Hybridization of Atomic Orbitals - Sigma & Pi Bonds - Sp Sp2 Sp3

Summary

This educational video delves into the concept of atomic orbital hybridization, explaining how atomic orbitals combine to form hybrid orbitals like sp3, sp2, and sp. It details the probability distribution of electrons within orbitals, influenced by the Heisenberg Uncertainty Principle. The video explores carbon's electron configuration and how it forms sp3, sp2, and sp hybrid orbitals, emphasizing their energy levels relative to s and p orbitals. It also discusses degenerate orbitals, the formation of sigma and pi bonds, and the relative strengths of single, double, and triple bonds, providing a foundational understanding of chemical bonding.

Takeaways

• 🌐 Hybridization is the process of combining atomic orbitals to form hybrid orbitals, such as sp3, sp2, and sp, which are blends of s and p orbitals.
• 🔬 The sp3 hybrid orbital is a combination of one s orbital and three p orbitals, resulting in four equivalent orbitals with 25% s character and 75% p character.
• 📊 The sp2 hybrid orbital is formed by combining one s orbital and two p orbitals, creating three equivalent orbitals with approximately 33% s character and 67% p character.
• 📈 The sp hybrid orbital is a mix of one s orbital and one p orbital, leading to two equivalent orbitals with 50% s character and 50% p character.
• 📍 Hybrid orbitals are positioned at energy levels that reflect their composition, with more p character placing them closer to the p orbitals' energy level.
• 🌀 Degenerate orbitals, like the sp3, sp2, and sp hybrids, have the same energy and are used to place electrons one at a time with parallel spins.
• 🔗 Sigma bonds are formed from the overlap of hybrid orbitals and are present in single, double, and triple bonds, with triple bonds being the strongest.
• 🔄 Unhybridized p orbitals are used to form pi bonds, which are weaker than sigma bonds and are found in double and triple bonds alongside sigma bonds.
• 🔢 The number of sigma bonds in a molecule can be counted as one for each bond, while pi bonds are counted as one for each double bond and two for each triple bond.
• 📚 Understanding hybridization and bond types is crucial for predicting molecular geometry and the strength of chemical bonds.

Q & A

What is the definition of hybridization in atomic orbitals?

Hybridization is the process of combining atomic orbitals to form hybrid orbitals. It involves mixing different types of orbitals, such as s, p, and d orbitals, to create new orbitals that are suitable for bonding.

What are the different types of hybrid orbitals mentioned in the script?

The script mentions sp3, sp2, and sp hybrid orbitals. These are created by combining one s orbital with three p orbitals, one s orbital with two p orbitals, and one s orbital with one p orbital, respectively.

How does the energy level of hybrid orbitals compare to the original atomic orbitals?

Hybrid orbitals generally have an energy level that is closer to the p orbitals than the s orbitals due to the higher proportion of p character in the hybrid orbitals. The energy level also depends on the number of p orbitals involved in the hybridization.

What is the significance of the term 'degenerate orbitals' in the context of hybridization?

Degenerate orbitals are orbitals that have the same energy. In the context of hybridization, all the sp3, sp2, or sp hybrid orbitals formed are degenerate, meaning they have the same energy level.

How does the electron configuration of carbon relate to its hybridization?

Carbon has an electron configuration of 1s2 2s2 2p2, with four valence electrons. When carbon forms sp3 hybrid orbitals, it uses all four orbitals (one s and three p orbitals) to create four sp3 hybrid orbitals.

Why is it important to add electrons to degenerate orbitals one at a time with parallel spins?

Adding electrons one at a time with parallel spins to degenerate orbitals maximizes the stability of the atom by minimizing electron-electron repulsion. This follows Hund's rule, which states that electrons will fill orbitals in a way that maximizes the number of unpaired electrons in degenerate orbitals.

What is the percentage of s and p character in an sp3 hybrid orbital?

An sp3 hybrid orbital has 25% s character and 75% p character, as it is formed by combining one s orbital with three p orbitals.

How many unhybridized p orbitals are left after forming sp2 hybrid orbitals?

After forming sp2 hybrid orbitals, one p orbital remains unhybridized because only two of the three p orbitals are used in the hybridization process.

What is the difference between sigma and pi bonds in terms of strength?

Sigma bonds are stronger than pi bonds. While a triple bond is stronger than a single bond due to the presence of three bonds (one sigma and two pi), when comparing individual bond types, a sigma bond is more difficult to break than a pi bond.

