CH 232 Chapter Notes - Chapter 16: Hydrazine, Lithium Aluminium Hydride, Bromine

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plumtermite154

26 Apr 2018

School

University of Alabama

Department

Chemistry

Course

CH 232

Professor

Silas Blackstock

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Document Summary

Section 16. 1: structure and bonding: the functional group of an aldehyde is a carbonyl group bonded to a hydrogen atom and a carbon atom. In methanal (formaldehyde), the simplest aldehyde, the carbonyl group is bonded to two hydrogen atoms. For unsaturated aldehydes, the presence of a carbon-carbon double or triple bond is indicated by the infix -en- or -yn- Section 16. 3: physical properties: oxygen is more electronegative than carbon; therefore, a carbon-oxygen double bond is polar, with oxygen bearing a partial negative charge and carbon bearing a partial positive charge. In addition, the resonance structure emphasizes the reactivity of the carbonyl oxygen as a. If none of the starting materials are chiral, the nucleophile will approach the carbonyl from either side with equal probability, resulting in a carbonyl addition product that consists of a racemic mixture. Nucleophilic addition of a grignard reagent to the electrophilic carbonyl carbon atom gives a tetrahedral carbonyl addition compound: add a proton.

Related Questions

Which statement correctly correlates s or p bonding atoms and theirrespective bonding orbitals in formaldehyde?

A)The oxygen atom (with its 2s orbital) forms a s bond with one ofthe three sp2 hybrid orbitals of the carbon atom; the two hydrogenatoms (with their 1s orbitals) each form a s bond with one of thethree sp2 hybrid orbitals of the carbon atom.
B)The oxygen atom (with its 2p orbital) forms a p bond with one ofthe three sp2 hybrid orbitals of the carbon atom; the two hydrogenatoms (with their 1s orbitals) each form a s bond with one of thethree sp2 hybrid orbitals of the carbon atom.
C)The oxygen atom (with its 2p orbital) forms a p bond with the pzorbital of the carbon atom; the two hydrogen atoms (with their 1sorbitals) each form a s bond with one of the two sp2 hybridorbitals of the carbon atom.
D)The oxygen atom (with its 2p orbital) forms a s bond with one ofthe three sp2 hybrid orbitals of the carbon atom; the two hydrogenatoms (with their 1s orbitals) each form a s bond with one of thethree sp2 hybrid orbitals of the carbon atom. The oxygen atom alsoforms a p bond with carbon which involves the 2pz orbitals ofoxygen and carbon.

cyanweasel854

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.

CH 232 Chapter Notes - Chapter 16: Hydrazine, Lithium Aluminium Hydride, Bromine

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