321637
The electronic configuration of transition element ' X ' is \({\mathrm{[\mathrm{Ar}] 3 \mathrm{~d}^{5}}}\) in its +3 oxidation state. What is its atomic number?
1 26
2 24
3 23
4 21
Explanation:
\({\mathrm{\mathrm{Fe}^{3+}=[\mathrm{Ar}] 3 \mathrm{~d}^{5}}}\) \({\mathrm{{ }_{26} \mathrm{Fe}=[\mathrm{Ar}] 3 \mathrm{~d}^{6} 4 \mathrm{~s}^{2}}}\) So atomic number is 26. So, the correct option is (1).
CHXII08:THE D- & F-BLOCK ELEMENTS
321638
In which one of the following pairs, both the elements does not have \({\text{(n - 1)}}{{\text{d}}^{{\text{10}}}}{{\text{ns}}^{\text{2}}}\) configuration in its elementary state?
321639
The number of d-electrons in \(\mathrm{\mathrm{Fe}^{2+}(\mathrm{Z}}\) of \(\mathrm{\mathrm{Fe}=}\) 26) is not equal to that of the :
1 p-electrons in \({\rm{Ne}}\,\,{\rm{(Z = 10)}}\)
2 s-electrons in \({\rm{Mg}}\,\,{\rm{(Z = 12)}}\)
3 d-electrons in \({\rm{Fe}}\,\,{\rm{(Z = 26)}}\)
4 p-electrons in \(\mathrm{\mathrm{Cl}^{-}(\mathrm{Z}}\) of \(\mathrm{\mathrm{Cl}=17)}\)
Explanation:
p-electrons in \(\mathrm{\mathrm{Cl}^{-}}\)(atomic number of \(\mathrm{\mathrm{Cl}}\) \(\mathrm{=17}\)) \({\rm{C}}{{\rm{l}}^{\rm{ - }}} \to {\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}\) \({\rm{F}}{{\rm{e}}^{{\rm{2 + }}}} \to {\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{\rm{6}}}\) In \(\mathrm{\mathrm{Fe}^{2+}}\), the total number of d-electrons is 6 , which is not equal to \(\mathrm{\mathrm{p}}\)-electrons in \(\mathrm{\mathrm{Cl}^{-}(=12)}\).
CHXII08:THE D- & F-BLOCK ELEMENTS
321640
Which of the following has maximum number of unpaired \(\mathrm{d}\) - electrons?
1 \(\mathrm{Fe}^{2+}\)
2 \(\mathrm{Cu}^{+}\)
3 \(\mathrm{Zn}\)
4 \(\mathrm{Ni}^{3+}\)
Explanation:
(1) \(\mathrm{Fe}^{2+}=[\mathrm{Ar}] 3 \mathrm{~d}^{6} 4 \mathrm{~s}^{0}\) \(\Rightarrow 4\) unpaired electrons (2) \(\mathrm{Cu}^{+}=[\mathrm{Ar}] 3 \mathrm{~d}^{10} 4 \mathrm{~s}^{0}\) \(\Rightarrow\) No unpaired electron (3) \(\mathrm{Zn}=[\mathrm{Ar}] 3 \mathrm{~d}^{10} 4 \mathrm{~s}^{2}\) \(\Rightarrow\) No unpaired electron (4) \(\mathrm{Ni}^{3+}=[\mathrm{Ar}] 3 \mathrm{~d}^{7} 4 \mathrm{~s}^{0}\) \(\Rightarrow 3\) unpaired electrons
AIIMS - 2017
CHXII08:THE D- & F-BLOCK ELEMENTS
321641
The number of d-electrons present in \(\mathrm{Ni}^{2+}\) ions is _____.
321637
The electronic configuration of transition element ' X ' is \({\mathrm{[\mathrm{Ar}] 3 \mathrm{~d}^{5}}}\) in its +3 oxidation state. What is its atomic number?
1 26
2 24
3 23
4 21
Explanation:
\({\mathrm{\mathrm{Fe}^{3+}=[\mathrm{Ar}] 3 \mathrm{~d}^{5}}}\) \({\mathrm{{ }_{26} \mathrm{Fe}=[\mathrm{Ar}] 3 \mathrm{~d}^{6} 4 \mathrm{~s}^{2}}}\) So atomic number is 26. So, the correct option is (1).
CHXII08:THE D- & F-BLOCK ELEMENTS
321638
In which one of the following pairs, both the elements does not have \({\text{(n - 1)}}{{\text{d}}^{{\text{10}}}}{{\text{ns}}^{\text{2}}}\) configuration in its elementary state?
