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Write the electron configurations for the following atoms or ions:(a) ${B}^{3+}$(b) ${O}^{-}$(c) ${C}^{3+}$(d) ${Ca}^{2+}$(e) Tì
Chemistry 101
Chapter 6
Electronic Structure and Periodic Properties of Elements
Electronic Structure
Periodic Table properties
Carleton College
University of Maryland - University College
University of Kentucky
Brown University
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All right. So for this problem, we want to write out the electron configurations for the ions given Orion's or elements given. Um, so I have those written here just to the right of the periodic table. Um, let's just walk through this and get started. So Boron three plus is going to have three less electrons than non charged forum. So if we walk back through the period of table, it's going to have the same electron configuration is helium, which means that it's just going to have to electrons and it's one s orbital. That's gonna be the complete electron configuration for four on three. Plus, we're just going to complete this. Repeat the same process for the other ions and element listed in this, um, list here. So we add an electron oxygen. It's going to have the same electron configuration is non charged flooring. So it's going to have those, uh, 21 US electrons to two s electrons. Because flooring is in group 17 we're going to have five electrons in the toupee. Orbital carbon three plus is going to remove three electrons from carbon giving it. The same electron configuration is lithium, which has an electron configuration of one s 22 s. One calcium to plus, We're going to pull calcium ZX +24 s electrons, and it's going to have the same electron configurations are gone. It means we're going to fill these ground state from left to right, increasing in energy levels until we fully fill this three p orbital. Finally, if we look at Valium, we're not that lamp. Sorry. Titanium, Um, looking a titanium titanium exists within this this D block here, So we're going to be having the process is going to be exactly the same. It's going to have the same electron configuration as are gone initially. And then we remember is we're actually going to fill the four s orbital before we fill the three D. For the purposes of writing this out, I'm actually going to write them in order of increasing energy level. So we've got two electrons in the three D and then two electrons and before s these are going to be the complete energy levels for these elements. And I am
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