Tag: d and f block elements
Questions Related to d and f block elements
Which of the following is not correct?
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${\text{TiC}}{{\text{l}} _{\text{4}}}$ is a colourless compound.
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$\left[ {{\text{Cr}}{{\left( {{\text{N}}{{\text{H}} _{\text{3}}}} \right)} _{\text{6}}}} \right]{\text{C}}{{\text{L}} _{\text{3}}}$ is a coloured compound
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${{\text{K}} _{\text{3}}}\left[ {{\text{V}}{{\text{F}} _{\text{6}}}} \right]$ is a colourless compound
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$\;\left[ {{\text{Cu}}{{\left( {{\text{NCC}}{{\text{H}} _{\text{3}}}} \right)} _{\text{4}}}} \right]\left[ {{\text{B}}{{\text{F}} _{\text{4}}}} \right]$ is a colourless compound
The colour imparted by $Co(II)$ compounds to glass is
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green
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deep blue
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yellow
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red
Vanadium | yellow-green |
---|---|
Chrome | emerald green |
Iron | Coke bottle green |
Manganese | amethyst |
Cobalt | violet blue |
Copper | greenish blue to blue |
Nickel | grayish brown |
Selenium | salmon pink |
Cerium- Titanium | yellow |
Neodymium | dichroic violet-pink |
Uranium | yellow (fluorescent |
Which of the ions will give colorless aqueous solution?
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${Ni}^{2+}$
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${Fe}^{2+}$
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${Cu}^{2+}$
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${Cu}^{+}$
${Ni}^{2+}$ is light green, ${Fe}^{2+}$ is pale green,
The color of the transition metal ions is due to:
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$d-d$ transition
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charge transfer
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change in the geometry
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none
In case of transition elements, where the d-level is not completely filled, it is possible to promote an electron from a lower energy d-orbital to a higher energy d-orbital by absorption of a photon of electromagnetic radiation having an appropriate energy. Electromagnetic radiations in the visible region of the spectrum often possess the appropriate energy for such transitions.
Which of the following statements are correct with reference to the ferrous and ferric ions?
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${Fe}^{3+}$ gives brown color with potassium ferricyanide
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${Fe}^{2+}$ gives blue precipitate with potassium ferricyanide
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${Fe}^{3+}$ gives red color with potassium thiocyanate
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${Fe}^{2+}$ gives brown color with ammonium thiocyanate
Which one of the following ionic species will not impart color to an aqueous solution?
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${Ti}^{4+}$
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${Cu}^{+}$
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${Zn}^{2+}$
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${Cr}^{3+}$
The colorless species is:
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$V{Cl} _{3}$
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$VO{SO} _{4}$
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${Na} _{3}{VO} _{4}$
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$\left[ V{ \left( { H } _{ 2 }O \right) } _{ 6 }{ SO } _{ 4 } \right] .{ H } _{ 2 }O$
$ VCl _3$ is green.
The aqueous solution of the salt will colored in the case of:
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$Zn{({NO} _{3})} _{2}$
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$Li{NO} _{3}$
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$Co{({NO} _{3})} _{2}$
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$Cr{Cl} _{3}$
$ Co^{2+}$ = $3d^7$
What is/are true statement?
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Ions of $d$-block elements are colored due to $d-d$ transition
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Ions of $f$-block elements are colored due to $f-f$ transtition
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${ \left[ Sc{ \left( { H } _{ 2 }O \right) } _{ 6 } \right] }^{ 3+ },{ \left[ Ti{ \left( { H } _{ 2 }O \right) } _{ 6 } \right] }^{ 4+ }$ are colored complexes.
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${Cu}^{+}$ is colorless ion.
The aqueous solutions of the following salts will be colored in the case of:
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$Zn{({NO} _{3})} _{2}$
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$Li{NO} _{3}$
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$Co{({NO} _{3})} _{2}$
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$Cr{Cl} _{3}$
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Potash alum