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प्रश्न
Interstitial compounds are formed when small atoms are trapped inside the crystal lattice of metals. Which of the following is not the characteristic property of interstitial compounds?
पर्याय
They have high melting points in comparison to pure metals.
They are very hard.
They retain metallic conductivity.
They are chemically very reactive.
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उत्तर
They are chemically very reactive.
Explanation:
Interstitial compounds/alloys are substances that are formed when a small atom like carbon, hydrogen, boron, nitrogen can occupy space in their lattices. All the properties mentioned above are true for interstitial compounds except, they are chemically inert.
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संबंधित प्रश्न
Why do interstitial compounds have higher melting points than corresponding pure metals?
Account for the following:
Cr2+ is a strong reducing agent.
Out of Mn3+ and Cr3+, which is more paramagnetic and why ?
(Atomic nos. : Mn = 25, Cr = 24)
How would you account for the irregular variation of ionization enthalpies (first and second) in the first series of the transition elements?
Which is a stronger reducing agent, Cr2+ or Fe2+ and why?
Calculate the ‘spin only’ magnetic moment of \[\ce{M^{2+}_{( aq)}}\] ion (Z = 27).
Compare the stability of +2 oxidation state for the elements of the first transition series.
How would you account for the following?
Transition metals and their compounds act as catalysts.
Explain why transition metals and their compounds act as a catalyst.
Transition metals with lowest melting point is ______.
Transition elements show high melting points. Why?
Match the catalysts given in Column I with the processes given in Column II.
| Column I (Catalyst) | Column II (Process) |
| (i) \[\ce{Ni}\] in the presence of hydrogen | (a) Zieglar Natta catalyst |
| (ii) \[\ce{Cu2C12}\] | (b) Contact process |
| (iii) \[\ce{V2O5}\] | (c) Vegetable oil to ghee |
| (iv) Finely divided iron | (d) Sandmeyer reaction |
| (v) \[\ce{TiCl4 + Al (CH3)3}\] | (e) Haber's Process |
| (f) Decomposition of KCIO3 |
Match the solutions given in Column I and the colours given in Column II.
| Column I (Aqueous solution of salt) |
Column II (Colour) |
| (i) \[\ce{FeSO2.7H2O}\] | (a) Green |
| (ii) \[\ce{NiCl2.4H2O}\] | (b) Light pink |
| (iii) \[\ce{MnCl2.4H2O}\] | (c) Blue |
| (iv) \[\ce{CoC12,6H2O}\] | (d) Pale green |
| (v) \[\ce{Cu2 Cl2}\] | (e) Pink |
| (f) Colourless |
Assertion: Separation of \[\ce{Zr}\] and \[\ce{Hf}\] is difficult.
Reason: Because \[\ce{Zr}\] and \[\ce{Hf}\] lie in the same group of the periodic table.
Answer the following question:
Which element of the first transition series has highest third ionisation enthalpy?
Which of the following statements is not correct?
Which one of the following characters tie of the transition metal is associated with higher catalytic activity?
Which of the following ions will exhibit colour in aqueous solution?
A complex in which dsp2 hybridisation takes place is ______.
The trend of which property is represented by the following graph?
