Group 1 and group 2 metals react with water to form metallic hydroxides and hydrogen gas. These reactions are vigorously exothermic, and can result in the hydrogen gas igniting, causing an impressive explosion. For example, when pure sodium (Na) is added to water, it reacts quickly to produce bubbles of hydrogen gas. If enough sodium is used, the reaction will be sufficiently exothermic to burn the hydrogen. The initial reaction is: 2Na + 2H2O --> 2NaOH + H2 and the burning of hydrogen is: 2H2 + O2 --> 2H2O.
This is because gold is not reactive enough. Metals below hydrogen in the reactive series will not react with sulphuric acid.
Neptunium is a reactive metal and can react with the majority of non metals.
Very reactive metals - from group 1 and 2 of the periodic table - can react with water.
Vinegar (acetic acid) can react with some reactive metals as alkaline metals.
Metals higher up the reactivity series (more reactive) will react more readily with oxygen to form the respective metal oxide
Because metals are often very reactive, as are acid.
Electronegativities of metals are very different: alkali metals are very reactive, platinum metals very unreactive. Metals react with nonmetals.
Electronegativities of metals are very different: alkali metals are very reactive, platinum metals very unreactive. Metals react with nonmetals.
Alkali metals are more reactive than alkaline earth metals.
Alkali Earth metals are the most reactive metals on the periodic table.
Yes, alkali metals will react with anything to get rid of that one valence electron, which makes them highly reactive.
Metals which are more reactive than aluminium. Eg= Sodium, Magnesium, Potassium, etc