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Questions and Answers
What is the angle between the sp2 hybrid orbitals in ethene?
Which type of bond is formed by the overlapping of sp3 orbitals of carbon and 1s orbitals of hydrogen in alkanes?
How many pi bonds are present in ethene?
What is the primary difference between sp3 hybridization and sp2 hybridization?
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What is the shape of the sp3 hybrid orbitals?
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What is the total number of bonds in ethene, including sigma and pi bonds?
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Which type of hybridization is used in the formation of bonds in alkenes?
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What is the difference in energy between sp3 and 2p orbitals?
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How many unpaired electrons are present in each sp3 orbital?
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What is the angle between the unhybridized 2p orbitals in ethene that overlap to form a pi bond?
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Study Notes
Orbitals and Quantum Numbers
- Each orbital is described by three sets of quantum numbers: principal (n), azimuthal (l), and magnetic (M), and spin quantum number.
- The principal quantum number (n) determines the main energy level and size of orbitals.
- The azimuthal quantum number (l) defines the shape of the orbitals.
- The magnetic quantum number (M) specifies the spatial orientation of orbitals.
- The spin quantum number describes the spin of electrons in orbitals.
Rules of Electron Arrangement
- The Aufbau principle, Pauli exclusion principle, and Hund's rule govern electron arrangement.
- Electrons fill orbitals starting with the lowest energy level.
- No orbital can contain more than two electrons with opposite spins.
Electron Arrangement in Carbon
- Carbon's electron arrangement follows the Aufbau principle, Pauli exclusion principle, and Hund's rule.
- Electrons are distributed among 1s and 2s orbitals, and the three 2p orbitals.
Orbital Hybridization
- Hybridization is the formation of new orbitals by combining two or more orbitals with different energy, shape, and size.
- Carbon atoms typically bond with other atoms using their orbitals and unpaired electrons.
sp3 Hybridization and Bond Formation in Alkanes
- sp3 hybridization involves mixing the 2s orbital and all three 2p orbitals of carbon to form four new hybrid orbitals.
- The sp3 orbitals have a tetrahedral shape and are arranged at 109.5° to each other in the excited state.
- sp3 hybridization is used in the formation of bonds in alkanes, such as methane.
sp Hybridization and Bond Formation in Alkynes
- sp hybridization involves promoting one electron from the 2s orbital to the empty 2p orbital, resulting in two hybrid orbitals of equal energy.
- The hybrid orbitals are linear and oriented at 180° to each other.
- Two of the 2p orbitals remain unhybridized and are oriented perpendicular to the plane of the linear sp orbitals and to each other.
- sp hybridization is used in the formation of bonds in alkynes, such as ethyne.
sp2 Hybridization and Bond Formation in Alkenes
- sp2 hybridization involves promoting one electron from the 2s orbital to the 2p orbital, resulting in three new hybrid orbitals.
- The sp2 hybrid orbitals are of equivalent energy and are displayed along the apex of a triangle with an angle of 120° between them.
- sp2 hybridization is used in the formation of bonds in alkenes, such as ethene.
Electronic Theory of Valency and Molecular Orbital Theory
- The electronic theory of valency suggests that chemical bonding involves the electrons in the outer shells of atoms.
- The octet rule applies to elements in the second period, including carbon, which exhibits a valency of four.
- The sp3 orbitals have higher energy than 2s but lower than 2p orbitals and contain one unpaired electron each.
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Description
Test your knowledge on quantum numbers and electron configuration with this quiz. Learn about the different sets of quantum numbers that describe orbitals, as well as the rules governing electron arrangement.
