객관식
Which of the following best represents the overall molecular dipole moment of a water (H_2O) molecule using a vector arrow?
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11. Bonding & Molecular Structure
Dipole Moment
객관식
Which of the following correctly shows the direction of polarity and partial charges for the H–Cl bond?
A
H^{\(\text{δ-}\)}–Cl^{\(\text{δ-}\)}
B
H^{\(\text{δ-}\)}–Cl^{\(\text{δ+}\)}
C
H^{\(\text{δ+}\)}–Cl^{\(\text{δ+}\)}
D
H^{\(\text{δ+}\)}–Cl^{\(\text{δ-}\)}
검증된 단계별 안내1
Step 1: Understand that polarity in a bond arises due to differences in electronegativity between the two atoms involved. Electronegativity is the tendency of an atom to attract shared electrons in a chemical bond.
Step 2: Identify the electronegativities of hydrogen (H) and chlorine (Cl). Chlorine is more electronegative than hydrogen, meaning it attracts the bonding electrons more strongly.
Step 3: Because chlorine attracts electrons more strongly, the shared electron pair in the H–Cl bond will be closer to chlorine, creating a partial negative charge (δ-) on Cl and a partial positive charge (δ+) on H.
Step 4: Represent the polarity direction with an arrow pointing from the less electronegative atom (H) to the more electronegative atom (Cl), indicating the shift of electron density.
Step 5: Conclude that the correct representation of the bond polarity is \(\mathrm{H^{\delta+} - Cl^{\delta-}}\), showing hydrogen with a partial positive charge and chlorine with a partial negative charge.
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