Periodic trends are specific patterns found in the periodic table, illustrating different aspects of a given element including their size and properties with electrons. I will compare and contrast how the underlying causes of the left and right and up and down configurations of the periodic table are the same in all of these four trends. Trends can be predicted using the periodic table and can be explained by analyzing the electronic configurations of the elements. Elements tend to gain or lose valence electrons to achieve stable octet formation. The atomic radius is half the distance between the nuclei of two atoms is just like a radius equal to half the diameter of a circle. The idea is that not all atoms are normally bonded together in the same way. Some are bound by covalent bonds in molecules, some are attracted to each other in ironic crystals, and some are held in metallic crystals. Atomic size gradually decreases from left to right through a period of elements. This is because within a period or family of elements. , they are all added to the same shell. At the same time, protons are also added to the nucleus, making it more positively charged. The increasing number of protons is greater than that of the increasing number of electrons; so there is a greater nuclear attraction. So as you go down the periodic table the atomic radius increases. Valence electrons have higher levels due to the increase in quantum number. The atomic radius decreases from left to right within a period, this is caused by the increase in the number of protons and electrons in a period. A proton has a greater effect than an electron, so many electrons will be attracted towards the nucleus, which with... half of the paper... differently depending on the trend. As you can see, each trend has a similarity of properties within the groups. You will notice that these properties change depending on the position of the element in the periodic table. Eventually you will notice that as you move from left to right in the periodic table, there is a trend or change in a number of properties. The same thing happens if you go up and down the periodic table and compare the properties of the elements. Periodic trends influence how certain elements of the periodic table react with each other. For example, the trend of ionization energy: metals want to give up electrons, non-metals want to gain them. This trend is essentially about which elements could react together and how they would react together, i.e. the formation of electron ions through a reaction.