How many types of hybrid orbitals do we use to describe each molecule? b. C 2 H 5 NO (four C-H bonds and one O-H bond)

Hi everyone here, we have a question asking us to determine the total number of hybrid orbital's in acetone I trial. So first let's draw our LewiS structure. We have a central carbon Single bonded to three hydrogen single bonded to a carbon, Which is triple bonded to a nitrogen with one lone pair. So our central carbon has a linear electron geometry And two sp hybrid orbital's. Our CH three Group as tetra. He'd rel electron geometry And has four sp 3 hybrid total rebuttals. Our nitrogen has linear electron geometry, It has two sp hybrid orbital's. So there are a total of eight hybrid orbital's and that is our final answer. Thank you for watching. Bye.

Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory

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Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory

Problem 97b

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Chapter 10, Problem 97b

How many types of hybrid orbitals do we use to describe each molecule? b. C₂H₅NO (four C-H bonds and one O-H bond)

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Identify the central atoms in the molecule C_2H_5NO. The central atoms are typically carbon (C) and nitrogen (N) in organic molecules.

Determine the hybridization of each central atom based on the number of atoms bonded to it and lone pairs.

For each carbon atom in C_2H_5NO, count the number of sigma bonds and lone pairs to determine the hybridization. Carbon typically forms four sigma bonds, leading to sp^3 hybridization.

For the nitrogen atom, count the number of sigma bonds and lone pairs. Nitrogen in this molecule is likely to form three sigma bonds and have one lone pair, leading to sp^3 hybridization.

Consider the oxygen atom, which forms one sigma bond and has two lone pairs, leading to sp^3 hybridization.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Hybridization

Hybridization is the process of combining atomic orbitals to form new hybrid orbitals that can accommodate the bonding requirements of a molecule. In the case of carbon, for example, the 2s and three 2p orbitals can hybridize to form four equivalent sp³ hybrid orbitals, which are used to form sigma bonds with other atoms.

Types of Hybrid Orbitals

There are several types of hybrid orbitals, including sp, sp², and sp³. The type of hybridization depends on the number of electron domains around the central atom. For instance, sp hybridization occurs in linear geometries with two electron domains, while sp³ hybridization occurs in tetrahedral geometries with four electron domains, as seen in molecules like C₂H₅NO.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule, which is influenced by the types of hybrid orbitals involved. The geometry helps predict the bond angles and overall shape of the molecule, which is crucial for understanding reactivity and properties. In C₂H₅NO, the presence of different types of bonds (C-H and O-H) will affect its hybridization and geometry.