Advertisements
Advertisements
Questions
Account for the following:
Cr2+ is a strong reducing agent.
Give reasons for the following statement:
Cr2+ is a strong reducing agent.
Advertisements
Solution
Cr2+ is strongly reducing in nature. It has a d4 configuration. While acting as a reducing agent, it gets oxidised to Cr3+ (with electronic configuration d3). This d3 configuration can be written as \[\ce{t^3_{2g}}\] configuration, which is a more stable configuration.
APPEARS IN
RELATED QUESTIONS
In 3d series (Sc to Zn), which element has the lowest enthalpy of atomisation and why?
What are the transition elements? Write two characteristics of the transition elements.
Out of Mn3+ and Cr3+, which is more paramagnetic and why ?
(Atomic nos. : Mn = 25, Cr = 24)
An antifriction alloy made up of antimony with tin and copper, which is extensively used in machine bearings is called _______.
(A) Duralumin
(B) Babbitt metal
(C) Spiegeleisen
(D) Amalgam
Give reasons: Sc3+ is colourless in aqueous solution whereas Ti3+ is coloured.
Highest oxidation state of manganese in fluoride is \[\ce{+4 (MnF4)}\] but highest oxidation state in oxides is \[\ce{+7 (Mn2O7)}\] because ______.
Transition elements show high melting points. Why?
Ionisation enthalpies of Ce, Pr and Nd are higher than Th, Pa and U. Why?
Account for the following:
Ce4+ is a strong oxidising agent.
Give a reason for the following:
Transition metals possess a great tendency to form complex compounds.
