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171. Write down the number of 3d electrons in each of the following ions : Ti²⁺, V²⁺, Cr³⁺, Mn²⁺, Fe²⁺, Fe³⁺, Co²⁺, Ni²⁺ and Cu²⁺. Indicate how would you expect the five 3d orbitals to be occupied for these hydrated ions (octahedral)

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172.

Comment on the statement that elements of the first transition series possess many properties different from those of heavier transition elements.

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173.

Mention the direct consequence of the following factors on the chemical behaviour of the transition elements.
(i) They have in completely filled d-orbitals in the ground state or in one of the oxidised states of their atoms.
(ii) They contribute more valence electrons per atom in the formation of metallic bonds?

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174. Why do the d-block elements exhibit a large number of oxidation states than the f-block elements?

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175. How do the transition elements form interstitial compounds? State an industrial advantage of such occurrence.

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176. Of the ions Co²⁺, Sc³⁺ and Cr³⁺ which one will give coloured aqueous solutions and will have each of them respond to a magnetic field and why? [Atomic numbers, Co = 27, Sc = 21, Cr = 24]

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177. Except La³⁺, Ce⁴⁺ and Yb²⁺, Lu³⁺ all lanthanoids are paramagnetic. Why?

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178.

What is the general trend of the ionisation enthalpies in the lanthanoids?

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179.

Explain the following facts:
Transition metals acts as catalyst.

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180.
Explain the following facts:
Chromium group elements have highest melting points in their respectively series.

Chromium has a highest melting oint because of the half filled stability, it has configuration 4s¹ 3d⁵
Due to the half filled d- orbital due to presence of unpaired electron they form strong intermetallic bonds (formed by valence electrons and covalent bonds formed due to d-d overlapping of impaired d-electrons.) hence result in high melting point.

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