CHEMICAL BOND
Chapter 5 Form 4 Chemistry KSSM
Prepared by: Pn. Nurulkamilah binti Khairir
Chemical
Bond
5.1
Basics of Compound Formation
5.2
Ionic Bond
5.3
Covalent Bond
5.4
Hydrogen Bond
5.5
Dative Bond
5.6
Metallic Bond
5.7
Properties of Ionic Compounds and
Covalent Compound
5.1 Basics of Compound Formation
Learning Standard
At the end of the lesson, pupils are able to
5.1.1 Explain the basics of compound formation
Video of Formation of Compounds
Ionic bond
Covalent bond
5.1 Basics of Compound Formation
Noble gases exists as monoatomic gases
and are not reactive chemically
Because they have achieved stable duplet
or octet electron arrangement
However, for atoms of other elements,
stability of electron arrangement can be
achieved by transferring or sharing of
electrons
Chemical bonds are formed when electron
transfer or electron sharing takes place
There are two types of chemical bonds;
ionic bond and covalent bond and only
involve the valence electrons
5.1 Basics of Compound Formation
5.1 Basics of Compound Formation
5.1 Basics of Compound Formation
Test Yourself 5.1
Page 111 Chemistry Form 4 KSSM Text Book
5.2 Ionic Bond
Learning Standard
At the end of the lesson, pupils are able to
5.2.1 Explain with examples the formation of ionic bond
5.2 Ionic Bond
5.2 Ionic Bond
Metal atom
donates
valence
electron to
form cation
Non-metal
atom receives
electron to
form anion
5.2 Ionic Bond
5.2 Ionic Bond
5.2 Ionic Bond
5.2 Ionic Bond
5.2 Ionic Bond – Magnesium oxide, MgO
Magnesium atom has 12 electrons.
The electron arrangement for
magnesium atom is 2.8.2.
Oxygen atom has 8 electrons. The
electron arrangement for oxygen
atom is 2.6.
Mg
O
5.2 Ionic Bond – Magnesium oxide, MgO
Magnesium atom donates 2 electrons
to form magnesium ion, Mg2+
To achieve stable octet electron
arrangement
Oxygen atom receives 2 electrons
to form oxide ion, O2To achieve stable octet electron
arrangement
2+
Mg
Mg 🡪 Mg2+ + 2e-
2-
O
O + 2e- 🡪 O2-
5.2 Ionic Bond – Magnesium oxide, MgO
Magnesium ion, Mg2+ ion and oxide ion, O2- are attracted by strong electrostatic
force. A compound magnesium oxide, MgO is formed
2+
Mg
2-
O
5.2 Ionic Bond – Sodium chloride, NaCl
Sodium atom has 11 electrons. The
electron arrangement for sodium
atom is 2.8.1.
Na
Chlorine atom has 17 electrons.
The electron arrangement for
chlorine atom is 2.8.7.
Cl
5.2 Ionic Bond – Sodium chloride, NaCl
Sodium atom donates 1 electron to
form sodium ion, Na+
To achieve stable octet electron
arrangement
Chlorine atom receives 1 electron to
form chloride ion, ClTo achieve stable octet electron
arrangement
_
+
Na
Na 🡪 Na+ + e-
Cl
Cl + e- 🡪 Cl-
5.2 Ionic Bond – Sodium chloride, NaCl
Sodium ion, Na+ and chloride ion, Cl- are attracted by strong electrostatic force. A
compound sodium chloride, NaCl is formed
_
+
Na
Cl
5.2 Ionic Bond – Sodium oxide, Na2O
Sodium atom has 11 electrons. The
electron arrangement for sodium
atom is 2.8.1.
Na
Oxygen atom has 8 electrons. The
electron arrangement for oxygen
atom is 2.6.
