Ionic bonds form when electrons are transferred from a metal atom to a non-metal atom, creating oppositely charged ions. Covalent bonds form through the sharing of electrons between non-metal atoms. Ionic compounds contain ionic bonds and transfer electrons, while covalent compounds share electrons. Examples of ionic compounds are sodium chloride and magnesium oxide, while examples of covalent compounds are hydrogen gas, oxygen gas, and carbon dioxide. Ionic compounds are generally solids with high melting points that conduct electricity when molten or dissolved, while covalent compounds can be solids, liquids or gases with varied properties depending on molecular complexity.

1. CHEMICAL BONDS
XYLENE AR

2. IONIC BOND
• Transfer of electrons from metal atom to non-metal atom
COVALENT BOND
Sharing of electrons between non-metal atoms
 Attraction force between ions/ electrostatic force
Three types of covalent bond: single bond, double bond and triple bond
 For example:
H
H-N-H
H
H-C=H H-C=C-H
Double bond
Single bond
Triple bond
Single bond
Single bond

3. Why?
• Stability of atom
• Outer shell filled with electrons
• Duplet configuration (2 electrons) – H, Li, Be, B
• Octate configuration (8 electrons) – others
How?
1. Atom donates/ losses of electrons
2. Atom accepts electrons
Ion formation

4. POSITIVE & NEGATIVE IONS
Positive ions  metal atom donates/ losses of
electrons towards non-metal atom
Cation
Negative ions  non-metal atom
accepts electrons from metal atom
Anion

5. POSITIVE ION
Na
Electron arrangement= 2,8,1
Positive charge= +11
Negative charge = -11
Total charge = 0
Donate 1 electron
Stability of atom???
Na – metal atom
Donate 1 electron
11p
12n
Electron arrangement= 2,8 (octate)
Na+
Positive charge= +11
Negative charge = -10
Total charge = +1
Natrium ION
Natrium ATOM
11p
12n
Half equation: Na  Na+ + e

6. Mg
Electron arrangement = 2,8,2
Positive charge = +12
Negative charge = -12
Total charge = 0 Donates 2 electrons
Stability of atom???
Mg – metal atom
Donates 2 electrons
Electron arrangement = 2,8 (octate)
Mg 2+
Positive charge = +12
Negative charge = -10
Total charge = +2
12p
12n
12p
12n
Magnesium ATOM Magnesium ION
Half equation : Mg  Mg2+ + 2e
POSITIVE ION

7. NEGATIVE ION
O
Electron arrangement = 2,6
Positive charge = +8
Negative charge = -8
Total charge = 0 Accept 2 electrons
O – non-metal atom
Accept 2 electrons
Electron arrangement = 2,8 (octate)
O2-
Positive charge = +8
Negative charge = -10
Total charge = -2
Oxide ION
Oksigen ATOM
8p
8n
8p
8n
Half equation : O + 2e  O2-

8. Cl
Electron arrangement = 2,8,7
Positive charge = +17
Negative charge = -17
Total charge = 0
Accept 1 electron
Cl – non-metal atom
Accept 1 electron
Electron arrangement = 2,8,8 (octate)
Cl-
Positive charge = +17
Negative charge = -18
Total charge = -1
Chloride ION
Chlorine ATOM
17p
18n
17p
18n
Half equation : Cl + e  Cl-
NEGATIVE ION

