Bonding
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Transcript of Bonding
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At the end of this lesson we will be able to understand :-
Why an atom gets bonded with other atom or atoms.
Different types of solids depending upon type ofbonding between their particles.
Properties of different solids.
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Group zero elements
Element Electronic configuration
Behavior of atoms
2He4 2 Helium atoms do not bond
10Ne20 2 , 8 Neon atoms do not bond
18Ar40 2 ,8, 8 Argon atoms do not bond
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Argon: 18Ar40
Nucleus
First shell: 2electrons
Second shell : 8 electrons
Third shell : 8 electrons
Each shell is full .
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Magnesium :12 Mg24
Nucleus
First shell ; 2 electrons
Second shell : 8 electrons
Third shell : 2 electrons
Outer shell not full : only 2 electrons in it
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Press Enter to continue
Now I am sure you can tell me that why bonding takes place between two atoms.
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Types of solidsDepending on the type of bonding solids
are of Four types – Molecular solids Macromolecular solids Metallic solids Ionic solids
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I I
I I
Two atoms of iodine
Two atoms bonding together
Iodine : a molecular solid
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I I
Two Iodine atoms
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I I
An Iodine molecule
I - I
A covalent bond between two Iodine atoms is formed
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I I I I
I I
A Collection of iodine atoms Iodine molecules, full shells
I I
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C C
C
C
C
Carbon is in IV group –each atom has 4 outer shell electron
Carbon (diamond) : a macromolecular solid
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C
CC
C C
Central carbon atom now has a full outer shell
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Carbon lattice
The whole lattice is held together by covalent bonds. These are strong forces of attraction, so a considerable amount of energy is needed to break up the lattice.
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Lattice of iodine molecules
The forces of attraction between molecules is weak , however – they all have full shells – so lattice is easily broken up.
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sodium atom Na
sodium ion Na+
11 protons, 11 electrons: neutral 11 protons, 10 electrons:+ charged
Sodium : a metallic solid
Removed electron
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repulsion
attraction
Metallic Bonding
Metal ion
- Delocalized electron
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Metals are malleable and ductile : they can be bent , shaped and drawn into wires.
Force applied
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delocalized electrons moving though the lattice carrying negative charge
Metals conduct electricity well
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HOT ENDCOLD END
ELECTRONS MOVING QUICKLY
ELECTRONS MOVING SLOWLY
Metals conduct heat well
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Na
Cl Cl
Na+
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atoms ions
Salt : an ionic solid
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Electrovalent bond between cat ions and anions
cat ion
anion
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repel
Force applied
Although ionic solids are hard , they are brittle. They shatter when hit by a hammer.
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+
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+
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electrode electrode
solvent particles
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Summary• Properties of a solid depend on the type of particle
in the lattice & the way in which they attract each other in the lattice.
• There are three types of bonding – covalent bonding, metallic bonding, ionic bonding .
• In all these bonding, the atoms achieve full electron shells .
• An ion is a particle which has gained or lost electrons, so is charged .