Electronegativity TrendĮlectronegativity is the ability of an atom to attract electrons. Therefore, the atomic size and atomic radius increase from top to bottom. Hence, they are further away from the nucleus. The inner electrons shield the valence electrons and prevent them from getting closer to the nucleus. It is evident that as the atomic number increases down a group, the valence electrons occupy higher shells. In other words, the atomic radius increases from right to left, as shown in the image below. Thus, the atomic size and radius gradually decrease from left to right of a period. As a result, the electrostatic attraction between the electrons and the nucleus increases, and the valence electrons are held closer to the nucleus. Protons are also added to the atomic nucleus, making the nucleus more positively charged. Across a PeriodĪlong a period, electrons are added to the same shell of an atom as we go from left to right. Hence, the discussion in this section will be of atomic radius. The atomic and ionic radii follow the same trend in the periodic table. On the other hand, the ionic radius is half the distance between two ions that barely touch each other in a compound. Atomic Radius and Ionic Radius TrendĪtomic radius is the distance between an atom’s nucleus and its outermost or valence electrons. Properties of Elements Based on Periodic Trends 1. These changes occur within their respective period from left to right and group from top to bottom in the periodic table. These observed patterns allude to the changes in atomic structure, including size and radius, as well as properties of the elements. Periodic trends are specific patterns observed among the chemical elements of the periodic table. Properties of Elements Based on Periodic Trends.
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