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A step-by-step explanation of how to draw the NaCl Lewis Dot Structure. For the NaCl Lewis structure, calculate the total number of valence electrons for the NaCl molecule. Since Na is a metal and Cl is a non-metal we have an ionic compound for the Lewis dot structure for NaCl. This means that the metal (Na) will transfer its electron to the non-metal (Cl). Sodium has 1 valence electron and there are 7 valence electrons for Cl. Be sure to include the charge on the bonded atoms and to place brackets around the Chlorine atom in the NaCl Lewis structure. Get more chemistry help at http://www.thegeoexchange.org/chemistry/bonding/
Practice drawing Lewis Structures with answers and explanation. The video covers the basic Lewis structures for a general chemistry class. The five steps are: 1. Find the total valence electrons for the molecule. 2. Put the least electronegative atom in the center. Note: Hydrogen (H) always goes outside. 3. Put two electrons between atoms to form a chemical bond. 4. Complete octets on outside atoms. 5. If central atom does not have an octet, move electrons from outer atoms to form double or triple bonds. Lewis Structures are also called Electron Dot Structures/Diagrams and Lewis Dot Structures. Get more practice at http://www.thegeoexchange.org/chemistry/bonding --- Drawing done in Inkscape and captured with Camtasia Studio on a Dell Dimension laptop. Audio recording using a Yeti Blue microphone.
Examples of writing formulas from names of compounds (both ionic and molecular). Part 1 of 2 Dinitrogen pentoxide, manganese (II) hydroxide, Ammonium acetate, Lead (IV) carbonate, Selenium dioxide, Nitrogen monoxide, Calcium sulfate, Potassium fluoride, Chromium (III) oxide, Sodium nitrate, Beryllium sulfite, Barium cyanide, Palladium (IV) acetate, Iodine monofluoride
Subject : Chemistry Courses name : IIT PAL Name of Presenter : Prof. S. Sankararaman Keyword : Swayam Prabha
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A step-by-step explanation of how to draw the BaBr2 Lewis Dot Structure.
For BaBr2 we have an ionic compound and we need to take that into account when we draw the Lewis Structure. We’ll first draw the metal and put it in brackets with its charge on the outside (video: finding ionic charge: https://youtu.be/M22YQ1hHhEY).
Next, we'll draw the Lewis Structure for the Br- ion and add brackets. We put the two ions together to complete the Lewis structure for BaBr2. Note that BaBr2 is also called Barium bromide.
For a complete tutorial on drawing Lewis Structures, see my video: https://youtu.be/1ZlnzyHahvo
For more practice, see https://youtu.be/DQclmBeIKTc
To learn to find the valence electrons: https://youtu.be/VBp7mKdcrDk
Note that is it more common to draw Lewis Structures for covalent (molecular) compounds where valance electrons are shared. In the case of ionic compounds, where we have a metal bonded to a non-metal (or group of non-metals), the Lewis diagram represents a formula unit. Many of these formula units make up a crystal lattice. So when we talk about the structure for BaBr2 we think of it together with other BaBr2 formula units in a crystal (NaCl is a good example of this: https://en.wikipedia.org/wiki/Sodium_chloride).
Get more chemistry help at http://www.thegeoexchange.org/chemistry/bonding
Drawing/writing done in InkScape. Screen capture done with Camtasia Studio 4.0. Done on a Dell Dimension laptop computer with a Wacom digital tablet (Bamboo).