Why is steric strain most evident in cyclic molecules?

Steric strain is most evident in cyclic molecules because the ring structure prevents the groups from getting away from each other.

Steric strain is the increase in potential energy of a molecule due to repulsion between groups on non-neighbouring carbons.

Consider a non-cyclic molecule such as 1,3-dichloropropane. We could draw it as

Here, the electron clouds of the Cl atoms are close together, and they repel each other. But there is free rotation about the C-C σ bonds. The CH₂Cl groups can rotate to get the Cl atoms further apart.

This rotation is severely hindered when the C atoms are in a ring.

For example, a cyclohexane ring is most stable in a chair conformation.

If you had a cyclohexane with two groups in axial positions, you would get steric strain because these groups would be too close and they would repel each other.

The molecule below has steric strain from many 1,3-diaxial interactions.

Most of these can be relieved by flipping the cyclohexane chair. But then the Br would be axial and have its own 1,3-diaxial steric repulsions.