Notice that the general trend is upwards, but this is broken by falls between magnesium and aluminium, and between phosphorus and sulphur. For facts, physical properties, chemical properties, structure and atomic properties of the specific element, click on the element symbol in the below periodic table. This is because, the effect of increasing proton number is greater than that of the increasing effective nuclear charge; therefore, there is a greater nuclear attraction. These topics are covered in various places elsewhere on the site and this page simply brings everything together - with links to the original pages if you need more information about particular points. It is a soft, silvery-white alkali metal. The 3p electron is slightly more distant from the nucleus than the 3s, and partially screened by the 3s electrons as well as the inner electrons. Like all alkali metals, lithium is highly reactive and flammable, and is stored in mineral oil. Joap's interactive graph and data of "Atomic Radius of Period 3 Elements" is a scatter chart, showing Col2; with Elements in the x-axis and Atomic Radius (10^-12 m) in the y-axis.. Atomic radius is determined as the distance between the nuclei of two identical atoms bonded together. atomic radius of the elements decreases from 134 pm to 69 pm across the period from left to right Atomic radius generally decreases across Period 2 from left to right as the nuclear charge increases. Sodium, magnesium and aluminium are all good conductors of electricity. As you go across the period, the bonding electrons are always in the same level - the 3-level. Atomic radius is determined as the distance between the nuclei of two identical atoms bonded together. Periodic Trend in Atomic Radius Along the Period: The atomic radii of the elements of the second period and the graphical representation of variation for the second period are given below. D. K and Br 2 (Total 1 mark) 4. In these and similar cases, the atomic radius is designated as a covalent radius. Commercial copying, hiring, lending is prohibited. To understand these, you first have to understand the structure of each of the elements. For which element are the group number and the period … Atomic radius across period 3. Going across period 3: the nuclear charge increases … the atomic radius decreases … there are more electrons, but the increase in shielding is negligible because each extra electron enters the same shell … so electrons will be more strongly attracted to the nucleus. The chemical symbol for Lithium is Li.. Atomic radius of period 3 elements Na Mg Al Si P S Cl Ar Period 3 element 0.08 0.10 0.12 0.14 0.16 0.18 0.20 Atomic radius /nm In each of these cases, before bonding happens, the existing s and p orbitals are reorganised (hybridised) into new orbitals of equal energy. Moving across Period 3, the number of protons in the nucleus increases - for example sodium has 11 protons, and chlorine has 17 protons. Atomic Radius of all the elements in the Periodic Table. All that differs is the number of protons in the nucleus. Chlorine, Cl2, is a much smaller molecule with comparatively weak van der Waals attractions, and so chlorine will have a lower melting and boiling point than sulphur or phosphorus. In the whole of period 3, the outer electrons are in 3-level orbitals. I don't know why there is such a small increase in melting point as you go from magnesium to aluminium. Both of these factors offset the effect of the extra proton. shown in the data table below. Trends of atomic radius in 3rd period elements. It is fair to compare metallic and covalent radii because they are both being measured in tightly bonded circumstances. However, excluding the particles in argon from the term "molecule" just adds unnecessary complications to the flow of this page - for example, it makes life difficult if you are talking about "molecular elements" and intermolecular forces. (b) Atomic radius decreases on moving from left to right in a period of the periodic table. The first three are metallic, silicon is giant covalent, and the rest are simple molecules. As the atomic number increases within a period, the atomic radius decreases. It is measured or calculated in different ways, so values vary from source to source. After studying this page, you should be able to: The table shows atomic radius values for the elements Na to Ar. Home This is due to the increase in nuclear charge across these periods Hence increasing its electrostatic pull between electrons and nucleus, resulting in decrease in atomic … In Period 3 of the Periodic Table, the 3s and 3p orbitals are filling with electrons. 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