O
5.2 Ionic Bond – Sodium oxide, Na2O
Sodium atom donates 1 electron to
form sodium ion, Na+
To achieve stable octet electron
arrangement
Oxygen atom receives 2 electrons
to form oxide ion, O2To achieve stable octet electron
arrangement
+
+
2-
Na
O
Na 🡪 Na+ + e-
O + 2e- 🡪 O2-
Na
5.2 Ionic Bond – Sodium oxide, Na2O
Sodium ion, Na+ and oxide ion, O2- are attracted by strong electrostatic force. A
compound sodium oxide, Na2O is formed
+
Na
2-
O
+
Na
Test Yourself 5.2
Page 114 Chemistry Form 4 KSSM Text Book
Test Yourself 5.2
5.3 Covalent Bond
Learning Standard
At the end of the lesson, pupils are able to
5.3.1 Explain with examples the formation of covalent
bond
5.3.2 Compare ionic bond and covalent bond
5.3 Covalent Bond
Diamond is the hardest substances
in the world
The property of diamond is caused
by the formation of covalent bond
between carbon atoms
5.3 Covalent Bond
Non-metal
Non-metal
Covalent bonds are formed when non-metal atoms share their electrons
to achieve a stable duplet or octet electron arrangement
5.3 Covalent Bond
Single covalent bond
01
Formed when two atoms
share a pair of electrons
Triple covalent bond
03
Formed when two atoms
share three pairs of
electrons
Double covalent bond
02
Formed when two atoms
share two pairs of electrons
5.3 Covalent Bond
5.3 Covalent Bond
The formation of covalent bond can be visualised using the Lewis
structure.
Lewis structure only shows the valence electrons of the atoms
involved.
A pair of electrons shared, is represented with a line between the
two atoms
5.3 Covalent Bond
5.3 Covalent Bond
5.3 Covalent Bond
5.3 Covalent Bond – Hydrogen, H2
Hydrogen atom has 1 electron. The electron arrangement for hydrogen atom is 1.
H
5.3 Covalent Bond – Hydrogen, H2
Each hydrogen atom contributes one electron for sharing with each other to achieve
stable duplet electron arrangement.
H
H
H
H
Two hydrogen atoms share one pair of electrons to form one single covalent bond.
Hydrogen molecule, H2 is formed
Lewis structure:
5.3 Covalent Bond – Hydrogen chloride, HCl
Hydrogen atom has 1 electron.
The electron arrangement for
hydrogen atom is 1.
Chlorine atom has 17 electrons.
The electron arrangement for
chlorine atom is 2.8.7.
H
Cl
5.3 Covalent Bond – Hydrogen chloride, HCl
The hydrogen atom contributes one electron for sharing to achieve stable duplet electron arrangement.
The chlorine atom contributes one electron for sharing to achieve stable octet electron arrangement.
H
Cl
H
Cl
One hydrogen atom and one chlorine atom share one pair of electrons to form one single covalent bond.
Hydrogen chloride molecule, HCl is formed
Lewis structure:
5.3 Covalent Bond – Oxygen, O2
Oxygen atom has 8 electrons. The electron arrangement for oxygen atom is 2.6.
O
5.3 Covalent Bond – Oxygen, O2
Each oxygen atom contributes two electrons for sharing with each other to achieve
stable octet electron arrangement.
O
O
O
Two oxygen atoms share two pairs of electrons to form one double covalent bond.
Oxygen molecule, O2 is formed
Lewis structure:
O
5.3 Covalent Bond – Carbon dioxide, CO2
Carbon atom has 6 electron.
The electron arrangement for
carbon atom is 2.4.
C
Oxygen atom has 8 electrons. The
electron arrangement for oxygen
atom is 2.6.
O
5.3 Covalent Bond – Carbon dioxide, CO2
The carbon atom contributes four electrons for sharing to achieve stable octet electron arrangement.
Each oxygen atom contributes two electrons for sharing to achieve stable octet electron arrangement.
O
C
O
One carbon atom and two oxygen atoms share four pair of electrons to form two double covalent bond.
Carbon dioxide molecule, CO2 is formed
Lewis structure:
5.3 Covalent Bond – Nitrogen, N2
Nitrogen atom has 7 electrons. The electron arrangement for nitrogen atom is 2.5.
