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