Advanced searches left 3/3
Search only database of 8 mil and more summaries

Chlorine Dot Diagram

Summarized by PlexPage
Last Updated: 19 October 2020

* If you want to update the article please login/register

General | Latest Info

During chemical bonding, it is valence electrons which move amongst different atoms. In order to keep track of the valence of electrons for each atom and how they may be shared in bonding, we use the Lewis Dot Structure for Atoms and molecules. In this approach, we represent valence electrons as dots around the element symbol. For example, oxygen has 6 valence electrons, so we write the symbol O for oxygen and surround it with 6 dots: unpaired electrons are represented as single dots, and paired electrons as double dots. Placement of single or double dots around symbol is not critical. Alternatively, we can represent paired electrons as line. That is, we replace double dots as shown below: let's consider other examples. Sodium atom has 11 electrons, but only one is valence electron. The other 10 are inside close shell with Neon electron configuration. Thus, we draw the Lewis Structure for Sodium atom as symbol Na with a single dot: chlorine atom has 17 electrons, but only 7 of these are valence electrons. Thus, we draw the Lewis Structure as: in Ionic Bonds valence electrons are completely transfer. Thus, we write Lewis Structure for NaCl as: as you can see, Chlorine is now surrounded by 8 electrons in N = 3 shell and Sodium has lost its one valence electron in N = 3 shell. Of course, sodium, is still surrounded by 8 electrons of N = 2 shell, but we do not show electrons in inner close shells. For period 2 elements, where all valence electrons of an atom are in s and p orbitals, we find that the Lewis Dot Structure of molecules will often follow the Octet Rule: Octet Rule - Atoms tend to gain, lose, or share electrons until they are surrounded by eight electrons. Using Lewis Dot structures and Octet Rule, we can predict and represent the electronic structure of covalently bonded molecules. For example, when two Chlorine atoms, each with 7 valence electrons, come together to form a diatomic Chlorine molecule, Lewis Structure shows that there will be sharing of two electrons between two Chlorine atoms, which allows both Chlorine to be surrounded by 8 electrons. Of course, hydrogen is period 1 element, with only 1s Orbital, so it has a maximum of two electrons allowed in its valence shell. When two hydrogen atoms come together into a diatomic H 2 molecule, the Lewis Structure shows that there will be sharing of two electrons between two hydrogen, allowing both hydrogen to be surrounded by a closed N = 1 shell of 2 electrons: We can represent the electronic structure and reaction of hydrogen and Chlorine Atoms to form HCl with Lewis structures: for diatomic oxygen, Lewis Dot Structure predict double bond. While the Lewis diagram correctly predicts that there is a double bond between o atoms, it incorrectly predicts that all valence electrons are pair.

* Please keep in mind that all text is machine-generated, we do not bear any responsibility, and you should always get advice from professionals before taking any actions.

* Please keep in mind that all text is machine-generated, we do not bear any responsibility, and you should always get advice from professionals before taking any actions

logo

Plex.page is an Online Knowledge, where all the summaries are written by a machine. We aim to collect all the knowledge the World Wide Web has to offer.

Partners:
Nvidia inception logo

© All rights reserved
2021 made by Algoritmi Vision Inc.

If you believe that any of the summaries on our website lead to misinformation, don't hesitate to contact us. We will immediately review it and remove the summaries if necessary.

If your domain is listed as one of the sources on any summary, you can consider participating in the "Online Knowledge" program, if you want to proceed, please follow these instructions to apply.
However, if you still want us to remove all links leading to your domain from Plex.page and never use your website as a source, please follow these instructions.