Which of the following elements are capable of forming...

Key Concepts

Electronegativity and Atomic Size Considerations

Atomic size and electronegativity also play significant roles in determining whether an element can form hypervalent compounds. Generally, larger atoms with lower electronegativity are more capable of dispersing the increased electron density associated with hypervalency. Conversely, smaller and highly electronegative atoms tend to resist having an expanded number of electrons in their valence shell.

Availability of d-Orbitals in Period 3 and Beyond

Elements in the third period and beyond have access to low-lying d-orbitals that can be used to accommodate extra electrons. This availability makes it possible for these atoms to form bonds that result in more than eight electrons around the central atom, thus facilitating the formation of hypervalent compounds.

Hypervalency

Hypervalency refers to the ability of an atom to accommodate more than eight electrons in its valence shell when forming compounds. This phenomenon occurs in certain molecules where the central atom forms more bonds than would be predicted by the classic octet rule, thus resulting in an expanded valence shell.

Octet Rule and Its Exceptions

The octet rule is the principle that atoms tend to form bonds in such a way that they have eight electrons in their valence shell, mirroring the electron configuration of a noble gas. However, exceptions exist for elements that can exceed this limit, leading to hypervalent molecules. Such exceptions are typically observed in heavier elements that have available d-orbitals.

Transcript

00:01 Hello everyone, let us see the following question.

00:03 Which of the following elements are capable of forming hypervalent compounds? so here we are talking about hypervalent compounds.

00:17 So, first let us know the meaning about hypervalent compounds.

00:21 So, it is any component that contains more than formally assignable electrons in the valence shape.

00:28 So it is the any compound which contains more than.

00:36 Than which contains more than 8 formally assignable electrons in valent shell.

01:05 So, in fact, it is connected directly associated with the central atom.

01:10 In turn, it has to be connected to the ligands.

01:13 So let us see the elements given here.

01:16 So, the element carbon whose electronic configuration will be helium 2s2 and 2p2.

01:26 So, there are no d orbital.

01:27 So, total valency it has to undergo.

01:30 It has four bond pairs.

01:32 So, it requires four bonded electrons from other element.

01:35 So it will have only eight valence electrons.

01:39 So let us see in terms of phosphorus.

01:42 So, phosphorus has a configuration of a neon.

01:46 3 s2 and 3p3.

01:49 However, it has empty 3d orbital.

01:52 So, it can have 5 bonded electrons.

01:55 So, if it has 5, up to 5 bond pairs it can have, that means 5 bond pairs it can get from the ligands, totally it can have 10 electrons.

02:05 So, this is a hypervalent compound.

02:08 However, the one which shows only 8 is not a hypervalent compound.

02:12 So let us check in the case of oxygen.

02:14 Oxygen's configuration is helium 2 s2 and 2 p 4 so here also no d orbital so totally it has got two bond pairs and two loan pairs the two lone pairs would be taking two loan pairs sorry two loan pair plus it has got two bond pair the two bond pairs will get two bond pairs from the neighboring electrons so total four so each loan pair has two so two into four so it will have only 8 electrons so it is not a hypervalent compound.

02:48 So, coming to fluorine, florence configuration will be helium, 2s2 and 2p5.

02:55 It has actually 3 loan pair and 1 bond pair, that one bond pair takes another bond phase, so totally 2 electrons here.

03:04 See here each loan pair has 2 electrons, so 2 3s are 6 electrons plus 2.

03:09 So it also shows 8 electrons, hence it is not hypervalent.

03:13 Now coming to next is a chlorine...

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