CHE 106 Lecture Notes - Lecture 35: Sigma Bond, Pi Bond, Vsepr Theory

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14 Nov 2018

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CHE 106 Lecture Notes - Lecture 34: Valence Bond Theory, Covalent Bond, Vsepr Theory

CHE 106 Lecture Notes - Lecture 35: Sigma Bond, Pi Bond, Vsepr Theory

CHE 106 Lecture 36: CHE 106 Notes Lecture 32 (36)

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Vsepr: number of bonds formed by an atom=unpaired electrons, exception: carbon (2 unpaired electrons, form 4 bonds) Hybrid orbitals: form by mixing of atomic orbitals to create new orbitals of equal energy, called degenerate orbitals; process called hybridization: number of hybrid orbitals=sum of atomic orbitals. Hybridization: s3 geometric arrangement of hybrid orbitals same as vsepr theory sigma bond: head-to-head overlap of orbitals, cylindrical symmetry about internucleus axis pi bond: side-to-side overlap, electron density above and below internucleus axis, weaker bond.

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Benzene is an organic chemical compound with the molecular formula C6H6. In the benzene molecule, carbon atoms form a ring with alternating single and double bonds connecting them. Thus, each individual carbon atom forms one ? bond with another carbon atom and one ? and one ? bond with another carbon atom. Each carbon atom also forms one ? bond with a hydrogen atom. Identify which types of orbitals overlap to form the bonds between the atoms in a benzene molecule. Drag the appropriate labels to their respective targets.

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Chemical bonds are formed by linear combinations of atomic orbital's. These atomic orbital's should have compatible energies. An axial overlap of these orbitals results in the formation of a sigma bond, whereas a lateral overlap results in the formation of a pi bond. When two atomic orbitai's on different atoms approach each other, two molecular orbital's are formed: one bonding molecular orbital and one antibonding molecular orbital. The bonding molecular orbital has a lower energy than the corresponding atomic orbital's: antibonding orbital's have higher energies than the corresponding atomic orbital's. An example using the hydrogen molecule is shown here. However, the same rule applies to systems with multiple atomic orbital's. For each atomic orbital that overlaps, one molecular orbital must form. In the diagram below. 1s orbitais from two hydrogen atoms combine to form one bonding sigma1 orbital and one antibonding orbital. The total number of bonding and antibonding orbital's is always equal to the number of orbital's that overlap. Similarly, molecular orbital's can also be formed by the overlapping of hybrid orbital's. The hybrid orbital's are formed by the linear combination of different atomic orbital's of nearly equal energy on the same atom. The atomic orbital's of nearly equal energy undergo a process of mixing and reorientation to form new orbital's of lower energy. This process is called hybridization For example, hybridization of one s and two p orbital's on an atom forms three sp2 hybrid orbital's. Benzene is an organic chemical compound with the molecular formula C6H6. In the benzene molecule, carbon atoms form a ring with alternating single and double bonds connecting them. Thus, each individual carbon atom forms one sigma bond with another carbon atom and one sigma and one pi bond with another carbon atom. Each carbon atom also forms one sigma bond with a hydrogen atom. Identify which types of orbital's overlap to form the bonds between the atoms in a benzene molecule.

CHE 106 Lecture Notes - Lecture 35: Sigma Bond, Pi Bond, Vsepr Theory

CHE 106 Lecture Notes - Lecture 34: Valence Bond Theory, Covalent Bond, Vsepr Theory

CHE 106 Lecture Notes - Lecture 35: Sigma Bond, Pi Bond, Vsepr Theory

CHE 106 Lecture 36: CHE 106 Notes Lecture 32 (36)

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