Lewis structures are strictly based on valence electrons and the octet rule. b. Step 4: Determine whether the substance is paramagnetic or diamagnetic. 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…. Answer: Logic & Solution: Ni(CO) 4 = Ni + 4CO * The valence shell electronic configuration of ground state Ni atom is 3d 8 4s 2. Exercise \(\PageIndex{2}\) Indicate whether F-ions are paramagnetic or diamagnetic. Using the Crystal-Field Theory, account for the fact that Co(NH3)6^3+ is diamagnetic while. 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. Yes. CO is Diamagnetic (absence of unpaired electron) . B 2 is paramagnetic because it has two unpaired electrons, one in each of its p orbitals. C 2 is diamagnetic because all … Cu2+ paramagnetic. Answer. Why is [Ni(NH 3) 6]Cl 2 paramagnetic but [Co(NH 3) 6]Cl 3 is diamagnetic ? The atomic number of nickel atom, 28 and that of Ni(II)ion is 26 . Because, with 6 2p electrons, in a MO energy level diagram, all 6 electrons can be paired. Because there are no unpaired electrons, Zn atoms are diamagnetic. C 2 c. O 2 d. NO e. CO a. B 2 b. Zn2+ diamagnetic. What is Paramagnetic and Diamagnetic ? 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. Paramagnetic character depend on the number of unpaired electron present in any complex. 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. Therefore it has 4 unpaired electrons and would be paramagnetic. Use words and orbital diagrams. if you have a level with unpaired electrons (spins) then that makes it paramagnetic. Just understand that if it has a 2+ charge it has 2 less electrons than its natural state. The complex ion $\ce{[Co(H2O)6]^3+}$ has $\ce{Co}$ in the $+3$ oxidation state, meaning it has an electron configuration of $[Ar] 4s^0 3d^6$. 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 it has no unpaired electrons, it is diamagnetic. Ni2+ paramagnetic. c) Ni(CO) 4 and [Ni(CN) 4] 2-are diamagnetic; and NiCl 4 2-is paramagnetic. 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. d) Ni(CO) 4 is diamagnetic; [Ni(CN) 4] 2-and NiCl 4 2-are paramagnetic. One of the major breakthroughs of molecular orbital theory was to prove that #"O"_2# was paramagnetic. Co2+ paramagnetic. 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. In case of [Ni(NH 3 ) 6 ]Cl 2 complex , the oxidation state of nickel atom is +2 . 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) … a. By constructing a molecular orbital picture for each of the following molecules, determine whether it is paramagnetic or diamagnetic. 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