Question

question 31 of 60
for each molecule, specify the polarity of the bonds and the overall polarity of the molecule.
bonds
molecule
bonds
molecule
bonds
molecule

Explanation:

1. For $\text{BeCl}_2$:

• Bond polarity: Beryllium (Be) and chlorine (Cl) have different electronegativities, so $\text{Be-Cl}$ bonds are polar.
• Molecular polarity: The molecule has a linear, symmetrical geometry. The polar bond dipoles point in opposite directions and cancel each other out, making the overall molecule nonpolar.

1. For $\text{H}_2\text{O}$:

• Bond polarity: Hydrogen (H) and oxygen (O) have different electronegativities, so $\text{O-H}$ bonds are polar.
• Molecular polarity: The molecule has a bent, asymmetrical geometry. The polar bond dipoles do not cancel, creating a net molecular dipole, so the overall molecule is polar.

1. For $\text{O}_2$:

• Bond polarity: The bond is between two identical oxygen atoms, which have identical electronegativities, so the $\text{O=O}$ bond is nonpolar.
• Molecular polarity: The molecule is symmetrical, and with nonpolar bonds, there is no net dipole, so the overall molecule is nonpolar.

Answer:

1. $\text{BeCl}_2$

• bonds: Polar
• molecule: Nonpolar

1. $\text{H}_2\text{O}$

• bonds: Polar
• molecule: Polar

1. $\text{O}_2$

• bonds: Nonpolar
• molecule: Nonpolar