How many of the following species are diamagnetic? \mathrm{Cd}^{2+… 🎉 The Study-to-Win Winning Ticket number has been announced! Hg^2+: [Xe] 4f^14 5d^10: 0 unpaired e⁻s diamagnetic. Calculate the total energy (in kJ) contained in 1.0 mol of photons, all with a frequency of 2.75 x 10^8 MHz? How Many Of The Following Species Are Diamagnetic? Choose the paramagnetic species from below. See the answer. Diamagnetic … Cs Zr2 Al3 Hg2 4 0 2; Question: How Many Of The Following Species Are Diamagnetic? Hence, is Paramagnetic. Ca. A paramagnetic electron is an unpaired electron. Because the e-s are unpaired the cmplx will be paramagnetic. When forming the cation the 5s e-s are removed first hence Mo(III) is [Kr]4d^3 (a common oxdn state of Mo). 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! 3) Al3+ : [Ne]. Show transcribed image text. Write orbital diagrams for each ion and indicate whether the ion is diamagnetic or paramagnetic. If you don't get what I get go back and repeat! This problem has been solved! Now Neon has all its orbitals filled with electrons, hence NO unpaired electrons so it is Diamagnetic. 68. \begin{equation}\begin{array} \\ {\text { a. } Diamagnetic has no unpaired e-, while paramagnetic does. Fr Zr2+ Al3+ Hg2+ 2. (make sure to take into account the charge) Then slowly fill in the orbitals and check if the end result has unpaired electrons. Look e⁻ configuration up in Wikipedia/element (RH panel) and subtract e⁻s to give appropriate +charge. Paramagnetic has unpaired e⁻s; weakly attracted into by a magnetic field. \begin{equation}\begin{array}\\ {\text { a. } Add up the amount bonding valence electrons it has. Expert Answer 100% (5 … 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). Write orbital diagrams for each ion and indicate whether the ion is diamagnetic or paramagnetic. a. Cd2+ b. Write orbital diagrams for each ion and determine if the ion is diamagnetic or paramagnetic. An atom could have ten diamagnetic electrons, but as long as it also has one paramagnetic electron, it is still considered a paramagnetic atom. a. Cd2+ b. Au+ c. Mo3+ d. Zr2+ \mathrm{V}^{5+} … 🎉 The Study-to-Win Winning Ticket number has been announced! Cs Zr2 Al3 Hg2 4 0 2. An atom is considered paramagnetic if even one orbital has a net spin. Au + C. Mo3+ d. Zr2+ Cu+: [Ar] 3d^10: 0 unpaired e⁻s diamagnetic Write orbital diagrams for each ion and indicate whether the ion is diamagnetic or paramagnetic. 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