321414
Which of the following compounds is coloured?
1 \(\mathrm{TiCl}_{3}\)
2 \(\mathrm{FeCl}_{3}\)
3 \(\mathrm{CoCl}_{2}\)
4 All of these
Explanation:
The compounds having metal ions with unpaired electrons, are coloured. Thus, (1) In \(\mathrm{TiCl}_{3}, \mathrm{Ti}^{3+}=[\mathrm{Ar}] 3 \mathrm{~d}^{1}\) (one unpaired electron) (2) In \(\mathrm{FeCl}_{3}, \mathrm{Fe}^{3+}=[\mathrm{Ar}] 3 \mathrm{~d}^{5}\) (Five unpaired electrons) (3) In \(\mathrm{CoCl}_{2}, \mathrm{Co}^{2+}=[\mathrm{Ar}] 3 \mathrm{~d}^{7}\) (three unpaired electrons) Hence, all compounds given are coloured.
AIIMS - 2008
CHXII08:THE D- & F-BLOCK ELEMENTS
321415
Identify the oxidation states of titanium \(\mathrm{(Z=22)}\) and copper \(\mathrm{(Z=29)}\) in their colourless compounds.
1 \(\mathrm{\mathrm{Ti}^{3+}, \mathrm{Cu}^{2+}}\)
2 \(\mathrm{\mathrm{Ti}^{2+}, \mathrm{Cu}^{2+}}\)
3 \(\mathrm{\mathrm{Ti}^{4+}, \mathrm{Cu}^{+}}\)
4 \(\mathrm{\mathrm{Ti}^{4+}, \mathrm{Cu}^{2+}}\)
Explanation:
Electronic configuration of titanium (Ti) \(\mathrm{(\mathrm{Z}=22)}\) is \({{\rm{[Ar]}}_{{\rm{18}}}}{\rm{3}}{{\rm{d}}^{\rm{2}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}\). In case of \(\mathrm{\mathrm{Ti}^{4+}}\), the electronic configuration will be \({{\rm{[Ar]}}_{{\rm{18}}}}{\rm{3}}{{\rm{d}}^{\rm{0}}}{\rm{4}}{{\rm{s}}^{\rm{0}}}\) Similarly, electronic configuration of copper \(\mathrm{(\mathrm{Cu})}\) \(\mathrm{(Z=29)}\) is \(\mathrm{[A r]_{18} 3 d^{10} 4 s^{1}}\). On loosing one electron it acquires stable electronic configuration, i.e \({{\rm{[Ar]}}_{{\rm{18}}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}\). In both \({\rm{T}}{{\rm{i}}^{{\rm{4 + }}}}\) and \(\mathrm{\mathrm{Cu}^{+}}\)no unpaired electron is present. As a result, no d-d transition occur and therefore these are colourless in nature.
MHTCET - 2018
CHXII08:THE D- & F-BLOCK ELEMENTS
321416
d - d transition is not a reason for the colour of which of the following compounds?
1 \(\mathrm{FeI}_{3}\)
2 \(\mathrm{CrCl}_{3}\)
3 \(\mathrm{PbI}_{2}\)
4 None
Explanation:
Pb is a p - block metal. So d-d transition is not observed here.
CHXII08:THE D- & F-BLOCK ELEMENTS
321417
Match the following: Column I Column II A \({\mathrm{\mathrm{Zn}^{2+}}}\) P \({\mathrm{\mathrm{d}^{8}}}\) configuration B \({\mathrm{\mathrm{Cu}^{2+}}}\) Q Colourless C \({\mathrm{\mathrm{Ni}^{2+}}}\) R \({\mathrm{\mu=1.73 \,\mathrm{BM}}}\)
\({\mathrm{\mathrm{Zn}^{+2}}}\) - no unpaired electrons, so colourless. \({\mathrm{\mathrm{Cu}^{+2}-\mu-1.73}}\) B.M, due to 1 unpaired \({\mathrm{\mathrm{e}^{-}}}\). \({\mathrm{\mathrm{Ni}^{+2}-\mathrm{d}^{8}}}\) configuration, as it lost \({\mathrm{2 \mathrm{e}^{-}}}\).
