Deposition of salt from evaporated water

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When a saturated solution of NaCl evaporates on a flat surface, the salt tends to concentrate at the outer edges rather than forming a uniform distribution. This phenomenon is attributed to temperature variations across the surface during evaporation, which can affect the rate of water loss. Additionally, the movement of water is more pronounced in shallower areas, leading to higher salt concentration at the edges. The combination of these factors results in the observed pattern of salt deposition. Understanding these dynamics can provide insights into evaporation processes and crystallization patterns.
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When a small volume, say 5ml, of saturated solution of NaCl is left on a flat surface and evaporates, why does the salt always become concentrated on the outer edge of the base where the solution was? Why doesn't it form a uniform distribution of salt throughout the entire area which the solution previously took?
 
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It could be something to do with the temperature distribution over the surface (due to evaporation) or the rate of water movement where the liquid is more shallow - the outside edge being a bit more concentrated..
 

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