Can you explain the answer of this question below:Which one of the following is a diamagnetic ion?A:CO2+B:Cu2+C:Mn2+D:Sc3+The answer is d.

Question

Answer

Electronic Configuration is given below :

Sc3+ = [Ar] 3d0 4s0

In Sc3+ , it has paired electrons so it is diamagnetic.

Answer

The Sc atom has a 4s2 3d1 configuration. On attaining the Sc 3+ state, it loses the 4s and 3d electrons. Since there are no unpaired electrons, it is diamagnetic in nature.

Answer

It has paired electrons so it is diamagnetic.

Answer

Answer is d because not unpaired electron

Answer

Co⁺²= [Ar] 3d⁷
Cu²⁺ = [Ar] 3d⁹
Mn⁺² = [Ar] 3d⁵
Sc⁺³ = [Ar]
We can see that only Sc⁺³ has no unpaired electron, so it is a diamagnetic ion.

Answer

Diamagnetic ions are those ions that have all of their electrons paired up in their atomic or molecular orbitals, resulting in a net magnetic field of zero. In other words, they are not attracted to a magnetic field.

To determine which of the given options is a diamagnetic ion, we need to examine the electron configurations of each ion.

a) CO2: CO2 is a molecule composed of one carbon atom and two oxygen atoms. Carbon has an atomic number of 6, and the electron configuration of a neutral carbon atom is 1s^2 2s^2 2p^2. Oxygen has an atomic number of 8, and the electron configuration of a neutral oxygen atom is 1s^2 2s^2 2p^4. Therefore, the electron configuration of CO2 is (1s^2 2s^2 2p^2)(1s^2 2s^2 2p^4)(1s^2 2s^2 2p^4), and there are unpaired electrons present. Hence, CO2 is not a diamagnetic ion.

b) Cu2: Cu2 is the copper ion with a charge of +2. Copper has an atomic number of 29, and the electron configuration of a neutral copper atom is [Ar] 3d^10 4s^1. When copper loses two electrons to form Cu2+, the electron configuration becomes [Ar] 3d^9. In this configuration, there is one unpaired electron present, indicating that Cu2 is not a diamagnetic ion.

c) Mn2: Mn2 is the manganese ion with a charge of +2. Manganese has an atomic number of 25, and the electron configuration of a neutral manganese atom is [Ar] 3d^5 4s^2. When manganese loses two electrons to form Mn2+, the electron configuration becomes [Ar] 3d^5. In this configuration, there are five unpaired electrons present, indicating that Mn2 is not a diamagnetic ion.

d) Sc3: Sc3 is the scandium ion with a charge of +3. Scandium has an atomic number of 21, and the electron configuration of a neutral scandium atom is [Ar] 3d^1 4s^2. When scandium loses three electrons to form Sc3+, the electron configuration becomes [Ar] 3d^0. In this configuration, all of the electrons are paired up, resulting in a net magnetic field of zero. Therefore, Sc3 is a diamagnetic ion.

In conclusion, among the given options, the diamagnetic ion is Sc3.

Answer

Diamagnetic ions are those ions that have all of their electrons paired up in their atomic or molecular orbitals, resulting in no unpaired electrons. As a result, diamagnetic ions are not attracted to a magnetic field and are weakly repelled by it.

Let's analyze each option to determine which one is the diamagnetic ion:

a) CO2: Carbon dioxide is a molecule composed of one carbon atom and two oxygen atoms. Each oxygen atom contributes two unpaired electrons to the molecule, resulting in a total of four unpaired electrons. Since CO2 has unpaired electrons, it is paramagnetic, not diamagnetic.

b) Cu2: Copper ion (Cu2+) has lost two electrons compared to its neutral state. The electron configuration of Cu2+ is [Ar]3d9, which means it has one unpaired electron. Therefore, Cu2+ is paramagnetic, not diamagnetic.

c) Mn2: Manganese ion (Mn2+) has lost two electrons compared to its neutral state. The electron configuration of Mn2+ is [Ar]3d5, which means it has five unpaired electrons. Therefore, Mn2+ is paramagnetic, not diamagnetic.

d) Sc3: Scandium ion (Sc3+) has lost three electrons compared to its neutral state. The electron configuration of Sc3+ is [Ar]3d0, which means it has no unpaired electrons. Therefore, Sc3+ is diamagnetic.

Therefore, the correct answer is option D, Sc3. Scandium ion (Sc3+) is the only ion among the given options that has no unpaired electrons, making it diamagnetic.

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