![]() The elements classified as transition metals are strong and durable. The transition metals constitute one of the largest sets of the periodic table. Transition metals include metals from group 3, group 4, group 5, group 6 until group 12. ![]() The group 2 elements include Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), and Barium (Ba). These metals are named so because they are found in the earth's crust. ![]() Group 2: Group 2 elements are called alkali earth metals. The metals of group 1 include Lithium, Sodium, Potassium, Rubidium, Cesium, and Francium. The valency of these metals is 1 and these metals are highly reactive. Group 1: Group 1 consists of alkali metals. The elements belonging to a particular group have several similarities in their chemical properties and also form similar types of bonds, however, there are some exceptions.Įlements of each group have their characteristic features. All the elements in a group have similar properties and also have the same valency. A new subshell is added to the elements as we traverse down a group. As we traverse down a group the electronic configuration in groups changes hugely. The 6th and 7th periods could be classified as the longest periods in the modern periodic table, as they also host lanthanides and actinides.Īs we have seen earlier, the modern periodic table consists of 18 groups. The second period begins with lithium and boron which have 3 and 4 electrons respectively. The electronic configuration of hydrogen is 1s¹ whereas the electronic configuration of helium is 1s².Īs we proceed down a group, the period number increases and the number of subshells also increases. These two elements do not have a P subshell and have only an S subshell. The first period is the smallest period and hosts only two elements, hydrogen and helium. As we traverse from left to right across a period, the Electronic Configuration of the elements increases, and hence the energy level of the atoms also increases. The value of the principal quantum number, that is n is incremented by 1 as we traverse across a period. The electronic configuration between consecutive elements differs by only 1, across a period. Across a period the atomic number of every consecutive element differs by 1. As we see in the image above, the modern periodic table has 7 periods and 18 groups. The periods are basically the horizontal rows and the groups are the vertical columns of the modern periodic table. The elements in a periodic table are arranged in: Hence, the electronic configuration does play a huge role in the existence of every object in the surrounding.Įlectronic Configuration in Periods of the Periodic Table The electronic configuration also determines which element would combine with which other element and in what ratio. Each element, in the ground state, has a unique electronic configuration and hence, each one of them differs from the other in many ways.Įlectrons, although they are so tiny, have a detrimental role in several reactions. If we look at it on a wider scale, electronic configuration determines every single chemical property of an element. It plays a major role in determining the chemical properties of the atoms such as valency, conductance, reactivity. ![]() This electronic configuration of the elements determines their several properties. Each atom belonging to every single group and period has a characteristic electronic configuration.
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