The magnetic moment (mu) values for
Cs2 (MnCl4), k4 (Mn (CN) 6) and K2 (Ni (CN) 4) are
5.9 , 1.8 and 0 B.M, respectively. Explain the difference of these values based on the Valence bond theory.?
Ah, the world of magnetic moments. Let's dive into the Valence bond theory to explain the stark differences in these values!
First up, Cs2(MnCl4)! This little fella has a magnetic moment of 5.9 B.M. Well, Mn in this compound has an oxidation state of +4, which means it lost some of its electronegativity pizzazz. The unpaired electrons from the d-orbital of Mn create a net magnetic moment resulting from good old spin. They're just really into spinning!
Next, we have k4(Mn(CN)6). This compound boasts a magnetic moment of 1.8 B.M. Here, Mn exhibits an oxidation state of +2. As a result, all of its electrons are paired up in the d-orbital, leading to a lowered magnetic moment. It's like they brought along a magnetic partner and decided to do a synchronized dance routine!
Lastly, we encounter K2(Ni(CN)4), meandering in with its feeble magnetic moment of 0 B.M. In this compound, Ni proudly showcases an oxidation state of +2. Consequently, all of its d-electrons are paired up, rendering its magnetic moment as nonexistent as my social life at a clown party.
So, in a nutshell, the differences in magnetic moments among these compounds can be explained by the oxidation states and the electron pairing in the d-orbitals. It's like a symphony of unpaired electrons, synchronized dances, and lonely clowns in the world of magnetism!
According to the Valence Bond Theory, the magnetic moment of a compound depends on the number of unpaired electrons present on the central metal atom. Unpaired electrons generate magnetic moments, which can be measured in units of Bohr magnetons (B.M).
Let's analyze the compounds mentioned: Cs2(MnCl4), K4(Mn(CN)6), and K2(Ni(CN)4).
1. Cs2(MnCl4):
In this compound, each Mn atom is surrounded by four chloride (Cl) ligands. Chloride is a strong field ligand, which causes the electrons to pair up in the d orbitals of the Mn atom. As a result, all the electrons are paired, resulting in a diamagnetic compound with no unpaired electrons, and hence, a magnetic moment of 0 B.M.
2. K4(Mn(CN)6):
Here, each Mn atom is surrounded by six cyanide (CN) ligands. Cyanide is a weak field ligand, which doesn't strongly influence the electrons' pairing. The Mn atom in this compound has one unpaired electron, leading to a magnetic moment of 1.8 B.M.
3. K2(Ni(CN)4):
In this compound, each Ni atom is coordinated with four cyanide ligands. Similar to the previous compound, cyanide is a weak field ligand, allowing some unpaired electrons on the central Ni atom. The Ni atom in this compound has two unpaired electrons, resulting in a greater magnetic moment of 2.0 B.M.
In summary, the difference in magnetic moments of Cs2(MnCl4), K4(Mn(CN)6), and K2(Ni(CN)4) can be explained by the different ligand influences on the unpaired electrons present on the central metal atom according to the Valence Bond Theory.
To explain the difference in magnetic moment values of Cs2(MnCl4), K4(Mn(CN)6), and K2(Ni(CN)4) based on the Valence Bond Theory, we need to understand the concept of magnetic moment and its relationship with the bonding in these compounds.
Magnetic moment (μ) refers to the property of a substance to generate a magnetic field in response to an external magnetic field. It is influenced by various factors, including the number of unpaired electrons and their spin orientation.
According to the Valence Bond Theory, the magnetic properties of a compound depend on the nature and overlap of atomic orbitals involved in the bond formation. In this context, we will examine each compound individually to understand its magnetic moment value:
1. Cs2(MnCl4):
MnCl4 has a coordination number of 4, indicating that each Mn atom is bonded to four chloride ions. The manganese ion (Mn2+) has a d5 electron configuration, with five unpaired electrons. The magnetic moment (μ) value of 5.9 B.M indicates a high spin state, suggesting that all the electrons occupy degenerate d orbitals.
2. K4(Mn(CN)6):
Mn(CN)6 has a coordination number of 6, consisting of six cyanide ligands bonded to the central Mn atom. The manganese ion (Mn2+) has a d5 electron configuration, similar to Cs2(MnCl4). However, the presence of a larger number of ligands in the coordination sphere results in strong ligand field effects. These ligand field effects cause the d-orbitals to split into two sets, known as the t2g and eg orbitals. As a result, the five unpaired electrons preferentially enter the lower energy t2g orbitals. Thus, the reduced number of unpaired electrons leads to a lower magnetic moment value of 1.8 B.M.
3. K2(Ni(CN)4):
Ni(CN)4 also has a coordination number of 4, with four cyanide ligands bonded to the central Ni atom. The nickel ion (Ni2+) has a d8 electron configuration, with eight electrons in the d orbitals. As per Valence Bond Theory, due to the ligand field effects, the d orbitals split into two sets, t2g and eg, similar to the previous case. The t2g set is occupied by six electrons, leaving only two unpaired electrons in the eg set. This configuration results in a lower magnetic moment value of 0 B.M.
In summary, the difference in the magnetic moment values of Cs2(MnCl4), K4(Mn(CN)6), and K2(Ni(CN)4) can be explained by considering the coordination numbers and ligand field effects. The presence of more ligands leads to stronger ligand field effects, which cause the d orbitals to split and result in a lower number of unpaired electrons, thereby reducing the magnetic moment value.