Prove the Correct Order of Reactivity of Metals :: Metal Reactivity Science Experiments Essays

Prove the Correct Order of Reactivity of Metals Aim The aim of this experiment is to find a method of mathematically analysing the order of metal reactivity. This involved finding a safe, dependant variable which is numerically measurable. After testing all the metals and measuring such a variable, is my hope to set all of the metals into a proven, accurate order of activity. Plan Every element of the periodic table is made up of atoms. Each of the atoms consists of subatomic particles which make up a nucleus and outer orbits. The nucleus contains positively charged protons, and neutrally charged neutrons. These make up the relative mass of the atom. Orbiting the nucleus, attracted by the positive charge of the protons, are the electrons. This are arranged in layers, called energy levels, and have no mass. Only a certain number of electrons fit on each energy level, and it is this which affects the reactivity of certain materials and is also the way that the periodic table is arranged. The number of electrons in the outer energy level is the group in which the element is placed. The first level (nearest the nucleus) will only hold 2 electrons, the second holds 8, and the third also seems to be full when it has 8 electrons. If all of the energy levels in the atom are full populated with electrons, it is said to be stable, and in most cases, is therefore unreactive. Examples of this include the noble (or inert) gases such as neon or argon. However if the outer energy level of the atom is not stable, it will automatically try to either gain or lose electrons to become stable. This is achieved by an ionic reaction. Ionic bonding occurs when the outer atoms of on material changes orbit and joins another material for example: Sodium chloride As you can see, sodium is a group one metal (it has one electron on its outer energy level) so is therefore unstable. Chlorine on the other hand is a group 7 element. It is much easier for sodium to lose its outer electron to become stable, than it is for it to gain 7. The same is true for the chlorine gaining 1 as opposed to losing seven. Therefore the outer electron of the sodium switches orbits to the chlorine. This creates a Na+ ion and a Cl- ion. Because opposites attract, it means that the two substances create an ionic bond and form sodium chloride! Group one metals are the most reactive as they only have one, easily removed, electron. However if you view the periodic table: