Can gas to solid be called …

The reverse process of sublimation is <a href="https://en.wikipedia.org/wiki/Deposition_(phase_transition)" title="Deposition (phase transition)">deposition</a> or desublimation, in which a substance passes directly from a gas to a solid phase. Sublimation has also been used as a generic term to describe a solid-to-gas transition (sublimation) followed by a gas-to-solid transition (<a href="https://en.wikipedia.org/wiki/Deposition_(phase_transition)" title="Deposition (phase transition)">deposition</a>).

 While a transition from liquid to gas is described as <a href="https://en.wikipedia.org/wiki/Evaporation" title="Evaporation">evaporation</a> if it occurs below the boiling point of the liquid, and as <a href="https://en.wikipedia.org/wiki/Boiling" title="Boiling">boiling</a> if it occurs at the boiling point, there is no such distinction within the solid-to-gas transition, which is always described as sublimation.

The term <i>sublimation</i> refers to a <a href="https://en.wikipedia.org/wiki/Physical_change" title="Physical change">physical change</a> of <a href="https://en.wikipedia.org/wiki/State_of_matter" title="State of matter">state</a> and is not used to describe the transformation of a solid to a gas in a chemical reaction. For example, the dissociation on heating of solid <a href="https://en.wikipedia.org/wiki/Ammonium_chloride" title="Ammonium chloride">ammonium chloride</a> into hydrogen chloride and ammonia is <i>not</i> sublimation but a chemical reaction. Similarly the combustion of candles, containing <a href="https://en.wikipedia.org/wiki/Paraffin_wax" title="Paraffin wax">paraffin wax</a>, to <a href="https://en.wikipedia.org/wiki/Carbon_dioxide" title="Carbon dioxide">carbon dioxide</a> and <a href="https://en.wikipedia.org/wiki/Water_vapor" title="Water vapor">water vapor</a> is <i>not</i> sublimation but a chemical reaction with oxygen.

Sublimation is caused by the absorption of heat which provides enough energy for some molecules to overcome the <a href="https://en.wikipedia.org/wiki/Intermolecular_force" title="Intermolecular force">attractive forces</a> of their neighbors and escape into the vapor phase. Since the process requires additional energy, it is an <a href="https://en.wikipedia.org/wiki/Endothermic" title="Endothermic">endothermic</a> change.