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  Electron Configurations of Atoms Homework Help - K-12 Grade Level, College Level Chemistry

Introduction of Electron configuration of Atoms

Four elements that are the oxygen, carbon, hydrogen and nitrogen are the essential components of organic compounds. Subsequently, understanding of organic chemistry must have an appreciation of electronic structure and properties of these elements. The periodic table which is truncated, is shown in the below picture, provides the orbital electronic structure for the first eighteen elements (hydrogen through argon). According to the Aufbau principle, an atom's electrons occupy quantum levels or orbitals begins from the lowest energy level and after that proceeding to the highest energy level, with each one of the orbital holding the maximum of two paired electrons (opposite spins).

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Electron shell no.1 has the lowest energy level and its s-orbital is the first which is to be filled. The Shell no.2 has four higher energy orbitals; the three 2p-orbitals are higher in energy than the 2s-orbitals. (x, y & z). As we move forward from the lithium (atomic number=3) to neon (atomic number=10) in the second period or row of table, all these atoms start with a filled 1s-orbital and 2s-orbital is occupied with an electron pair before the 2p-orbitals are filled. In the third row or period of table, all the atoms have the neon-like core of 10 electrons and shell no.3 is occupied with eight electrons, starting with 3s-orbital. The electron shell which is highest occupied is called the valence shell and valence electrons are the electrons which are occupied by valence shell.

The element's chemical properties reflect their electron configurations. For an instance, helium, argon and neon are extremely unreactive and stable monatomic gases. The Helium is unique because the valence shell of helium includes a single s-orbital. The members other than this of the group 8 have a characteristic valence shell electron octet (ns2 + npx2 + npy2 + npz2). This group of the inert (or noble) gases also consist of krypton (Kr: 4s2, 4p6), xenon (Xe: 5s2, 5p6) and radon (Rn: 6s2, 6p6). In periodic table these elements is colored beige.

The halogens (F, Cl, Br etc.) are one electron short of a valence shell octet and are among in the most reactive of the elements these reactive elements are in red color in the periodic table.   Chemical reactions of the halogen atoms achieve a valence shell octet by capturing or borrowing the eighth electron from another atom or molecule. Alkali metals that are Li, Na, K etc. (colored violet above) are also very reactive, but for opposite reason. In valence shell these atoms have only one electron and on losing this electron arrive at the lower shell valence octet. As result of this electron loss, these elements are generally encountered as cations (positively charged atoms).

The elements in the groups from 2 to 7 demonstrate the characteristic reactivates and bonding patterns that can in large part be rationalized by their electron configurations. Note that the hydrogen is unique. The location of hydrogen in periodic table should not suggest a kinship to the chemistry of the alkali metals and its role in the properties and structure of organic compounds is different or unique from the any other element.

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