N
5.3 Covalent Bond – Nitrogen, N2
Each nitrogen atom contributes three electrons for sharing with each other to achieve
stable octet electron arrangement.
N
N
N
Two hydrogen atoms share one pair of electrons to form one single covalent bond.
Hydrogen molecule, H2 is formed
Lewis structure:
N
5.3 Covalent Bond
Test Yourself 5.3
Page 117 Chemistry Form 4 KSSM Text Book
Test Yourself 5.3
Test Yourself 5.3
Test Yourself 5.3
Test Yourself 5.3
5.4 Hydrogen Bond
Learning Standard
At the end of the lesson, pupils are able to
5.4.1 Explain with examples the formation of hydrogen
bond
5.4.2 Explain the effect of the hydrogen bond on physical
properties of substances
5.4 Hydrogen Bond
An iceberg weighing thousands of
tonnes is able to float on the
surface of the sea
This is because the density of ice is
lower than water
This is due to the presence of
hydrogen bond in water
5.4 Hydrogen Bond
Hydrogen bonds are attraction forces between hydrogen atom, H
that has bonded with an atom of high electronegativity such as
N, O or F with N, O or F in another molecule.
5.4 Hydrogen Bond
5.4 Hydrogen Bond in hydrogen fluoride, HF
H-F
Fluorine atom, F has high
electronegativity
H-F
Attraction forces between hydrogen
atom, H in hydrogen fluoride
molecule with fluorine atom, F, from
another hydrogen fluoride molecule
forms a hydrogen bond
5.4 Hydrogen Bond in ammonia, NH3
H
H-N-H
Nitrogen atom, N has high
electronegativity
H
N-H
H
Attraction forces between hydrogen
atom, H in ammonia molecule with
nitrogen atom, N, from another
ammonia molecule forms a
hydrogen bond
5.4 Hydrogen Bond – Role in Daily Life
There are protein molecules that form hydrogen bonds
among one another in the hair structure.
5.4 Hydrogen Bond – Role in Daily Life
When hair is wet, protein molecules no longer form
hydrogen bond between themselves.
Instead, protein molecules will form hydrogen bonds with
water molecules, H2O.
Water molecules also form hydrogen bonds with other hair
protein molecules.
This causes hair to stick together.
5.4 Hydrogen Bond – Role in Daily Life
5.4 Hydrogen Bond – Role in Daily Life
When turning the pages of a book, you lick your finger
before turning the pages.
5.4 Hydrogen Bond – The Effect on Physical
Properties of Substances
01
Compounds in the form of liquids reach boiling point when the attraction
forces between molecules are overcome
02
In the covalent compound of ethanol, C2H5OH, there are hydrogen bonds
formed between molecules, other than weak Van der Waals attraction forces
03
Strong hydrogen bonds are difficult to break. More heat energy is required to
overcome the weak Van der Waals attraction forces, besides breaking the
hydrogen bonds
04
As a result, the boiling point of ethanol is high. Cl2 molecules do not form
hydrogen bonds have lower boiling point compared to ethanol
5.4 Hydrogen Bond – The Effect on Physical
Properties of Substances
5.4 Hydrogen Bond
Test Yourself 5.4
Page 119 Chemistry Form 4 KSSM Text Book
Test Yourself 5.4
Test Yourself 5.4
Test Yourself 5.4
5.5 Dative Bond
Learning Standard
At the end of the lesson, pupils are able to
5.5.1 Explain with examples the formation of dative bond
5.5 Dative Bond
5.5 Dative Bond
5.5 Dative Bond
5.5 Dative Bond in ammonium ion, NH4
+
Test Yourself 5.5
Page 121 Chemistry Form 4 KSSM Text Book
Test Yourself 5.5
Test Yourself 5.5
Test Yourself 5.5
5.6 Metallic Bond
Learning Standard
At the end of the lesson, pupils are able to
5.6.1 Explain the formation of a metallic bond
5.6.2 Reason out the electrical conductivity of metal
5.6 Metallic Bond
Why can metals conduct electricity?
