Question

which of the following compounds has an overall molecular dipole moment (even a small one)? select all that apply however marks will be deducted for incorrect answers. select one or more: chf₃ cf₄ co₂ bh₃ hcl co

Explanation:

To determine if a molecule has a molecular dipole moment, we analyze its molecular geometry and polarity of bonds:

• \( \text{CHF}_3 \): Tetrahedral geometry. The \( \text{C-H} \) and \( \text{C-F} \) bonds have different electronegativities. The dipole moments of \( \text{C-F} \) bonds do not cancel the \( \text{C-H} \) dipole, so there is a net dipole.
• \( \text{CF}_4 \): Tetrahedral, symmetric. All \( \text{C-F} \) bonds are identical, so dipole moments cancel (non - polar).
• \( \text{CO}_2 \): Linear, symmetric (\( \text{O}=\text{C}=\text{O} \)). Bond dipoles cancel (non - polar).
• \( \text{BH}_3 \): Trigonal planar, symmetric. Bond dipoles cancel (non - polar).
• \( \text{HCl} \): Diatomic, polar bond (\( \text{H - Cl} \)), so there is a net dipole.
• \( \text{CO} \): Diatomic, polar bond (\( \text{C - O} \)), so there is a net dipole.

Answer:

\( \text{CHF}_3 \), \( \text{HCl} \), \( \text{CO} \)