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