Advertisements
Advertisements
Question
Generally transition elements form coloured salts due to the presence of unpaired electrons. Which of the following compounds will be coloured in solid-state?
Options
\[\ce{Ag2SO4}\]
\[\ce{CuF2}\]
\[\ce{ZnF2}\]
\[\ce{Cu2Cl2}\]
Solution
\[\ce{CuF2}\]
Explanation:
\[\ce{Cu^{2+}}\] has 1 unpaired electron in \[\ce{CuF2}\], hence, it is coloured in solid state.
APPEARS IN
RELATED QUESTIONS
Explain why is Fe3+ more stable than Fe2+?
How would you account for the following : Transition metals form coloured compounds
Why are Mn2+ compounds more stable than Fe2+ towards oxidation to their +3 state?
How is the variability in oxidation states of transition metals different from that of the non-transition metals? Illustrate with examples.
Dissociation of H2S is suppressed in acidic medium.
Transition metals with lowest melting point is:
The halides of transition elements become more covalent with increasing oxidation state of the metal. Why?
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?
Write the number of unpaired electrons in Cr3+.
(Atomic number of Cr = 24)
A pair of coloured ions is ______.
