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When a Group 1 metal, such as lithium, sodium, or potassium, reacts with water, the typical reaction produces a metal hydroxide and hydrogen gas. This reaction is characterized by the metal displacing hydrogen ions from water, leading to the formation of the corresponding metal hydroxide (for instance, sodium hydroxide from sodium) and the release of hydrogen gas.

This reaction is exothermic and often vigorous, with the hydrogen gas produced potentially igniting due to the heat of the reaction, especially with more reactive metals like potassium. The hydroxides of Group 1 metals are also soluble in water and strongly alkaline, a key characteristic of these compounds.

In contrast, the other options do not accurately represent the typical products formed by the interaction of Group 1 metals with water. For example, metal oxides are usually formed through different reactions involving oxygen, not directly from water. Similarly, metal chlorides involve reactions with halogens rather than water. Oxygen does not form as a product in this specific reaction, and thus is not observed in the typical output when water is involved.