CHEM10003 Lecture Notes - Lecture 1: Sigma Bond, Covalent Bond, Isobutane

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rosedog575

8 Aug 2018

School

University of Melbourne

Department

Chemistry

Course

CHEM10003

Professor

Mark Rizzacasa

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Document Summary

Structure of methane, carbon forms 4 covalent bonds, 4 orbitals with electron in each orbital and each are required to overlap to form the 2 electron for covalent sigma bonds that are required in the molecule methane. All the bonds in methane are the same length and energy. C in ground state is not like that! (electrons are in diff orbitals of diff energies) and carbon in the ground state is not gonna form a ch4 molecule. Cannot 4 hydrogen s orbitals with single electrons with the 4 orbitals because that would make very unstable bonds and we"re going forward to minimize energy (unstable bonds. Hybridisation (combine the 4 orbitals 2s + 2px + 2py + 2pz) = 1 s x 3 p = 4 sp3 orbitals (contains characteristics of both s and p). Hybridisation = a theory to help explain why carbon form 4 covalent bonds. Sigma carbon-carbon bond = bond that holds most organic molecules.

Related Questions

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.

Attached is picture. Please explain/show work, will give 5 stars to correct answer, thank you very much! :)

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.

Answer True or false for the following questions.

1) There are eleven Ï bonds in this molecule?

2) There are three lone pairs of electrons in the complete Lewisstructure?

3) The C-N bond is formed from overlap of an sp3 hybrid orbitalfrom the carbon atom with an sp2 hybrid orbital from the nitrogenatom?

4) An sp2 hybrid orbital on C-1 overlaps with an sp3 hybrid orbitalon C-2 to form the sigma bond between C-1 and C-2?

5) There are four Ï bonds in this molecule?

6)The C-2 and C-3 atoms cannot rotate about the internuclear axisbetween the two atoms since the Ï bond would break?

7) The Ï bond between C-3 and O is formed by overlap ofunhybridized p atomic orbitals?

please help me...it should be finished within 1 hour. I cannotdo this. thanks.

CHEM10003 Lecture Notes - Lecture 1: Sigma Bond, Covalent Bond, Isobutane

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