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sp3 Hybridisation in Ethane
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Today, we will learn about hybridisation, starting with the sp3 hybridisation in ethane, C2H6. Can anyone tell me how hybridisation affects molecular structure?
Does it help in understanding the shape of the molecule?
Exactly! In ethane, each carbon atom undergoes sp3 hybridisation, meaning one s orbital and three p orbitals mix to form four equivalent sp3 hybrid orbitals.
So, how do these orbitals interact?
Great question! One sp3 hybrid orbital from each carbon atom overlaps axially to form a sigma bond between the two carbons. The other three sp3 orbitals from each carbon bond with hydrogen atoms.
What are the bond lengths in C2H6?
The CβC bond length is 154 pm while each CβH bond measures about 109 pm. This illustrates how bond lengths can indicate hybridisation types.
To recap, in sp3 hybridisation, the orbitals adopted are equivalent in shape and energy, and they form tetrahedral arrangements around the carbon atoms.
sp2 Hybridisation in Ethene
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Now let's shift to sp2 hybridisation in ethene, C2H4. Can anyone describe what happens during its formation?
Doesn't it involve two p orbitals and one s orbital?
Correct! Here, one s and two p orbitals combine to create three sp2 hybrid orbitals. These orbitals arrange themselves in a trigonal planar shape.
What about the bonds formed in ethene?
One sp2 hybrid orbital overlaps with that from another carbon to form a sigma bond. The remaining two sp2 orbitals bond with hydrogen atoms. Additionally, the unhybridised p orbitals produce a pi bond.
So thereβs a double bond between the carbons?
Exactly! The carbon-carbon bond consists of one sigma and one pi bond, leading to bond lengths of 134 pm and HβC bonds measuring 108 pm.
In summary, sp2 hybridisation creates planar structures where p orbitals can work together to form pi bonds.
sp Hybridisation in Ethyne
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Let's conclude with sp hybridisation, specifically in ethyne, C2H2. What do you know about this hybridisation?
Isnβt it when one s orbital and one p orbital mix to create two sp hybrid orbitals?
Exactly! These sp hybrid orbitals allow for a linear arrangement, aligned with the z-axis. Each carbon forms a sigma bond with the other carbon via their sp hybrid orbitals.
And what about the triple bond?
Great observation! The triple bond consists of one sigma bond from the sp hybrid orbitals and two pi bonds formed by the remaining unhybridised p orbitals, creating a strong bond structure.
So, what are the bond lengths in ethyne?
The CβC bond length is quite short at about 120 pm, demonstrating the strength associated with triple bonds. Remember, linear structures emerge from sp hybridisation.
In summary, ethyne showcases how hybridised orbitals dictate molecular shapes and bond structures.
Introduction & Overview
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Quick Overview
Standard
The section covers hybridisation in various molecules, detailing the formation of different hybridised orbitals. Specific examples such as ethane (C2H6), ethene (C2H4), and ethyne (C2H2) are examined to elucidate sp3, sp2, and sp hybridisation, respectively.
Detailed
Detailed Summary
In this section, hybridisation is explored with practical examples demonstrating how molecular geometry is defined based on the hybridisation of atomic orbitals.
Key Points:
- sp3 Hybridisation in C2H6 (Ethane): Ethane has carbon atoms adopting sp3 hybrid states. Each carbon forms sp3-sp3 sigma bonds with each other and sp3-s sigma bonds with hydrogens. CβC and CβH bond lengths are specified, demonstrating the typical bond characteristics of an ethane molecule.
- sp2 Hybridisation in C2H4 (Ethene): In ethene, one sp2 hybrid orbital on each carbon overlaps to form a CβC sigma bond, with the remaining hybrid orbitals forming bonds with two hydrogens. An unhybridised orbital from each carbon overlaps sidewise to create a pi bond, essential for double bond formation, and several angles are defined to characterize the geometry accurately.
- sp Hybridisation in C2H2 (Ethyne): In ethyne, carbon atoms use sp hybridisation, allowing the formation of a strong triple bond consisting of one sigma and two pi bonds. Each carbon occupies two unhybridised p orbitals to facilitate this bonding.
The detailed examination of these examples highlights how hybridisation explains the molecular structures and the bond behaviors in organic compounds.
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sp3 Hybridisation in C2H6
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In ethane molecule both the carbon atoms assume sp3 hybrid state. One of the four sp3 hybrid orbitals of carbon atom overlaps axially with similar orbitals of other atom to form sp3-sp3 sigma bond while the other three hybrid orbitals of each carbon atom are used in forming sp3βs sigma bonds with hydrogen atoms as discussed in section 4.6.1(iii). Therefore in ethane CβC bond length is 154 pm and each CβH bond length is 109 pm.
Detailed Explanation
In ethane (C2H6), each carbon atom undergoes sp3 hybridisation, meaning each carbon mixes one s and three p orbitals to form four new equivalent orbitals. These sp3 hybrid orbitals are arranged in a tetrahedral geometry around each carbon atom. When two carbon atoms come together, one sp3 hybrid orbital from each carbon overlaps to create a strong sigma bond between them. Additionally, the remaining hybrid orbitals form bonds with hydrogen atoms. This results in specific bond lengths; the CβC bond is 154 pm long, while each CβH bond is 109 pm long. This arrangement allows ethane to have its characteristic structure and stability.