NEET Test Series from KOTA - 10 Papers In MS WORD
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CHXII08:THE D- & F-BLOCK ELEMENTS
321414
Which of the following compounds is coloured?
1 \(\mathrm{TiCl}_{3}\)
2 \(\mathrm{FeCl}_{3}\)
3 \(\mathrm{CoCl}_{2}\)
4 All of these
Explanation:
The compounds having metal ions with unpaired electrons, are coloured. Thus, (1) In \(\mathrm{TiCl}_{3}, \mathrm{Ti}^{3+}=[\mathrm{Ar}] 3 \mathrm{~d}^{1}\) (one unpaired electron) (2) In \(\mathrm{FeCl}_{3}, \mathrm{Fe}^{3+}=[\mathrm{Ar}] 3 \mathrm{~d}^{5}\) (Five unpaired electrons) (3) In \(\mathrm{CoCl}_{2}, \mathrm{Co}^{2+}=[\mathrm{Ar}] 3 \mathrm{~d}^{7}\) (three unpaired electrons) Hence, all compounds given are coloured.
AIIMS - 2008
CHXII08:THE D- & F-BLOCK ELEMENTS
321415
Identify the oxidation states of titanium \(\mathrm{(Z=22)}\) and copper \(\mathrm{(Z=29)}\) in their colourless compounds.
1 \(\mathrm{\mathrm{Ti}^{3+}, \mathrm{Cu}^{2+}}\)
2 \(\mathrm{\mathrm{Ti}^{2+}, \mathrm{Cu}^{2+}}\)
3 \(\mathrm{\mathrm{Ti}^{4+}, \mathrm{Cu}^{+}}\)
4 \(\mathrm{\mathrm{Ti}^{4+}, \mathrm{Cu}^{2+}}\)
Explanation:
Electronic configuration of titanium (Ti) \(\mathrm{(\mathrm{Z}=22)}\) is \({{\rm{[Ar]}}_{{\rm{18}}}}{\rm{3}}{{\rm{d}}^{\rm{2}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}\). In case of \(\mathrm{\mathrm{Ti}^{4+}}\), the electronic configuration will be \({{\rm{[Ar]}}_{{\rm{18}}}}{\rm{3}}{{\rm{d}}^{\rm{0}}}{\rm{4}}{{\rm{s}}^{\rm{0}}}\) Similarly, electronic configuration of copper \(\mathrm{(\mathrm{Cu})}\) \(\mathrm{(Z=29)}\) is \(\mathrm{[A r]_{18} 3 d^{10} 4 s^{1}}\). On loosing one electron it acquires stable electronic configuration, i.e \({{\rm{[Ar]}}_{{\rm{18}}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}\). In both \({\rm{T}}{{\rm{i}}^{{\rm{4 + }}}}\) and \(\mathrm{\mathrm{Cu}^{+}}\)no unpaired electron is present. As a result, no d-d transition occur and therefore these are colourless in nature.
MHTCET - 2018
CHXII08:THE D- & F-BLOCK ELEMENTS
321416
d - d transition is not a reason for the colour of which of the following compounds?
1 \(\mathrm{FeI}_{3}\)
2 \(\mathrm{CrCl}_{3}\)
3 \(\mathrm{PbI}_{2}\)
4 None
Explanation:
Pb is a p - block metal. So d-d transition is not observed here.
CHXII08:THE D- & F-BLOCK ELEMENTS
321417
Match the following: Column I Column II A \({\mathrm{\mathrm{Zn}^{2+}}}\) P \({\mathrm{\mathrm{d}^{8}}}\) configuration B \({\mathrm{\mathrm{Cu}^{2+}}}\) Q Colourless C \({\mathrm{\mathrm{Ni}^{2+}}}\) R \({\mathrm{\mu=1.73 \,\mathrm{BM}}}\)
\({\mathrm{\mathrm{Zn}^{+2}}}\) - no unpaired electrons, so colourless. \({\mathrm{\mathrm{Cu}^{+2}-\mu-1.73}}\) B.M, due to 1 unpaired \({\mathrm{\mathrm{e}^{-}}}\). \({\mathrm{\mathrm{Ni}^{+2}-\mathrm{d}^{8}}}\) configuration, as it lost \({\mathrm{2 \mathrm{e}^{-}}}\).
