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प्रश्न
Give reasons for the following statement:
Transition metals and most of their compounds show paramagnetic behaviour.
Give reasons:
Transition metals show paramagnetism.
Why do most of the transition metals show paramagnetic behaviour?
Why do most of the transition metals and their compounds exhibit paramagnetic behaviour?
Explain giving reasons:
Transition metals and many of their compounds show paramagnetic behaviour.
Why do most of the transition metals and their compounds exhibit paramagnetic behaviour? How is their paramagnetic behaviour related to the number of unpaired electrons?
Explain the following:
Transition metals and their compounds generally exhibit a paramagnetic behaviour.
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उत्तर
- They have unpaired electrons in their (n − 1)d orbitals.
- The presence of these unpaired electrons causes attraction towards a magnetic field, resulting in paramagnetic behavior.
- The number of unpaired electrons increases from left to the middle of the transition series, so paramagnetism increases and then decreases towards the end.
- Transition metals or ions with all paired electrons show diamagnetism, not paramagnetism.
Thus, paramagnetism in transition metals arises from unpaired electrons in d-orbitals, causing magnetic moments.
Notes
Students can refer to the provided solutions based on their preferred marks.
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संबंधित प्रश्न
Calculate the ‘spin only’ magnetic moment of \[\ce{M^{2+}_{( aq)}}\] ion (Z = 27).
Use Hund’s rule to derive the electronic configuration of Ce3+ ion and calculate its magnetic moment on the basis of ‘spin-only’ formula.
Match the properties given in Column I with the metals given in Column II.
| Column I (Property) | Column II (Metal) | |
| (i) | Element with highest second ionisation enthalpy |
(a) \[\ce{Co}\] |
| (ii) | Element with highest third ionisation enthalpy |
(b) \[\ce{Cr}\] |
| (iii) | \[\ce{M}\] in \[\ce{M(CO)6}\] is | (c) \[\ce{Cu}\] |
| (iv) | Element with highest heat of atomisation |
(d) \[\ce{Zn}\] |
| (e) \[\ce{Ni}\] |
Assertion: \[\ce{Cu^2+}\] iodide is not known.
Reason: \[\ce{Cu^2+}\] oxidises \[\ce{I^-}\] to iodine.
Identify the metal and justify your answer.
\[\ce{MO3F}\]
Transition metals can act as catalysts because these can change their oxidation state. How does \[\ce{Fe(III)}\] catalyse the reaction between iodide and persulphate ions?
Why are fluorides of transition metals more stable in their higher oxidation state as compared to the lower oxidation state?
The number of terminal oxygen atoms present in the product B obtained from the following reactions is:
\[\ce{FeCr2O4 + Na2CO3 + O2 -> A + Fe2O3 + CO2}\]
\[\ce{A + H^+ -> B + H2O + Na^+}\]
Account for the following:
Eu2+ with electronic configuration [Xe]4f76s2 is a strong reducing agent.
Explain the magnetic properties of d-block (or transition) elements.
