![]() It is a dimensionless property because it is only a tendency. The tendency of an atom in a molecule to attract the shared pair of electrons towards itself is known as electronegativity. Main article: Electronegativity Periodic variation of Pauling electronegativities In that case, the ionization energy decreases as atomic size increases due to adding a valence shell, thereby diminishing the nucleus's attraction to electrons. However, suppose one moves down in a group. The decrease in the atomic size results in a more potent force of attraction between the electrons and the nucleus. Trend-wise, as one moves from left to right across a period in the modern periodic table, the ionization energy increases as the nuclear charge increases and the atomic size decreases. The energy needed to remove the second electron from the neutral atom is called the second ionization energy and so on. The first ionization energy is the amount of energy that is required to remove the first electron from a neutral atom. It is also referred to as ionization potential. The ionization energy is the minimum amount of energy that an electron in a gaseous atom or ion has to absorb to come out of the influence of the attracting force of the nucleus. ![]() These trends give a qualitative assessment of the properties of each element. ![]() These trends exist because of the similar electron configurations of the elements within their respective groups or periods they reflect the periodic nature of the elements. Major periodic trends include atomic radius, ionization energy, electron affinity, electronegativity, valency and metallic character. They were discovered by the Russian chemist Dmitri Mendeleev in 1863. In chemistry, periodic trends are specific patterns that are present in the periodic table that illustrate different aspects of certain elements when grouped by period and/or group. These trends explain the periodicity observed in the elemental properties of atomic radius, ionization energy, electron affinity, and electronegativity.Specific recurring patterns that are present in the modern periodic table The periodic trends in properties of elements. This happens because the number of filled principal energy levels (which shield the outermost electrons from attraction to the nucleus) increases downward within each group. Second, moving down a column in the periodic table, the outermost electrons become less tightly bound to the nucleus. As this happens, the electrons of the outermost shell experience increasingly strong nuclear attraction, so the electrons become closer to the nucleus and more tightly bound to it. First, electrons are added one at a time moving from left to right across a period. In addition to this activity, there are two other important trends. Stable octets are seen in the inert gases, or noble gases, of Group VIII of the periodic table. ![]() Elements tend to gain or lose valence electrons to achieve stable octet formation. These trends can be predicted merely by examing the periodic table and can be explained and understood by analyzing the electron configurations of the elements. The periodic table arranges the elements by periodic properties, which are recurring trends in physical and chemical characteristics. ![]()
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