Examples & Analogies
Imagine two friends (the carbon atoms) sitting across a table (the bond) and each holding hands with others (hydrogens) on both sides. Their hands (the bonds) will stretch comfortably, not too tight, creating a cozy setting, reminiscent of the bond lengths in the ethane molecule. This comfortable arrangement keeps the friends close while allowing space to move, as in the tetrahedral shape of ethane.
sp2 Hybridisation in C2H4
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In the formation of ethene molecule, one of the sp2 hybrid orbitals of carbon atom overlaps axially with sp2 hybridised orbital of another carbon atom to form CβC sigma bond. While the other two sp2 hybrid orbitals of each carbon atom are used for making sp2βs sigma bond with two hydrogen atoms. The unhybridised orbital (2px or 2py) of one carbon atom overlaps sidewise with the similar orbital of the other carbon atom to form weak Ο bond, which consists of two equal electron clouds distributed above and below the plane of carbon and hydrogen atoms. Thus, in ethene, the carbon-carbon bond consists of one sp2βsp2 sigma bond and one Ο bond.
Detailed Explanation
In ethene (C2H4), each carbon atom uses sp2 hybridisation, mixing one s and two p orbitals to create three equivalent sp2 orbitals. These orbitals arrange in a trigonal planar configuration. When two carbon atoms unite, one sp2 hybrid orbital from each overlaps to form a strong sigma bond (CβC bond). The remaining sp2 orbitals bond with hydrogen atoms, while the leftover p orbital from each carbon overlaps sidewise to form a Ο bond, which is not as strong but exists above and below the plane of the molecule. The presence of this Ο bond gives ethene its characteristic reactivity in addition to the sigma bond.
Examples & Analogies
Consider two dancers (the carbon atoms) in a competition who hold each other's hands (creating the CβC bond) while their other arms are extended out to touch the hands of other dancers (the hydrogen atoms). Together they create a beautiful formation where thereβs a strong connection in the middle (the sigma bond) and a light, flowing movement around them (the pi bond) that adds grace to their performance, reminiscent of the double bond in ethene.
sp Hybridisation in C2H2
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In the formation of ethyne molecule, both the carbon atoms undergo sp-hybridisation having two unhybridised orbital i.e., 2py and 2px. One sp hybrid orbital of one carbon atom overlaps axially with sp hybrid orbital of the other carbon atom to form CβC sigma bond, while the other hybridised orbital of each carbon atom overlaps axially with the half filled s orbital of hydrogen atoms forming Ο bonds. Each of the two unhybridised p orbitals of both the carbon atoms overlaps sidewise to form two Ο bonds between the carbon atoms. Thus, the triple bond between the two carbon atoms is made up of one sigma and two pi bonds.
Detailed Explanation
In ethyne (C2H2), the carbon atoms undergo sp hybridisation, combining one s orbital and one p orbital to create two equivalent sp hybrid orbitals. These two sp hybrid orbitals arrange in a linear fashion. When the two carbon atoms come closer, they overlap to create a strong sigma bond (CβC bond). Additionally, each carbon's remaining half-filled p orbital overlaps to form two sidewise Ο bonds, resulting in a triple bond. This combination of one sigma bond and two pi bonds provides ethyne its stability and unique geometrical structure.
Examples & Analogies
Imagine two strong ropes (the carbon atoms) pulled tightly to form a straight line (the CβC bond). Now, as the ropes pull together, there are also some ribbons (the hydrogen atoms) tied onto the ropes, pulling them in different directions (the sigma bonds). Overlapping the ribbons creates a double wrap around the ropes (the pi bonds), creating a strong and stable connection. This illustrates the triple bond structure in ethyne.
Definitions & Key Concepts
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Key Concepts
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sp Hybridisation: A type of hybridisation creating two hybrid orbitals.
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sp2 Hybridisation: Hybridisation that results in three equivalent orbitals.
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sp3 Hybridisation: A hybridisation resulting in four orbitals used for bonding.
Examples & Real-Life Applications
See how the concepts apply in real-world scenarios to understand their practical implications.
Examples
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C2H6 (Ethane): Each carbon undergoes sp3 hybridisation.
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C2H4 (Ethene): Features sp2 hybridisation with double bonds.
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C2H2 (Ethyne): Demonstrates sp hybridisation with triple bonds.
Memory Aids
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π΅ Rhymes Time
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In ethane, sp3 leads to four bonds galore, join with C and H, then you have more.
π Fascinating Stories
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Imagine carbon at a dance, spinning with three friends, perfectly arranging themselves in a tetrahedral stance.
π§ Other Memory Gems
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For sp3, think of Three (H) and One (C): '3 is one more!'
π― Super Acronyms
SP2 = Sum of Parts
- 1S + 2P = 3 Total!
Flash Cards
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Glossary of Terms
Review the Definitions for terms.
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Term: sp Hybridisation
Definition:
Hybridisation where one s and one p orbital combine to form two equivalent sp hybrid orbitals.
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Term: sp2 Hybridisation
Definition:
Hybridisation involving one s and two p orbitals resulting in three equivalent sp2 hybrid orbitals.
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Term: sp3 Hybridisation
Definition:
Hybridisation involving one s and three p orbitals leading to four equivalent sp3 hybrid orbitals.
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Term: Sigma Bond
Definition:
A bond formed by the head-to-head overlap of orbitals.
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Term: Pi Bond
Definition:
A bond resulting from the sidewise overlap of p orbitals.