A LITTLE LIGHTBULB MOMENT
Bonding, functional groups and nomenclature
Bond polarity follows electronegativity differences
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The stronger pull shifts electron density toward one atom.
The idea behind the cue
Covalent bonds are polarized when atoms differ in electronegativity, creating partial charges and bond dipoles. More electronegative atoms pull electron density toward themselves. The dipole points toward the negative end in chemistry convention, and bond polarity influences solubility and reactivity patterns.
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Short & simple
The stronger pull shifts electron density toward one atom.
Acronym
EDP — Exhausted Donuts Pout.
Story
On a tug-of-war rope, the kid with the bigger gloves drags the center line off-center. In a bond, the more electronegative atom pulls shared electrons closer and becomes partially negative.
Connect the pieces
- E (Exhausted) → Electronegativity: The atom with higher electronegativity pulls shared electrons toward itself.
- D (Donuts) → Dipole: A polar bond has a dipole that points toward the negative end in chemistry convention.
- P (Pout) → Partial charges: Unequal sharing creates delta-plus and delta-minus regions that affect solubility and reactivity.
- Exhausted · Electronegativity: The atom with higher electronegativity pulls shared electrons toward itself.
- Donuts · Dipole: A polar bond has a dipole that points toward the negative end in chemistry convention.
- Pout · Partial charges: Unequal sharing creates delta-plus and delta-minus regions that affect solubility and reactivity.
Know the limits
A symmetric molecule can contain polar bonds yet have little or no net molecular dipole because the bond dipoles cancel.
Further reading · OpenStax Organic Chemistry ↗Check your understanding
Which bond is expected to be the most polar?
A. C–C
B. C–H
C. C–O
D. O–O
Reveal explanation
C–O
Oxygen is significantly more electronegative than carbon or hydrogen, so a C–O bond is more polarized than the others listed.