HgCl₂ and SnCl₂

HgCl₂ and SnCl₄

SnCl₄ and FeCl₃

SnCl₄ and PbCl₄

Fe⁺³

Mn⁺²

Co⁺²

Cu⁺²

59

95

102

104

V>Cr>Mn

V<Cr<Mn

V<Cr>Mn

V>Cr<Mn

Red precipitate

Blue precipitate

Yellow precipitate

No precipitate

O₂ oxidises Mn²⁺ to Mn³⁺

O₂ oxidises both Mn⁺² to Mn⁺³ and Fe²⁺ to Fe³⁺

Fe³⁺ oxidises H₂O to O₂

Mn³⁺ oxidised H₂O to O₂

Re-Re bond length is abnormally short

Re-Re bond is comprised of one $\mathrm{\sigma }, \mathrm{two} \mathrm{\pi } \mathrm{and} \mathrm{one} \mathrm{\delta } \mathrm{bond}$

If Re-Re bond points along z-axis, then square planar ReX₄ unit will use s, p_x, p_y and d_x²-y² orbitals for the formation of four Re-X $\mathrm{\sigma }$ bonds

d_xy orbitals will overlap to form $\mathrm{\delta }$-bond

(I), (II)

(I), (III)

(II), (III)

(I), (II) & (III)

Ce⁺³

Pm⁺²

Lu⁺³

Eu⁺²

Na₂CrO₄ and Na₂Cr₂O₇

Cr(OH)₃ and Na₂Cr₂O₇

Cr₂(CO₃)₃ and Fe₂(SO₄)₃

Cr(OH)₃ and Na₂CrO₄

V²⁺ < Cr²⁺ < Mn²⁺ < Fe²⁺ : Paramagnetic behaviour

Ni²⁺ < Co²⁺ < Fe²⁺ < Mn²⁺ : Ionic size

Co³⁺ < Fe³⁺ < Cr³⁺ < Sc³⁺ : Stability in aqueous solution

Sc < Ti < Cr < Mn : Number of oxidation states

[Rn]7s²

[Xe]4f⁷5d¹6s²

[Xe]5d¹6s²

[Rn]5f⁷6d¹7s²

Sm, Tb, Gd

Sm, Eu, Yb

La, Gd, Lu

Yb, Pm, Sm

Cu(NO₃)₂, and NO₂

 $\mathrm{Cu}{\left({\mathrm{NO}}_3\right)}_{\mathrm{2,}} \mathrm{and}$ NO

 $\mathrm{Cu}{\left({\mathrm{NO}}_3\right)}_2, \mathrm{NO,} \mathrm{and} {\mathrm{NO}}_2$

 $\mathrm{Cu}{\left({\mathrm{NO}}_3\right)}_{\mathrm{2,}} \mathrm{and} {\mathrm{N}}_2\mathrm{O}$

4.90 BM

5.92 BM

2.84 BM

3.87 BM

  The transition metals and their compounds are known for their catalytic activity due to their ability to adopt multiple oxidation states and to form complexes. 

  Interstitial compounds are those that are formed when small atoms like H, C or N are trapped inside the crystal lattices of metals.

  The oxidation states of chromium in $Cr{O}_4^{2-}$ and $C{r}_2{O}_7^{2-}$ are not the same.

  $C{r}^{2+}\left(d^4\right)$ is a stronger reducing agent than $F{e}^{2+}\left(d^6\right)$ in water. 

(Molecular weight)/2

(Molecular weight)/6

(Molecular weight)/3

same as molecular weight

3

4

5

6

Iron, and ${\mathrm{H}}_2{\mathrm{SO}}_4$ (aq)

Iron, and steam

Copper, and HCl(g)

Sodium, and ethyl alcohol

4,3,1,5

1,5,3,7

1,3,4,5

3,5,7,1

 $S{O}_2$

 $FeC{l}_3$

 $H_2{O}_2$

 $FeS{O}_4$

In the highest oxidation states of the first five transition element (Sc to

Once the d${}^5$ configuration is exceeded, the tendency to involve all the 3d

In the highest oxidation states, the transition metal show basic character

In addition to the normal oxidation states, the zero oxidation state is also

The ionic sizes of Ln (III) decrease in general with increasing atomic

Ln (III) compounds are generally colourless. 

Ln (III) hydroxides are mainly basic in character.

Because of the large size of the Ln (III) ions the bonding in its compounds

(a)-(i), (b)-(iv) ,(c)-(ii), (d)-(iii)

(a)-(iii), (b)-(iv), (c)-(i) ,(d)-(ii)

(a)-(iii) ,(b)-(i) ,(c)-(iv), (d)-(ii)

(a)-(ii), (b)-(iv), (c)-(i), (d)-(iii)

Zirconium, and Hofnium have identical radii of 160 pm and 159 pm, respectively as a consequence of lanthanoid contraction.

Lanthanoids reveal only a +3 oxidation state.

The lanthanoid ions other than the ${\mathrm{f}}^0$ types and the ${\mathrm{f}}^{14}$ type are all paramagnetic.

The overall decrease in atomic, and ionic radii from lanthanum to lutetium is called lanthanoid contraction.

 $3 \mathrm{Cu}+8{\mathrm{HNO}}_3 \to 3\mathrm{Cu} {\left({\mathrm{NO}}_3\right)}_2 + 2\mathrm{NO} + 4{\mathrm{H}}_2\mathrm{O}$

 $\mathrm{Cu} +\hspace{0.17em}4{\mathrm{HNO}}_3 \to 3\mathrm{Cu}{\left({\mathrm{NO}}_3\right)}_2 +\hspace{0.17em}2{\mathrm{NO}}_2 +\hspace{0.17em}2{\mathrm{H}}_2\mathrm{O}$

Both (1), and (2)

None of the above

25

26

27

24

Fe 

Ni

Co

Cu

Ag₂SO₄

CuF₂

ZnF₂

Cu₂Cl₂