That describes just about any Bronsted-Lowry acid, from citric to hydrofluoric...although it is unbelievably important that you do NOT try to find out what hydrofluoric acid tastes like!
Acid
there are some alkali metals. It can be sodium or potassium.
Non-metals tend to react with oxygen to form oxides when heated. The reaction can be violent or slow, depending on the element. For example, carbon reacts with oxygen to form carbon dioxide, sulfur reacts to form sulfur dioxide, and nitrogen reacts to form nitrogen oxides.
An acid, such as hydrochloric acid or sulfuric acid, produces hydrogen gas when it reacts with some metals like zinc or aluminum. The reaction releases hydrogen gas along with a salt as a byproduct.
All the other alkali metals (sodium, potassium, rubidium, and cesium) reacts with water with increasing violence. Some of the alkaline earth metals (calcium, strontium, and barium) and a few other metals (such as europium) react in similar manner to produce hydrogen gas and the corresponding metal hydroxide.
which reacts with some metals causing it to break down.
Nitric acid reacts strongly with many metals.
When non-metals react with water, they may not produce hydrogen gas like metals do. Instead, some non-metals may form acidic solutions, releasing hydrogen ions. Others may simply dissolve or form oxides upon reacting with water.
Heating carbon with metal compounds can help extract the metal because carbon can act as a reducing agent. During the heating process, carbon reacts with the metal compound, and the carbon removes oxygen from the metal compound, leaving behind the pure metal. This process is known as a reduction reaction.
A common compound of curium is curium oxide (Cm2O3), which is formed when curium reacts with oxygen. Another compound is curium fluoride (CmF3), formed when curium reacts with fluorine. These compounds are used in research and nuclear applications.
Some metals in the table do not react with water
The most prominent constituent in the atmosphere which reacts with some metals, though not all, is oxygen. The resultant chemical would be an oxide of the metal concerned.