Which simple ion would each of the following elements be expected to form? What noble gas has an

Which simple ion would each of the following elements be...

Key Concepts

Ion Formation

Ion formation involves atoms either losing or gaining electrons to achieve a more stable electron configuration, often resembling that of a noble gas. This process is driven by the desire of atoms to attain a full outer electron shell, which minimizes the system's overall energy and increases chemical stability.

Electron Configuration

Electron configuration describes the distribution of electrons among the orbitals of an atom or ion. Understanding the arrangement of electrons is crucial for predicting how elements behave chemically, particularly in relation to ion formation and bonding.

Periodic Trends and Valence Electrons

Periodic trends, such as atomic size, effective nuclear charge, and ionization energy, influence the number of valence electrons and an element's tendency to gain or lose electrons. The behavior of valence electrons is key in determining the type of ion an element will form.

Noble Gas Electron Configurations

Noble gas electron configurations refer to the stable arrangement of electrons found in noble gases, which have completely filled valence shells. Many elements form ions by either losing or gaining electrons to achieve a similar configuration, thereby gaining the stability characteristic of noble gases.

Transcript

00:02 So we're looking to find the ion or the charge of an atom, depending on its electron configuration and in comparison to some noble gas.

00:14 So first we're going to be looking at chlorine, which has this electron configuration here.

00:21 And we see its outermost shell in the 3s and the 3p orbital.

00:26 We have a 2 and a 5.

00:28 We have 7 valence electrons.

00:31 So we know in its outer most shell, chlorine, has seven valence electrons.

00:36 It's trying to get the perfect eight, the octet, so we know it needs to gain one.

00:42 So if chlorine gets this octet and it gains one, it is going to be gaining a negative charge, and so it is going to have a charge of negative one.

00:51 So the simple ion that chlorine likes to form is cl minus one.

00:58 And if we have gained this minus one electron, we can add it to the outermost orbital and so this becomes 3p6 here and this is for chlorine minus 1.

01:15 So this is its desired electron configuration and if we're going to compare this to a noble gas configuration we can look at the periodic table we have chlorine here and we know that with non -metals they like to gain electrons in order to get their perfect octet, so it is going to be gaining one.

01:41 So we're going to look at the atom to the right, one space, when it gains an electron, so it's going to have the same electron configuration of the noble gas argon.

01:54 So that is that.

01:57 So chlorine likes to form a negative one ion, which has the same electron configuration as neutral argon.

02:06 So now let's look at the next which is the metal strontium.

02:12 Now, strontium is way over here in period 5, group 2.

02:20 Now we know that this fulfills the 5s2 orbital, and in order to save some time, i've written the krypton noble gas in brackets, so that just represents the electron configuration all the way up through krypton, through 3s, 3p, then you'd have to do 4s, 4d, 4p, and just to save some time, this electron configuration is written here as this bracket plus the 5s2 that represents strontium.

02:57 So we have some strontium atom here, and in its outermost shell in the 5s orbital, it has two electrons.

03:07 Now strontium, if it wants to have a perfect octet, can either try and gain six more to make the perfect octet, but that's a lot of work to find six valence electrons from other atoms, or it can simply try to get rid of these two and drop back down to a different orbital.

03:29 And that is the much easier thing to do.

03:33 So strontium is going to lose to electrons.

03:35 It's losing two negative charges, so it is going to have a positive two charge...

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