Paramagnetic Paramagnetism is a form of magnetism whereby certain materials are weakly attracted by an externally applied magnetic field, and form internal, induced magnetic fields in the direction of the applied magnetic field. Let's see the picture: Pls note that as NH3 is a strong field ligand that's why it has d2sp3 hybridization.If it is week field ligand then it has sp3d2 hybridization…I will give you a chart of week and strong field ligand…. In case of [Ni(NH 3 ) 6 ]Cl 2 complex , the oxidation state of nickel atom is +2 . The complex ion $\ce{[Co(H2O)6]^3+}$ has $\ce{Co}$ in the $+3$ oxidation state, meaning it has an electron configuration of $[Ar] 4s^0 3d^6$. Why is [Ni(NH 3) 6]Cl 2 paramagnetic but [Co(NH 3) 6]Cl 3 is diamagnetic ? Zn2+ diamagnetic. Answer. Step 4: Determine whether the substance is paramagnetic or diamagnetic. Because there are no unpaired electrons, Zn atoms are diamagnetic. d) Ni(CO) 4 is diamagnetic; [Ni(CN) 4] 2-and NiCl 4 2-are paramagnetic. Cu2+ paramagnetic. By constructing a molecular orbital picture for each of the following molecules, determine whether it is paramagnetic or diamagnetic. Click hereto get an answer to your question ️ Given the species N2, CO, NO^ + and CN^ - which of the following statements are true for this :(I) All the species are diamagnetic(II) All the species are isostructural(III) All the species have identical bond order(IV) … One of the major breakthroughs of molecular orbital theory was to prove that #"O"_2# was paramagnetic. CO is Diamagnetic (absence of unpaired electron) . b. Yes. 1. However, in the octahedral complex ion, the d orbitals split into two levels, with three lower-energy orbitals and two higher-energy ones. CoF6^3+ paramagnetic. The bond order and magnetism (paramagnetic or diamagnetic) found through molecular orbital theory is not always reflected in the Lewis structure for a molecule. Lewis structures are strictly based on valence electrons and the octet rule. B 2 b. In [CoF6]3–, Co is having four unpaired electrons as F– does not cause pairing of electrons in d-orbitals, whereas in case of [Co(C2O4)3]3–, C2O4 causes pairing of unpaired electrons in d–orbitals and thus there is no unpaired electron, hence it is diamagnetic in nature. Because, with 6 2p electrons, in a MO energy level diagram, all 6 electrons can be paired. c) Ni(CO) 4 and [Ni(CN) 4] 2-are diamagnetic; and NiCl 4 2-is paramagnetic. C 2 c. O 2 d. NO e. CO a. Ni2+ paramagnetic. C 2 is diamagnetic because all … This MO diagram should be in your textbook, and is also in anor's answer, where #"O"_2# has two unpaired electrons in its #pi^"*"# antibonding molecular orbitals. Therefore it has 4 unpaired electrons and would be paramagnetic. Paramagnetic character depend on the number of unpaired electron present in any complex. Exercise \(\PageIndex{2}\) Indicate whether F-ions are paramagnetic or diamagnetic. What is Paramagnetic and Diamagnetic ? The F-ion has 2s 2 2p 6 has the electron configuration. Answer: Logic & Solution: Ni(CO) 4 = Ni + 4CO * The valence shell electronic configuration of ground state Ni atom is 3d 8 4s 2. So do the electron configuration and the diagram with the appropriate (2 less spins) electrons. if you have a level with unpaired electrons (spins) then that makes it paramagnetic. Because it has no unpaired electrons, it is diamagnetic. Co2+ paramagnetic. Using the Crystal-Field Theory, account for the fact that Co(NH3)6^3+ is diamagnetic while. The atomic number of nickel atom, 28 and that of Ni(II)ion is 26 . Use words and orbital diagrams. B 2 is paramagnetic because it has two unpaired electrons, one in each of its p orbitals. a. Just understand that if it has a 2+ charge it has 2 less electrons than its natural state. Just understand that if it has no unpaired electrons, one in each of the breakthroughs... Would be paramagnetic complex ion, the d orbitals split into two,. 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