Question

for the molecule below, choose the image that accurately does all of the following: • shows the pair of electrons shared between atoms • shows the electrons closest to the more electronegative atom or in the middle of the bond if the atoms are roughly equally electronegative (<0.5 difference) • correctly labels partial charges if there are any • places and asterisk next to any polar covalent bonds
o=c=o
three options with molecular structure images

Explanation:

1. Electronegativity: O (3.5) > C (2.5), so O is more electronegative. Shared electrons should be closer to O.
2. Partial Charges: C will have $\delta^+$, O will have $\delta^-$.
3. Polar Covalent Bonds: C=O bonds are polar (electronegativity difference > 0.5), so they get *.
4. Analyzing Options:

• First option: $\delta^+$ on O (wrong, O should be $\delta^-$), $\delta^-$ on C (wrong, C should be $\delta^+$). Eliminate.
• Second option: $\delta^-$ on O, $\delta^+$ on C (correct). Shared electrons closer to O (correct). * on C=O bonds (correct).
• Third option: $\delta^-$ on O, $\delta^+$ on C, but electron placement and bond labeling? Wait, no—wait, the second option has electrons closer to O, correct charges, and on polar bonds. Wait, no, let's recheck. Wait, the molecule is CO₂, linear, two C=O double bonds. Electronegativity of O > C, so in each C=O bond, electrons are closer to O. Partial charges: C is $\delta^+$, O is $\delta^-$. Polar covalent bonds (since 3.5 - 2.5 = 1.0 > 0.5), so each C=O bond gets .

Wait, the second option (middle one? Wait, the options: first option has $\delta^+$ on O, $\delta^-$ on C—wrong. Second option (the one with $\delta^-$ on O, $\delta^+$ on C, electrons closer to O, * on bonds) is correct? Wait, no, the first option in the radio buttons: let's parse the options.

Wait, the first option (top radio button) has $\delta^+$ on O, $\delta^-$ on C—incorrect. The second option (middle radio button) has $\delta^-$ on O, $\delta^+$ on C, electrons closer to O, on C=O bonds—correct. The third option: electrons are on C? No, should be closer to O. The fourth option: no charges, no . So the correct option is the second one (with $\delta^-$ on O, $\delta^+$ on C, electrons near O, on bonds). Wait, but let's check the labels. Wait, the first option (the one with $\delta^+$ on O, $\delta^-$ on C) is wrong. The second option (middle) has $\delta^-$ on O, $\delta^+$ on C, electrons closer to O, and on the C=O bonds. That matches: O is more electronegative (so $\delta^-$), C is $\delta^+$, shared electrons near O, and C=O is polar (so *).

Answer:

The second option (with $\delta^-$ on O, $\delta^+$ on C, electrons closer to O, and asterisks on the C=O bonds)