NEET Test Series from KOTA - 10 Papers In MS WORD
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CHXII08:THE D- & F-BLOCK ELEMENTS
321517
Although \(\mathrm{\mathrm{Cr}^{3+}}\) and \(\mathrm{\mathrm{Co}^{2+}}\) ions have same number of unpaired electrons but the magnetic moment of \(\mathrm{\mathrm{Cr}^{3+}}\) is 3.87 B.M and that of \(\mathrm{\mathrm{Co}^{2+}}\) is 4.87 B.M because
1 Half filled configurations show no orbital contribution to magnetic moment due to symmetry.
2 Incompletely filled configurations show orbital contribution to magnetic moment.
3 Half filled configurations show orbital contribution in maganetic moment due to symmetry.
4 Both (1) & (2)
Explanation:
Due to symmetrical electronic configuration there is no orbital contribution in \(\mathrm{\mathrm{Cr}^{3+}}\) ion. However appreciable orbital contribution takes place in \(\mathrm{\mathrm{Co}^{2+}}\) ion.
CHXII08:THE D- & F-BLOCK ELEMENTS
321518
The element which shows only one oxidation state other than its elemental form is
1 cobalt
2 nickel
3 scandium
4 titanium
Explanation:
Sc shows only +3 oxidation state other than elemental state. \({\mathrm{\mathrm{Ni}, \mathrm{Ti}}}\) and Co show \({\mathrm{+2,+3}}\) and \({\rm{ + 4}}\) oxidation states. So, the correct option is (3).
JEE Main - 2024
CHXII08:THE D- & F-BLOCK ELEMENTS
321519
A transition metal ion exists in its highest oxidation state. It is expected to behave as
1 a chelating agent
2 a central metal in a coordination compound
3 an oxidising agent
4 a reducing agent.
Explanation:
When a transition metal ion exists in its highest oxidation state, it act as an oxidising agent. For example, \(\mathrm{\mathrm{Mn}}\) (VII) in \(\mathrm{\mathrm{KMnO}_{4}}\) is one of the strongest oxidising agent in solution.
KCET - 2006
CHXII08:THE D- & F-BLOCK ELEMENTS
321520
The halides of transition elements become more covalent with increasing oxidation state \(\left( {{\rm{OS}}} \right)\) of the metal. Why?
1 As OS increases ionic character increases
2 As OS increases covalent character increases.
3 As OS increases covalent character decreases
4 OS has nothing to do with covalent character
Explanation:
As the oxidation state increases, size of the ion of transition element decreases. As per Fajan's rule, as the size of metal ion decreases, covalent character of the bond formed increases.
321517
Although \(\mathrm{\mathrm{Cr}^{3+}}\) and \(\mathrm{\mathrm{Co}^{2+}}\) ions have same number of unpaired electrons but the magnetic moment of \(\mathrm{\mathrm{Cr}^{3+}}\) is 3.87 B.M and that of \(\mathrm{\mathrm{Co}^{2+}}\) is 4.87 B.M because
1 Half filled configurations show no orbital contribution to magnetic moment due to symmetry.
2 Incompletely filled configurations show orbital contribution to magnetic moment.
3 Half filled configurations show orbital contribution in maganetic moment due to symmetry.
4 Both (1) & (2)
Explanation:
Due to symmetrical electronic configuration there is no orbital contribution in \(\mathrm{\mathrm{Cr}^{3+}}\) ion. However appreciable orbital contribution takes place in \(\mathrm{\mathrm{Co}^{2+}}\) ion.
CHXII08:THE D- & F-BLOCK ELEMENTS
321518
The element which shows only one oxidation state other than its elemental form is
1 cobalt
2 nickel
3 scandium
4 titanium
Explanation:
Sc shows only +3 oxidation state other than elemental state. \({\mathrm{\mathrm{Ni}, \mathrm{Ti}}}\) and Co show \({\mathrm{+2,+3}}\) and \({\rm{ + 4}}\) oxidation states. So, the correct option is (3).
JEE Main - 2024
CHXII08:THE D- & F-BLOCK ELEMENTS
321519
A transition metal ion exists in its highest oxidation state. It is expected to behave as
1 a chelating agent
2 a central metal in a coordination compound
3 an oxidising agent
4 a reducing agent.
Explanation:
When a transition metal ion exists in its highest oxidation state, it act as an oxidising agent. For example, \(\mathrm{\mathrm{Mn}}\) (VII) in \(\mathrm{\mathrm{KMnO}_{4}}\) is one of the strongest oxidising agent in solution.
KCET - 2006
CHXII08:THE D- & F-BLOCK ELEMENTS
321520
The halides of transition elements become more covalent with increasing oxidation state \(\left( {{\rm{OS}}} \right)\) of the metal. Why?
1 As OS increases ionic character increases
2 As OS increases covalent character increases.
3 As OS increases covalent character decreases
4 OS has nothing to do with covalent character
Explanation:
As the oxidation state increases, size of the ion of transition element decreases. As per Fajan's rule, as the size of metal ion decreases, covalent character of the bond formed increases.
