PRE MI UM ACT I VE- LE A RN IN G WO RK BOO K
Polarity, Dipoles & Intermolecular Forces
Chemistry Deep Dive
General Chemistry • Active-Learning Edition
How to use this workbook
1. Read the concept explanation. 2. Study the worked example. 3. Try the practice problems yourself.
4. Check your work against the Answer Key. 5. Revisit anything you missed.
, 1. Electronegativity
Electronegativity is the ability of an atom to attract electrons toward itself in a chemical bond, and it's a key
factor in determining the nature of the bonds atoms form.
● Key idea: a larger electronegativity difference between two atoms means more uneven electron sharing
→ a more polar bond.
● Trend: electronegativity increases up a group and to the right across a period. Fluorine (F) has the
highest electronegativity of any element.
✏ TRY IT YOURSELF
1. Which is more electronegative: oxygen or nitrogen? How do you know from periodic trends?
2. Rank these bonds from least to most polar: C–H, O–H, N–H (using electronegativity differences).
2. Polar Bonds & Dipoles
Term Definition
Forms when electrons are shared unequally between two atoms, creating a dipole
Polar Bond
moment.
The more electronegative atom becomes partially negative (δ⁻); the other becomes
δ⁻ / δ⁺
partially positive (δ⁺).
Points toward the more electronegative atom, showing the direction of electron
Dipole Arrow
density.
WORKED EXAMPLE — Identifying a Dipole
In the H–Cl bond, Cl is more electronegative than H.
The dipole is drawn H → Cl, and Cl carries the δ⁻ charge while H carries the δ⁺ charge.
✏ TRY IT YOURSELF
1. Draw the dipole arrow for the C–O bond. Which atom is δ⁻?
2. Is the bond between two identical atoms (e.g. Cl–Cl) polar or nonpolar? Why?
3. Molecular Polarity
A molecule is polar if it has a net dipole moment — meaning the individual bond dipoles don't cancel out.
3-Step Method to Determine Polarity
● Step 1 — Check if the bonds are polar at all. If no, the molecule is nonpolar.
● Step 2 — Determine the molecular shape using VSEPR theory.
● Step 3 — Check whether the dipoles cancel. If they cancel → nonpolar. If not → polar.
Polarity, Dipoles & Intermolecular Forces
Chemistry Deep Dive
General Chemistry • Active-Learning Edition
How to use this workbook
1. Read the concept explanation. 2. Study the worked example. 3. Try the practice problems yourself.
4. Check your work against the Answer Key. 5. Revisit anything you missed.
, 1. Electronegativity
Electronegativity is the ability of an atom to attract electrons toward itself in a chemical bond, and it's a key
factor in determining the nature of the bonds atoms form.
● Key idea: a larger electronegativity difference between two atoms means more uneven electron sharing
→ a more polar bond.
● Trend: electronegativity increases up a group and to the right across a period. Fluorine (F) has the
highest electronegativity of any element.
✏ TRY IT YOURSELF
1. Which is more electronegative: oxygen or nitrogen? How do you know from periodic trends?
2. Rank these bonds from least to most polar: C–H, O–H, N–H (using electronegativity differences).
2. Polar Bonds & Dipoles
Term Definition
Forms when electrons are shared unequally between two atoms, creating a dipole
Polar Bond
moment.
The more electronegative atom becomes partially negative (δ⁻); the other becomes
δ⁻ / δ⁺
partially positive (δ⁺).
Points toward the more electronegative atom, showing the direction of electron
Dipole Arrow
density.
WORKED EXAMPLE — Identifying a Dipole
In the H–Cl bond, Cl is more electronegative than H.
The dipole is drawn H → Cl, and Cl carries the δ⁻ charge while H carries the δ⁺ charge.
✏ TRY IT YOURSELF
1. Draw the dipole arrow for the C–O bond. Which atom is δ⁻?
2. Is the bond between two identical atoms (e.g. Cl–Cl) polar or nonpolar? Why?
3. Molecular Polarity
A molecule is polar if it has a net dipole moment — meaning the individual bond dipoles don't cancel out.
3-Step Method to Determine Polarity
● Step 1 — Check if the bonds are polar at all. If no, the molecule is nonpolar.
● Step 2 — Determine the molecular shape using VSEPR theory.
● Step 3 — Check whether the dipoles cancel. If they cancel → nonpolar. If not → polar.
