONa+ \underset{\text{lead chromate}}{PbCrO _{4}}$
$CrO _{2} Cl _{2}+4 NaOH \longrightarrow 2 NaCl + Na _{2} CrO _{4}+2 H _{2} O$
$Na _{2} CrO _{4}+\left( CH _{3} COO \right)_{2} Pb \longrightarrow 2 CH _{3} COONa+ \underset{\text{lead chromate}}{PbCrO _{4}}$
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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