![]() ![]() This particle contains two more negatively-charged electrons than positively-charged protons therefore, it bears an overall net –2 charge. This particle is now an ion, a charged particle, as a result of the imbalance between the number of positively-charged protons (+16) and negatively-charged electrons (–18) that it possesses. Therefore, this new particle is no longer a sulfur (S) atom which, as stated above, contains 16 electrons. However, since this new particle was formed through the gain of two valence electrons, it now has 18 (16 + 2) electrons. Since the identity of an element is defined by the number of protons that it contains, due to the association between atomic number and proton-count, this new particle is still a form of sulfur. Note that the number of protons was unchanged in the process described above, so this new particle still contains 16 protons. Therefore, this new particle has 8 valence electrons and has achieved, through the process described above, a highly-stable octet configuration. The superscripts associated with these orbitals now sum to 8. In this new electron configuration, the number of valence electrons contained in the corresponding particle are still determined by totaling the electrons found within the the 3 s and 3 p orbitals. Simplification of the 3 p orbital's superscript results in a new electron configuration, as shown below. The rules presented in Section 2.6 dictate that if two additional electrons are added, they must both be placed in the 3 p orbital, in order to fill that orbital to its maximum capacity. Therefore, sulfur will gain two additional valence electrons.Ĭonsider the impact that this will have on sulfur's electron configuration. Unlike in the calcium example presented in the previous section, gaining this number of electrons is possible, as doing so would not exceed the maximum gain-limit of three electrons. Sulfur would need to gain 2 electrons in order to achieve an octet configuration. In order to be stable, a particle must possess an octet, or eight, fully-paired valence electrons. Sulfur has 6 valence electrons, as determined either by totaling the electrons found within the orbitals in the highest occupied energy level, which, in this case, includes both the 3 s and 3 p orbitals, or by identifying the "A/B System" group number for the column in which the element is found. Sulfur's electron configuration, which was first determined in Section 2.6, is shown below. For reasons identical to those described in the previous section, the neutron count for this particular sulfur atom is irrelevant to the analysis that will be performed in the following paragraphs and will not be discussed further. You can effortlessly find every single detail about the elements from this single Interactive Periodic table.\)Īnions are negatively-charged ions that are most often formed when non-metals, which are found on the right side of the periodic table, gain valence electrons.Īn atom of sulfur contains 16 protons, because its atomic number is 16, and 16 electrons, in order to be net-neutral. Let me tell you how this Interactive Periodic Table will help you in your studies.ġ). Free Gift for you: Interactive Periodic Table In this way, the elements of the same group show similar chemical properties and they also have the same number of valence electrons. They are soft and can be cut easily with a kitchen knife.Īlso all the elements of group 1 have one valence electron.Īll the elements of group 18 are chemically inert (that means they do not easily react with other elements).Īnd all the elements of group 18 have a complete octet (that means they have 8 electrons in their outer shell). The elements lying in the same groups show similar chemical properties and they also have same number of valence electrons.Īll the elements of group 1 are highly reactive to water. There are total 18 vertical columns on periodic table. Groups are the vertical columns on the periodic table. ![]()
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