Sp² Hybridization in Ethene: The Secret of Double Bonds

Sp² Hybridization in Ethene: The Secret of Double Bonds

Assessment

Interactive Video

Chemistry, Science, Physics

10th Grade - University

Practice Problem

Hard

Created by

Wayground Content

FREE Resource

The video tutorial explains the structure and bonding of ethane, focusing on its carbon-carbon double bond, which consists of a sigma and a pi bond. Ethane's SP2 hybridization results in a trigonal planar structure with a bond angle close to 120°. The double bond is strong, with a bond energy of 146 kcal/mol, and the pi bond has a shorter bond length of 1.34 angstroms. The tutorial visualizes the orbital structure, showing how SP2 hybrid orbitals form sigma bonds and how unhybridized p orbitals form pi bonds through lateral overlap, resulting in a delocalized orbital. The structure of ethane is also represented in different ways.

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5 questions

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1.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the hybridization of carbon atoms in ethane?

SP

SP2

None of the above

SP3

2.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the bond angle in the trigonal planar structure of ethane?

180°

120°

109.5°

90°

3.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the bond energy of the double bond in ethane?

100 kilocalories per mole

146 kilocalories per mole

250 kilocalories per mole

200 kilocalories per mole

4.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which orbitals overlap to form the sigma bond in ethane?

SP2 and SP2

P and P

S and P

SP3 and SP3

5.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the nature of the pi orbital in ethane?

Delocalized

Non-existent

Hybridized

Localized

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