Transition metal ions show colour because
they absorb light
They emit light
They are paramagentic
they exhibit d-d transition
Transitional metal ions have an ability of complex formation. They have this tendency due to
catalytic property
high enthalpy of atomisation
high nuclear charge
All of the above
In the reduction of KMnO4 by warm acidified oxalic acid, the oxidation number of Mn changes from
+4 to +2
+6 to +4
+7 to +2
+7 to +4
Transition metals have the electronic configuration (n -1)d1-10ns1-2. The d-orbitals are degenerate. Colour of transition metal ions is due to absorption of some wavelength. This result is
d-s transition
s-d transition
s-s transition
d-d transition
Manganese salt + PbO2 + conc. HNO3 → the solution acquires purple colour. The colour is due to
Mn(NO3)2
Pb(NO3)2
HMnO4
MnO
Acidified solution of chromic acid on treatment with H2O2 yields
CrO3 + H2O + O2
Cr2O3 + H2O + O2
CrO5 + H2O
H2Cr2O7 + H2O + O2
What is the change in the oxidation state of Mn in the reaction of MnO with H2O4 in acidic medium?
7 ➔4
6➔4
7➔2
6➔2
The following reaction occurs in acidic medium KMnO4 + 8H+ + 5e- → K+ + Mn2+ + 4H2O. What is the equivalent weight of KMnO4 ?
(Molecular weight of KMnO4 = 158)
79.0
31.6
158.0
39.5