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Compare And Contrast The Reaction Between Group 1 And Group 2 Elements

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As the elements went down Group I, the reactions became quicker and more reactive. This is because of the decreasing electronegativity.
Each element in this group has one valence electron each, but a different number of shells. The increasing number of shells means that the valence electron surrounding the nucleus of the atom gets farther away as the elements go down the group. The electron experiences less of a pull towards the nucleus, so the atom can give the electron away a lot easily. This gives each element a more violent reaction than the one above it in the Periodic Table.
As with the Group I elements, the reactions of the Group II elements get more vigourous as they go down the group. Calcium has a stronger reaction than Magnesium, because of the increase in atomic size. Just like with the Group I elements, its valence electrons are further away from the nucleus, so it gives them away easier than Magnesium does. …show more content…
The electronegativity increases across periods. Because of the increase of valence electrons in the Group II elements (2 electrons), they are more unreactive than the Group I elements (1 electron). For an atom, it’s a lot easier to give away one valence electron than it is to give away two.
Using Calcium and Potassium as an example: Calcium is rather reactive in water, Potassium is even more so. They both have the same number of shells, but Potassium has one less valence electron than

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