How can you determine the number of sigma and pi bonds in a molecular structure?

In a molecular structure, every single bond contains one sigma bond, and every double bond contains one sigma and one pi bond. A triple bond contains one sigma and two pi bonds. By counting the number of single, double, and triple bonds, you can determine the total number of sigma and pi bonds.

Outlines

00:00

🌌 Introduction to Atomic Orbital Hybridization

This paragraph introduces the concept of atomic orbital hybridization, explaining it as the process of combining atomic orbitals to form hybrid orbitals. It discusses different types of hybrid orbitals such as sp3, sp2, and sp, and how they are formed by mixing s and p orbitals in different proportions. The paragraph also touches on the nature of s and p orbitals, their shapes, and their significance in determining the probability of finding an electron within an atom. The focus is on carbon's electron configuration and how it forms sp3 hybrid orbitals using all four of its valence electrons, with a discussion on the energy levels of these orbitals in relation to the 2s and 2p orbitals.

05:05

🔬 Deep Dive into Hybrid Orbitals and Bonding

The second paragraph delves deeper into the specifics of sp2 and sp hybrid orbitals, detailing the process of hybridization and the resulting energy levels. It explains that sp2 hybridization involves one s and two p orbitals, leading to a 33% s character and 67% p character, while sp hybridization involves one s and one p orbital, resulting in an equal 50% s and p character. The paragraph also discusses the formation of sigma and pi bonds, with sigma bonds formed from the overlap of hybrid orbitals and pi bonds from the overlap of unhybridized p orbitals. It emphasizes the strength of different types of bonds, stating that sigma bonds are stronger than pi bonds, and that triple bonds are stronger than single bonds due to the presence of additional pi bonds.

10:06

🔍 Counting Sigma and Pi Bonds in Molecular Structures

The final paragraph provides a practical application of the concepts discussed, focusing on how to count sigma and pi bonds in a given molecular structure. It explains that each single bond contains one sigma bond, and each double bond contains one sigma bond and one pi bond. The paragraph uses an example structure to illustrate the counting process, showing that there are seven sigma bonds and two pi bonds in the given structure. This section reinforces the understanding of bond types and their significance in molecular structures.

Keywords

💡Hybridization

Hybridization refers to the process where atomic orbitals combine to form new hybrid orbitals. In the context of the video, hybridization is crucial for understanding molecular geometry and bonding. For example, sp3 hybridization involves one s orbital and three p orbitals blending to form four sp3 hybrid orbitals, which is central to the discussion on the structure of carbon compounds.

💡s orbital

An s orbital is a type of atomic orbital that has a spherical shape, representing the region around the nucleus where there is a high probability of finding an electron. The video mentions that s orbitals are involved in hybridization, such as in sp3, sp2, and sp hybrid orbitals, to create different molecular geometries.

💡p orbital

P orbitals are a set of three atomic orbitals that are dumbbell-shaped and oriented along the x, y, and z axes. The video explains that there are three types of p orbitals (px, py, and pz) and they play a significant role in hybridization, contributing to the formation of sp, sp2, and sp3 hybrid orbitals.

💡Degenerate orbitals

Degenerate orbitals are orbitals that have the same energy level. In the video, it is mentioned that the four sp3 hybrid orbitals are degenerate, meaning they all have the same energy. This concept is important for understanding how electrons fill these orbitals in molecular structures.

💡Electron configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. The video uses carbon's electron configuration (1s2 2s2 2p2) as a basis for discussing how its valence electrons participate in hybridization to form sp3, sp2, and sp orbitals.

💡Valence electrons

Valence electrons are the electrons in the outermost shell of an atom that are involved in chemical bonding. The video highlights that carbon has four valence electrons, which are crucial for its ability to form various types of hybrid orbitals and engage in different bonding configurations.

💡Sigma bonds

Sigma bonds are the first type of covalent bond formed between atoms, resulting from the end-to-end overlap of atomic orbitals. The video explains that sigma bonds are formed from the overlap of hybrid orbitals and are present in single, double, and triple bonds.

💡Pi bonds

Pi bonds are a type of covalent bond that forms from the side-to-side overlap of unhybridized p orbitals. The video discusses that pi bonds are weaker than sigma bonds and are found in double and triple bonds, contributing to the overall bond strength.

