* Low electron density: Hydrogen atoms only have one electron each, and these electrons are tightly bound to the nucleus. This means there are very few free electrons available to carry an electric current.

* No free electrons: In its gaseous state, hydrogen exists as individual molecules (H2), not as a free electron gas.

However, liquid hydrogen can be conductive, especially under high pressure. The increased pressure forces the hydrogen molecules closer together, increasing the likelihood of electron transfer and improving conductivity.

Furthermore, metallic hydrogen, a hypothetical state of hydrogen under extremely high pressure, is predicted to be a superconductor, with zero electrical resistance.

So, the conductivity of hydrogen depends on its state:

* Gaseous hydrogen: Poor conductor

* Liquid hydrogen: Conductor (under high pressure)

* Metallic hydrogen: Superconductor (hypothetical)