Why is k4fe CN 6 diamagnetic but k3fe CN 6 is paramagnetic?

Since CN− ion is a strong field ligand, it causes the pairing of unpaired 3d electrons. CN– will cause pairing of electrons. It is diamagnetic in nature due to the unpaired electron.

Is the complex Fe CN 6 ]- 4 diamagnetic or paramagnetic?

Magnetic Moments of Molecules and Ions Many transition metal complexes have unpaired electrons and hence are paramagnetic. Molecules such as N2 and ions such as Na+ and [Fe(CN)6]4− that contain no unpaired electrons are diamagnetic.

How many unpaired electrons does the octahedral complex ion Fe CN 6 4 have in its low spin configuration?

[Fe(H2O)6]2+ is high spin d6, with μ = 4.9 µB; [Fe(CN)6]4– is low spin d6 , with μ = 0 µB. The average value is then 2 × 4.9/3 = 3.3 µB. 2.67 unpaired electrons gives μ = 2.67 × 4.67 = 3.53 µB. μ = n(n+ 2) = 3.9, 3.9, and 1.7 μB, respectively.

Which is a diamagnetic complex Fe?

[Fe(CN)6]4− In the above coordination complex, iron exists in the +II oxidation state. Since CN- is strong field ligand it cause pairing. hence it is diamagnetic. In this complex, the oxidation state of Fe is +3.

Why is K Fe CN paramagnetic?

As CN is a strong field ligand. So, it causes the pairing of electrons. So, As one electron is not paired, so potassium ferricyanide is paramagnetic in nature.

Is FeF6 3 an outer orbital complex?

[Fe(CN)6]3– is an inner orbital complex whereas [FeF6]3– is an outer orbital complex.

Is paramagnetic while is diamagnetic explain why?

Also, NH3 is a weak field ligand that does not cause the pairing of the electrons in the 3d orbital. Therefore, it undergoes d2sp3 hybridization and the electrons in the 3d orbitals remain unpaired. Hence, it is paramagnetic in nature. As there are no unpaired electrons, it is diamagnetic.

Is FeF6 3 paramagnetic?

[FeF6]^3 – is paramagnetic due to the presence of unpaired electrons in the complex.

Why is cof6 3 paramagnetic?

Because, the compound contain weak field ligand so electrons are not paired up. hence the compound is said to be paramagnetic. F is a weak field ligand so there will be 4 unpaired electrons in the d-orbital. so the compound is paramanetic.

Do you expect Fe CN 63 to be diamagnetic or paramagnetic explain?

Since CN− ion is a strong field ligand, it causes the pairing of unpaired 3d electrons. CN– will cause pairing of electrons. It is diamagnetic in nature due to the unpaired electron. Since there are 2 unpaired electrons in this case, it is paramagnetic in nature.

Is k3fe CN 6 paramagnetic or diamagnetic?

So, As all electrons are paired, potassium ferrocyanide is diamagnetic in nature. Similarly we have to find out the magnetic character of potassium ferricyanide. The formula of potassium ferricyanide is K3[Fe(CN)6].

Is CoF6 3 paramagnetic?

[CoF6]3- is paramagnetic. This complex is called high spin or spin free complex. When NH3 ligand attacks the central metal ion Co3+ , pairing of electrons in 3d orbital occurs against Hund’s rule.

Is [Fe(CN) 6] 4– complex ion diamagnetic in nature?

From the above crystal field splitting diagram of Fe (II) ion, it is evidently shown that, the Fe (II)ion have no unpaired electrons in its outer 3d-orbital. That is, all electrons are paired, hence [Fe (CN) 6] 4– complex ion is diamagnetic in nature.

Is [F E(C N)6]3+ ion paramagnetic or paramagnetic?

The given statement is true. [F e(C N)6 ]3+ ion strongly paramagnetic. ]3− ion. In both the complexes, Fe is in +3 oxidation state. F e3+ has [Ar]3d5 electronic configuration. Water is a weak field ligand. Spin pairing is not favored. Hence, [F e(H 2 ]3+ is high spin complex with 5 unpaired electrons. Cyanide ion is strong field ligand.

What is the hybridization of the complex ion [Fe(CN) 6]3-?

For the complex ion [Fe (CN) 6]3- , state (1) The type of hybridisation. (2) The magnetic behaviour (3) The oxidation number of the central metal atom. CN is a powerful field ligand and uses inner 3d-orbitals to form a low spin complex. Because there are 6 ligands, it has octahedral geometry. So the hybridization of the complex is d 2 sp 3.

What is the electronic configuration of Fe(II) ion under octahedral crystal field?

The ligand CN– which is a strong field ligand. Now, the valence shell electronic configuration of Fe (II) ion is [ Ar ] d6 . Again, since the ligand CN – is a strong field ligand, hence the complex is low spin one. Therefore, under the influence of the octahedral crystal field, the possible electronic arrangement of Fe (II) ion is t2g6, eg0.