Sodium is highly soluble in water, forming sodium hydroxide (NaOH) and hydrogen gas (H2). It also dissolves in other solvents like ammonia and ethanol, but to a lesser extent. The solubility of sodium in water is influenced by temperature, with higher temperatures generally increasing solubility. For instance, at 20°C, sodium has a solubility of approximately 40 grams per 100 milliliters of water. This high solubility in water is due to the strong ionic bond between sodium and the oxygen atom in water molecules, which breaks down the sodium chloride lattice structure, allowing the sodium ions to be surrounded by water molecules.

The high solubility of sodium in water is a result of the strong electrostatic attraction between the sodium cation (Na+) and the oxygen atom in the water molecule (H2O). Water is a polar molecule, meaning it has a partial positive charge on the hydrogen atoms and a partial negative charge on the oxygen atom. This polarity allows water molecules to surround and stabilize the sodium cation, effectively dissolving the sodium. The process can be represented by the following equation:

Na(s) + H2O(l) → NaOH(aq) + 1/2 H2(g)

This reaction is exothermic, releasing heat as the sodium dissolves. The solubility of sodium in water also increases with temperature due to the increased kinetic energy of the water molecules, which allows them to more effectively break apart the sodium chloride lattice structure.

In addition to water, sodium can dissolve in other solvents, such as ammonia (NH3) and ethanol (C2H5OH). In ammonia, sodium forms sodium amide (NaNH2), while in ethanol, it forms sodium ethoxide (C2H5ONa). The solubility of sodium in these solvents is lower than in water, but it is still significant. The solubility of sodium in ammonia at 25°C is approximately 40 grams per 100 milliliters, and in ethanol, it is around 30 grams per 100 milliliters.

The solubility of sodium in these solvents is also influenced by the strength of the ionic bond between sodium and the solvent molecules. In ammonia, the lone pairs of electrons on the nitrogen atom can form coordinate bonds with the sodium cation, stabilizing it and allowing for dissolution. Similarly, in ethanol, the oxygen atom can also form coordinate bonds with the sodium cation. However, the strength of these bonds is generally weaker than the ionic bond between sodium and water, resulting in lower solubility.

In conclusion, sodium is highly soluble in water due to the strong ionic bond between sodium and the oxygen atom in water molecules. It also dissolves in other solvents like ammonia and ethanol, although to a lesser extent. The solubility of sodium in these solvents is influenced by the strength of the ionic bond and the ability of the solvent molecules to stabilize the sodium cation.