Examples of Polar Covalent Bonds

🧪 Quick Study Guide

• ⚛️ A polar covalent bond occurs when electrons are unequally shared between atoms in a molecule.
• ⚡ This unequal sharing arises from differences in electronegativity between the bonded atoms.
• 📈 Electronegativity is the measure of an atom's ability to attract electrons in a chemical bond.
• 💧 Common examples include water ($H_2O$) and hydrogen fluoride ($HF$).
• ➕ The atom with higher electronegativity gains a partial negative charge ($\delta^-$), while the other atom gains a partial positive charge ($\delta^+$).
• 📐 The greater the difference in electronegativity, the more polar the bond.
• ⚖️ Dipole moment ($\mu$) is used to quantify the polarity of a bond, given by $\mu = q \times d$, where $q$ is the magnitude of the charge and $d$ is the distance between the charges.

Practice Quiz

1. Which of the following molecules contains a polar covalent bond?
   1. $O_2$
   2. $CH_4$
   3. $NaCl$
   4. $HCl$
2. What causes a polar covalent bond to form?
   1. Equal sharing of electrons
   2. A large difference in electronegativity between the bonded atoms
   3. Identical electronegativity values
   4. Formation of ions
3. In a molecule of water ($H_2O$), which atom has a partial negative charge?
   1. Hydrogen
   2. Oxygen
   3. Both hydrogen and oxygen have equal negative charges
   4. Neither hydrogen nor oxygen
4. Which of the following bonds is the MOST polar?
   1. C-H
   2. N-H
   3. O-H
   4. F-H
5. What is the symbol used to represent a partial charge in a polar covalent bond?
   1. +
   2. -
   3. $\delta$
   4. $\pm$
6. Which molecule is NOT an example of a polar covalent compound?
   1. $NH_3$
   2. $H_2S$
   3. $CO_2$
   4. $Cl_2$
7. The dipole moment is a measure of:
   1. Bond length
   2. Bond energy
   3. Bond polarity
   4. Bond angle