DSE Chemistry: Chemical Bonding — Tutor Lesson Plan (ionic, covalent, metallic)

2026-10-27

Tutor lesson-prep guides · Secondary chemistry

Students can name three bond types but cannot explain why salt melts high and sugar low. One question organises the lesson: what is holding what together?

Objectives — the student can predict the bond type from element positions, write ionic formulas from charges, and link bond type to melting point and conductivity.

01 Prerequisites (3-minute check)

If any of these fails, fix it before the lesson starts.

Skill	Quick check	Pass mark
Arrangements	Sodium and chlorine	2,8,1 and 2,8,7
Ions	How to write sodium and chloride ions	Na⁺ and Cl⁻
Table sides	Where metals sit	Left, non-metals right

02 Lesson flow (60 minutes)

Time	Stage	Tutor does	Student does
0-10 min	Three bonds	Metal plus non-metal is ionic	Sort five compounds
10-26 min	Ionic	Electron transfer and attraction	Write three formulas
26-42 min	Covalent	Shared pairs	Draw two structures
42-54 min	Metallic	Electron sea, malleability	Explain two observations
54-57 min	Properties	Melting point, conductivity, solubility	Complete a table
57-60 min	Exit check	Three questions marked	Finish alone

03 Teaching script (read it out)

Scene 1: Read the elements before the bond

Metal plus non-metal gives ionic bonding, as in NaCl and MgO.
Non-metal plus non-metal gives covalent bonding, as in water and carbon dioxide.
Metal plus metal gives metallic bonding.

Student sorts KBr, CH4 and Al.

Scene 2: Ionic bonding: transfer then attract

Sodium gives chlorine one electron, so Na⁺ and Cl⁻ attract in a giant lattice.
Formulas balance charge: Mg²⁺ with Cl⁻ gives MgCl2.

Note: write the ions first, then cross the charges, then simplify.

Scene 3: Bond type sets the properties

Ionic: high melting point, conducts when molten or dissolved, not when solid.
Simple molecular: low melting point, no conduction.
Metallic: conducts and is malleable because the electron sea moves with the layers.

Student explains why copper draws into wire and salt shatters.

04 Question types and worked steps

Type	Example	Steps	Answer
Bond type	KBr	Metal plus non-metal	Ionic
Formula	Mg²⁺ and Cl⁻	Balance charge	MgCl2
Melting point	NaCl against water	Lattice against intermolecular forces	NaCl much higher
Conductivity	Solid NaCl	Ions cannot move	Does not conduct

Sanity check (teach this): Formulas must balance charge: MgO is one to one because +2 meets -2, never Mg2O2.

05 Independent practice (3 questions)

Question	Answer	What to watch
Formula for Ca²⁺ and O²⁻	CaO	Charge balance
Bond type in CO2	Covalent	Non-metal plus non-metal
Why metals are malleable	Layers slide, electron sea still binds	Metallic bonding

06 Common mistakes and what to say

Mistake	Student writes	Say this
Covalent whenever a non-metal appears	calls NaCl covalent	Check for a metal first.
Formula not simplified	Mg2O2	Simplify to MgO.
Melting point confused with hardness	assumes molecular means soft	Low melting point is not softness.
Conduction rule missed	says solid NaCl conducts	Only molten or dissolved.

07 Homework (paper, section and question numbers)

Secondary chemistry chapter index — Use the three questions on this page

08 Exit check (last 5 minutes)

Question	Answer	Decision
Formula for Ca²⁺ and O²⁻	CaO	All right: move to acids
Bond type in CO2	Covalent	One wrong: re-teach sorting
Why metals are malleable	Layers slide, sea still binds	Two wrong: repeat scene 3

09 Tutor FAQ

Memorise many formulas?

No; charge balance gives them.

Giant covalent structures?

Know diamond and graphite for DSE.

Link to acids?

Most ionic compounds dissolve, so acid reactions happen in water.

Find a tutor — free

A TutorZone lesson-prep guide. Written by the TutorZone team; questions and lesson flow are original and are not taken from any school or publisher material.