Loading presentation...

Present Remotely

Send the link below via email or IM


Present to your audience

Start remote presentation

  • Invited audience members will follow you as you navigate and present
  • People invited to a presentation do not need a Prezi account
  • This link expires 10 minutes after you close the presentation
  • A maximum of 30 users can follow your presentation
  • Learn more about this feature in our knowledge base article

Do you really want to delete this prezi?

Neither you, nor the coeditors you shared it with will be able to recover it again.


Make your likes visible on Facebook?

Connect your Facebook account to Prezi and let your likes appear on your timeline.
You can change this under Settings & Account at any time.

No, thanks

Alloys & Metallic Bonding

Explanation of how metallic bonds are formed and the usefulness of alloys

Maria Heininger

on 30 March 2015

Comments (0)

Please log in to add your comment.

Report abuse

Transcript of Alloys & Metallic Bonding

Metallic bonds are formed when the
valance electrons
of a metal atom become
or detached from the rest of the atom.
How Metallic Bonds
are formed...

How are atoms in a metal held together?
How are metallic bonds formed?
Common Alloys
Main Points of Metallic Bonding
Why are alloys more useful than pure metals?
All metal atoms are held together through
metallic bonds

Metallic bonds can be between
atoms of the same metals
or between
atoms of different metals.
Valance electrons in metals are

(free to move around & not connected to the cation)
Alloys are chemical substances where the
main component is a metal

However, the metal is
mixed (not bonded!)
with other elements.
Brass - 67% copper, 33% zinc

Bronze - 60% copper, 39% tin, 1% aluminum & other elements

Steel - 98% iron, 1% carbon, 1% other
Has different properties then that of the pure metal (enhances the properties)
Does not rust as easily
Harder to break or damage
Light weight
Metal cations are held together via a

Metals have a
crystalline structure
due to the organization of their metal cations. This is why metals are relatively hard (not easy to break).
However, metals are
flexible, malleable & ductile
because the

cations in the
sea of electrons
are able to move around and not locked into place.

Delocalized electrons - free to move around between the stable cations
Stable cations
Sea of Electrons
Properties of Pure Metals
rust easily
very soft (malleable)
Do these sound like ideal properties for making something out of metal?
Look at the list of everyday items:

Baseball bats
Kitchen appliances
While these are all made from metals, are they PURE metals?
14 karat gold - NOT PURE GOLD!

59% Gold
14% Silver
23% Copper
3.5% Zinc
0.5% Cobalt
Sterling silver - NOT PURE SILVER!

92.5% Silver
7.5% Copper
The Structure of
Pure Metals vs. Alloys
The atoms in pure metals are very
, which allows them to easily
slide over one another
when a force is applied
The atoms in an alloy are
due to the mixture of the different metals and elements. When a force is applied, the atoms are
NOT able to slide over one another
. This makes the alloy extremely strong.
How are alloys made?
Alloys can be made 2 different ways:

Melting each metal and then mixing them together.

Taking a solid piece of metal, chemically coating it with a thin layer of the second metal (callled plating) and heating until they physically combine.
Full transcript