Ionisation energy increases on moving horizontally across a period, whereas on moving in the downward direction, the ionisation energy decreases.Ītomic radii – the distance between the outermost electron and the nucleus is known as the atomic radius. Ionisation energy – this energy helps the atoms to remove the electrons. An exception in group 3 elements is present where electronegativity increases towards thallium. On moving in the downward direction, the electronegativity decreases. On moving from left to right horizontally in a periodic table, there is an increase in electronegativity. The Pauling scale is used to measure electronegativity. Some periodic trends and chemical reactivity in the periodic table are as follows –Įlectronegativity – measures the ability of a molecule to gain electrons within a chemical bond. The trends of the elements in a periodic table depend on various factors like electronegativity, ionisation energy, electron affinity, atomic radii, metallic character, and chemical reactivity. Periodic trends refer to the patterns of the properties of the chemical elements. The periodic trends and chemical reactivities of elements are shared below. The gas elements do not gain or lose their electrons because the electronic configuration is filled. Hence the elements on the left side in the downwards direction are the highly reactive elements. In a period, the chemical reactivity decreases on moving towards the right, whereas in a group, chemical reactivity increases on moving downwards. Hence the electronegativity and the ionisation energy determine a chemical reaction. The higher the reactivity of the element, the easier it is to combine. The electrons between the elements are shared, or the elements lose or gain the electrons. The rate at which a chemical substance or an element undergoes a chemical reaction is known as reactivity.
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