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

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DochEvi

10 days ago

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

xsafari

Chemistry

1 answer:

alisha [964] · Answer 1 · 2026-02-23T21:53:24+03:00

Response: Below are the orbitals responsible for each bond identified in citric acid per the attachment.

Response 1) σ Bond a: Carbon uses $SP^{2}$ and Oxygen employs $SP^{2}$ .

Clarification: The sigma bonds are formed through the hybrid orbitals of carbon and oxygen. This occurs at the 'a' location in the citric acid structure.

Response 2) π Bond a: Both Carbon and Oxygen have π orbitals.

Clarification: The π-bond at position 'a' consists of interactions between the π orbitals of carbon and oxygen.

Response 3) Bond b: Oxygen $SP^{3}$ and Hydrogen solely utilizes the S orbital.

Clarification: The bonding at position 'b' includes oxygen and hydrogen atoms, with hydrogen utilizing its S orbital.

Response 4) Bond c: Carbon is $SP^{3}$ and Oxygen is also $SP^{3}$ .

Clarification: The bonding process at position 'c' involves both carbon and oxygen atoms with their respective hybrid orbitals.

Response 5) Bond d: Carbon atom has $SP^{3}$ and the second carbon has $SP^{3}$ .

Clarification: In position 'd', the bond formed between carbon atoms is $SP^{3}$ , utilizing orbitals that underwent $SP^{3}$ hybridization which are $SP^{3}$ .

Response 6) Bond e: C1 has O $SP^{2}$ .

C2 has $SP^{3}$ .

Clarification: The carbon that contains oxygen and a double bond utilizes $SP^{2}$ hybridized orbitals; conversely, carbon at C2 employs $SP^{3}$ hybridized orbitals in this bonding at position 'e'.