![]() This causes the electrons to experience a greater force of attraction as you move along the period, making it easier for an atoms to gain more electrons to become ions. The charge on the atomic nucleus increases as you move go across the period but the electron shielding caused by the two inner electrons remains the same.The reactivity increases as you go across the period because: Measurements are taken of metallic radii for metals and covalent radii for molecules. State and explain the general trend in atomic radius across Period 3 (excluding Argon). The periodic trends allow for a partial inference of any elements unknown properties There are a few exceptions, such as the ionization energy trend of group 3. ![]() As the atomic size reduces, it becomes more difficult to eliminate an electron nearer to a more central nucleus. c) the trend in reactivity of the halogens Cl, Br and I, illustrated by reaction with other halide ions Scotland. Dependence of chemical properties of elements on their electronic structure. As you move across a period, the first ionization energy increases. (ii) across a period (main group elements) and for exceptions to the general trends across a period. The low ones elements tend to be reducing agents. Nitrogen, Oxygen and Fluorine can all gain electrons to become negative ions in certain reactions. Periodic Trends 4.1.3 4.1.3 Atomic Radius across Period 3 1. The ionization energy of an element can be used to determine its reactivity. This causes the electrons to experience a greater force of attraction as you move along the period, making it harder for the atoms to lose electrons and become ions. The outer electrons are all roughly the same distance away from the nucleus.trends that are not followed by the transition metals in groups 3-12. Trends in reactivity Terms in this set (98) 3.1.1 PERIODICITY 3.1. The reactivity decreases as you go across the period because: The repeating pattern across the periods of the periodic table is the filling of. The pH of typical solutions will, like sulphuric acid, be around 0. Chlorine (VII) oxide reacts with water to give the very strong acid, chloric (VII) acid - also known as perchloric acid. For the first 3 elements Lithium, Beryllium and Boron all lose electrons in chemical reactions. It continues the trend of the highest oxides of the Period 3 elements towards being stronger acids.
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