321414
Which of the following compounds is coloured?
1 \(\mathrm{TiCl}_{3}\)
2 \(\mathrm{FeCl}_{3}\)
3 \(\mathrm{CoCl}_{2}\)
4 All of these
Explanation:
The compounds having metal ions with unpaired electrons, are coloured. Thus, (1) In \(\mathrm{TiCl}_{3}, \mathrm{Ti}^{3+}=[\mathrm{Ar}] 3 \mathrm{~d}^{1}\) (one unpaired electron) (2) In \(\mathrm{FeCl}_{3}, \mathrm{Fe}^{3+}=[\mathrm{Ar}] 3 \mathrm{~d}^{5}\) (Five unpaired electrons) (3) In \(\mathrm{CoCl}_{2}, \mathrm{Co}^{2+}=[\mathrm{Ar}] 3 \mathrm{~d}^{7}\) (three unpaired electrons) Hence, all compounds given are coloured.
AIIMS - 2008
CHXII08:THE D- & F-BLOCK ELEMENTS
321415
Identify the oxidation states of titanium \(\mathrm{(Z=22)}\) and copper \(\mathrm{(Z=29)}\) in their colourless compounds.
1 \(\mathrm{\mathrm{Ti}^{3+}, \mathrm{Cu}^{2+}}\)
2 \(\mathrm{\mathrm{Ti}^{2+}, \mathrm{Cu}^{2+}}\)
3 \(\mathrm{\mathrm{Ti}^{4+}, \mathrm{Cu}^{+}}\)
4 \(\mathrm{\mathrm{Ti}^{4+}, \mathrm{Cu}^{2+}}\)
Explanation:
Electronic configuration of titanium (Ti) \(\mathrm{(\mathrm{Z}=22)}\) is \({{\rm{[Ar]}}_{{\rm{18}}}}{\rm{3}}{{\rm{d}}^{\rm{2}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}\). In case of \(\mathrm{\mathrm{Ti}^{4+}}\), the electronic configuration will be \({{\rm{[Ar]}}_{{\rm{18}}}}{\rm{3}}{{\rm{d}}^{\rm{0}}}{\rm{4}}{{\rm{s}}^{\rm{0}}}\) Similarly, electronic configuration of copper \(\mathrm{(\mathrm{Cu})}\) \(\mathrm{(Z=29)}\) is \(\mathrm{[A r]_{18} 3 d^{10} 4 s^{1}}\). On loosing one electron it acquires stable electronic configuration, i.e \({{\rm{[Ar]}}_{{\rm{18}}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}\). In both \({\rm{T}}{{\rm{i}}^{{\rm{4 + }}}}\) and \(\mathrm{\mathrm{Cu}^{+}}\)no unpaired electron is present. As a result, no d-d transition occur and therefore these are colourless in nature.
MHTCET - 2018
CHXII08:THE D- & F-BLOCK ELEMENTS
321416
d - d transition is not a reason for the colour of which of the following compounds?
1 \(\mathrm{FeI}_{3}\)
2 \(\mathrm{CrCl}_{3}\)
3 \(\mathrm{PbI}_{2}\)
4 None
Explanation:
Pb is a p - block metal. So d-d transition is not observed here.
CHXII08:THE D- & F-BLOCK ELEMENTS
321417
Match the following: Column I Column II A \({\mathrm{\mathrm{Zn}^{2+}}}\) P \({\mathrm{\mathrm{d}^{8}}}\) configuration B \({\mathrm{\mathrm{Cu}^{2+}}}\) Q Colourless C \({\mathrm{\mathrm{Ni}^{2+}}}\) R \({\mathrm{\mu=1.73 \,\mathrm{BM}}}\)
\({\mathrm{\mathrm{Zn}^{+2}}}\) - no unpaired electrons, so colourless. \({\mathrm{\mathrm{Cu}^{+2}-\mu-1.73}}\) B.M, due to 1 unpaired \({\mathrm{\mathrm{e}^{-}}}\). \({\mathrm{\mathrm{Ni}^{+2}-\mathrm{d}^{8}}}\) configuration, as it lost \({\mathrm{2 \mathrm{e}^{-}}}\).