321639
The number of d-electrons in \(\mathrm{\mathrm{Fe}^{2+}(\mathrm{Z}}\) of \(\mathrm{\mathrm{Fe}=}\) 26) is not equal to that of the :
1 p-electrons in \({\rm{Ne}}\,\,{\rm{(Z = 10)}}\)
2 s-electrons in \({\rm{Mg}}\,\,{\rm{(Z = 12)}}\)
3 d-electrons in \({\rm{Fe}}\,\,{\rm{(Z = 26)}}\)
4 p-electrons in \(\mathrm{\mathrm{Cl}^{-}(\mathrm{Z}}\) of \(\mathrm{\mathrm{Cl}=17)}\)
Explanation:
p-electrons in \(\mathrm{\mathrm{Cl}^{-}}\)(atomic number of \(\mathrm{\mathrm{Cl}}\) \(\mathrm{=17}\)) \({\rm{C}}{{\rm{l}}^{\rm{ - }}} \to {\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}\) \({\rm{F}}{{\rm{e}}^{{\rm{2 + }}}} \to {\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{\rm{6}}}\) In \(\mathrm{\mathrm{Fe}^{2+}}\), the total number of d-electrons is 6 , which is not equal to \(\mathrm{\mathrm{p}}\)-electrons in \(\mathrm{\mathrm{Cl}^{-}(=12)}\).
CHXII08:THE D- & F-BLOCK ELEMENTS
321640
Which of the following has maximum number of unpaired \(\mathrm{d}\) - electrons?
1 \(\mathrm{Fe}^{2+}\)
2 \(\mathrm{Cu}^{+}\)
3 \(\mathrm{Zn}\)
4 \(\mathrm{Ni}^{3+}\)
Explanation:
(1) \(\mathrm{Fe}^{2+}=[\mathrm{Ar}] 3 \mathrm{~d}^{6} 4 \mathrm{~s}^{0}\) \(\Rightarrow 4\) unpaired electrons (2) \(\mathrm{Cu}^{+}=[\mathrm{Ar}] 3 \mathrm{~d}^{10} 4 \mathrm{~s}^{0}\) \(\Rightarrow\) No unpaired electron (3) \(\mathrm{Zn}=[\mathrm{Ar}] 3 \mathrm{~d}^{10} 4 \mathrm{~s}^{2}\) \(\Rightarrow\) No unpaired electron (4) \(\mathrm{Ni}^{3+}=[\mathrm{Ar}] 3 \mathrm{~d}^{7} 4 \mathrm{~s}^{0}\) \(\Rightarrow 3\) unpaired electrons
AIIMS - 2017
CHXII08:THE D- & F-BLOCK ELEMENTS
321641
The number of d-electrons present in \(\mathrm{Ni}^{2+}\) ions is _____.
321637
The electronic configuration of transition element ' X ' is \({\mathrm{[\mathrm{Ar}] 3 \mathrm{~d}^{5}}}\) in its +3 oxidation state. What is its atomic number?
1 26
2 24
3 23
4 21
Explanation:
\({\mathrm{\mathrm{Fe}^{3+}=[\mathrm{Ar}] 3 \mathrm{~d}^{5}}}\) \({\mathrm{{ }_{26} \mathrm{Fe}=[\mathrm{Ar}] 3 \mathrm{~d}^{6} 4 \mathrm{~s}^{2}}}\) So atomic number is 26. So, the correct option is (1).
CHXII08:THE D- & F-BLOCK ELEMENTS
321638
In which one of the following pairs, both the elements does not have \({\text{(n - 1)}}{{\text{d}}^{{\text{10}}}}{{\text{ns}}^{\text{2}}}\) configuration in its elementary state?
321639
The number of d-electrons in \(\mathrm{\mathrm{Fe}^{2+}(\mathrm{Z}}\) of \(\mathrm{\mathrm{Fe}=}\) 26) is not equal to that of the :
1 p-electrons in \({\rm{Ne}}\,\,{\rm{(Z = 10)}}\)
2 s-electrons in \({\rm{Mg}}\,\,{\rm{(Z = 12)}}\)
3 d-electrons in \({\rm{Fe}}\,\,{\rm{(Z = 26)}}\)
4 p-electrons in \(\mathrm{\mathrm{Cl}^{-}(\mathrm{Z}}\) of \(\mathrm{\mathrm{Cl}=17)}\)
Explanation:
p-electrons in \(\mathrm{\mathrm{Cl}^{-}}\)(atomic number of \(\mathrm{\mathrm{Cl}}\) \(\mathrm{=17}\)) \({\rm{C}}{{\rm{l}}^{\rm{ - }}} \to {\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}\) \({\rm{F}}{{\rm{e}}^{{\rm{2 + }}}} \to {\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{\rm{6}}}\) In \(\mathrm{\mathrm{Fe}^{2+}}\), the total number of d-electrons is 6 , which is not equal to \(\mathrm{\mathrm{p}}\)-electrons in \(\mathrm{\mathrm{Cl}^{-}(=12)}\).
