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TRANSCRIPT
CHEMICAL BONDING
K. FALING
EDITED: R. BASSON
SUTHERLAND HIGH SCHOOL
GRADE 10
PHYSICAL SCIENCE
TB . 103
HOW DOES BONDING WORK?
• The chemical reaction between elements leads to compounds, which have new
physical and chemical properties.
• A bond is the force that holds atoms together to form molecules. This happens so that the
millions of different substances found on earth can be formed.
• Intermolecular bonds/forces – between MOLECULES
Intramolecular bonds/forces – between ATOMS
• There are ATTRACTIVE forces between the nucleus of one atom (+) and the electrons of
the other atom and there are REPULISIVE forces between the electrons of different atoms.
When the attractive force is GREATER than the REPULSIVE force that exists between them.
• Elements will bond with each other to become stable = full energy levels.
• Only valence electrons are involved in bonding.
TB . 103
3 TYPES OF INTRAMOLECULAR BONDING
1. COVALENT BONDS - Between atoms of non-metals
2. IONIC BONDS - Between atoms of metals and non – metals
3. METALLIC BONDS - Between atoms of metals
O O
Na Cl
Cu Cu
TB . 103
REPRESENTING BONDING
•Bonding is illustrated by using LEWIS DIAGRAMS.
Requirements
• Only valence electrons are drawn.
• Electrons are represented as dots or crosses around
the symbol of the element.
EXAMPLEVALENCE
ELECTRONS?
GROUP
NUMBER?TB . 103
IMPORTANT INFO ABOUT LEWIS DIAGRAMS
• VALENCE ELECTRONS ARE DRAWN.
• THEY ARE REPRESENTED AS DOTS BUT ALSO CONTAINS LINES TO
REPRESENT SHARED PAIRS IN A CHEMICAL BOND.
• EXCESS ELECTRONS THAT FORM LONE PAIRS ARE REPRESENTED AS PAIRS
OF DOTS, AND ARE PLACED NEXT TO THE ATOMS.
• EACH ELEMENT WILL GAIN, LOOSE OR SHARE ELECTRONS UNTIL THEY
HAVE RECEIVED AN OCTET OF ELECTRONS = FULL VALENCE SHELL
ELECTRON CONFIGURATION.
PRACTICEDRAW LEWIS DIAGRAMS FOR THE FOLLOWING STRUCTURES
Ar
H
Ca
Zn
HOMEWORK
EXERCISE 8
1. COVALENT BONDS
• BETWEEN NON-METAL ATOMS
• ORBITALS WITH HALF-FILLED ORBITALS WILL OVERLAP AND ELECTRONS ARE SHARED
• SMALLEST PARTICLE IS A MOLECULE
• THE TYPE OF COVALENT BOND IS DETERMINED BY THE DIFFERENCE IN ELECTRONEGATIVITY
• NON-POLAR COVALENT - DIFFERENCE < 0.9 Attraction is shared equally
• POLAR COVALENT - 0.9 < DIFFERENCE < 1.7 One atom attracts the
shared pair more than the
other.
• IONIC - DIFFERENCE > 1.7
• EXAMPLE:𝐻20
• Single
• Double
• Triple
TB . 104
PRACTICEDRAW LEWIS DIAGRAMS FOR THE FOLLOWING BONDS
Hydrogen 𝐻2
Water 𝐻20
Nitrogen 𝑁2
TB . 104
IONIC BONDS
• OCCUR BETWEEN A METAL AND NON-METAL ATOMS
• INVOLVES THE TRANSFER OF ELECTRONS
• METALS TEND TO GIVE AWAY ELECTRONS AND BECOME POSITIVE IONS (CATIONS) AND THE NON-
METALS TEND TO ACCEPT THE ELECTRONS AND BECOME NEGATIVE IONS (ANIONS)
• SO: METALS – LOW IONISATION ENERGY AND NON-METALS: HIGH ELECTRON AFFINITY.
• THE CATIONS AND ANIONS ATTRACT EACH OTHER WITH STRONG ELECTROSTATIC OR
COULOMBIC FORCES
• LARGE CRYSTAL LATTICES ARE FORMED
• THE SMALLEST PARTICLE MAKING UP AN IONIC CRYSTAL LATTICE IS AN ION
• EXAMPLES INCLUDE: NACℓ; KMNO4; MGSO4; CACO3
TB . 106
DRAWING LEWIS DIAGRAMS THE IONIC BONDS
𝐶𝑙2𝑁𝑎
TB . 106
METALLIC BONDS• OCCUR BETWEEN METAL ATOMS
• THE ATOMIC NUCLEI WITH THE INNER ELECTRON SHELLS ARE TIGHTLY PACKED
• TOGETHER IN AN ORGANISED CRYSTAL STRUCTURE
• THE OUTERMOST ORBITALS OVERLAP
• THE VALENCE ELECTRONS ARE DELOCALISED AND CAN MOVE INTO ADJACENT ORBITALS
OF NEARBY ATOMS.
• THE SMALLEST PARTICLE OF A METALLIC CRYSTAL IS A POSITIVE METAL ION
• EXAMPLE: PIECES OF ZN, FE, CU AND AG
TB . 107
QUICK SUMMARY
Property Ionic bond Covalent
bond
Metallic bond
Smallest particle Ion Molecules Atom
Types of
elements
Metals &
non-metals
Non-metals Metals
How does bond
occur?
Electron
transfer
Sharing of
electrons
Positive atomic
core with sea of
delocalized
electrons
TB . 110
HOMEWORK
EXERCISE 9
• ALL MATTER IS MADE UP OF SMALL PARTICLES CALLED ATOMS
• A MOLECULE (NON-METALS) CONSISTS OF 2 OR MORE ATOMS THAT ARE BOUND
TOGETHER BY STRONG ATTRACTIVE FORCES
• A CHEMICAL COMPOUND IS A GROUP OF TWO OR MORE ATOMS OF DIFFERENT
TYPES THAT ARE HELD TOGETHER BY STRONG FORCES OR BONDS. THESE ATOMS
ALWAYS BOND IN A SPECIFIC RATIO.
TB . 111
• MOLECULAR FORMULA
• The actual number and type of atoms in the compound.
• Example: 02 03 𝐻20 𝐶8𝐻18
• EMPIRICAL FORMULA
• The simplest ratio in which atoms combine.
• STRUCTUAL FORMULA
• Shows the arrangement of the atoms and bonds
TB . 117
BALL AND STICK SPACE FILLING DIAGRAM LEWIS STRUCTURE
TB . 118
HOMEWORK
EXERCISE 10
TEST EXAMPLES
• Molecules (molecular
substances) are due to covalent
bonding.
• Ionic substances are due to ionic
bonding.
When the electrons of atoms are transferred from one atom to
another atom to form positive and negative ions, the ions bond
with ionic bonds and the resulting solid is called an ionic
substance (or salt or ionic compound).
As a general rule ionic substances are usually composed of both
metallic elements (usually forming positive ions) and nonmetallic
elements (usually forming negative ions)
• When metal atoms lose their outer electrons to form a
lattice of regularly spaced positive ions and the outer electrons
form a delocalized “pool” of electrons that surround the positive
ions, the atoms are bonded by metallic bonding and the resulting
collection of atoms is called a metal • Give examples of
molecules based on the above description e.g. • Covalent
molecular structures consist of separate molecules: oxygen,
water, petrol, CO2, S8, C60 (buckminsterfullerene or buckyballs)