💡Hund's rule

Hund's rule states that electrons will fill degenerate orbitals singly and with parallel spins before pairing up. The video mentions this rule in the context of adding electrons to degenerate sp3 hybrid orbitals, emphasizing the importance of this principle in molecular orbital theory.

💡Molecular geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. The video connects the concept of hybridization with molecular geometry, explaining how different hybrid orbitals (sp3, sp2, sp) result in different molecular shapes, such as tetrahedral, trigonal planar, and linear.

💡Heisenberg's uncertainty principle

Heisenberg's uncertainty principle states that the exact position and momentum of an electron cannot be simultaneously determined. The video briefly touches on this principle to explain that orbitals provide a probability distribution of where an electron might be found, rather than a precise location.

Highlights

Hybridization is the process of combining atomic orbitals to form hybrid orbitals.

sp3 hybrid orbital is a blend of one s orbital and three p orbitals.

sp2 hybrid orbital is a hybrid of an s orbital and two p orbitals.

sp hybrid orbital is a hybrid of an s orbital and one p orbital.

d2sp3 hybridization involves combining two d orbitals, one s orbital, and three p orbitals.

An s orbital is spherical and represents the probability of finding an electron within an atom.

P orbitals are oriented along the x, y, and z axes and come in three different types.

Carbon's electron configuration is 1s2 2s2 2p2, with four valence electrons.

sp3 hybrid orbitals have 25% s character and 75% p character, placing them closer to the 2p energy level.

sp3 hybrid orbitals are degenerate, meaning they have the same energy.

Electrons should be added one at a time to degenerate orbitals with parallel spins.

sp2 hybrid orbitals have 33% s character and 67% p character, resulting in three hybrid orbitals.

sp hybrid orbitals have an equal 50% s and p character, placing them between s and p orbitals in energy.

Hybrid orbitals are used to form sigma bonds, while unhybridized p orbitals form pi bonds.

Sigma bonds are stronger than pi bonds due to their head-on overlap.

A triple bond is stronger than a single bond because it contains one sigma and two pi bonds.

Triple bonds are shorter than single bonds due to the closer proximity of overlapping orbitals.

Every single bond contains one sigma bond, and every double bond contains one sigma and one pi bond.

A triple bond contains one sigma and two pi bonds, making it the strongest type of covalent bond.

