All molecules with polar bonds have dipole moment.

Explanation

To determine whether the statement "All molecules with polar bonds have dipole moment" is true or false, we can analyze the concept of polar bonds and dipole moments step by step.

### Step-by-Step Solution:

1. **Understanding Polar Bonds**:
- A polar bond occurs when there is a difference in electronegativity between the two atoms involved in the bond. This difference causes a partial positive charge (δ+) on one atom and a partial negative charge (δ-) on the other atom.

2. **Definition of Dipole Moment**:
- The dipole moment is a vector quantity that measures the separation of positive and negative charges in a molecule. It is represented by the formula:
\[ \text{Dipole Moment} (\mu) = q \times d \]
where \( q \) is the charge and \( d \) is the distance between the charges.

3. **Analyzing Molecular Geometry**:
- The overall dipole moment of a molecule is not only dependent on the presence of polar bonds but also on the molecular geometry. The shape of the molecule can lead to the cancellation of dipole moments.

4. **Example of CCl₄**:
- Consider the molecule carbon tetrachloride (CCl₄). Each C-Cl bond is polar due to the difference in electronegativity between carbon and chlorine.
- However, CCl₄ has a tetrahedral geometry. The dipole moments of the four C-Cl bonds are equal in magnitude but oriented in such a way that they cancel each other out.

5. **Conclusion**:
- Although CCl₄ has polar bonds, the overall dipole moment of the molecule is zero due to the symmetrical arrangement of the bonds. Therefore, not all molecules with polar bonds have a net dipole moment.

6. **Final Answer**:
- The statement "All molecules with polar bonds have dipole moment" is **false**.