[NiCl4]2- is paramagnetic while [Ni(CO)4] is diamagnetic though both are tetrahedral. Why?in [NiCl4]2- and Ni(CO)4 nickel is in +2 and 0 oxidation state.in the A paramagnetic substance is one that contains one or more unpaired electrons.. On the other hand, a diamagnetism substance is one that does not contain any odd electrons. Which of the following solutions is the most concentrated? Since there are 2 unpaired electrons in this case, it … [NiCl4]2− is paramagnetic while [Ni(CO)4] is diamagnetic though both are tetrahedral.Why? Just draw the orbitals with the electrons. Welcome to Sarthaks eConnect: A unique platform where students can interact with teachers/experts/students to get solutions to their queries. is done on EduRev Study Group by IIT JAM Students. It is diamagnetic in nature due to the unpaired electron. Why is [NiCl4]^2- paramagnetic while [Ni(CN)4]^2- is diamagnetic. ? Join Yahoo Answers and get 100 points today. Since there are 2 unpaired electrons in this case, it … The complex [Ni(CN)4]2- is diamagnetic, but [NiCl4]2- is paramagnetic with two unpaired electrons. Therefore, it causes the pairing of unpaired 3d electrons. (ii) [Ni(Cl 4)] 2– In case of [NiCl4] 2−, Cl − ion is a weak field ligand. [NiCl4]2- is paramagnetic while [Ni(CO)4] is diamagnetic though both are tetrahedral. Therefore, it does not lead to the pairing of unpaired 3d electrons. [NiCl4]^2- is paramagnetic while [Ni (CO)4] is diamagnetic though both are tetrahedral. Does the difficulty of pronouncing a chemical’s name really follow the trend: the easier, the less harmful, and the harder, the more harmful? [NiCl4]2− is paramagnetic, while [Ni (CO)4] is diamagnetic, though both are tetrahedral. Dec 26,2020 - The complexes [Pt(CN)4]2 and [NiCl4]2, respectively, area)paramagnetic, paramagneticb)diamagnetic, diamagneticc)paramagnetic, diamagneticd)diamagnetic, paramagneticCorrect answer is option 'D'. 161 views. Therefore, it causes the pairing of unpaired 3d electrons. Why? Calculate the vapor pressure of water above the solution.? [NiCl4]2− is paramagnetic while [Ni(CO)4] is diamagnetic though both are tetrahedral. Therefore, it undergoes sp3 hybridization. Trump becomes an interloper in Palm Beach, Biden's 'Amazon tax' could make things complicated, Biden's granddaughters turn heads at inauguration, Hoops team cancels season after coach accused of abuse, New dad Josh Hartnett: Why I dropped off the radar, New Time cover depicts chaos Biden must address, GOP Rep: Give stimulus check to those who get vaccine, Mickelson denies lobbying Trump on gambler's behalf, Teigen: 'Incredible' to be at Biden's inauguration, Official names U.S.'s most significant strategic threat, Biden needs to account for lost jobs at Keystone XL. The molecule $\ce{[PdCl4]^2-}$ is diamagnetic, which indicates a square planar geometry as all eight d electrons are paired in the lower-energy orbitals. [NiCl4]2- is paramagnetic while [Ni(CO)4] is diamagnetic though both are tetrahedral. Now, Ni +2 ion is 3d 8 system. The Questions and Answers of K2(NiF6). Still have questions? Deduce the structures of these complexes [NiCl 4 ] 2- is tetrahedron and [Ni(CN) 4 ] 2- is square planar [NiCl 4 ] 2- is square planar and [Ni(CN) 4 ] 2- is tetrahedron Will this recipe make diamonds ? Why ? Cr(NH3)6]3+ is paramagnetic while [Ni(CN)4]2− is diamagnetic. The magnetic nature of the complex, [NiCl 4] 2 … Explain (provide structures and orbital diagrams). Paramagnetic or Diamagnetic? Since there are 2 unpaired electrons in this case, it … Why ? Therefore, it undergoes sp3 hybridization. But CO is a strong field ligand. Why? Explain why? Therefore, it does not lead to the pairing of unpaired 3d electrons. This gives rise to a diamagnetic configuration, as expected. So, the #d_(z^2)# and #d_(x^2 - y^2)# fill with one electron each, then the #d_(xy)#, #d_(xz)#, and #d_(yz)# with one electron each, and then pairing occurs only after that, filling the #d_(z^2)#, #d_(x^2-y^2)#, and #d_(xy)# completely. [NiCl4]^2 - is paramagnetic while [Ni (CO)4] is diamagnetic though both are tetrahedral. Since there are 2 unpaired electrons in this case, it … Why? (ii) [Ni(Cl 4)] 2– In case of [NiCl4] 2−, Cl − ion is a weak field ligand. In recording your answer , be sure to also provide the name of each molecule and include a well -articulated explanation of the origin of the observed magnetism by showing a d … Please Help me with my Chemistry problem? 