![]() The stability of lewis structure can be checked by using a concept of formal charge. Now you have come to the final step in which you have to check the stability of lewis structure of ClO3- ion. Step 6: Check the stability of lewis structure Total valence electrons in ClO 3 – ion = valence electrons given by 1 chlorine atom valence electrons given by 3 oxygen atoms 1 more electron is added due to 1 negative charge = 7 6(3) 1 = 26. You can see the 6 valence electrons present in the oxygen atom as shown in the above image. Hence the valence electrons present in oxygen is 6. Oxygen is group 16 element on the periodic table. → Valence electrons given by oxygen atom: You can see the 7 valence electrons present in the chlorine atom as shown in the above image. Hence the valence electrons present in chlorine is 7. ![]() → Valence electrons given by chlorine atom:Ĭhlorine is group 17 element on the periodic table. Here, I’ll tell you how you can easily find the valence electrons of chlorine as well as oxygen using a periodic table. (Valence electrons are the electrons that are present in the outermost orbit of any atom.) In order to find the total valence electrons in ClO3- ion (chlorate ion), first of all you should know the valence electrons present in chlorine atom as well as oxygen atom. The shared electrons are not located in a fixed position between the nuclei.Step 1: Find the total valence electrons in ClO3- ion In Lewis structures the bonding pair of electrons is usually displayed as a line, and the unshared electrons as dots: When two chlorine atoms covalently bond to form \(Cl_2Cl_2\), the following sharing of electrons occurs:Įach chlorine atom shared the bonding pair of electrons and achieves the electron configuration of the noble gas argon. In a sense, it has the electron configuration of the noble gas helium. The shared pair of electrons provides each hydrogen atom with two electrons in its valence shell (the 1 s) orbital. The diatomic hydrogen molecule (H 2) is the simplest model of a covalent bond, and is represented in Lewis structures as: Although it is said that atoms share electrons when they form covalent bonds, they do not usually share the electrons equally. Nonmetals will readily form covalent bonds with other nonmetals in order to obtain stability, and can form anywhere between one to three covalent bonds with other nonmetals depending on how many valence electrons they posses. By sharing their outer most (valence) electrons, atoms can fill up their outer electron shell and gain stability. Atoms will covalently bond with other atoms in order to gain more stability, which is gained by forming a full electron shell. The arrow indicates the transfer of the electron from sodium to chlorine to form the Na metal ion and the Cl - chloride ionĬovalent bonding occurs when pairs of electrons are shared by atoms. The Lewis Structure of this reaction is (here we will consider one chlorine atom, rather than Cl 2) is: ![]() Thus the chlorine gains an electron from the sodium atom. The chlorine has a high affinity for electrons, and the sodium has a low ionization potential. ![]()
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