A micelle has its hydrophobic ends directed:

To understand the structure of a micelle, we need to look at the properties of surfactant or soap molecules. These molecules are amphiphilic, meaning they contain two distinct regions:
1. A hydrophilic (water-loving) polar head group.
2. A hydrophobic (water-fearing) non-polar hydrocarbon tail.

When these molecules are dispersed in an aqueous (water-based) medium at or above the critical micelle concentration (CMC), they self-assemble to minimize free energy.

Since water is a highly polar solvent, the hydrophobic hydrocarbon tails experience unfavorable interactions with water molecules (the hydrophobic effect). To minimize these contact areas, the hydrophobic ends orient themselves inward, pointing towards the center of the aggregate structure, completely shielded from the surrounding water.

Meanwhile, the hydrophilic polar heads point outwards, facing the water molecules, where they can form favorable electrostatic interactions and hydrogen bonds. This spherical or cylindrical aggregate is called a micelle.

Therefore, in a micelle, the hydrophobic ends are directed towards the center, away from the water.