9. PERIODIC TABLE OF ELEMENTS
1
H
Hydrogen
1
2
He
Helium
4
3 (2,1)
Li
Lithium
7
4 (2,2)
Be
Beryllium
9
5 (2,3)
B
Boron
11
6 (2,4)
C
Carbon
12
7 (2,5)
N
Nitrogen
14
8 (2,6)
O
Oxygen
16
9 (2,7)
F
Flourine
19
10 (2,8)
Ne
Neon
20
11 (2,8,1)
Na
Sodium
23
12 (2,8,2)
Mg
Magnesiu
m
24
13 (2,8,3)
Al
Aluminiu
m
27
14 (2,8,4)
Si
Silicon
28
15 (2,8,5)
P
Phosphor
us
31
16 (2,8,6)
S
Sulphur
32
17 (2,8,7)
Cl
Chlorine
35.5
18 (2,8,8)
Ar
Argon
40
19
(2,8,8,1)
K
Potassiu
m
39
20
(2,8,8,2)
Ca
Calcium
40
5
B
Boron
11
Proton
number
Name of
element Nucleon
number
Symbol of
element
+ 2
+
3
+
3- 2- -

10. IONIC BOND
• Transfer of electron from metal atom to non-metal atom
• Ionic compound is the compound containing ionic bond
• An example of ionic compound: sodium chloride
11p
12n
17p
18n
Na Cl
11p
12n
17p
18n
Na+ Cl-

11. Mg O Mg2+ O2-
12p
12n
8p
8n
12p
12n
8p
8n
2
2
IONIC BOND
• Transfer of electron from metal atom to non-metal atom
• Ionic compound is the compound containing ionic bond
• An example of ionic compound: magnesium oxide

12. O
Na +
O2-
8p
8n 8p
8n
2
11p
12n
11p
12n
Na
Na 11p
12n
11p
12n
Na +
IONIC BOND
• Transfer of electron from metal atom to non-metal atom
• Ionic compound is the compound containing ionic bond
• An example of ionic compound: sodium oxide

13. COVALENT BOND
• Sharing of electron between non-metal atoms. Three types of bonds: single, double bond and triple bond
• Examples for single bond covalent compund: hydrogen molecule (H2) and hydrogen chloride (HCl)
1
H
H
H
H
Electron arrangement for hydrogen atom = 2
H – H
1 Single bond
Cl
H Cl
H
Single bond
H – Cl
Electron arrangement for hydrogen atom = 2
Electron arrangement for chlorine atom = 2,8,8
Structural formula
1
2,8,7
A pair of electron shared between 2 atoms = 1 bond

14. • Examples for double bond covalent compound: oxygen molecule (O2) and carbon dioxide (CO2)
Electron arrangement for oxygen atom = 2
O = O
2,6
Double bond
O=C=O
Electron arrangement for oxygen atom = 2,8
Electron arrangement for carbon atom = 2,8
Structural formula
O
2,6
O O
O
2 pairs of electrons shared between 2 atoms = 2 bonds
C
O
O
2,6 2,6
2,4
C O
O
COVALENT BOND

15. • Examples for triple bond covalent compound : nitrogen molecule (N2)
Electron arrangement for nitrogen atom = 2,8
2,5
Triple bond
Structural formula
2,5
N
3 pairs of electrons shared between 2 atoms = 3 bonds
N N
N
N N
COVALENT BOND

16. COMPARISON ON IONIC BOND AND COVALENT
BOND
SIMILARITIE
S
DIFFERENCE
S
1. Produce stable molecules
2. Exothermic reaction
3. Only valence electrons involved in the
reactions
4. Neutral molecules produced
5. Number of particles involved is in fixed
amount
Characteristics Ionic bond Covalent bond
1. Force of
attraction among
particles
Very strong Weak (for simple molecule)
Very strong (for complex
molecule)
2.
Electronegativity
Very strong None

17. CHARACTERISTICS FOR IONIC AND COVALENT COMPOUND
Characteristics Ionic compound Covalent compound
State of matter Solid Solid, liquid, gas
Melting point High Low (for simple molecule)
High (for complex molecule)
Boiling point High Low (for simple molecule)
High (for complex molecule)
Electrical
conductivity
Only in molten and aqueous solution Do not conduct electricity
Solubility Soluble in water
Insoluble in organic solvent
Insoluble in water
Soluble in organic solvent
State at room
temperature
Solid Solid, liquid, gas