![]() ![]() These electrons screen or shield the outer electrons from the nuclear charge. Metal reactivity increases down a group because as nuclear shielding increases and the nucleus' hold on the valence electron weakens, therefore it is easier to remove valence electrons. This is because of the screening effect of the filled inner electron levels. That is why as you go up a group Chemical Reactivity increases because it is easier for elements to gain electrons when they have high electronegativity. The greater attraction between the increased number of protons (increased nuclear charge) and electrons, pulls the electrons closer together, hence the smaller size.Īs you move down a group in the periodic table, the covalent radius increases. The covalent radius (a measure of how large individual atoms are) shows different trends if you are moving across a period or down a group.Ī comparison of the relative covalent radii of atoms is shown in the diagram below.Īcross a period from left to right, the covalent radius decreases.Īs you move from left to right across the periodic table, atoms have more electrons in their outer energy level and more protons in their nucleus. Why does reactivity decrease as you go down group 7 Reactivity decreases down the group. ![]() Patterns and trends in the periodic tableĬhemists observe patterns in different properties of elements as they are arranged in the periodic table. As you go down group 1 (the alkali metals) in the periodic table, the elements get more reactive.
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