Ca. See the answer. Paramagnetic has unpaired e⁻s; weakly attracted into by a magnetic field. Write orbital diagrams for each ion and determine if the ion is diamagnetic or paramagnetic. Write orbital diagrams for each ion and indicate whether the ion is diamagnetic or paramagnetic. 68. Au + C. Mo3+ d. Zr2+ Write orbital diagrams for each ion and indicate whether the ion is diamagnetic or paramagnetic. Diamagnetic has no unpaired e-, while paramagnetic does. Cs Zr2 Al3 Hg2 4 0 2. When forming the cation the 5s e-s are removed first hence Mo(III) is [Kr]4d^3 (a common oxdn state of Mo). \begin{equation}\begin{array} \\ {\text { a. } a. Cd2+ b. Au+ c. Mo3+ d. Zr2+ Write orbital diagrams for each ion and indicate whether the ion is diamagnetic or paramagnetic. Hg^2+: [Xe] 4f^14 5d^10: 0 unpaired e⁻s diamagnetic. Expert Answer 100% (5 … Fr Zr2+ Al3+ Hg2+ 2. An atom could have ten diamagnetic electrons, but as long as it also has one paramagnetic electron, it is still considered a paramagnetic atom. Calculate the total energy (in kJ) contained in 1.0 mol of photons, all with a frequency of 2.75 x 10^8 MHz? Therefore, Zr2+ has 2 unpaired electrons (Study about Hunds Rule, Aufbau Priciple, Pauli's exclusion principle before you attempt to write electronic configuration of D-block transition elements). Look e⁻ configuration up in Wikipedia/element (RH panel) and subtract e⁻s to give appropriate +charge. \begin{equation}\begin{array}\\ {\text { a. } Cu+: [Ar] 3d^10: 0 unpaired e⁻s diamagnetic No matter what the size of the d-d splitting (Δoct) the three 4d electrons will occupy the lowest energy t2g set: ↑↑↑ with their spins parallel (Hund's Rule). Show transcribed image text. \mathrm{V}^{5+} … 🎉 The Study-to-Win Winning Ticket number has been announced! Paramagnetic: Gold: Diamagnetic: Zirconium: Paramagnetic: Mercury: Diamagnetic: Up to date, curated data provided by Mathematica's ElementData function from Wolfram Research, Inc. Click here to buy a book, photographic periodic table poster, card deck, or 3D print based on the images you see here! How many of the following species are diamagnetic? Because the e-s are unpaired the cmplx will be paramagnetic. 3) Al3+ : [Ne]. a. Cd2+ b. An atom is considered paramagnetic if even one orbital has a net spin. How Many Of The Following Species Are Diamagnetic? Hence, is Paramagnetic. Cs Zr2 Al3 Hg2 4 0 2; Question: How Many Of The Following Species Are Diamagnetic? Now Neon has all its orbitals filled with electrons, hence NO unpaired electrons so it is Diamagnetic. A paramagnetic electron is an unpaired electron. This problem has been solved! \mathrm{Cd}^{2+… 🎉 The Study-to-Win Winning Ticket number has been announced! Choose the paramagnetic species from below. 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