CHXII08:THE D- & F-BLOCK ELEMENTS
321640
Which of the following has maximum number of unpaired \(\mathrm{d}\) - electrons?
1 \(\mathrm{Fe}^{2+}\)
2 \(\mathrm{Cu}^{+}\)
3 \(\mathrm{Zn}\)
4 \(\mathrm{Ni}^{3+}\)
Explanation:
(1) \(\mathrm{Fe}^{2+}=[\mathrm{Ar}] 3 \mathrm{~d}^{6} 4 \mathrm{~s}^{0}\) \(\Rightarrow 4\) unpaired electrons (2) \(\mathrm{Cu}^{+}=[\mathrm{Ar}] 3 \mathrm{~d}^{10} 4 \mathrm{~s}^{0}\) \(\Rightarrow\) No unpaired electron (3) \(\mathrm{Zn}=[\mathrm{Ar}] 3 \mathrm{~d}^{10} 4 \mathrm{~s}^{2}\) \(\Rightarrow\) No unpaired electron (4) \(\mathrm{Ni}^{3+}=[\mathrm{Ar}] 3 \mathrm{~d}^{7} 4 \mathrm{~s}^{0}\) \(\Rightarrow 3\) unpaired electrons
AIIMS - 2017
CHXII08:THE D- & F-BLOCK ELEMENTS
321641
The number of d-electrons present in \(\mathrm{Ni}^{2+}\) ions is _____.
321637
The electronic configuration of transition element ' X ' is \({\mathrm{[\mathrm{Ar}] 3 \mathrm{~d}^{5}}}\) in its +3 oxidation state. What is its atomic number?
1 26
2 24
3 23
4 21
Explanation:
\({\mathrm{\mathrm{Fe}^{3+}=[\mathrm{Ar}] 3 \mathrm{~d}^{5}}}\) \({\mathrm{{ }_{26} \mathrm{Fe}=[\mathrm{Ar}] 3 \mathrm{~d}^{6} 4 \mathrm{~s}^{2}}}\) So atomic number is 26. So, the correct option is (1).
CHXII08:THE D- & F-BLOCK ELEMENTS
321638
In which one of the following pairs, both the elements does not have \({\text{(n - 1)}}{{\text{d}}^{{\text{10}}}}{{\text{ns}}^{\text{2}}}\) configuration in its elementary state?
321639
The number of d-electrons in \(\mathrm{\mathrm{Fe}^{2+}(\mathrm{Z}}\) of \(\mathrm{\mathrm{Fe}=}\) 26) is not equal to that of the :
1 p-electrons in \({\rm{Ne}}\,\,{\rm{(Z = 10)}}\)
2 s-electrons in \({\rm{Mg}}\,\,{\rm{(Z = 12)}}\)
3 d-electrons in \({\rm{Fe}}\,\,{\rm{(Z = 26)}}\)
4 p-electrons in \(\mathrm{\mathrm{Cl}^{-}(\mathrm{Z}}\) of \(\mathrm{\mathrm{Cl}=17)}\)
Explanation:
p-electrons in \(\mathrm{\mathrm{Cl}^{-}}\)(atomic number of \(\mathrm{\mathrm{Cl}}\) \(\mathrm{=17}\)) \({\rm{C}}{{\rm{l}}^{\rm{ - }}} \to {\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}\) \({\rm{F}}{{\rm{e}}^{{\rm{2 + }}}} \to {\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{\rm{6}}}\) In \(\mathrm{\mathrm{Fe}^{2+}}\), the total number of d-electrons is 6 , which is not equal to \(\mathrm{\mathrm{p}}\)-electrons in \(\mathrm{\mathrm{Cl}^{-}(=12)}\).
CHXII08:THE D- & F-BLOCK ELEMENTS
321640
Which of the following has maximum number of unpaired \(\mathrm{d}\) - electrons?
