Urea, a compound formed in the liver, is one of the ways humans excrete nitrogen. The Lewis stru

step 1 Let's talk about urea. So we have its dual structure here, C double bond O with its two long pai

Urea, a compound formed in the liver, is one of the ways...

Key Concepts

Hybrid Orbital Theory

Hybrid orbital theory is a model that explains the observed geometries of molecules by mixing atomic orbitals into new hybrid orbitals that are oriented in specific directions. This theory helps predict bond angles and the type of bonding (sigma and pi) in molecules.

Orbital Overlap

Orbital overlap refers to the way in which atomic orbitals from different atoms combine to form chemical bonds. The effective overlap of orbitals with similar energies and proper orientation is crucial for forming strong covalent bonds.

Sigma Bond Formation

Sigma (?) bonds are formed by the head-on overlap of hybrid orbitals or a hybrid orbital with an unhybridized orbital. In hybrid orbital theory, sigma bonds in molecules are typically created through the overlap of sp2 (or other hybridized) orbitals along the internuclear axis, providing the primary bond framework.

Pi Bond Formation

Pi (?) bonds arise from the side-on overlap of unhybridized p orbitals that remain after hybridization has occurred. In double bonds, for example, one bond is a sigma bond and the other is a pi bond, with the pi bond contributing to the molecule's reactivity and electron distribution.

Transcript

00:01 Let's talk about urea.

00:03 So we have its dual structure here, c double bond o with its two long pairs, and then nitrogen that is attached to two hydrogens with one loan pair, another nitrogen attached to two hydrogens with another loan pair.

00:22 Before we begin talking about the hybrid orbitals that overlap, what i want to do or what i always do is i figure out the hybridization of, atom in this structure and we start with carbon half balanced electron four there's two monovalent atoms because it shares a single bond with the two nitrogen on either side there's no charge on it so we put zeros in here six divided by two will give you three and you have sb two hybridization now let's number the nitrogen atoms you have nitrogen one and nitrogen hybridization of nitrogen 1 is half, 5 valance electrons, 3 monovalent atoms around it, no charge on it.

01:16 So you get 8 divided by 2, which gives you 4, and this is indicative of an sp3 hybridization.

01:24 The other nitrogen atom, which is n2, is half, 5 balance electrons, 3 monovolent atoms, charges 0 on it.

01:34 So 8 divided by 2, for sb3 hybridization.

01:39 And last but not the least, you have oxygen, which has a balanced electrons of 6 plus 0, minus 0, plus 0, and then 6 divided by 2 will give you 3, and this tells you that it has an sp2 hybridization.

01:59 So now that we have all the hybridizations are figured out, i'll just put them here so that we remember what the hybridization were we have sp2 sp2 on these two plants and sp3 sp3 for the two nitrogen now let's deal with the orbitals you have a carbon in the center which is an sp2 sp2 always has a trigonal planner structure so you have three of the sp2 lobes in this manner sp2 then you have oxygen which is also sp2 also has a trigonal planner structure so they overlap.

02:49 They overlap trigonial planner.

02:54 These are the two other lobes with the electrons in it, the lone pair of electrons in it.

03:01 And this is also sp2.

03:03 This forms a sigma bond.

03:06 On either side of the carbon, you have nitrogen, which is sb3 hybridized.

03:13 So these orbitals of the nitrogen are, they follow a tetrahedral pattern.

03:21 There's an overlap here and so you have another sigma orbital here and the individual orbitals on nitrogen is sp3.

03:31 The other nitrogen on the other side follows the same pattern.

03:35 The orbitals are arranged around it in a tetrahedral fashion.

03:39 Individual orbitals are sv3 and because of the overlap with the sp2 orbitals of carbon you form another sigma bond.

03:49 There's overlap from the hydrogen 1s orbital, which forms two more sigma bonds for the nitrogen on either side...

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