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Lesson 4 | Ionic and Covalent Compounds - Coggle Diagram
Lesson 4 | Ionic and Covalent Compounds
Ionic Compounds
These are formed when a metal, which tends to lose electrons, bonds with a nonmetal, which tends to receive electrons, because of the electrostatic force between the two
Covalent Compounds
These are formed when two nonmetals share electrons from their outer shell in order to get a full valence shell in both atoms
The bonds in these compounds are stronger than the bonds in ionic compounds.
Naming
Ionic Bonds
Name of the metal always comes first, then the nonmetal, with the ending -ide rather than its normal (e.g. Sodium ChlorIDE)
Covalent Bonds
Simple atoms
The element that is furthest left or up the periodic goes first, with the root of how many of that element there is (e.g. mono, di, tri, tetra, penta, etc.)
The other element goes after, with the same root, and ending in -ide
Complex atoms (carbonate, nitrate, etc.)
Same as normally, but no -ide ending
Forming compound formulae
Lewis Dot Structure
A structure that is used to represent covalent bonds
You only draw valence shell of electron
Cross Diagram (Ionic bonds)
If an ionic bond is made, you first figure out the amount of valence electrons the atom would receive or give away in order to become an ion, then do it for both atoms in a compound, then cross both charges to the other atom's subscript
If there is a common factor or simpler ratio to achieve a common charge, then you must simplify it as much as possible