Citric acid is a naturally occurring compound. what orbitals are used to form each indicated bond? be sure to answer all parts.2
xsafari
1 answer:
Response: Below are the orbitals responsible for each bond identified in citric acid per the attachment.
Response 1) σ Bond a: Carbon uses and Oxygen employs
.
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 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 and Oxygen is also
.
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 and the second carbon has
.
Clarification: In position 'd', the bond formed between carbon atoms is , utilizing orbitals that underwent
hybridization which are
.
Response 6) Bond e: C1 has O .
C2 has .
Clarification: The carbon that contains oxygen and a double bond utilizes hybridized orbitals; conversely, carbon at C2 employs
hybridized orbitals in this bonding at position 'e'.
You might be interested in
The answer is - 0.138 M. The buffer pH can be determined using the Henderson equation. Here, 
acts as a weak acid and 
serves as its corresponding conjugate base. The weak acid has two protons, while the base contains one. The equation can therefore be expressed in terms of protons transferred. Phosphoric acid can donate protons in three stages; the equation we’ve referenced pertains to the second stage, as the acid then has only two protons available and the base only one. Given the concentration of the acid as 0.10 M, we need to calculate the concentration of the base necessary to form a buffer with a pH of exactly 7.0. Substituting the values into the equation leads us to the solution. Cross-multiplying, we find that [base] = 1.38(0.10), yielding [base] = 0.138. Therefore, the concentration of the base needed for the buffer is 0.138 M.
Response:
The specific heat of the alloy
Clarification:
Weight of the alloy = 25 gm
Initial temperature = 100°c = 373 K
Weight of the water = 90 gm
Initial temperature of water = 25.32 °c = 298.32 K
Final temperature = 27.18 °c = 300.18 K
Using the energy balance equation,
Heat released by the alloy = Heat absorbed by the water
[[
-
] =
(
-
)
25 × × ( 373 - 300.18 ) = 90 × 4.2 (300.18 - 298.32)
This gives us the specific heat of the alloy.