Assertion (A): | The [Fe(NH3)2(CN)4]– shows geometrical isomerism. |
Reason (R): | [Fe(NH3)2(CN)4]– also show optical isomerism. |
1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
2. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
3. | (A) is True but (R) is False. |
4. | (A) is False but (R) is True. |
Given below are two statements:
Assertion (A): | Geometrical isomerism not possible in tetrahedral complexes. |
Reason (R): | Square planar complex may show geometrical isomerism. |
1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
2. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
3. | (A) is True but (R) is False. |
4. | (A) is False but (R) is True. |
The correct statements among the following are:
(I) | Valence bond theory cannot explain the color exhibited by transition metal complexes. |
(II) | Valence bond theory can predict quantitatively the magnetic properties of transition metal complexes. |
(III) | Valence bond theory cannot distinguish ligands as weak and strong field ones. |
1. (I), (II), and (III)
2. (II), and (III) only
3. (I), and (II) only
4. (I), and (III) only
Column I | Column II | ||
a. | K3[Fe(C2O4)3] | i. | Diamminechlorido(methylamine) platinum(II) chloride |
b. | [Co(NH3)5Cl]Cl2 | ii. | Potassium trioxalatoferrate(III) |
c. | [Pt(NH3)2Cl(NH2CH3)]Cl | iii. | Potassium tetrachlorido palladate(II) |
d. | K2[PdCl4] | iv. | Pentaamminechloridocobalt(III) chloride |
Statement I: | [Ni(CN)4]2− structure is tetrahedral and diamagnetic in nature. |
Statement II: | [NiCl4]2− structure is tetrahedral and diamagnetic in nature. |
Given below are two statements:
Assertion (A): | [NiCl4]2− is paramagnetic while [Ni(CO)4] is diamagnetic though both are tetrahedral. |
Reason (R): | CO is a strong field ligand, thus pairing of electrons takes place in [Ni(CO)4]. |
1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
2. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
3. | (A) is True but (R) is False. |
4. | (A) is False but (R) is True. |
I: | [Fe(H2O)6]3+ is strongly paramagnetic whereas [Fe(CN)6]3− is weakly paramagnetic. |
II: | [Fe(H2O)6]3+ has 4 unpaired electrons while [Fe(CN)6]3− has 5 unpaired electrons. |
1. Both I and II are true.
2. I is true and II is false.
3. Both I and II are false.
4. I is false but II is true.
a. | The hexaquamanganese(II) ion contains five unpaired electrons, while the hexacyanomanganese(II) ion contains only one unpaired electron. |
b. | [Mn(H2O)6]2+ is an outer sphere complex, and [Mn(CN)6]4− is an inner sphere complex. |
c. | Arrangement of the electrons in [Mn(CN)6]4− is t2g5eg0. |
Assertion (A): | ion shows magnetic moment corresponding to two unpaired electrons. |
Reason(R): | Because it has type hybridization. |
1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
2. | Both (A) and (R) are True and (R) is not the correct explanation of (A). |
3. | (A) is True but the (R) is False. |
4. | (A) is False but the (R) is True. |
Given below are two statements:
Assertion (A): | Complexes of the types MX6 and MX5L (where X and L represent unidentate ligands) do not exhibit geometrical isomerism. |
Reason (R): | Complexes with a coordination number of 6 do not display geometrical isomerism. |
1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
2. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
3. | (A) is True but (R) is False. |
4. | (A) is False but (R) is True. |