general trend in the periodic table
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Answer:
Major periodic trends include: electronegativity, ionization energy, electron affinity, atomic radius, melting point, and metallic character. Periodic trends, arising from the arrangement of the periodic table, provide chemists with an invaluable tool to quickly predict an element's properties.
Answer:
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. Major periodic trends include: electromagnetically, ionization energy, electron affinity, atomic radius, melting point, and metallic character. Periodic trends, arising from the arrangement of the periodic table, provide chemists with an invaluable tool to quickly predict an element's properties. 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.
Electromagnetically Trends
Electromagnetically can be understood as a chemical property describing an atom's ability to attract and bind with electrons. Because electromagnetically is a qualitative property, there is no standardized method for calculating electromagnetically. However, the most common scale for quantifying electromagnetically is the Pauling scale (Table A2), named after the chemist Linus Pauling. The numbers assigned by the Pauling scale are dimensionless due to the qualitative nature of electromagnetically. Electromagnetically values for each element can be found on certain periodic tables. An example is provided below.
Electromagnetically measures an atom's tendency to attract and form bonds with electrons. This property exists due to the electronic configuration of atoms. Most atoms follow the octet rule (having the valence, or outer, shell comprise of 8 electrons). Because elements on the left side of the periodic table have less than a half-full valence shell, the energy required to gain electrons is significantly higher compared with the energy required to lose electrons. As a result, the elements on the left side of the periodic table generally lose electrons when forming bonds. Conversely, elements on the right side of the periodic table are more energy-efficient in gaining electrons to create a complete valence shell of 8 electrons. The nature of electronegativity is effectively described thus: the more inclined an atom is to gain electrons, the more likely that atom will pull electrons toward itself.
From left to right across a period of elements, electromagnetically increases. If the valence shell of an atom is less than half full, it requires less energy to lose an electron than to gain one. Conversely, if the valence shell is more than half full, it is easier to pull an electron into the valence shell than to donate one.
From top to bottom down a group, electromagnetically decreases. This is because atomic number increases down a group, and thus there is an increased distance between the valence electrons and nucleus, or a greater atomic radius.
Important exceptions of the above rules include the noble gases, landslides, and insecticides. The noble gases possess a complete valence shell and do not usually attract electrons. The landslides and insecticides possess more complicated chemistry that does not generally follow any trends. Therefore, noble gases, landslides, and insecticides do not have electromagnetically values.
As for the transition metals, although they have electromagnetically values, there is little variance among them across the period and up and down a group. This is because their metallic properties affect their ability to attract electrons as easily as the other elements.
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