Explain how the atoms in covalent molecules achieve electron configurations similar to those of

Explain how the atoms in covalent molecules achieve electron...

Key Concepts

Ionic Bonding

Ionic bonding is another type of chemical bonding that involves the transfer of electrons from one atom to another, resulting in the formation of ions. In this bonding process, one atom loses electrons to achieve a noble gas configuration while another gains electrons to complete its valence shell, with the resulting ions being held together by electrostatic attractions.

Octet Rule

The octet rule is a guiding principle in chemistry where atoms tend to combine in such a way that they each have eight electrons in their valence shell, similar to the electron configuration of the noble gases. This rule helps explain the stability that atoms gain when they achieve a full outer electron shell through various bonding methods.

Covalent Bonding

Covalent bonding is a type of chemical bonding where atoms share pairs of electrons to fill their valence shells and reach stability. Through covalent bonds, atoms achieve electron configurations similar to the noble gases by sharing electrons, allowing them to complete their octet collectively without transferring electrons completely.

Transcript

00:01 So we're going to talk about the electron configurations in covalently bonded molecules and how these electron configurations will be similar to that of the noble gases.

00:14 So first, let's look at diatomic oxygen here.

00:18 We have oxygen, which has six valence electrons.

00:25 And if we have two oxygen molecules here, we know that covalent bonds are sharing of electrons.

00:36 So each one needs two valence electrons to get to the desired octet.

00:42 So if they share an electron from each of these lone pairs, we can rewrite this then as oxygen here, with its six, and then it's two shared here.

01:02 So now they have the octet they want, and we can see how this electron configuration stacks up.

01:09 So let's just take a look at that.

01:13 Now, each oxygen is in the 2p orbital here, and it's in the fourth spot of that orbital, counting left to right, one, two, three, four.

01:27 So each oxygen has an electron configuration of 1s2, 2s2, 2p4.

01:37 And they want the perfect octet in their, outermost shells in the valence shells so they already have two here in the outer s orbital and they have four in the outer p orbital which gives a total of six now they want eight and we know that they share two so by sharing two we're going to add two to the outermost orbital and then the electron configuration becomes one s2 two s2 two p six they both have the octet they want, and they have done this by sharing electrons through covalent bonding.

02:19 And if we look at the periodic table, this electron configuration here is the same as that of neon, which is the next closest noble gas.

02:33 So the electron configuration of an oxygen model, in 02 is going to be equal to that of neon.

02:42 Now we can look at another example of covalent bonding here.

02:46 We have cyanide here, which is when a carbon atom, which has four valence electrons, and a nitrogen, which has five, share six electrons here to form carbon, which is going to be triple bonded, basically, by sharing three sets of two.

03:16 With nitrogen here and it still has one lone one, which can be written here as c triple bonded to n with the extra electron here giving it its minus one charge.

03:33 So this is how carbon bonds with nitrogen here to give cyanide.

03:39 So let's look at the electron configuration of this.

03:43 So carbon typically has a electron configuration, of 1s2, 2s2, 2p2, if we look at the periodic table, and then nitrogen has just one more electron, so it is going to be 2p3.

04:06 Now, we know that they share three electrons, so if we are going to add three to their outermost shell here, then this is is going to be 2p5 and 2p6.

04:26 Now, nitrogen has a perfect octet in its outermost shells.

04:32 We have eight.

04:33 But carbon, which still has a lone electron, is going to get another plus one to the outermost shell, also giving it a 2p6 electron configuration, which is a perfect octet, and again is the same electron configuration.

04:51 As the noble gas neon.

04:54 So the way covalent bonds form the noble gas electron configuration is through the sharing of electrons.

05:06 As you can see, carbon has shared its electron and has a lone pair to get its octet of eight and nitrogen has done the same thing.

05:16 Now, this is a little different in ionic bonding, however, because we remember ionic bonding has to do with the charge.

05:25 It's not sharing electrons, it's using different charges, but they still are trying to get to that perfect octet.

05:33 So we're going to look at simple nacl.

05:36 We have our metal positive ion and the non -metal negative ion.

05:41 And we're going to take a look...

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