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प्रश्न
Why do interstitial compounds have higher melting points than corresponding pure metals?
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उत्तर
The melting points of interstitial compounds are higher than those of pure metals because of bonding between the metal and the non-metal, which is stronger than metal–metal bonding.
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संबंधित प्रश्न
How would you account for the following?
Transition metals exhibit variable oxidation states.
ln which pair highest oxidation states of transition metals are found:
How would you account for the following : Transition metals form coloured compounds
Which is a stronger reducing agent, Cr2+ or Fe2+ and why?
Which of the d-block elements may not be regarded as the transition elements?
What are inner transition elements?
NF3 is possible, but NF5 is not. Why?
Give reasons: Sc3+ is colourless in aqueous solution whereas Ti3+ is coloured.
Explain why Mn2+ is more stable than Fe2+ towards oxidation to +3 state. (At. no. of Mn = 25, Fe = 26)
Maximum magnetic moment is shown by ____________.
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\[\ce{KMnO4}\] acts as an oxidising agent in acidic medium. The number of moles of \[\ce{KMnO4}\] that will be needed to react with one mole of sulphide ions in acidic solution is ______.
Although Zirconium belongs to 4d transition series and Hafnium to 5d transition series even then they show similar physical and chemical properties because ______.
Why is \[\ce{HCl}\] not used to make the medium acidic in oxidation reactions of \[\ce{KMnO4}\] in acidic medium?
EΘ of Cu is + 0.34V while that of Zn is – 0.76V. Explain.
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 |
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The orientation of an atomic orbital is governed by
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On adding NaOH, solution to the aqueous solution of K2CrO7 the colour of the solution changes from
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[Ti(H2O)]3+ is coloured while [Sc(H2O)6]3+ is colourless.
How is the variability in oxidation states of transition metals different from that of p-block elements?
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(Round off to the nearest integer).
[Given: `sqrt3 = 1.73, sqrt2 = 1.41`]
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Explain the use of different transition metals as catalysts.
Decide which of the following atomic numbers are the atomic numbers of the inner transition elements:
29, 59, 74, 95, 102, 104
