The Internet belongs to everyone. Let’s keep it that way.

Protect Net Neutrality
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.


Atomic Bonding - 8th grade

No description

William Begoyan

on 5 October 2016

Comments (0)

Please log in to add your comment.

Report abuse

Transcript of Atomic Bonding - 8th grade

Atomic Bonding
Page 15 in ISN
(page 174-202 in textbook)

By: Mr. Begoyan
Electron Orbits
Electrons (e-) in an element are arranged into orbits.
The first orbit can only hold
2 e-
, while every other orbital can hold up to
8 e-
It is the
of every element (except noble gasses), to have
complete orbitals
Valence Electrons
Electrons in the outermost shells are called
valence electrons.
They are the only e- that are available for bonding.
Lewis Dot Structure
The symbol of the element is surrounded just by the
valence electrons.
Also known as the
electron dot diagram.
Chemical Bonds
Every element, besides inert gasses, has incomplete final shells.
They complete their shells by swapping or sharing electrons.
There are two types of bonds:
Ionic Bonding
One way an atom can reach stability is by gaining or dropping e-.
Elements with 3 or fewer valance e- will drop, while elements with 5-7 valance e- will gain electrons.
When an element loses e-, it becomes more positive, and when e- are gained, the element becomes more negative.
As e- are transferred, and elements gain a charge, they are called ions (ex: Lithium ion).
Ions with opposite charges attract each other, thus forming ionic bonds (Na+ and Cl-).
Covalent Bonding
Ionic bonds almost always take place between a


and a

Covalent bonds almost always take place between two
Ions form
ionic compounds
, which usually have a crystalline structure.
Negative ions are called
, and receive an
Ex: Chlorine becomes Chlor
Positive ions are called
, and have
added after their name.
Ex: Lithium becomes Lithium
Another way atoms can reach stability is by sharing e-.
Elements with 4 valence e- almost always share.
Compounds formed by covalent bonding are called
molecular compounds.
Molecular compounds do not have ordered crystalline structures, and are thus softer and have lower melting points than ionic compounds.
Non-Polar Covalent
Polar Covalent
In these covalent bonds, the e- is
shared equally
(mostly between 2
identical elements
The e- is not attracted to one nucleus more than the other.
In these covalent bonds, the e- is
not shared equally
One of the elements will have a larger nucleus, which means more protons, which means stronger positive pull.
The e- is attracted to the larger element.
Metallic Bonding
Solid metals consist of cations surrounded by a sea of moving electrons.
The free flowing e- allow metals to have all of their properties, including conductivity.
The metallic ions can easily shift position, allowing for malleability and ductility.
are formed when a metal and another element are melted together. The resulting combination greatly alters the original metal.

Elements can share more than one e- in a covalent bond.
electrons is called a
double bond
, sharing
is called a
Weird + Complex
In a Lewis structure, single bonds are designated as 1 line (2 e-), double bonds as 2 lines (4 e-), and triple bonds as 3 lines (6 e-).
How many e- can each orbital hold?
What is the goal of every element?
What are valence electrons?
Ionic bonds always take place between.....?
Describe a Lewis Dot Structure.
How does an Ionic Bond work?
What are the two types of ions and what do we call them?
Covalent bonds always take place between.....?
How does a Covalent Bond work?
What is the difference between the 2 types of covalent bonds?
How does a Metallic Bond work?
Describe double and triple bonds.
What is an alloy?
On page 16, describe the different types of bonds. Use of visuals and colors are required!
Full transcript