(a) Se os orbitais atômicos de valência de um átomo são...

(a) $\mathrm{Se}$ os orbitais atômicos de valência de um átomo são hibridizados $s p$, quantos orbitais $p$ não hibridizados permanecem na camada de valência? Quantas ligações $\pi$ o átomo pode formar? (b) Imagine que você pudesse segurar dois átomos que estão ligados um ao outro, rotacioná-los sem mudar o comprimento da ligação. Seria mais fácil rotacionar uma ligação simples $\sigma$ ou uma ligação dupla ( $\sigma$ e $\pi$ ), ou não faria diferença?

Key Concepts

Sigma (?) Bonds and Bond Rotation

Sigma bonds are characterized by head-on orbital overlaps and typically allow free rotational movement around the bond axis. In contrast, bonds that also include a pi component, such as double bonds, restrict rotation because disrupting the pi bond requires extra energy.

Pi (?) Bonds

Pi bonds are formed through the side-by-side overlap of unhybridized p orbitals. Each unhybridized p orbital is capable of forming one pi bond, and these bonds contribute to the double or triple bond character in molecules by supplementing a sigma bond.

Unhybridized Atomic Orbitals

Not all atomic orbitals necessarily participate in hybridization. For atoms where only some orbitals are hybridized, remaining unhybridized orbitals (often p orbitals) can still be available to form additional bonds or interactions, such as pi bonds.

Hybridization

Hybridization involves the mixing of atomic orbitals to form new, equivalent orbitals that direct the bonding geometry of a molecule. For example, in sp hybridization one s and one p orbital combine to create two sp orbitals, altering the bonding arrangement compared to pure s or p orbitals.

Transcript

00:01 All right, guys.

00:02 We're doing problem 56 of chapter 9 of chemistry or central science.

00:06 So if the valence of electrons, if the valent atomic orbitals of an atom are sp hybridized, how many unhybridized p orbitals remain in the valent show? so we can talk about hybridization, we can have sp hybrid.

00:20 We can have sp2, or we can have sp3 hybridization.

00:28 So if our atom is sp hybridized, that means we have two.

00:33 That's that means that we have two p orbitals that are non -hybridized in the in the valent shell now they want to know how many pi bonds can the atom can the atom form and that's very simple so when we use pie so we when we form us when we four pie bonds we're adding p orbitals into us we're adding p orbitals so that means that so let me phrase when we are adding p -orbitals, sorry, when we are making p -bonds, we have a sigma bond, we're making pie bonds.

01:20 Those are what our p -orbitals are used for.

01:24 Those are what are free p -orbitals are used for.

01:27 They're used to make pie bonds.

01:29 So if we have two free p -orbitals, two non -hyperidized p -orbitals, else we can form two more pie bonds.

01:48 So now, imagine you could hold two items our bonds together, twist them and not change bond life.

01:54 Would it be easier to twist or rotate around a single bond or a double bond? so this is actually a pretty standard question...

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