Question

agrocybin is isolated from edible mushrooms and is reported to be an antifungal molecule. predict the indicated bond angles in agrocy... molecular structure: ho - c (with h, h, and (1), (2) arrows) - c≡c - c (with (3) arrow) ≡c - c≡c - c (with (4) arrow) =o - nh₂. below: (1) select dropdown, (2) select dropdown, (3) select dropdown, (4) select dropdown, with reset and close buttons.

Explanation:

To solve for the bond angles in the agrocybin molecule, we analyze the hybridization of each carbon atom (or relevant atom) at each labeled position:

(1) Bond Angle Analysis

The first carbon (attached to \( \text{HO} \), \( \text{H} \), \( \text{H} \), and a triple - bonded carbon) has \( \boldsymbol{sp^3} \) hybridization (four electron groups: single bonds to \( \text{O} \), \( \text{H} \), \( \text{H} \), and a \( \sigma \) - bond to the adjacent carbon). For \( sp^3 \) hybridization, the electron - group geometry is tetrahedral, and the bond angle is approximately \( \boldsymbol{109.5^\circ} \).

(2) Bond Angle Analysis

The second carbon (part of the \( \text{C}\equiv\text{C} \) triple bond and bonded to the \( sp^3 \) carbon and a triple - bonded carbon) has \( \boldsymbol{sp} \) hybridization (two electron groups: a \( \sigma \) - bond to the \( sp^3 \) carbon and a \( \sigma \) - bond to the triple - bonded carbon, plus two \( \pi \) - bonds in the triple bond). For \( sp \) hybridization, the electron - group geometry is linear, and the bond angle is approximately \( \boldsymbol{180^\circ} \).

(3) Bond Angle Analysis

The third carbon (part of the \( \text{C}\equiv\text{C} \) triple bond, bonded between two triple - bonded carbons) has \( \boldsymbol{sp} \) hybridization (two electron groups: \( \sigma \) - bonds to the adjacent triple - bonded carbons, plus two \( \pi \) - bonds in each triple bond). For \( sp \) hybridization, the electron - group geometry is linear, and the bond angle is approximately \( \boldsymbol{180^\circ} \).

(4) Bond Angle Analysis

The fourth carbon (double - bonded to \( \text{O} \) and single - bonded to a triple - bonded carbon and \( \text{NH}_2 \)) has \( \boldsymbol{sp^2} \) hybridization (three electron groups: a \( \sigma \) - bond to the triple - bonded carbon, a \( \sigma \) - bond to \( \text{NH}_2 \), and a \( \pi \) - bond in the \( \text{C}=\text{O} \) double bond). For \( sp^2 \) hybridization, the electron - group geometry is trigonal planar, and the bond angle is approximately \( \boldsymbol{120^\circ} \).

Answer:

s:
(1) \( 109.5^\circ \)
(2) \( 180^\circ \)
(3) \( 180^\circ \)
(4) \( 120^\circ \)