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https://www. texasgateway. org/resource/ionic-and-covalent-bon ding

I. Ionic Bonding
An is formed when the atom of an element some of its electrons and reaches a electron formation. During the bond, one or more atoms electrons; the other atoms them in order to produce a noble gas electron configuration. The element that loses the electrons becomes charged, and the element that gains the electrons becomes charge
One ionic compound is referred to as a . Ionic compounds are often called .
Ionic compounds must have an and a .

Sketch a diagram to show the transfer of e- and the bond between magnesium and oxygen.

List the five properties of ionic bonds in compounds: Click on each property for more information.
1. 2.
3.
4.
5.

II. COVALENT BONDING
Covalent bonding most commonly occurs between .

How many electrons does oxygen need to fill its outer energy level?
How many electrons does carbon need to fill its outer energy level?
In the case of carbon dioxide, two oxygen atoms can bond with carbon and share electrons such that all atoms have a full outer energy level. Show this bond in the box below:

The most element in the compound has the greatest strength in holding the electrons that are shared. Think of a game of tug of war when one of the participants is slightly stronger than the other. The rope is being pulled closer to that end. This type of sharing in a compound is referred to as a bond. If the elements in a covalent compound are the there is an sharing of electrons. This equal sharing of electrons is referred to as covalent compounds.
A is the smallest unit of a covalent compound.

List five properties of covalent compounds:
1. 2.
3.
4. 5.

III. METALLIC BONDING
https://www. texasgateway. org/resource/chemical-bonding-metal lic-bonds

A metal is an element or compound with high electrical conductivity usually has a shiny luster, and it can be melted, hammered into sheets, or drawn into wires. In a metal, atoms atoms lose electrons easily and form positive ions or cations. Those ions are surrounded by electrons, which roam the metal structure. The "roaming" electrons are called delocalized electrons.
If you could look at a metal at a molecular level, you would see a sea or of negative electrons randomly buzzing around the positive charged metal ions. This is because of the metal's inability to hold onto its outermost

Research items/substances in your home. Classify them as ionic, covalent or metallic.