How Does The Environment Affect The Reactivity Of An Electron?

Atomic radius is defined as the distance from the outermost ring, referred to the valence shell, to the centre of the atom. On the periodic table, going across from left to right, the atom’s relative size decreases. However, going down the group, the atomic radius increases in size. From left to right there is an increase of positive charges in the neutron and the electrons. Due to the increase of the number of positive charges, the electron’s attractive force becomes stronger, thus (the electrons) being drawn close to the nucleus. The stronger the attractions causes the electrons move closer to the nucleus, decreasing the size. When going down the column (group), the number of electron shells that are occupied increases, creating a shield. The shield are the inner shells that have electrons making the outermost level being far from the nucleus. The distance from the outermost level to the nucleus is far, making the attraction decrease. Atomic radius affects the reactivity of an atom, as the bigger it is the bonds become weaker. As electrons are further away from the nucleus, the attraction between it (negative and positive forces) are not as strong, where electrons are able to move easily. A smaller atomic radius has a stronger bond between electrons and nucleus making it harder for other atoms to get it’s electrons. The
As you go down a group, the ionization energy decreases due to the shielding. This affects the reactivity of the element as the lower ionization energy level, the more reactive it is, as electrons can be easily removed by the pull of another atom. The greater the distance of the outermost shell to the nucleus, the easier it is to pull on the electrons. It can give away its electrons easily and reacting with the other atom. Also, the ionization energy increases from left to right. However, noble gases are not included as they do not have any electrons to