Advertisements
Advertisements
प्रश्न
Give reasons Iron has the higher enthalpy of atomization than that of copper.
Advertisements
उत्तर १
Iron has more number of the unpaired electron. Hence, it will have strong interatomic interaction than copper.
उत्तर २
Metallic bond in iron is stronger than that of copper. This is due to the presence of higher number of
unpaired electrons in iron.
APPEARS IN
संबंधित प्रश्न
Which metal in the first transition series (3d series) exhibits + 1 oxidation state most frequently and why?
How would you account for the following?
Transition metals exhibit variable oxidation states.
Calculate magnetic moment of `Fe_((aq))^(2+) ion (Z=26).`
Calculate the number of unpaired electrons in the following gaseous ions:
Mn3+, Cr3+, V3+ and Ti3+. Which one of these is the most stable in an aqueous solution?
NF3 is possible, but NF5 is not. Why?
Following are the transition metal ions of 3d series:
Ti4+, V2+, Mn3+, Cr3+
(Atomic numbers: Ti = 22, V = 23, Mn = 25, Cr = 24)
Answer the following:
1) Which ion is most stable in an aqueous solution and why?
2) Which ion is a strong oxidising agent and why?
3) Which ion is colourless and why?
Which of the following maxm magnetic moment?
Assertion (A): Transition metals have high enthalpy of atomisation.
Reason (R): Greater number of unpaired electrons in transition metals results in weak metallic bonding.
The given graph shows the trends in melting points of transition metals:
Explain the reason why Cr has the highest melting point and manganese (Mn) has a lower melting point.
Compare the general characteristics of the first series of the transition metals with those of the second and third series metals in the respective vertical columns. Give special emphasis on the following point:
Atomic sizes
