Chemical Bonding
Just a quick definition.

Electronegativity: The amount of attraction
an element has for electrons when forming a
Chemical Bond.
Metals & Non-Metals
Properties of Metals:

Typically:
 Good
conductors.
 Malleable
& pliable.
 High
melting point.
 Solid
at room temperature (Hg being an exception).
 Low
electronegativity.
Properties of Non-Metals:

Typically:
 Poor
conductors.
 Brittle
 Low
melting point.
 Liquid
 High
& fragile.
or gaseous at room temperature.
electronegativity.
Side-note: Metalloids

Metalloids share characteristics of both metals and nonmetals.

They are best known as semiconductors, most notably,
Silicon (symbol Si).
How they appear on the Periodic Table:
Metals vs. Non-metals in
Chemical Bonding

Metals and non-metals tend to behave differently when
they form chemical bonds. This is due mostly to the
differing electronegativity.
Covalent Bonds: Sharing is Caring

Covalent Bonds: When two bound molecules share
electrons

However, they do not always share equally.

In a polar covalent bond, electrons are more attracted
to the element with the higher electronegativity.

In a non-polar covalent bond, electrons are equally
attracted to the two elements.

They must have equal (or close to equal) electronegativity.
An important note…

The most equal sharing of electrons comes from atoms
that are the same element.
A couple examples:
 Polar
Covalent:
 Water.
The
“Universal” Solvent.
A couple examples:

(Nitrogen) N2

(Carbon Dioxide) CO2
Ionic Bonds: All for me, myself, and I.

Occur when electronegativity of the two elements is
very different.

Occurs most often between a metal and a non-metal.
A common example: Salt
Where would the electrons want to go?
Hydrogen Bonds: The Honorary Bonds.

Water molecules are attracted to each other because
they are polar.

Forms a very weak attraction among molecules.