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

Prove the Correct Order of Reactivity of MetalsAimThe aim of this experiment is to find a method of mathematicallyanalysing the order of metal reactivity. This involved finding a safe,dependant variable which is numerically measurable. After testing allthe metals and measuring such a variable, is my hope to set all of themetals into a proven, accurate order of activity.PlanEvery element of the periodic table is made up of atoms. individually of theatoms consists of subatomic particles which make up a nucleus andouter orbits. The nucleus contains positively charged protons, andneutrally charged neutrons. These make up the relative mass of theatom. Orbiting the nucleus, attracted by the positive charge of theprotons, are the electrons. This are arranged in layers, called slide fastenerlevels, and have no mass. Only a certain number of electrons fit oneach energy level, and it is this which affects the reactivity ofcertain materials and is also the way that the periodic table isarran ged.The number of electrons in the outer energy level is the groupin which the element is placed. The first level (nearest the nucleus)will only hold 2 electrons, the second holds 8, and the third alsoseems to be full when it has 8 electrons.If all of the energy levels in the atom are full populated withelectrons, it is said to be stable, and in most cases, is thereforeunreactive. Examples of this include the noble (or inert) gases suchas nor-east or argon. However if the outer energy level of the atom is notstable, it will automatically try to either gain or lose electrons to mystify stable. This is achieved by an ionic reaction. Ionic bondingoccurs when the outer atoms of on material changes orbit and joinsanother material for example Sodium chlorideAs you can see, atomic number 11 is a group one metal (it has one electron onits outer energy level) so is therefore unstable. Chlorine on theother mint is a group 7 element. It is much easier for atomic number 11 to loseits outer electron to become stable, than it is for it to gain 7. Thesame is true for the chlorine gaining 1 as opposed to losing seven.Therefore the outer electron of the sodium switches orbits to thechlorine. This creates a Na+ ion and a Cl- ion. Because oppositesattract, it means that the two substances create an ionic bond andform sodium chlorideGroup one metals are the most reactive as they only have one, easilyremoved, electron. However if you view the periodic table