Question

Citric acid is a naturally occurring compound. what orbitals are used to form each indicated bond? be sure to answer all parts.2xsafari

Answer 1

Answer : The orbitals that are used to form each indicated bond in citric acid is given below as per the attachment.

Answer 1) σ Bond a : C has
`SP^(2)` O has
`SP^(2)` .

Explanation : The orbitals of oxygen and carbon which are involved in
`SP^(2)` hybridization to form sigma bonds. This is observed at 'a' position in the citric acid molecule.

Answer 2) π Bond a: C has π orbitals and O also has π orbitals.

Explanation : The pi-bond at the 'a'position has carbon and oxygen atoms which undergoes pi-bond formation. And has pi orbitals of oxygen and carbon involved in the bonding process.

Answer 3) Bond b: O
`SP^(3)` H has only S orbital involved in bonding.

Explanation : The bonding at 'b' position involves oxygen
`SP^(3)` hydrogen atoms in it. It has
`SP^(3)` hybridized orbitals and S orbital of hydrogen involved in the bonding.

Answer 4) Bond c: C is
`SP^(3)` O is also
`SP^(3)`

Explanation : The bonding involved at 'c' position has carbon and oxygen atoms involved in it. Both the atoms involves the orbitals of
`SP^(3)` hybridized bonds.

Answer 5) Bond d: C atom has
`SP^(3)` C atom has
`SP^(3)`

Explanation : At the position of 'd' the bonding between two carbon atoms is found to be
`SP^(3)`. Therefore, the orbitals that undergo
`SP^(3)` hybridization are
`SP^(3)`.

Answer 6) Bond e : C1 containing O
`SP^(2)`

C2 is
`SP^(3)`

Explanation : The carbon atom which contains oxygen along with a double bond has
`SP^(2)` hybridized orbitals involved in the bonding process; whereas the carbon at C2 has
`SP^(3)` hybridized orbitals involved during the bonding. This is for the 'e' position.