Transcripts

in this video we're going to talk about

hybridization of atomic orbitals

so what exactly is hybridization

hybridization is basically

combining atomic orbitals to make hybrid

orbitals

so for example

the sp3 hybrid orbital

is a blend

of one s orbital and three p orbitals

as you can see it's s1p3

sp2 squared

is a hybrid of an s orbital

and two p orbitals

sp

is a hybrid of s and 1p orbital

so now you know what these terms mean

so let's say if you were to see d2

sp3

this means that you're combining two d

orbitals

one s orbital

and three p orbitals

so what exactly is an s orbital

an s orbital

looks like a sphere

and an orbital tells you the probability

of finding an electron somewhere within

an atom

keep in mind electrons

they can behave as particles and as

waves

so an orbital simply tells you the most

probable location in which you could

find an electron

according to heisenberg's uncertainty

principle

we cannot know precisely the exact

location of an electron

now let's talk about the p orbital

there's one s orbital but there's three

different types of p orbitals

you can have a p orbital

in the x axis

so this is known as p x

you have a p orbital that's oriented

along the y axis

so that's called a py

and then there's one

oriented about the z axis

which we'll call pz

so there's three types of p orbitals

now we're going to talk about the

hybridization of carbon

and the electron configuration of carbon

is 1s2

2s2

2p2

so this is the electron configuration of

carbon

now let's focus on this portion

let's say the 2s

is at an energy level here and let's say

this is 2p

i want to highlight something

so carbon has four valence electrons

now when carbon

forms an sp3 hybrid orbital

it uses

all four orbitals

keep in mind sp3 means that

we need to mix one s with three p

orbitals

so where should we put the sp3 orbitals

should we put them at the same energy

level with the 2s orbital

or with the 2p orbital or somewhere in

between

and should it be like halfway

closer to 2s or closer to 2p what would

you say

now to make an sp3 orbital it requires

four orbitals as you can see here

so one out of those four orbitals is s

which means that the sp3 orbital

has 25 percent

s character

now there's three p orbitals out of four

orbitals three out of four correlates to

75 percent

so the 75 p character

so because the sp3 hybrid orbital

is

has more p character than s

the energy level should be closer to 2p

than it is a 2s

so it should be somewhere over here

now all four of these sp3 hybrid

orbitals they're called degenerate

orbitals degenerate orbitals are those

that have the same energy

so these four electrons

will be placed

in these four sp3 hybrid orbitals

and you want to place the electrons one

at a time when you're adding electrons

to

degenerate orbitals or orbitals of the

same energy

and that's

uh the main idea behind hundred

you want to add electrons with parallel

spins one at a time

if you're adding them

to orbitals of the same energy

now let's talk about

the sp2 hybrid orbital

let's talk about its energy first

so to make an sp2 hybrid orbital we need

one s orbital and two p orbitals

so

we have three p orbitals we're not going

to use all three of them we only need to

use two

that means one of them will remain after

hybridization

so the green arrow would represent the

process of hybridization

so here's the unhybridized 2p orbital it

has the same energy

and now we have sp2

so one out of the three orbitals is s so

this is

we have 33 s character

and

two

out of the three orbitals

is p

two out of three is about sixty seven

percent if you round it

so it's 67 percent p character

so we still have more p character than s

so therefore

the sp2 hybrid orbital should still be

closer

to 2p than 2s

it should be less than sp3

so these three orbitals

will have the same energy

since we use three orbitals to make them

we're going to get three hybrid orbitals

so i'm going to put one orbital in each

i mean one electron in each orbital

so we should have something that looks

like this

so these are the three

sp2 hybrid orbitals

now let's talk about the sp hybrid

orbital

so after hybridization

to make the sp hybrid orbital

we need one s orbital and one p orbital

so we're going to use this s orbital and

only one of the p orbitals

which means the other two p orbitals are

unhybridized

so therefore

they will be unaffected

now if we have an s p orbital

one is s one is p one out of two is

fifty percent

so therefore we have fifty percent s

character

and 50 p character

so therefore

the sp hybrid orbital

should be right in between the s orbital

and the p orbital

and there's two of them since we use one

s and one p orbital or two orbitals to

make the sp hybrid orbital therefore

there must be two hybrid orbitals

so if you were to mix three atomic

orbitals you should get three hybrid

orbitals if you mix four atomic orbitals

you should get four hybrid orbitals

we're mixing one s one p that's a total

of two atomic orbitals

so that will give us two hybrid orbitals

and they will have the same energy

by the way you need to know that

hybrid orbitals are used to form sigma

bonds

the unhybridized orbitals in this case

the p orbitals that were unaffected

and hybridized orbitals are used to make

pi bonds which we'll talk more about

later

so just keep that in mind

so pi bonds are always made from

unhybridized p orbitals when you're

dealing with carbon atoms

and sigma bonds

they form from the overlap of atomic

orbitals

and they consist of hybrid orbitals for

the most part

every single bond that you see

contains one

sigma bond

every double bond

has at least one sigma and it has one pi

bond

a triple bond

contains one sigma

and two bipods

by the way a triple bond is stronger

than a sigma bond or a single bond

three bonds are more stronger than uh

one bond it's harder to break three

pencils than it is to break one so keep

this in my triple bonds are stronger

than single bonds but triple bonds are

shorter than single bonds single bonds

are longer

but now if you compare

one bond to another

you need to know that

well before i say it which one do you

think is stronger a sigma bond or a pi

bond

what do you think about that

sigma bonds are stronger than pi bonds

the reason why a triple bond is stronger

than a single bond

is because you're comparing

three bonds as opposed to one

so these two sigma bonds let's assume

they're equal

the triple bond is going to win because

it has two additional pi bonds

so when comparing a triple bond versus

the signal bond

the triple bond is stronger because you

compare three bonds compared to one but

if we compare one sigma

versus a pi bond the pi bond is weaker

it's easier to break a pi bond but it's

harder to break a sigma bond so just

keep that in mind

sigma bonds are stronger than

pi bonds

now let's say if you have a structure

that looks like this

how many sigma bonds

are in this structure and how many pi

bonds are there

so every bond contains one sigma so one

two three four

five six seven therefore there are seven

sigma bonds and every double bond has

one pi bond so one two two pi bonds

and that's a simple and easy way to

count the number of sigma and pi bonds