The Electron Configuration: Ions - Video Tutorials & Practice Problems
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The Electron Configuration of Ions involves either adding or removing electrons from a given orbital of an element.
Electron Configuration of Ions
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concept
The Electron Configuration: Ions
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Recall that when elements lose or gain electrons, they become ions. We're going to say here that cations are positive ions. We're gonna say with a cation, we first remove electrons from the highest shell number, and the highest shell number is connected to our principal quantum number or the n value. Now, the principal quantum number provides the shell number or energy level of the electron. So here we have 1 s 2, 2 s 2, 2p63s23p6. The number is related to the principal quantum number n. 1 s 2 would have an n value of 1, 2 s 2 and 2 p would have n values equal to 2, 3 s and 3 p would have n values equal to 3. So just remember, we look at the number before the sublevel or subshell letters of s, p, d, or f to determine our n value. And when we're removing electrons, we remove them from the orbitals that have the highest n value. But let's say we wanted to remove electrons and we only had 3 s and 3 p to choose from. Both of them have the highest n value, but we say that since 3p is listed after 3 s, it would have more energy, and therefore, if we had to choose between 3 s and 3 p, we remove the electron first from 3 p. Same thing can be said between 2 s and 2 p. Since Since 2p is listed after 2 s, it has more energy, and therefore if we had to take electrons away it'd come out of the 2p orbitals before we even look at the 2s orbitals. So just remember, first look at the highest n value. If a set of orbitals have the same n value, then the higher energy one is the one that was listed last. That's where we will remove electrons first.
For Cations, remove electrons from highest shell number (n).
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example
The Electron Configuration: Ions Example 1
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So here it says write the condensed electron configuration for the titanium 3 ion. Alright. So titanium 3 is t I three plus. Step 1 tells us to provide the electron configuration for the neutral form of the element. Alright. So titanium neutral has an atomic number of 22. If we're doing its condensed electron configuration, looking at the periodic table, we would see argon as a noble gas right before it, then we'd have here 4s2, and then we'd have 3d2. So this would be the electron configuration of the neutral titanium atom. Step 2, begin removing electron or electrons from the highest numbered shell to obtain to the desired charge. When in the same shell 2 s versus 2 p, use Aufbau principle to remove the higher energy electrons first. Alright. So coming back to the titanium 3 ion, 3 plus means we've lost 3 electrons. Looking at our condensed electron configuration for the neutral ion, our neutral element, will help guide us to the new electron configuration of the ion. So we don't touch what's within these brackets, that's our noble gas. So we're looking here because it's 4 s that means n equals 4, and because it's 3 d that means n equals 3. We remove our electrons first from the highest shell number, so we need to lose 3 electrons. Here we're gonna lose our first 2 from the 4 s, so 4 s is now completely gone. Next, we need to lose one more electron because we need to lose 3 electrons, so that's gonna come from the 3 d. That means titanium 3 at the end will be argon 3d1 as the electron configuration of our ion.
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concept
The Electron Configuration: Ions
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Now for an anion, remember anions are negatively charged ions. We become anions when we accept electrons. We're gonna say with an anion, you add an electron or electrons to the orbitals with available space. Now note, for an anion, the nonmetal keeps its base name, but had its ending changed to ide. So if we hear oxide, fluoride, or horide, that means we're dealing with the anion form of that element. So keep that in mind when asked to find the electron configurations of anions.
For Anions, add electrons to orbital with available space.
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example
The Electron Configuration: Ions Example 2
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Here it says, write the full electron configuration for the nitride ion. So it ends with ide, which means we're dealing with the anion form of nitrogen. So nitrogen is in group 3 a, so its charge is minus 3 or 3 minus. 3 minus means that we have gained 3 electrons, so we'll take that into account when we're doing its electron configuration. So the steps we're gonna do here is we're gonna provide the electron configuration for the neutral form of the element. So nitrogen, when it's neutral, it has an atomic number of 7. Its full electron configuration is 1 s 2, 2 s 2, 2p3. Next step 2, we're gonna add electron or electrons to the orbitals that can accommodate more electrons. Alright. So for the Nitride ion, here we have this. S can only hold up to 2 electrons max. So 1 s 2 and 2 s 2 stay the way that they are. Remember, the p sub level can hold up to 6 electrons. Right now it only has 3. We're gaining 3 additional electrons, so all of them can be tossed into this 2p set of orbitals to give us 2p6. So this would represent the full electron configuration of the nitride ion. So we can say this as an acceptable answer. One more thing we can also say is that it now has the same electron configuration as a noble gas, and then noble gas would be neon. So both of these answers are acceptable. You can show the full electron configuration here, and you can say that it is the same electron configuration as neon. Technically in this answer I'm asking for the full electron configuration, so this would be the best answer. But just keep in mind, it now also has the same electron configuration as a noble gas. So if we wanted to do a shorthand or condensed electron configuration, you could just write this as an answer.
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Problem
Problem
What is the full electron configuration of the selenide ion?
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Problem
Determine the electron configuration for the Cl+ ion.
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Problem
Problem
Determine the electron configuration and electron orbital diagram for the silver ion.