The structure of OF₂ (oxygen difluoride) is bent or V-shaped, not linear, due to the following reasons:

1. Electronegativity: Oxygen is more electronegative than fluorine. This means that the oxygen atom attracts the shared electrons in the O-F bonds more strongly, resulting in a partial negative charge on oxygen and a partial positive charge on the fluorine atoms.

2. Lone Pairs: Oxygen has two lone pairs of electrons in its valence shell. These lone pairs exert a strong repulsive force on the bonding pairs of electrons in the O-F bonds.

3. VSEPR Theory: According to the Valence Shell Electron Pair Repulsion (VSEPR) theory, electron pairs, both bonding and non-bonding, try to minimize repulsion by positioning themselves as far apart as possible. In the case of OF₂, the optimal arrangement to minimize repulsion is a bent shape with a bond angle of approximately 103.3 degrees.

Therefore, the combination of oxygen's electronegativity and the presence of lone pairs on oxygen leads to the bent shape of OF₂, rather than a linear structure.