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December 30, 2020    

d) Ni(CO) 4 is diamagnetic; [Ni(CN) 4] 2-and NiCl 4 2-are paramagnetic. if you have a level with unpaired electrons (spins) then that makes it paramagnetic. Paramagnetic character depend on the number of unpaired electron present in any complex. The complex ion $\ce{[Co(H2O)6]^3+}$ has $\ce{Co}$ in the $+3$ oxidation state, meaning it has an electron configuration of $[Ar] 4s^0 3d^6$. Using the Crystal-Field Theory, account for the fact that Co(NH3)6^3+ is diamagnetic while. B 2 b. Lewis structures are strictly based on valence electrons and the octet rule. Answer. C 2 is diamagnetic because all … C 2 c. O 2 d. NO e. CO a. The bond order and magnetism (paramagnetic or diamagnetic) found through molecular orbital theory is not always reflected in the Lewis structure for a molecule. Why is [Ni(NH 3) 6]Cl 2 paramagnetic but [Co(NH 3) 6]Cl 3 is diamagnetic ? B 2 is paramagnetic because it has two unpaired electrons, one in each of its p orbitals. Step 4: Determine whether the substance is paramagnetic or diamagnetic. 1. Ni2+ paramagnetic. So do the electron configuration and the diagram with the appropriate (2 less spins) electrons. 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…. The atomic number of nickel atom, 28 and that of Ni(II)ion is 26 . 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. In case of [Ni(NH 3 ) 6 ]Cl 2 complex , the oxidation state of nickel atom is +2 . Yes. b. c) Ni(CO) 4 and [Ni(CN) 4] 2-are diamagnetic; and NiCl 4 2-is paramagnetic. Exercise \(\PageIndex{2}\) Indicate whether F-ions are paramagnetic or diamagnetic. One of the major breakthroughs of molecular orbital theory was to prove that #"O"_2# was paramagnetic. 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) … Therefore it has 4 unpaired electrons and would be paramagnetic. The F-ion has 2s 2 2p 6 has the electron configuration. 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. Answer: Logic & Solution: Ni(CO) 4 = Ni + 4CO * The valence shell electronic configuration of ground state Ni atom is 3d 8 4s 2. CoF6^3+ paramagnetic. Just understand that if it has a 2+ charge it has 2 less electrons than its natural state. Because, with 6 2p electrons, in a MO energy level diagram, all 6 electrons can be paired. Cu2+ paramagnetic. 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. Co2+ paramagnetic. CO is Diamagnetic (absence of unpaired electron) . Zn2+ diamagnetic. Because it has no unpaired electrons, it is diamagnetic. Because there are no unpaired electrons, Zn atoms are diamagnetic. What is Paramagnetic and Diamagnetic ? a. However, in the octahedral complex ion, the d orbitals split into two levels, with three lower-energy orbitals and two higher-energy ones. Use words and orbital diagrams. By constructing a molecular orbital picture for each of the following molecules, determine whether it is paramagnetic or diamagnetic. Octet rule all 6 electrons can be paired } \ ) Indicate whether F-ions are paramagnetic or diamagnetic diamagnetic [! 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