Textbook Question
What orbitals are used to form the carbon–carbon s bond between the highlighted carbons?
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1. A Review of General Chemistry
Hybridization
2:01 minutesProblem 11b
Textbook Question
Predict the hybridization of the indicated atoms.
(b) 
Verified step by step guidance1
Identify the atom in question and examine its bonding environment. Count the number of sigma bonds (single bonds) and lone pairs of electrons around the atom.
Use the formula for hybridization: Hybridization = (Number of sigma bonds + Number of lone pairs). This will help determine the steric number of the atom.
Match the steric number to the corresponding hybridization: steric number 2 = sp, steric number 3 = sp², steric number 4 = sp³, steric number 5 = sp³d, steric number 6 = sp³d².
Consider the geometry of the molecule to confirm the hybridization. For example, sp corresponds to linear geometry, sp² to trigonal planar, and sp³ to tetrahedral.
Verify your prediction by checking the molecular structure and ensuring that the hybridization aligns with the observed bond angles and geometry.
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2mKey Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Hybridization
Hybridization is the concept in chemistry where atomic orbitals mix to form new hybrid orbitals, which can explain the geometry of molecular bonding. For example, in carbon, the mixing of one s and three p orbitals results in four sp3 hybrid orbitals, leading to a tetrahedral shape. Understanding hybridization helps predict molecular shapes and bond angles.
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VSEPR Theory
Valence Shell Electron Pair Repulsion (VSEPR) Theory is used to predict the geometry of molecules based on the repulsion between electron pairs around a central atom. According to VSEPR, electron pairs will arrange themselves to minimize repulsion, leading to specific molecular shapes such as linear, trigonal planar, or tetrahedral. This theory is essential for visualizing molecular structures.
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Bonding and Lone Pairs
In molecular structures, bonding pairs of electrons are shared between atoms, while lone pairs are non-bonding electrons localized on a single atom. The presence of lone pairs can significantly affect the hybridization and geometry of a molecule, as they occupy space and influence the arrangement of bonding pairs. Recognizing the role of lone pairs is crucial for accurate predictions of molecular shape.
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