321517
Although \(\mathrm{\mathrm{Cr}^{3+}}\) and \(\mathrm{\mathrm{Co}^{2+}}\) ions have same number of unpaired electrons but the magnetic moment of \(\mathrm{\mathrm{Cr}^{3+}}\) is 3.87 B.M and that of \(\mathrm{\mathrm{Co}^{2+}}\) is 4.87 B.M because
1 Half filled configurations show no orbital contribution to magnetic moment due to symmetry.
2 Incompletely filled configurations show orbital contribution to magnetic moment.
3 Half filled configurations show orbital contribution in maganetic moment due to symmetry.
4 Both (1) & (2)
Explanation:
Due to symmetrical electronic configuration there is no orbital contribution in \(\mathrm{\mathrm{Cr}^{3+}}\) ion. However appreciable orbital contribution takes place in \(\mathrm{\mathrm{Co}^{2+}}\) ion.
CHXII08:THE D- & F-BLOCK ELEMENTS
321518
The element which shows only one oxidation state other than its elemental form is
1 cobalt
2 nickel
3 scandium
4 titanium
Explanation:
Sc shows only +3 oxidation state other than elemental state. \({\mathrm{\mathrm{Ni}, \mathrm{Ti}}}\) and Co show \({\mathrm{+2,+3}}\) and \({\rm{ + 4}}\) oxidation states. So, the correct option is (3).
JEE Main - 2024
CHXII08:THE D- & F-BLOCK ELEMENTS
321519
A transition metal ion exists in its highest oxidation state. It is expected to behave as
1 a chelating agent
2 a central metal in a coordination compound
3 an oxidising agent
4 a reducing agent.
Explanation:
When a transition metal ion exists in its highest oxidation state, it act as an oxidising agent. For example, \(\mathrm{\mathrm{Mn}}\) (VII) in \(\mathrm{\mathrm{KMnO}_{4}}\) is one of the strongest oxidising agent in solution.
KCET - 2006
CHXII08:THE D- & F-BLOCK ELEMENTS
321520
The halides of transition elements become more covalent with increasing oxidation state \(\left( {{\rm{OS}}} \right)\) of the metal. Why?
1 As OS increases ionic character increases
2 As OS increases covalent character increases.
3 As OS increases covalent character decreases
4 OS has nothing to do with covalent character
Explanation:
As the oxidation state increases, size of the ion of transition element decreases. As per Fajan's rule, as the size of metal ion decreases, covalent character of the bond formed increases.
NEET Test Series from KOTA - 10 Papers In MS WORD
WhatsApp Here
CHXII08:THE D- & F-BLOCK ELEMENTS
321517
Although \(\mathrm{\mathrm{Cr}^{3+}}\) and \(\mathrm{\mathrm{Co}^{2+}}\) ions have same number of unpaired electrons but the magnetic moment of \(\mathrm{\mathrm{Cr}^{3+}}\) is 3.87 B.M and that of \(\mathrm{\mathrm{Co}^{2+}}\) is 4.87 B.M because
1 Half filled configurations show no orbital contribution to magnetic moment due to symmetry.
2 Incompletely filled configurations show orbital contribution to magnetic moment.
3 Half filled configurations show orbital contribution in maganetic moment due to symmetry.
4 Both (1) & (2)
Explanation:
Due to symmetrical electronic configuration there is no orbital contribution in \(\mathrm{\mathrm{Cr}^{3+}}\) ion. However appreciable orbital contribution takes place in \(\mathrm{\mathrm{Co}^{2+}}\) ion.
CHXII08:THE D- & F-BLOCK ELEMENTS
321518
The element which shows only one oxidation state other than its elemental form is
1 cobalt
2 nickel
3 scandium
4 titanium
Explanation:
Sc shows only +3 oxidation state other than elemental state. \({\mathrm{\mathrm{Ni}, \mathrm{Ti}}}\) and Co show \({\mathrm{+2,+3}}\) and \({\rm{ + 4}}\) oxidation states. So, the correct option is (3).
JEE Main - 2024
CHXII08:THE D- & F-BLOCK ELEMENTS
321519
A transition metal ion exists in its highest oxidation state. It is expected to behave as
1 a chelating agent
2 a central metal in a coordination compound
3 an oxidising agent
4 a reducing agent.
Explanation:
When a transition metal ion exists in its highest oxidation state, it act as an oxidising agent. For example, \(\mathrm{\mathrm{Mn}}\) (VII) in \(\mathrm{\mathrm{KMnO}_{4}}\) is one of the strongest oxidising agent in solution.
KCET - 2006
CHXII08:THE D- & F-BLOCK ELEMENTS
321520
The halides of transition elements become more covalent with increasing oxidation state \(\left( {{\rm{OS}}} \right)\) of the metal. Why?
1 As OS increases ionic character increases
2 As OS increases covalent character increases.
3 As OS increases covalent character decreases
4 OS has nothing to do with covalent character
Explanation:
As the oxidation state increases, size of the ion of transition element decreases. As per Fajan's rule, as the size of metal ion decreases, covalent character of the bond formed increases.