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Atomic Bonding - 8th grade
Transcript of Atomic Bonding - 8th grade
Page 15 in ISN
(page 174-202 in textbook)
By: Mr. Begoyan
Electrons (e-) in an element are arranged into orbits.
The first orbit can only hold
, while every other orbital can hold up to
It is the
of every element (except noble gasses), to have
Electrons in the outermost shells are called
They are the only e- that are available for bonding.
Lewis Dot Structure
The symbol of the element is surrounded just by the
Also known as the
electron dot diagram.
Every element, besides inert gasses, has incomplete final shells.
They complete their shells by swapping or sharing electrons.
There are two types of bonds:
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-).
Ionic bonds almost always take place between a
Covalent bonds almost always take place between two
, 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 do not have ordered crystalline structures, and are thus softer and have lower melting points than ionic compounds.
In these covalent bonds, the e- is
(mostly between 2
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.
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
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!