LESSON PLAN
Teacher: Howard Zulu Mr.
Date:……………Class. 10
Time: …………………………..
Duration: 80 MINUTES
Subject: CHEMISTRY
Topic: CHEMICAL BONDING
Sub-Topic: Chemical bonding-Metallic bonding
Rationale: This is the 3rd lesson in the series of 6 lesson to cover this topic. The learner will learn
about metallic bonding and properties of metallic .This will grow their appreciation and
awareness for metals and their properties as well as their use in every day lives. The method
used are demonstration, discussion, video demonstration, answer and question.
Lesson outcomes:


Describe metallic bonding.
Describe the electrical conductivity and ductility of metals.
References: IGCSE chemistry, Longman chemistry, Progress in science,
Teaching Resources/Aids: Periodic table, Chart, white board marker
TIME
LESSON CONTENT
LESON DEVELOPMENT
METALLIC BONDING
 Metallic bonding is the attraction between
the positively charged metal ions and the
free electrons in a metallic lattice.\
 In metals, the atoms are packed tightly
together in a regular lattice.
 The tight packing allows outer electrons to
separate from their atoms.
 The result is a lattice of ions in a ‘sea’ of
electrons that are free to move
 The electrons are free to move anywhere in
the metallic lattice. The electrons are said to
be delocalized.
 Copper atoms, for example, lose two single
electron from the outer most shell. When a
large number of sodium atoms lose these
electrons, the result is many free electron
NB:The metallic bond is the attraction between
metal ions and free electrons.
 It is the same with all metals. The ions sit in a
lattice, held together by their strong
attraction to the free electrons. And because
the ions are in a regular pattern, metals are
crystalline
METHODOLOGY
TEACHER ACTIVITY
LEARNER ACTIVITY

The teacher will
define metallic
bonding.

Learner
will
participat
e orally.

Techer will
engage learner
in comparing
the forces
attraction in
metallic bond
and forces of
attractions in a
covalent and
ionic bond

Learners
will
participat
e by
answering
and
asking
question
.
NB:The copper ions are held together by their
attraction to the free electrons between them. The
strong forces
of attraction
are called
metallic
bonds.
METALLIC PROPERTIES
 Metals usually have high melting points. That
is because it takes a lot of heat energy to
break up the lattice, with its strong metallic
bonds. Copper melts at 1083 8C, and nickel
at 1455 8C. (But there are exceptions.
Sodium melts at only 98 8C, for example.
And mercury melts at –39 8C, so it is a liquid
at room temperature.)
 Metals are malleable and ductile. Malleable
means they can be bent and pressed into
shape. Ductile means they can be drawn out
into wires. This is because the layers can
slide over each other.
 Metals are good conductors of heat.That is
because the free electrons take in heat
energy, which makes them move faster.
They quickly transfer the heat through the
metal structure:

Teacher will
explain the
diagrammatic
representation
of the metal.
Use copper

Learners
will
participat
e by
answering
and
asking
question

Teacher will
explain the
metallic
properties due
metallic bond.

Learners
will
participat
e by
asking
and
answering
questions

Teacher will
engage
learners in
comparing the
characteristic
of metallic
bond, of ionic
and covalent
compound.

Learners
will
participat
e by
answering
and
asking
question
.
CONCLUSION: The teacher will conclude the lesson by running through the main points and
giving an exercise.
EVALUATION:……………………………………………………………………………………………………
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