Question

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Answer 1

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(i) ${Cd}^{2+}$ salts are white because ${Cd}^{2+}$ has completely filled d orbitals due to which d-d transition will not take place.

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(ii) It is so because of lanthanoid contraction. This is associated with the intervention of the 4f orbitals which are filled before the 5d series of elements. This results in a regular decrease in atomic radii which compensates the expected increase in atomic size with increasing atomic number.

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(iii) Due to large size of transition metals, they can trap atoms of other elements that have small atomic size as such as H, C,N, in the interstitial sites of their crystal lattices. So, they are known to form interstitial compounds.

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(iv) This is due to the large number of unpaired electrons in D orbitals in the middle of the series.

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(v) ${Hg}^{+}$ has [Xe] 4${f}^{14}$ 5${d}^{10}$ 6${s}^{1}$ configuration and thus ${Hg}^{+}$ ion supposed to show paramagnetic nature due to unpaired electron but it shows diamagnetic nature that means it exists as ${Hg_2}^{2+}$.

${Cu}^{+}$ ions are diamagnetic with configuration [Ar] 3${d}^{10}$. Hence, they do not dimerize to ${Cu_2}^{2+}$ and thus written as ${Cu}^{+}$.

Answer 2

1. Transition elements exhibit color to d-d transition.
D-d transition will be possible only when d subshell us not fully filled. In the electronic configuration of Cd2 , d subshell is fully filled, thus d-d transition will not take place, hence cd+2 is white.

2. It is because of Lanthanoid Contraction

3. Because there are vacant spaces in the lattic of transtional metals which can be filled by small atoms like H, C, N etc.

4. In each of these elements the highest oxidation state is equal to the total number of 3d and 4s electrons.

5. Mercurous ions Hg2 are having Hg in +1 oxidation state. Cu also haves +1 oxidation state, Mercury ions is having a metal - metal bond, so we wrire in the Mercurous ion as Hg2+ to show that it also haves a metal - metal bond between mercury atoms.