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- https://chem.libretexts.org/Courses/Smith_College/Organic_Chemistry_(LibreTexts)/01%3A_Structure_and_Bonding/1.07%3A_sp_Hybrid_Orbitals_and_the_Structure_of_MethaneThe four identical C-H single bonds in methane form as the result of sigma bond overlap between the sp3 hybrid orbitals of carbon and the s orbital of each hydrogen.
- https://chem.libretexts.org/Courses/Oregon_Institute_of_Technology/OIT%3A_CHE_333_-_Organic_Chemistry_III_(Lund)/New_Page/2%3A_Introduction_to_Organic_Structure_and_Bonding_II/2.1%3A_Valence_Bond_TheoryValence bond theory is most often used to describe bonding in organic molecules. In this model, bonds are considered to form from the overlap of two atomic orbitals on different atoms, each orbital c...Valence bond theory is most often used to describe bonding in organic molecules. In this model, bonds are considered to form from the overlap of two atomic orbitals on different atoms, each orbital containing a single electron. In looking at simple inorganic molecules such as molecular hydrogen (H2) or hydrogen fluoride (HF), our present understanding of s and p atomic orbitals will suffice. In order to explain the bonding in organic molecules, however, we will need to introduce hybrid orbitals
- https://chem.libretexts.org/Courses/can/CHEM_231%3A_Organic_Chemistry_I_Textbook/01%3A_Structure_and_Bonding/1.07%3A_sp_Hybrid_Orbitals_and_the_Structure_of_MethaneThe four identical C-H single bonds in methane form as the result of sigma bond overlap between the sp3 hybrid orbitals of carbon and the s orbital of each hydrogen.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/09%3A_Covalent_Bonding/9.22%3A_Hybrid_Orbitals_-_spThis page explores hybridization in chemistry, centering on carbon's bonding in methane (CH4. Despite its electron configuration indicating it should form only two bonds, carbon actually for...This page explores hybridization in chemistry, centering on carbon's bonding in methane (CH4. Despite its electron configuration indicating it should form only two bonds, carbon actually forms four through sp3 hybridization, which mixes one s and three p orbitals. This process results in four equivalent hybrid orbitals, accounting for methane's tetrahedral geometry and bond angles.
- https://chem.libretexts.org/Courses/Alma_College/Organic_Chemistry_I_(Alma_College)/01%3A_Structure_and_Bonding/1.07%3A_sp_Hybrid_Orbitals_and_the_Structure_of_MethaneThe four identical C-H single bonds in methane form as the result of sigma bond overlap between the sp3 hybrid orbitals of carbon and the s orbital of each hydrogen.
- https://chem.libretexts.org/Courses/Chandler_Gilbert_Community_College/Fundamental_Organic_ala_Mech/02%3A_Molecular_Structure/2.04%3A_sp_Hybrid_Orbitals_and_the_Structure_of_MethaneThe four identical C-H single bonds in methane form as the result of sigma bond overlap between the sp3 hybrid orbitals of carbon and the s orbital of each hydrogen.
- https://chem.libretexts.org/Bookshelves/Organic_Chemistry/Organic_Chemistry_(Morsch_et_al.)/01%3A_Structure_and_Bonding/1.06%3A_sp_Hybrid_Orbitals_and_the_Structure_of_MethaneThe text explains the structure of methane (CH4) using the concept of sp3 hybridization of the central carbon atom. Methane exhibits a tetrahedral shape with an H-C-H bond angle of 109.5??. Valence bo...The text explains the structure of methane (CH4) using the concept of sp3 hybridization of the central carbon atom. Methane exhibits a tetrahedral shape with an H-C-H bond angle of 109.5??. Valence bond theory and Linus Pauling's hybridization model are highlighted to explain how carbon's 2s and 2p orbitals combine to form four equivalent sp3 orbitals. These hybrid orbitals allow the formation of four identical C-H sigma (??) bonds, accounting for methane's observed structure and bond properties
- https://chem.libretexts.org/Courses/Nassau_Community_College/CHE200_-_Introduction_to_Organic_Chemistry_(Resch)/02%3A_Introduction_to_Organic_Structure_and_Bonding_II/2.02%3A_Valence_Bond_TheoryValence bond theory is most often used to describe bonding in organic molecules. In this model, bonds are considered to form from the overlap of two atomic orbitals on different atoms, each orbital c...Valence bond theory is most often used to describe bonding in organic molecules. In this model, bonds are considered to form from the overlap of two atomic orbitals on different atoms, each orbital containing a single electron. In looking at simple inorganic molecules such as molecular hydrogen (H2) or hydrogen fluoride (HF), our present understanding of s and p atomic orbitals will suffice. In order to explain the bonding in organic molecules, however, we will need to introduce hybrid orbitals
- https://chem.libretexts.org/Courses/East_Tennessee_State_University/CHEM_3110%3A_Descriptive_Inorganic_Chemistry/03%3A_Bonding_TheoriesThis chapter discusses the different theories which can be used to describe bonding in molecules. Some of these theories should be familiar from general or organic chemistry and some may be new to you...This chapter discusses the different theories which can be used to describe bonding in molecules. Some of these theories should be familiar from general or organic chemistry and some may be new to you this semester. Not every theory is applicable in every situation so, so we will look at cases where these theories are successful and cases where they fail (can't explain or reproduce experimental observations). Apply Lewis and VSEPR theories to determine molecular geometry and bond angles
- https://chem.libretexts.org/Courses/Oregon_Institute_of_Technology/OIT%3A_CHE_331_-_Organic_Chemistry_(Lund)/01%3A_General_Chemistry_Recap/1.02%3A_Valence_Bond_TheoryValence bond theory is most often used to describe bonding in organic molecules. In this model, bonds are considered to form from the overlap of two atomic orbitals on different atoms, each orbital c...Valence bond theory is most often used to describe bonding in organic molecules. In this model, bonds are considered to form from the overlap of two atomic orbitals on different atoms, each orbital containing a single electron. In looking at simple inorganic molecules such as molecular hydrogen (H2) or hydrogen fluoride (HF), our present understanding of s and p atomic orbitals will suffice. In order to explain the bonding in organic molecules, however, we will need to introduce hybrid orbitals
- https://chem.libretexts.org/Courses/Smith_College/CHM_222_Chemistry_II%3A_Organic_Chemistry_(2025)/01%3A_Structure_and_Bonding/1.07%3A_sp_Hybrid_Orbitals_and_the_Structure_of_MethaneThe four identical C-H single bonds in methane form as the result of sigma bond overlap between the sp3 hybrid orbitals of carbon and the s orbital of each hydrogen.
