in the image below, which of the following correctly indicates shared electrons would be on the bold bonds and correctly labels the partial charges of the atoms involved in the bonds? chemical structure and options as shown in the image

Question

Accepted Answer

To solve this, we analyze electronegativity and partial charges:

1. **Nitrogen (N) in $ \boldsymbol{C-N} $ bond**: N is more electronegative than C, so shared electrons (dots) should be closer to N ($ \delta^- $ on N, $ \delta^+ $ on C? Wait, no—wait, the $ C-N $ bond: N is more electronegative, so N has $ \delta^- $, C has $ \delta^+ $? Wait, no, in the options, let's check the bold bonds (C-N, and the O bonds in the carboxyl/hydroxyl).

2. **Oxygen (O) in $ \boldsymbol{C=O} $ and $ \boldsymbol{O-H} $ bonds**: O is highly electronegative, so shared electrons (dots) are closer to O ($ \delta^- $ on O, $ \delta^+ $ on H in O-H, $ \delta^+ $ on C in C=O).

3. **Analyzing options**:
   - The correct option must show:
     - For $ C-N $: Shared electrons (dots) closer to N (since N > C in electronegativity, N is $ \delta^- $, C is $ \delta^+ $? Wait, no—wait, in the first part (left molecule: $ H_3C-NH_2 $), the $ C-N $ bond: N is more electronegative, so shared electrons (the bond’s electrons) are pulled toward N. So N should have $ \delta^- $, C $ \delta^+ $? Wait, no—wait, $ CH_3NH_2 $: C is $ \delta^+ $, N is $ \delta^- $ (since N is more electronegative). Then, in the right molecule (carboxylic acid-like), O in $ C=O $ and $ O-H $ is $ \delta^- $, H in $ O-H $ is $ \delta^+ $, C in $ C=O $ is $ \delta^+ $.

- The third option (middle one) has incorrect partial charges? Wait, no—let’s re-express:

The correct option is the one where:
   - $ C-N $ bond: Shared electrons (dots) near N (N is $ \delta^- $, C $ \delta^+ $? Wait, no, in the options, the first option has $ \delta^+ $ on N? No, that’s wrong. Wait, no—wait, N in $ NH_2 $ has lone pairs, and the $ C-N $ bond: N is more electronegative, so N should be $ \delta^- $, C $ \delta^+ $. Then, in the right molecule, O in $ C=O $ and $ O-H $ is $ \delta^- $, H in $ O-H $ is $ \delta^+ $, C in $ C=O $ is $ \delta^+ $.

Wait, the third option (middle) shows N with dots (shared electrons) but partial charges? No, let's check the last option: Wait, the correct answer is the third option? No, wait, let's think again.

Wait, the key is:
   - In $ C-N $ bond: N is more electronegative, so shared electrons (the bond’s electrons) are closer to N (so N has $ \delta^- $, C $ \delta^+ $).
   - In $ O-H $ bond: O is more electronegative, so shared electrons closer to O ($ \delta^- $ on O, $ \delta^+ $ on H).
   - In $ C=O $ bond: O is more electronegative, so shared electrons closer to O ($ \delta^- $ on O, $ \delta^+ $ on C).

Looking at the options, the third option (middle) has:
   - $ C-N $: Shared electrons (dots) near N (correct, N is $ \delta^- $? Wait, no, the partial charges: in the third option, N has no $ \delta $, but O has $ \delta^- $, H has $ \delta^+ $, C has $ \delta^+ $. Wait, no—maybe the correct option is the third one? Wait, no, let's check the first option: it has $ \delta^+ $ on N, which is wrong (N should be $ \delta^- $ relative to C). The last option: N is $ \delta^- $, H on N is $ \delta^+ $ (correct, since N is more electronegative than H), O is $ \delta^- $, H on O is $ \delta^+ $, C in $ C=O $ is $ \delta^+ $. Wait, the last option’s partial charges: N is $ \delta^- $, H on N is $ \delta^+ $; O is $ \delta^- $, H on O is $ \delta^+ $; C in $ C=O $ is $ \delta^+ $. And shared electrons (dots) are near N (C-N bond) and near O (C=O and O-H bonds). That matches.

Wait, the last option (bottom) has:
   - $ C-N $: N is $ \delta^- $, C $ \delta^+ $ (dots near N).
   - $ O-H $: O $ \delta^- $, H $ \delta^+ $ (dots near O).
   - $ C=O $: O $ \delta^- $, C $ \delta^+ $ (dots near O).

Yes, that’s correct. So the correct option is the last one (bottom) with $ \delta^- $ on N, $ \delta^+ $ on H (N-H), $ \delta^- $ on O, $ \delta^+ $ on H (O-H), and $ \delta^+ $ on C (C=O), with shared electrons (dots) near N (C-N) and near O (C=O, O-H).

# Brief Explanations:
To determine the correct option, we analyze electronegativity and partial charges:
1. **$ \boldsymbol{C-N} $ bond**: Nitrogen (N) is more electronegative than carbon (C), so shared electrons (dots) are closer to N (N has $ \boldsymbol{\delta^-} $, C has $ \boldsymbol{\delta^+} $).
2. **$ \boldsymbol{O-H} $ and $ \boldsymbol{C=O} $ bonds**: Oxygen (O) is more electronegative than hydrogen (H) and carbon (C), so shared electrons (dots) are closer to O (O has $ \boldsymbol{\delta^-} $, H (in $ O-H $) and C (in $ C=O $) have $ \boldsymbol{\delta^+} $).

The last option (bottom) correctly shows:
- Shared electrons near N (C-N) and O (C=O, O-H).
- Partial charges: $ \delta^- $ on N, $ \delta^+ $ on H (N-H); $ \delta^- $ on O, $ \delta^+ $ on H (O-H); $ \delta^+ $ on C (C=O).

# Answer:
The correct option is the bottom - most choice (with $ \delta^- $ on N, $ \delta^+ $ on H - N, $ \delta^- $ on O, $ \delta^+ $ on H - O, and $ \delta^+ $ on C in $ C = O $, with shared electrons near N and O).

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