Textbook Question
Refer to the following Lewis structures.
(c)
(d)
If an atom is sp² hybridized, how many sp²-hybridized orbitals does it use for bonding? How many p orbitals?
1. A Review of General Chemistry
Hybridization
2:46 minutesProblem 3a
Textbook Question
What is the hybridization of carbon in each of the following molecules?
(a) 
Verified step by step guidance1
Step 1: Understand the concept of hybridization. Hybridization is the mixing of atomic orbitals to form new hybrid orbitals that are degenerate in energy and suitable for bonding. The type of hybridization depends on the number of regions of electron density (bonds or lone pairs) around the atom.
Step 2: Identify the number of regions of electron density around the carbon atom in the given molecule. This includes single bonds, double bonds, triple bonds, and lone pairs. Each counts as one region of electron density.
Step 3: Determine the hybridization based on the number of regions of electron density: (a) 2 regions = sp hybridization, (b) 3 regions = sp² hybridization, (c) 4 regions = sp³ hybridization.
Step 4: For each carbon atom in the molecule, count the regions of electron density and assign the corresponding hybridization. For example, if a carbon is involved in a double bond and two single bonds, it has 3 regions of electron density and is sp² hybridized.
Step 5: Repeat the process for all carbon atoms in the molecule, ensuring to consider lone pairs or resonance structures if applicable, and summarize the hybridization for each carbon atom.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Hybridization
Hybridization is a concept in organic chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals. These hybrid orbitals are used to form covalent bonds in molecules. The type of hybridization (sp, sp2, sp3, etc.) depends on the number of bonds and lone pairs around the central atom, particularly carbon in organic compounds.
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Types of Hybridization
The main types of hybridization for carbon are sp3, sp2, and sp. In sp3 hybridization, carbon forms four equivalent bonds with a tetrahedral geometry. In sp2 hybridization, it forms three bonds with a trigonal planar geometry, and in sp hybridization, it forms two bonds with a linear geometry. Understanding these types is crucial for determining the geometry and reactivity of organic molecules.
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Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. It is influenced by the hybridization of the central atom and the presence of lone pairs. The geometry helps predict the shape and reactivity of the molecule, which is essential for understanding its chemical behavior and interactions with other substances.
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