Answer:
Ar⁺, S and Co are paramagnetic in nature
Explanation:
Paramagnetism is a property of a given chemical substance and it is <em>due to the presence of unpaired electrons. </em>
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Zinc (Zn)-
Electron configuration in ground state- Zn: [Ar] 3d¹⁰4s²
Since the transition metal zinc has completely filled (n-1)d and ns orbital.
<u>Therefore, the number of unpaired electrons = 0</u>
<u>⇒ Zn is not paramagnetic</u>
Sulphide (S²⁻)- anion of sulfur
Reduction reaction: S + 2e⁻ → S²⁻
Electron configuration in ground state- S: [Ne] 3s² 3p⁴
Electron configuration in excited state- S²⁻ : [Ne] 3s² 3p⁶
Since sulfide ion, S²⁻ has completely filled ns and np orbitals.
<u>Therefore, the number of unpaired electrons = 0</u>
<u>⇒ S²⁻ is not paramagnetic</u>
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Ar⁺- cation of argon
Oxidation reaction: Ar → Ar⁺ + e⁻
Electron configuration in ground state- Ar: [Ne] 3s² 3p⁶
Electron configuration in excited state- Ar⁺ : [Ne] 3s² 3p⁵
Since Ar⁺ has completely filled ns orbital and 5 electrons in np orbital.
<u>Therefore, the number of unpaired electrons = 1</u>
<u>⇒ Ar⁺ is paramagnetic</u>
Sulfur (S)-
Electron configuration in ground state- S: [Ne] 3s² 3p⁴
Since S has completely filled ns orbital and 4 electrons in the np orbital.
<u>Therefore, the number of unpaired electrons = 2</u>
<u>⇒ S is paramagnetic</u>
Cobalt (Co)-
Electron configuration in ground state- Co: [Ar] 3d⁷ 4s²
As, the transition metal cobalt has completely filled ns orbital and 7 electrons in the (n-1)d orbital.
<u>Therefore, the number of unpaired electrons = 3</u>
⇒ Co is paramagnetic