A valid Lewis structure for the molecule PH₃ is shown in the image attached.
Lewis structure of phosphine
The Lewis structure of phosphine shows three hydrogen atoms bound to phosphorus at the center. Every hydrogen atom and every phosphorus atom has its octet completed when valence electrons are dispersed to form single bonds.
The lone pair on phosphorus causes the resulting structure to have a pyramidal shape. Since there are no formal charges, the molecule is stable. Common uses for phosphorus include the production of semiconductors and as a reducing agent in chemical processes.