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Questions and Answers
What is the hybridization state of carbon in methane (CH4)?
What is the hybridization state of carbon in methane (CH4)?
Which hybridization corresponds to nitrogen in ammonia (NH3)?
Which hybridization corresponds to nitrogen in ammonia (NH3)?
What is the molecular geometry of water (H2O) based on its hybridization?
What is the molecular geometry of water (H2O) based on its hybridization?
What is the percentage of p-orbital character in the hybridized state of carbon?
What is the percentage of p-orbital character in the hybridized state of carbon?
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Which of the following describes the hybridization of oxygen in water (H2O)?
Which of the following describes the hybridization of oxygen in water (H2O)?
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In which molecule does nitrogen display a trigonal pyramidal geometry due to its hybridization?
In which molecule does nitrogen display a trigonal pyramidal geometry due to its hybridization?
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Which electron configuration represents the hybridized state of carbon?
Which electron configuration represents the hybridized state of carbon?
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How do you classify the arrangement of electron pairs around nitrogen in NH3?
How do you classify the arrangement of electron pairs around nitrogen in NH3?
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What type of hybridization does not occur in the elements discussed?
What type of hybridization does not occur in the elements discussed?
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What is the primary characteristic of the hybridization of carbon?
What is the primary characteristic of the hybridization of carbon?
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What orbital result is produced from the overlap of 1s orbitals in H2?
What orbital result is produced from the overlap of 1s orbitals in H2?
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In the ground state of carbon, how many half-filled p orbitals are present?
In the ground state of carbon, how many half-filled p orbitals are present?
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What is the cause for carbon to promote an electron from the 2s to a 2p orbital?
What is the cause for carbon to promote an electron from the 2s to a 2p orbital?
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What shape do the hybrid sp3 orbitals of carbon point towards?
What shape do the hybrid sp3 orbitals of carbon point towards?
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How many equivalent C–H bonds are present in methane?
How many equivalent C–H bonds are present in methane?
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What occurs during the hybridization of carbon's orbitals?
What occurs during the hybridization of carbon's orbitals?
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Which of the following describes the bonding orbital formed in H2?
Which of the following describes the bonding orbital formed in H2?
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What type of bond is described as having differing energies and bond lengths from the overlap of carbon and hydrogen orbitals?
What type of bond is described as having differing energies and bond lengths from the overlap of carbon and hydrogen orbitals?
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What is the electron configuration of carbon in its promoted state?
What is the electron configuration of carbon in its promoted state?
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What energy condition must be met for carbon to promote an electron into a higher energy orbital?
What energy condition must be met for carbon to promote an electron into a higher energy orbital?
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What hybridization is exhibited by a central atom with 4 electron pairs in its valence shell?
What hybridization is exhibited by a central atom with 4 electron pairs in its valence shell?
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In which compound does the central atom exhibit trigonal bipyramidal geometry?
In which compound does the central atom exhibit trigonal bipyramidal geometry?
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Which hybridization percentage character corresponds with the sp2 hybrid orbital?
Which hybridization percentage character corresponds with the sp2 hybrid orbital?
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What type of hybridization occurs in ethyne (C2H2)?
What type of hybridization occurs in ethyne (C2H2)?
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How many unhybridised orbitals are present in a carbon atom that is sp2 hybridised?
How many unhybridised orbitals are present in a carbon atom that is sp2 hybridised?
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Which of the following molecular geometries corresponds with sp hybridization?
Which of the following molecular geometries corresponds with sp hybridization?
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Which molecule is correctly represented by sp3 hybridisation?
Which molecule is correctly represented by sp3 hybridisation?
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In diborane (B2H6), how many valence electrons are involved?
In diborane (B2H6), how many valence electrons are involved?
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Which hybridization corresponds with the central atom in a molecule exhibiting tetrahedral geometry?
Which hybridization corresponds with the central atom in a molecule exhibiting tetrahedral geometry?
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Which of the following statements about aspirin (C9H8O4) is incorrect?
Which of the following statements about aspirin (C9H8O4) is incorrect?
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Study Notes
Orbital Hybridization and Bonding
- Orbital hybridization occurs when atomic orbitals combine to form new hybrid orbitals with different shapes and energies.
- Hybrid orbitals are utilized for explaining molecular geometry and bonding.
- Hybrid orbitals possess better directional properties than atomic orbitals, resulting in stronger, more stable bonds.
Methane (CH4)
- Each C atom in methane forms four identical C-H sigma bonds.
- The 2s and three 2p orbitals of the carbon atom hybridize to form four sp3 hybrid orbitals.
- The sp3 hybrid orbitals have a tetrahedral geometry, meaning they point towards the vertices of a tetrahedron.
Ammonia (NH3)
- The nitrogen atom in ammonia is sp3 hybridized, but it has a lone pair of electrons.
- The four sp3 hybrid orbitals are arranged in a tetrahedral geometry.
- Since there are three bonding pairs and one lone pair of electrons, the geometry is trigonal pyramidal.
Water (H2O)
- The oxygen atom in water is also sp3 hybridized, but it has two lone pairs of electrons.
- The four sp3 hybrid orbitals are in a tetrahedral arrangement.
- Because there are two bonding pairs and two lone pairs of electrons, the geometry is angular or bent.
Ethene (CH2=CH2)
- Each carbon atom forms two sigma bonds and one pi bond.
- The C atoms are sp2 hybridized, meaning they have three sp2 hybrid orbitals and one unhybridized 2p orbital.
- Each carbon atom forms a sigma bond with each of the two hydrogen atoms and a sigma bond with the other carbon atom.
- The unhybridized 2p orbitals overlap to form a pi bond between the two carbon atoms.
Ethyne (CH≡CH)
- Each carbon atom forms one σ bond and two π bonds.
- C atoms are sp hybridized, possessing two unhybridized 2p orbitals each.
- The sp hybrid orbitals form σ bonds with the hydrogen atoms and each other.
- The two unhybridized 2p orbitals overlap to form two pi bonds between the carbons.
Hybridisation Summary
- Linear molecules (sp hybridized) have 2 electron pairs.
- Trigonal planar (sp2 hybridized) molecules have 3 electron pairs.
- Tetrahedral molecules (sp3 hybridized) have 4 electron pairs.
Diborane (B2H6)
- Diborane is an exception to the normal rules of hybridization since its structure involves three-center two-electron (3c-2e) bonds.
- Two boron atoms each possess three valence electrons, while six hydrogen atoms contribute one electron each.
- The 3c-2e bonds are formed between two hydrogen atoms and a boron atom, creating a unique bonding pattern.
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Description
Test your understanding of orbital hybridization and bonding in molecules such as methane, ammonia, and water. This quiz covers the principles of hybrid orbitals, their geometries, and their impact on molecular bonding. Assess your knowledge of sp3 hybridization and its applications in various compounds.
