![]() ![]() Metallic character relates to the ability to lose electrons, and nonmetallic character relates to the ability to gain electrons.Īnother easier way to remember the trend of metallic character is that moving left and down toward the bottom-left corner of the periodic table, metallic character increases toward Groups 1 and 2, or the alkali and alkaline earth metal groups.Lattice energy increases as you move up the periodic table. Third, if the charges are the same look at the position on the periodic table. Second, place them in order of increasing or decreasing based on charge. Electron shielding causes the atomic radius to increase thus the outer electrons ionizes more readily than electrons in smaller atoms. How do you find lattice energy First, find the charges of the ions in the compound. Metallic characteristics increase down a group.This is caused by the decrease in radius (caused by Zeff, as stated above) of the atom that allows the outer electrons to ionize more readily. Metallic characteristics decrease from left to right across a period.The semi-metal boron also possesses a high melting point. The non-metal carbon possesses the highest melting point of all the elements.Most non-metals possess low melting points.Metals generally possess a high melting point.Electronegativity values for each element can be found on certain periodic tables. The numbers assigned by the Pauling scale are dimensionless due to the qualitative nature of electronegativity. However, the most common scale for quantifying electronegativity is the Pauling scale (Table A2), named after the chemist Linus Pauling. Because electronegativity is a qualitative property, there is no standardized method for calculating electronegativity. These trends exist because of the similar atomic structure of the elements within their respective group families or periods, and because of the periodic nature of the elements.Įlectronegativity can be understood as a chemical property describing an atom's ability to attract and bind with electrons. Periodic trends, arising from the arrangement of the periodic table, provide chemists with an invaluable tool to quickly predict an element's properties. Major periodic trends include: electronegativity, ionization energy, electron affinity, atomic radius, melting point, and metallic character. Periodic trends are specific patterns that are present in the periodic table that illustrate different aspects of a certain element, including its size and its electronic properties.
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