1 \(\mathrm{Fe}^{2+}\)
2 \(\mathrm{Cu}^{+}\)
3 \(\mathrm{Zn}\)
4 \(\mathrm{Ni}^{3+}\)
Explanation:
(1) \(\mathrm{Fe}^{2+}=[\mathrm{Ar}] 3 \mathrm{~d}^{6} 4 \mathrm{~s}^{0}\) \(\Rightarrow 4\) unpaired electrons (2) \(\mathrm{Cu}^{+}=[\mathrm{Ar}] 3 \mathrm{~d}^{10} 4 \mathrm{~s}^{0}\) \(\Rightarrow\) No unpaired electron (3) \(\mathrm{Zn}=[\mathrm{Ar}] 3 \mathrm{~d}^{10} 4 \mathrm{~s}^{2}\) \(\Rightarrow\) No unpaired electron (4) \(\mathrm{Ni}^{3+}=[\mathrm{Ar}] 3 \mathrm{~d}^{7} 4 \mathrm{~s}^{0}\) \(\Rightarrow 3\) unpaired electrons
AIIMS - 2017
CHXII08:THE D- & F-BLOCK ELEMENTS
321641
The number of d-electrons present in \(\mathrm{Ni}^{2+}\) ions is _____.
321637
The electronic configuration of transition element ' X ' is \({\mathrm{[\mathrm{Ar}] 3 \mathrm{~d}^{5}}}\) in its +3 oxidation state. What is its atomic number?
1 26
2 24
3 23
4 21
Explanation:
\({\mathrm{\mathrm{Fe}^{3+}=[\mathrm{Ar}] 3 \mathrm{~d}^{5}}}\) \({\mathrm{{ }_{26} \mathrm{Fe}=[\mathrm{Ar}] 3 \mathrm{~d}^{6} 4 \mathrm{~s}^{2}}}\) So atomic number is 26. So, the correct option is (1).
CHXII08:THE D- & F-BLOCK ELEMENTS
321638
In which one of the following pairs, both the elements does not have \({\text{(n - 1)}}{{\text{d}}^{{\text{10}}}}{{\text{ns}}^{\text{2}}}\) configuration in its elementary state?
321639
The number of d-electrons in \(\mathrm{\mathrm{Fe}^{2+}(\mathrm{Z}}\) of \(\mathrm{\mathrm{Fe}=}\) 26) is not equal to that of the :
1 p-electrons in \({\rm{Ne}}\,\,{\rm{(Z = 10)}}\)
2 s-electrons in \({\rm{Mg}}\,\,{\rm{(Z = 12)}}\)
3 d-electrons in \({\rm{Fe}}\,\,{\rm{(Z = 26)}}\)
4 p-electrons in \(\mathrm{\mathrm{Cl}^{-}(\mathrm{Z}}\) of \(\mathrm{\mathrm{Cl}=17)}\)
Explanation:
p-electrons in \(\mathrm{\mathrm{Cl}^{-}}\)(atomic number of \(\mathrm{\mathrm{Cl}}\) \(\mathrm{=17}\)) \({\rm{C}}{{\rm{l}}^{\rm{ - }}} \to {\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}\) \({\rm{F}}{{\rm{e}}^{{\rm{2 + }}}} \to {\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{\rm{6}}}\) In \(\mathrm{\mathrm{Fe}^{2+}}\), the total number of d-electrons is 6 , which is not equal to \(\mathrm{\mathrm{p}}\)-electrons in \(\mathrm{\mathrm{Cl}^{-}(=12)}\).
CHXII08:THE D- & F-BLOCK ELEMENTS
321640
Which of the following has maximum number of unpaired \(\mathrm{d}\) - electrons?
1 \(\mathrm{Fe}^{2+}\)
2 \(\mathrm{Cu}^{+}\)
3 \(\mathrm{Zn}\)
4 \(\mathrm{Ni}^{3+}\)
Explanation:
(1) \(\mathrm{Fe}^{2+}=[\mathrm{Ar}] 3 \mathrm{~d}^{6} 4 \mathrm{~s}^{0}\) \(\Rightarrow 4\) unpaired electrons (2) \(\mathrm{Cu}^{+}=[\mathrm{Ar}] 3 \mathrm{~d}^{10} 4 \mathrm{~s}^{0}\) \(\Rightarrow\) No unpaired electron (3) \(\mathrm{Zn}=[\mathrm{Ar}] 3 \mathrm{~d}^{10} 4 \mathrm{~s}^{2}\) \(\Rightarrow\) No unpaired electron (4) \(\mathrm{Ni}^{3+}=[\mathrm{Ar}] 3 \mathrm{~d}^{7} 4 \mathrm{~s}^{0}\) \(\Rightarrow 3\) unpaired electrons
AIIMS - 2017
CHXII08:THE D- & F-BLOCK ELEMENTS
321641
The number of d-electrons present in \(\mathrm{Ni}^{2+}\) ions is _____.
