1
2

Ionic- where atoms give or take
electrons to become ions (cations and
anions).
› An attraction between cations and anions
(positive attracted to negative).
› Always between a metal and non-metal

Covalent-where atoms share electrons
to reach an octet
› Always between non-metals
3
Between metals and non-metals
 Contain positive and negative ions
(strong force of attraction)
 Compounds w/ ionic bonds dissolve
quickly in water
 When melted or dissolved ionic
compounds tend to conduct electricity
 Ionic bonds have a high melting and
boiling point

5
Ionic Bonding
Look at the following diagram with regards to
sodium (Na) and chlorine (Cl)
Each ion needs to have an octet in their last shell.
What must each do to fulfill the octet rule?
7
Sodium gives up its valence e- and
becomes the cation (+1 charge).
 Chlorine has 7 e- and needs 1. It takes
sodium’s e- that it is getting rid of. When
chlorine takes it is becomes the anion (-1
charge).

8
The positively charged sodium ion and the negatively
charged chloride ion will be attracted to each other and
form an ionic bond.
Na +
Cl -
The ionic bond is due to the attractive forces
between the now positively charged sodium & the
negatively charged chloride.
Both atoms are now…
9
Salts form very ordered structures as seen
above and we call them crystals
(network of molecules).
10
1. Draw the lewis dot structures of each
2. Show the transfer of electrons with arrows
Na,F
 Ca, Cl
 Al, F
 Ca, O

11

Recall Question- What is an ionic bond?

Recall Question- Why are ionic bonds
necessary?

Recall Question- How are ionic bonds
formed?
12
Between non-metals (forming molecules)
 Contain neutral molecules (weak force
of attraction)
 When melted or dissolved, they do not
conduct electricity
 Lower melting and boiling points

13
Draw the Lewis structure for carbon and for
hydrogen. How can they share electrons so
that all the atoms have an octet?
Hint: You may need more than one hydrogen
There are several ways to represent molecules.
This molecule is called methane. It is similar to
gasoline in your car.
15
Different types of molecules containing carbon.
Notice the single, double and triple bonds.
What do you think is the difference?
16
Single bond-two atoms share two electrons
 Double bond-two atoms share four electrons
 Triple bond-two atoms share six electrons

17
Single Covalent Bond- chemical
bond resulting from sharing of an
electron pair between two atoms.
Double Covalent Bond- chemical
bond resulting from sharing of two
electron pairs between two atoms.
Triple Covalent Bond-chemical
bond resulting from sharing of
three electron pairs between two
atoms.
18
19
Covalent bonded
Molecules.
20
H2O
NH3
CH4
21

Recall Question- What is a covalent
bond?

Recall Question- Why are covalent
bonds necessary?

Recall Question- How are covalent
bonds formed?
22

Each of you will be given two element cards and a data
sheet.
› Those cards will contain “personal” information about you.

Each student will sit down at a station with their data sheet
and information cards.

When I say start you will have 2 minutes to have a
conversation to see if you are compatible.

From the information you acquire complete the data sheet.

When the bell rings move to the right to the next station and
repeat until the activity is over.

What was easy about the activity?

What was hard about the activity?

Were you able to make multiple
compounds or just one?