Ionic Bonding

By: Scott Tobin and Tony Hoyeck

Ionic bonding is between a metal and a non-metal MgO

CaCl2

K2O

The Metal gives up one or more electrons to the non-metal to form a

bond

The number of electrons must equal the number of protons. If they

don’t you have to balance them.

NaCO3 Na2CO3

Sometimes, there can be a bond with a polyatomic ion like carbonate. A polyamic ion is

tow or more elements bonded together covalently.

Ex)Na2CO3

Ex)CaCO3

Electronegativity

The way the bonds form is that the ions are pulled together by electronegativity. The farther to the top right that you go the more electronegative the element is and the farther to the bottom left the less electronegative the element is.

http://www.youtube.com/watch?v=xTx_DWboEVs&feature=player_detailpage

A stable octet is when the element already has 8 electrons in it’s final shell. These elements are called noble gases Noble Gases don’t usually make bonds

because they already have a stable octet

The noble gases are…

HeliumNeon ArgonKrypton Xenon Radon

There are two types of atoms, positive and negative. When an atom loses an electron

while bonding it becomes positive and when an atom gains an electron while bonding it

becomes positive

Examples of ionic bonding used in everyday things

NaCl - Sodium Chloride - Table Salt

Na2CO3 - Sodium Bicarbonate - Backing Soda

NaF - Sodium Fluoride - Used in tooth paste

CaCl - Calcium Chloride – Used in Tofu

Ions

• The atoms that are involved in ionic bonds are called ions. These ions were once normal atoms until they lost or gained electrons due to an interaction with another atom. Atoms that lose electrons become positive and are called cations. Atoms that gain electrons become positive and are called anions.

Electron Dot Symbols

• Electron dot diagrams are a way of portraying the events of an ionic bond.

Physical Properties

• Here are some physical properties of ionic compounds.

• State at room temperature-solid

• Electric Conductivity- Solid:no Liquid:yes Aqueous: Yes(if soluble)

• Boiling and Melting Point-high

• Solubility in water-Often high

• Thermal Conductivity-Low

Solubility

• Ionic compounds dissolve very well in polar solvents such as water and ionic liquids. They also dissolve in alcohols, acetone and dimetyl sulfoxide. Ionic compounds tend to not dissolve in non polar solvents such as diethyl ether or petrol.

The Crystal Array

• When a compound is matched perfectly with a 1:1 ratio it forms a crystal array.

Bibliography

• Chemistry 11 Notebookhttp://en.wikipedia.org/wiki/Ionic_bonding

www.saskschools.ca/curr_content/chem30_05/appendix/glossary.htm

http://www.youtube.com/watch?v=xTx_DWboEVs&feature=player_detailpage

Chem11 adv notebook