Bonding Basics
Back to Basics
_______________________ are pure substances that cannot be broken down by chemical or physical means. They
are listed on the ______________________________ in order of _____________________________. They
have a unique one or two letter ____________________. The _____________________ letter is always
____________________________.
_____________________ are substances made of 2 or more elements __________________ combined in a
specific ___________________.
Examples: water, carbon dioxide, trinitrotoluene, _______________________.
The smallest unit of a compound is a_____________________
We represent molecules/ compounds with a _____________________________.The most well know example
is_____________________.
What does this chemical formula tells us about a molecule of water?
A water molecule is made of:
________ atoms of hydrogen
________ atom of oxygen
How did you know this?
What if you saw 2 H20?
Words to Know:
_______________________- just like in math. A number in front of the formula that tells you how many
________________________ you have.
_______________________ - a little number to the left of an element symbol that tells you how ___________ of
that element are in the molecule.
Parentheses - __________________ around groups of ______________ that always stay together in a group.
How to Read a chemical Formula:
Coefficients show
how many
molecules you have.
2NH3
Subscripts show how
many of each type of
atom you have.
There are ______________ molecules of ammonia.
Each ammonia molecule has:
__________atoms of nitrogen ___________ atoms of hydrogen.
Totals
__________atoms of nitrogen ___________ atoms of hydrogen. _____________ atoms
4Al2(SO4)3
Lewis Dot Diagrams
Show the number of _________________________________ only.
They use dots and the element symbol. Electrons are shown in __________________________.
You try:
Oxygen
Sodium
Germanium
Nitrogen
IONS
These are a __________________ atom that has lost or gained one or more electrons.
If an atom loses electrons, it becomes a ___________ ion because it now has more protons than electrons. If an atom gains one or more electrons, it becomes a negative ion.
Remember:
Atoms want ________ electrons in their valence orbital.
Atoms with less than __________valence electrons will try to give up an electron. With more than 4 will try to ______________ electrons
Some ions and there charges are:
+
+2
Li ,
Ca ,
Cl ,
S
-2
Polyatomic Ions
Ions that are made of ______________ than one atom.
The prefix poly- means ____________________.
These can be the atoms you see in parentheses, but not always. Learn to recognize them.
Examples: Ammonium: NH 4+
Hydroxide: OH - Nitrate: NO 3
Sulfate: SO 24
Chemical Bonds
Type of Bond
Ionic
Covalent
Metallic
Who?
How?
Example
Drawing