![]() ![]() Ionic radius also follows the same trend as the atomic radius. The number of outer electrons (also known as Valence electrons) determines how that element will react.Ītomic radius decreases across a period from left to right, and increases down a group. Non-metals (right) are often gases or brittle solids at room temperature, poor conductors of heat and electricity, and tend to gain electrons in chemical reactions. Metals (left and centre) are often solid at room temperature, good conductors of heat and electricity, and tend to lose electrons in chemical reactions. Section 4: Understanding Patterns in the Periodic TableĪs you move down a group, the elements become more metallic and reactivity increases (for metals) and decreases (for non-metals).Īs you move across a period to the right, elements become less metallic and the reactivity of metals decreases and reactivity of non-metals increases.īy understanding an element’s position on the periodic table, you can predict its physical and chemical properties: Lanthanides and actinides are special groups of metals located at the bottom of the Periodic Table. Transition metals are found in the middle of the periodic table, between Group 2 and Group 3. Group 8 elements (Group 0 according to UK labelling) are the noble gases, which are very unreactive. Group 7 elements are the halogens, which are very reactive non-metals. Group 2 elements, the alkaline earth metals, are reactive but less so than Group 1. Group 1 elements, the alkali metals, are very reactive metals. Section 2: The Groups of The Periodic Table The atomic number on the periodic table represents the number of protons an atom of that element has. The vertical columns are called ‘groups’ and the horizontal rows are called ‘periods’.Įlements in the same group have the same number of electrons in their outermost shell and hence, have similar chemical properties.Įlements in the same period have the same number of energy levels or electron shells. The periodic table is a table of chemical elements arranged in order of their relative atomic numbers. Section 1: Understanding The Periodic Table
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