Q. Name the oxometal anions of the first series of the transition metals in which the metal exhibits the oxidation state equal to its group number.

Q. Describe the oxidising action of potassium dichromate and write the ionic equations for its reaction with:
(i) iodide (ii) iron(II) solution and (iii) $H_{2}S$

Q. What is meant by lanthanoid contraction? The actinoid contraction is greater than that of lanthanoid contraction. Why?

Q. In what way is the electronic configuration of the transition elements different from that of the non transition elements?

Q. Describe the preparation of potassium dichromate from iron chromite ore. What is the effect of increasing pH on a solution of potassium dichromate?

Q. To what extent do the electronic configurations decide the stability of oxidation states in the first series of the transition elements? Illustrate your answer with examples.

Q. Compare the chemistry of actinoids with that of the lanthanoids with special reference to: (i) electronic configuration (ii) atomic and ionic sizes and (iii) oxidation state (iv) chemical reactivity.

Q. What may be the stable oxidation state of the transition element with the following d electron configurations in the ground state of their atoms: $3d^3,3d^5,3d^8$ and $3d^4$?

Q. What are the different oxidation states exhibited by the lanthanoids?

Q. Explain briefly how $+2$ state becomes more and more stable in the first half of the first row transition elements with increasing atomic number?

Q. Predict which of the following will be coloured in aqueous solution? $T{i}^{3+},V^{3+},C{u}^{+},S{c}^{3+},M{n}^{2+},F{e}^{3+}$ and $C{o}^{2+}$. Give reasons for each

Q. What are the characteristics of the transition elements and why they are called as transition elements? Which of the d-block elements may not be regarded as the transition elements?

Q. How would you account for the following:
(i) Of the $d^4$ species, $C{r}^{2+}$ is strongly reducing while manganese(III) is strongly oxidising.
(ii) Cobalt(II) is stable in aqueous solution but in the presence of complexing reagents it is easily oxidised.
(iii) The $d^1$ configuration is very unstable in ions

Q. What are interstitial compounds? Why are such compounds well known for transition metals?

Q. Write down the electronic configuration of:
(i) $C{r}^{3+}$ (ii) $P{m}^{3+}$ (iii) $C{u}^{+}$ (iv) $C{e}^{4+}$ (v) $C{o}^2+$ (vi) $L{u}^{2+}$ (vii) $M{n}^{2+}$ (viii) $T{h}^{4+}$

Q. How is the variability in oxidation states of transition metals different from that of the non transition metals? Illustrate with examples

Q. Describe the preparation of potassium permanganate. How does the acidified permanganate solution react with (i) iron(II) ions (ii) $S{O}_2$ and (iii) oxalic acid? Write the ionic equations for the reactions.

Q. Explain given reasons:

Q. Compare the stability of $+2$ oxidation state for the elements of the first transition series.

Q. For $M^{2+}/M$ and $M^{3+}/M^{2+}$ systems the $E^{\ominus }$ values for some metals are as follows:

$C{r}^{2+}/Cr$	$-0.9V$$	$C{r}^3/C{r}^{2+}$	$-0.4V$
$M{n}^{2+}/Mn$	$-1.2V$	$M{n}^{3+}/M{n}^{2+}$	$+1.5V$
$F{e}^{2+}/Fe$	$-0.4V$	$F{e}^{3+}/F{e}^{2+}$	$+0.8V$

Use this data to comment upon:
(i) the stability of $F{e}^{3+}$ in acid solution as compared to that of $C{r}^{3+}$ or $M{n}^{3+}$ and
(ii) the ease with which iron can be oxidised as compared to a similar process for either chromium or manganese metal