The Elements of the Periodic Table

   When the Periodic Table was first being invented, people thought they should organize the elements by the element's atomic mass. Later on, scientists decided to arrange the elements by their atomic number as well as their chemical properties.

   The elements in Group 1 (except hydrogen) are known as the Alkali metals. They are the most reactive group of metals in the Periodic Table; these elements all have a +1 charge. The elements in Group 2 are known as the Alkali Earth metals. They are the second most reactive elements in the Periodic Table; all elements in this group have +2 charge. The elements in Groups 3-12 are the Transition Metals (not including the Lanthanides and Actinides); they all vary from a +1 to a +4 charge. Some elements at the bottom rows (Periods 6 and 7) of the Periodic Table are the Lanthanide series and the Actinide series. We will not go into too much detail on these elements, except for a couple of them, because their chemical properties are largely similar. Elements with an atomic number of higher than 92 are known as transuranium elements, which are all synthetic; many of them are radioactive with short half-lives. All the nonmetals are on the right side of the Periodic Table except for hydrogen; hydrogen is sometimes placed on the left side of the Periodic Table and sometimes on the right, because it shows both metallic and nonmetallic properties. The elements in Groups 13-16 also have their own unique group names. The halogens are in Group 17 and they have 7 electrons in their outermost energy level; they gain one electron to become stable, and so they have a -1 charge. The noble gases are the only naturally stable elements in the Periodic Table; they are used in many things like neon lights and lasers because they do not combine.

   This is a general overview of the elements in the Periodic Table. To find out more on a specific element, click the group number on the left.