A central atom in a molecule has two lone pairs of electrons and forms three single bonds. The shape of this molecule is:

The central atom has 2 lone pairs and forms 3 single bonds, giving a total of $$2 + 3 = 5$$ electron pairs around it. According to VSEPR theory, 5 electron pairs arrange themselves in a trigonal bipyramidal geometry to minimize repulsion.

In a trigonal bipyramidal arrangement, lone pairs preferentially occupy the equatorial positions because these positions have more space (only two 90-degree interactions with axial positions, compared to three 90-degree interactions if placed axially). With 2 lone pairs in equatorial positions, the 3 bonding pairs occupy the remaining positions: 1 equatorial and 2 axial.

This gives a T-shaped molecular geometry, where the three bonded atoms form a shape resembling the letter T. A classic example of this geometry is $$ClF_3$$.

Therefore, the shape of the molecule is T-shaped, which is option (C).