reactions of metal

• When a metal reacts with oxygen, it forms a metal oxide.
• Aluminium is a reactive metal that forms a layer on the outside of aluminium oxide, which helps to protect the metal and prevents it from corroding in air.
• Lithium, Sodium, Potassium, and other Group 1 and Group 2 metals tarnish and look dull because they react with oxygen.
• Metal plus water goes to metal hydroxide plus hydrogen.
• Group 1 metals, such as lithium, sodium, and potassium, become more reactive as they are added to water.
• Rubidium and cesium, which are in Group 1, are not commonly used in classrooms.
• Less reactive metals, such as iron, will react with water slowly and things will go rusty.
• Metal plus acid results in salt plus hydrogen.
• A more reactive metal is easier to take away its outer electrons.
• Sodium is more reactive than lithium because it is further away from the nucleus and the attraction of the nucleus is weaker.
• The metal displaces the hydrogen because it is more reactive than hydrogen.
• Potassium plus sulfuric acid results in potassium sulfate plus hydrogen.
• Sodium plus hydrochloric acid results in sodium chloride plus hydrogen.
• A salt is a product that is obtained when an acid is neutralized, and its properties depend on the metal and the acid used.
• Calcium plus sulfuric acid results in calcium sulfate plus hydrogen.
• Potassium is more reactive than sodium because it is further away from the nucleus and the attraction of the nucleus is weaker.
• The reactivity series shows that the more reactive metals will react with dilute acid, while the less reactive metals won't.