What noble gas has the same electron configuration as each of the ions in the following compound

What noble gas has the same electron configuration as each...

Key Concepts

Ion Formation and Electron Configurations

When atoms form ions by either losing or gaining electrons, they often attain an electron configuration that matches that of a noble gas. This process, which involves the removal of electrons (cation formation) or the addition of electrons (anion formation), enables the ion to reach a more stable, lower energy state similar to the complete electron shells of noble gases.

Noble Gas Electron Configurations

Noble gases have completely filled valence electron shells, leading to a very stable and low-energy electron configuration. In chemistry, the electron configurations of noble gases serve as benchmarks, and many ions or atoms change their electron count by losing or gaining electrons to achieve a similar stable configuration.

Isoelectronic Species

Isoelectronic species are atoms or ions that have the same number of electrons and, consequently, the same electron configuration. Despite being different elements or ions, these species exhibit similarities in their electronic structure because they have achieved a noble gas-like arrangement by either losing or gaining electrons.

Transcript

00:01 All right, in this question, we have a number of compounds and we're asked to find out what normal gas configuration the ions of those compounds have.

00:11 So first up, we have cesium sulfide.

00:17 So we have cs and we have sulfur.

00:22 Now we know that, you know what, we don't even need to balance this or write the empirical formula because we know the charges of these.

00:32 So cesium is going to lose an electron.

00:36 Sulfur is going to gain two electrons.

00:41 So when sulfur gains two electrons, it will reach argon configuration.

00:50 And when cesium loses an electron, it goes over here and forms the xenon configuration.

01:00 Yeah, we don't have to balance the equations or write the empirical formulas.

01:05 We can just figure out which elements there are.

01:10 So the way i solve that, if we look at sulfur, sulfur has six valence electrons.

01:19 For it to satisfy an octet, they'll need to gain two electrons.

01:26 And when it satisfies the octet, it reaches argon.

01:31 And cesium, we know that group 1a and group 2a elements like to lose their electrons.

01:37 So when cesium loses an electron, it goes to the row before, and it reaches the noble gas configuration of the row before.

01:47 Because it's just lost everything in this orbital, so it's kind of kicked off that row in terms of electrons.

01:55 All right.

01:55 So next up we have strontium fluoride.

01:58 So i'm not sure on the symbol of, i think it's st.

02:06 And i would be wrong.

02:07 It's sr.

02:08 Sr for strontium, for fluorine.

02:13 So, fluorine is over here.

02:16 We know that fluorine is the anion of this ionic bond, and we know that it's going to lose one electron.

02:22 Because it's in group, it gain one electron, because it's in group 7a, it needs one more electron.

02:27 It's going to get that electron.

02:29 So, fluorine, when it gains an electron, it reaches neon.

02:36 And strontium is an alkaline earth metal...

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