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Questions and Answers
What is the shape of the molecule formed through sp3 hybridization?
Which type of bond is formed by lateral overlap of atomic orbitals?
What is the shape of the molecule formed through spd2 hybridization?
What character does each sp3 hybrid orbital have?
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What is the reason for sigma bonds being stronger than pi bonds?
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What is the shape of the molecule formed through sp2 hybridization?
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How many electron domains are required for spd hybridization?
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What is the shape of the molecule formed through spd3 hybridization?
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How many hybrid orbitals are formed in sp3 hybridization?
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What type of bond is formed by head-on overlap of atomic orbitals?
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Study Notes
Hybridization in Chemistry
Sigma and Pi Bonds
- Sigma (σ) bonds: formed by head-on overlap of atomic orbitals, resulting in a cylindrical shape
- Pi (Ï€) bonds: formed by lateral overlap of atomic orbitals, resulting in a nodal plane
- Sigma bonds are stronger than pi bonds due to greater orbital overlap
- Multiple bonds (double, triple) contain one sigma bond and one or two pi bonds
Sp3 Hybridization
- Sp3 hybridization occurs when an atom has four electron domains (e.g., methane, CH4)
- The s orbital and three p orbitals mix to form four equivalent hybrid orbitals
- Each sp3 hybrid orbital has 25% s character and 75% p character
- The resulting molecule has a tetrahedral shape
spd, spd2, sp2, and spd3 Hybridization
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spd Hybridization: occurs when an atom has five electron domains (e.g., phosphorus, PF5)
- The s orbital, three p orbitals, and one d orbital mix to form five hybrid orbitals
- The resulting molecule has a trigonal bipyramidal shape
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spd2 Hybridization: occurs when an atom has six electron domains (e.g., sulfur, SF6)
- The s orbital, three p orbitals, and two d orbitals mix to form six hybrid orbitals
- The resulting molecule has an octahedral shape
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sp2 Hybridization: occurs when an atom has three electron domains (e.g., ethene, C2H4)
- The s orbital and two p orbitals mix to form three hybrid orbitals
- The resulting molecule has a trigonal planar shape
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spd3 Hybridization: occurs when an atom has seven electron domains (e.g., iodine, IF7)
- The s orbital, three p orbitals, and three d orbitals mix to form seven hybrid orbitals
- The resulting molecule has a pentagonal bipyramidal shape
Sigma and Pi Bonds
- Sigma bonds are formed by head-on overlap of atomic orbitals, resulting in a cylindrical shape
- Pi bonds are formed by lateral overlap of atomic orbitals, resulting in a nodal plane
- Sigma bonds are stronger than pi bonds due to greater orbital overlap
- Multiple bonds (double, triple) contain one sigma bond and one or two pi bonds
Sp3 Hybridization
- Sp3 hybridization occurs when an atom has four electron domains (e.g., methane, CH4)
- The s orbital and three p orbitals mix to form four equivalent hybrid orbitals
- Each sp3 hybrid orbital has 25% s character and 75% p character
- The resulting molecule has a tetrahedral shape
Other Hybridizations
- spd Hybridization: occurs when an atom has five electron domains (e.g., phosphorus, PF5)
- The s orbital, three p orbitals, and one d orbital mix to form five hybrid orbitals
- The resulting molecule has a trigonal bipyramidal shape
- spd2 Hybridization: occurs when an atom has six electron domains (e.g., sulfur, SF6)
- The s orbital, three p orbitals, and two d orbitals mix to form six hybrid orbitals
- The resulting molecule has an octahedral shape
- sp2 Hybridization: occurs when an atom has three electron domains (e.g., ethene, C2H4)
- The s orbital and two p orbitals mix to form three hybrid orbitals
- The resulting molecule has a trigonal planar shape
- spd3 Hybridization: occurs when an atom has seven electron domains (e.g., iodine, IF7)
- The s orbital, three p orbitals, and three d orbitals mix to form seven hybrid orbitals
- The resulting molecule has a pentagonal bipyramidal shape
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Description
Learn about the formation of sigma and pi bonds in chemistry, their differences, and the concept of sp3 hybridization. Understand the characteristics of single, double, and triple bonds.