1 Answer. Can you explain this answer? Explain (provide structures and orbital diagrams). asked Dec 25, 2017 in Chemistry by sforrest072 (127k points) [NiCl 4] 2− is paramagnetic while [Ni(CO) 4] is diamagnetic though both are tetrahedral. Use the magnetic behaviour of these complexes to deduce the geometric structures , I.e. Hence the geometry of, [ NiCl4 ] 2–complex ion would be tetrahedral. Answer Save. ← Prev Question Next Question → +1 vote . | EduRev Chemistry Question is disucussed on EduRev Study Group by 193 Chemistry Students. (ii) [Ni(Cl 4)] 2– In case of [NiCl4] 2−, Cl − ion is a weak field ligand. Ask Question + 100. Join Yahoo Answers and get 100 points today. Under this condition, all the 3d-electrons of Ni (II) ion are paired and hence the complex would be diamagnetic. * The valence shell electronic configuration of ground state Ni atom is 3d 8 4s 2. Since no unpaired electrons are present in this case, [Ni(CO)4] is diamagnetic. Why Ni +2 paramagnetic whereas Zn +2 diamagnetic?. [NI(CN)4]^2 is paramagnetic while [Ni(CO)4]^3- is diamagnetic though both are tetrahedral. Get your answers by asking now. Therefore, it does not lead to the pairing of unpaired 3d electrons. The complex [Ni(CN)4]^2- is diamagnetic and the the complex NiCl4]^2- is paramagnetic. 1 Answer +1 vote . molecular geometry, of each of these species. (ii) [Ni(Cl 4)] 2– In case of [NiCl4] 2−, Cl − ion is a weak field ligand. asked Dec 28, 2017 in Chemistry by sforrest072 (127k points) [NiCl 4] 2- is paramagnetic while [Ni(CO) 4] is diamagnetic though both are tetrahedral. coordinatian compounds; Share It On Facebook Twitter Email. [NiCl4]2– is paramagnetic while [Ni(CO)4] is diamagnetic though both are tetrahedral. * All of these 10 electrons are pushed into 3d orbitals and get paired up when strong field CO ligands approach Ni atom. magnetic nature ? #["Ni""Cl"_4]^(2-)#: The #d# orbitals here fill with #8# electrons, but instead, high spin. are solved by group of students and teacher of IIT JAM, which is also the largest student community of IIT JAM. 1 Answer +1 vote . Therefore, it undergoes sp3 hybridization. Para magnetism and diamagnetism of a substance depends on the number of electrons occupied by it. Paramagnetic or Diamagnetic? Why? Lv 7. ← Prev Question Next Question → +1 vote . 0 0. Also, it causes the 4s electrons to shift to the 3d orbital, thereby giving rise to sp. But CO is a strong field ligand. d) Ni(CO) 4 is diamagnetic; [Ni(CN) 4] 2-and NiCl 4 2-are paramagnetic. Found it on the deep web? Just draw the orbitals with the electrons. Also, it causes the 4s electrons to shift to the 3d orbital, thereby giving rise to sp3 hybridization. It is diamagnetic in nature due to the unpaired electron. Therefore, it undergoes sp3 hybridization. ag_iitkgp. 1 decade ago. NiCl4 2- is paramagnetic with two unpaired electrons while Ni(CN)4 -2 is diamagnetic.? [NiCl4]2− is paramagnetic while [Ni(CO)4] is diamagnetic though both are tetrahedral. Since there are 2 unpaired electrons in this case, it … coordinatian compounds; Share It On Facebook Twitter Email. [NiCl 4] 2- is paramagnetic while [Ni (CO) 4] is diamagnetic though both are tetrahedral. In [NiCl 4] 2-, Nickel is in +2 oxidation state and it has electronic configuration of 3d 8.It is a tetrahedral complex in which one s and three p orbitals are hybradized to form 4 orbitals that are oriented tetrahedrally. Still have questions? What can you conclude about their molecular geometries? Get your answers by asking now. Please HELP with my Chemistry assignment.. Now, in case of [ NiCl4 ] 2–complex ion, Ni (II) ion with co-ordination 4 involves ‘sp3’ hybridization. Students (upto class 10+2) preparing for All Government Exams, CBSE Board Exam, ICSE Board Exam, State Board Exam, JEE (Mains+Advance) and NEET can ask questions from any subject and get quick answers by subject teachers/ experts/mentors/students. If the answer is not available please wait for a while and a community member will probably answer this soon. Why? The complex [NiCl 4 ] 2- is green and paramagnetic with two unpaired electrons, while the solution of [Ni(CN) 4 ] 2- is colorless and diamagnetic. Therefore, it undergoes sp3 hybridization. Relevance. Why ? It is diamagnetic in nature due to the unpaired electron. Therefore, it does not lead to the pairing of unpaired 3d electrons. It is diamagnetic in nature due to the unpaired electron. Favorite Answer. 337 views. Just so, what is the hybridization of NI CN 4 2? It is diamagnetic in nature due to the unpaired electron. [NiCl4]^2- is paramagnetic while [Ni (CO)4] is diamagnetic though both are tetrahedral. (ii) [Ni(Cl 4)] 2– In case of [NiCl4] 2−, Cl − ion is a weak field ligand. [NiCl4]2− is paramagnetic while [Ni(CO)4] is diamagnetic though both are tetrahedral. 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