1. Metal atoms are arranged closely packed and orderly in the solid
state
2. Valence electrons of metal atoms can be donated easily and
delocalized although in the solid state
3. Metal ions that are positively-charged are formed when valence
electrons are delocalized
4. All delocalized valence electrons can move freely between the
metal structure and form a sea of electrons
5. Electrostatic attraction force between the sea of electrons and
the positively-charged metal ions form the metallic bond
5.6 Metallic Bond
5.6 Metallic Bond
5.6 Metallic Bond
6. When electrons of metal atoms are delocalised in the sea of
electrons, the metal can conduct electricity
7. Electrons that move freely in the metal structure carry the
charges from the negative terminal to the positive terminal when
electricity is supplied
5.6 Metallic Bond
Test Yourself 5.6
Page 122 Chemistry Form 4 KSSM Text Book
Test Yourself 5.6
5.7 Properties of Ionic Compounds and
Covalent Compounds
Learning Standard
At the end of the lesson, pupils are able to
5.7.1 Compare the properties of ionic compounds and
covalent compounds through experiment
5.7.2 Explain with examples the uses of ionic
compounds and covalent compounds in daily life
5.7 Properties of Ionic Compounds and Covalent
Compounds
5.7 Properties of Ionic Compounds and Covalent
Compounds
5.7 Properties of Ionic Compounds and Covalent
Compounds
5.7 Properties of Ionic Compounds and Covalent
Compounds
5.7 Properties of Ionic Compounds and Covalent
Compounds
5.7 Properties of Ionic Compounds and Covalent
Compounds
5.7 Properties of Ionic Compounds and Covalent
Compounds
5.7 Properties of Ionic Compounds and Covalent
Compounds
5.7 Properties of Ionic Compounds and Covalent
Compounds
5.7 Properties of Ionic Compounds and Covalent
Compounds
5.7 Properties of Ionic Compounds and Covalent
Compounds – Electrical Conductivity
5.7 Properties of Ionic Compounds and Covalent
Compounds – Electrical Conductivity
5.7 Properties of Ionic Compounds and Covalent
Compounds – Electrical Conductivity
5.7 Properties of Ionic Compounds and Covalent
Compounds – Solubility in Water and Organic
Solvents
5.7 Properties of Ionic Compounds and Covalent
Compounds – Solubility in Water and Organic
Solvents
5.7 Properties of Ionic Compounds and Covalent
Compounds – Solubility in Water and Organic
Solvents
5.7 Properties of Ionic Compounds and Covalent
Compounds – Solubility in Water and Organic
Solvents
5.7 Properties of Ionic Compounds and Covalent
Compounds – Solubility in Water and Organic
Solvents
5.7 Properties of Ionic Compounds and Covalent
Compounds – Melting Point and Boiling Point
5.7 Properties of Ionic Compounds and Covalent
Compounds – Melting Point and Boiling Point
5.7 Properties of Ionic Compounds and Covalent
Compounds – Melting Point and Boiling Point
5.7 Properties of Ionic Compounds and Covalent
Compounds – Structure of Covalent Compounds
5.7 Properties of Ionic Compounds and Covalent
Compounds – Uses in Our Daily Life
5.7 Properties of Ionic Compounds and Covalent
Compounds – Uses in Our Daily Life
5.7 Properties of Ionic Compounds and Covalent
Compounds
Test Yourself 5.7
Page 130 Chemistry Form 4 KSSM Text Book
5.7 Properties of Ionic Compounds and Covalent
Compounds
Test Yourself 5.7
Test Yourself 5.7
Test Yourself 5.7
ACHIEVEMENT
TEST 5
Achievement Test 5
Achievement Test 5
Achievement Test 5
Achievement Test 5
Achievement Test 5
Achievement Test 5
Achievement Test 5
Achievement Test 5
Achievement Test 5
Achievement Test 5
Achievement Test 5
Enrichment Corner
Enrichment Corner
THANK YOU
Prepared by: Puan Nurulkamilah binti Khairir