321414
Which of the following compounds is coloured?
1 \(\mathrm{TiCl}_{3}\)
2 \(\mathrm{FeCl}_{3}\)
3 \(\mathrm{CoCl}_{2}\)
4 All of these
Explanation:
The compounds having metal ions with unpaired electrons, are coloured. Thus, (1) In \(\mathrm{TiCl}_{3}, \mathrm{Ti}^{3+}=[\mathrm{Ar}] 3 \mathrm{~d}^{1}\) (one unpaired electron) (2) In \(\mathrm{FeCl}_{3}, \mathrm{Fe}^{3+}=[\mathrm{Ar}] 3 \mathrm{~d}^{5}\) (Five unpaired electrons) (3) In \(\mathrm{CoCl}_{2}, \mathrm{Co}^{2+}=[\mathrm{Ar}] 3 \mathrm{~d}^{7}\) (three unpaired electrons) Hence, all compounds given are coloured.
AIIMS - 2008
CHXII08:THE D- & F-BLOCK ELEMENTS
321415
Identify the oxidation states of titanium \(\mathrm{(Z=22)}\) and copper \(\mathrm{(Z=29)}\) in their colourless compounds.
1 \(\mathrm{\mathrm{Ti}^{3+}, \mathrm{Cu}^{2+}}\)
2 \(\mathrm{\mathrm{Ti}^{2+}, \mathrm{Cu}^{2+}}\)
3 \(\mathrm{\mathrm{Ti}^{4+}, \mathrm{Cu}^{+}}\)
4 \(\mathrm{\mathrm{Ti}^{4+}, \mathrm{Cu}^{2+}}\)
Explanation:
Electronic configuration of titanium (Ti) \(\mathrm{(\mathrm{Z}=22)}\) is \({{\rm{[Ar]}}_{{\rm{18}}}}{\rm{3}}{{\rm{d}}^{\rm{2}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}\). In case of \(\mathrm{\mathrm{Ti}^{4+}}\), the electronic configuration will be \({{\rm{[Ar]}}_{{\rm{18}}}}{\rm{3}}{{\rm{d}}^{\rm{0}}}{\rm{4}}{{\rm{s}}^{\rm{0}}}\) Similarly, electronic configuration of copper \(\mathrm{(\mathrm{Cu})}\) \(\mathrm{(Z=29)}\) is \(\mathrm{[A r]_{18} 3 d^{10} 4 s^{1}}\). On loosing one electron it acquires stable electronic configuration, i.e \({{\rm{[Ar]}}_{{\rm{18}}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}\). In both \({\rm{T}}{{\rm{i}}^{{\rm{4 + }}}}\) and \(\mathrm{\mathrm{Cu}^{+}}\)no unpaired electron is present. As a result, no d-d transition occur and therefore these are colourless in nature.
MHTCET - 2018
CHXII08:THE D- & F-BLOCK ELEMENTS
321416
d - d transition is not a reason for the colour of which of the following compounds?
1 \(\mathrm{FeI}_{3}\)
2 \(\mathrm{CrCl}_{3}\)
3 \(\mathrm{PbI}_{2}\)
4 None
Explanation:
Pb is a p - block metal. So d-d transition is not observed here.
CHXII08:THE D- & F-BLOCK ELEMENTS
321417
Match the following: Column I Column II A \({\mathrm{\mathrm{Zn}^{2+}}}\) P \({\mathrm{\mathrm{d}^{8}}}\) configuration B \({\mathrm{\mathrm{Cu}^{2+}}}\) Q Colourless C \({\mathrm{\mathrm{Ni}^{2+}}}\) R \({\mathrm{\mu=1.73 \,\mathrm{BM}}}\)
\({\mathrm{\mathrm{Zn}^{+2}}}\) - no unpaired electrons, so colourless. \({\mathrm{\mathrm{Cu}^{+2}-\mu-1.73}}\) B.M, due to 1 unpaired \({\mathrm{\mathrm{e}^{-}}}\). \({\mathrm{\mathrm{Ni}^{+2}-\mathrm{d}^{8}}}\) configuration, as it lost \({\mathrm{2 \mathrm{e}^{-}}}\).