Transcript Ionic Bonding

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…
Helium
Neon
Argon
Krypton
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 Notebook
http://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