Bonding and Structure Grade 10
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Bonding & Structure
K Warne
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Bonding
O
H2O
O
H2O
O
O
Bonding takes place when atoms react to form molecules.
Example: Two hydrogen molecules and one oxygen molecule react to form two
water molecules.
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Atomic Radius
Note the trends in atomic radius across the periodic table.
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VALENCY – No of BONDS
Valency – number of electrons lost or gained to have a FULL valence level. (Outer shell) = number of bonds made by element
H He
Li Be B C N O F Ne
Valence electrons – those in outer shell.
METALS –
valency = G No.
NON – METALS
valency = G.no - 8
1 2 3 4 3 2 1 0
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O x
xxx
xx
O x
x
xx
xx
O x
xxx
xx
O x
x
xx
xx
O xx
xx
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Ox
xx
x xx
O O
“Dot Cross Diagrams” - Lewis & Couper Notation
Lewis Diagrams
Couper Notation
Chemical Formulae
…………
Name:Oxygen
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Cl
Covalent Molecules
H2, O2, F2, Cl2, Br2, N2, HCl, H2O, NH3, CH4
CO2, NH4+,
CL
H X
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Ionic Bonding
Formed when there is a ………….
of …………………...
Formed between ………….. and ………………….
Metals …………………….. and
become ……………………... ions -CATIONS.
Non metals …………………... and become …………………………. ions - ANIONS.
…………………………… between oppositely charged ions bonds the ions together.
Na.
..
:Cl: -
..Na
+
.
:Cl:..
..
Na.
+ : Cl: --> [Na]+ [Cl]-
.
ELECTROSTATIC
ATTRACTION
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Lithium atom (Li)
3 protons (+3)
3 electrons (-3)
Total charge 0
Lithium ion (Li+)
3 protons (+3)
2 electrons (-2)
Total charge (+1)
+
Li. [Li]+ + e-
Ionic Bonding
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Ionic Crystal
The iond in ionic substances pack into GIANT IONIC structures called LATTICES, The
ions are arranged to give the lowest possible energy system. Strong ionic bonds exist
throughout the structure giving ionic substances HIGH melting & boiling points, HIGH
densities etc.
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ELECTRON AFFINITY
The amount of ENERGY RELEASED when an electron is
added to a gaseous atom. This always accompanies the
formation of an ionic bond.
e-
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Formation of Ionic Bond
A large amount of energy (lattice) is released when the gaseous ions bond together into the ionic crystal lattice.
Ionic compounds are therefore very stable and require large amounts of energy to break the bonding.
Ionic compounds have HIGH MELTING POINTS we say they are thermally stable.
Na(s) + 1/2 Cl2(g) NaCl(s)
Na(g) + 1/2 Cl2(g)
Na(g) + Cl(g)
Na+(g) + e- + Cl(g)
Na+(g) + Cl
-
(g)Ionisation Energy
Dissociation Energy
Sublimation Energy
Electron
Affinity
Lattice Energy
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MUST BE LEARNT BY HEART!
ONE TWO THREE
Hydrogen H+
Beryllium Be2+
Aluminium Al3+
Lithium Li+
Magnesium Mg2+
Iron(III) Fe3+
Sodium Na+
Calcium Ca2+
Potassium K+
Barium Ba2+
Silver Ag+
Lead Pb2+
Copper(I) Cu+
Zinc Zn2+
Ammonium NH4+
Iron(II) Fe2+
Oxonium H3O+
Copper(II) Cu2+
VALENCY TABLE 1
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Bonding - Metallic Bonding
- Exists between _________________.
- Metal electrons are _____________ - therefore they become______________________ (move from one atom to another).
- This leaves _______________ -which become surrounded by a ‘sea’ of ______________________ electrons.
- A force of _______________________exists between the delocalized ___________________ and the positive ___________- which forms the ___________________ bond.
All the _____________ of
metals can be explained
in terms of this bonding.
+ + + + + + +
+ + + + + + +
+ + + + + + +
+ + + + + + +
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Explaining Metal Properties
Property Explanation
Malleable
Ductile
Conductors of
electricity
Shiny (Luster)
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Bonding Summary
Covalent
Ionic
•
•
•
Metallic
•
•
H xH•
Cl-Na+
Properties•
•
•
•
•
Properties
•
•
•
•
•
Properties•
•
•
•
• .
H-H
Eg
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Strong covalent bonds
Network Solids
Properties:
• Strong hard
• conducts electricity - delocalised electrons -
Weaker (van der waals) forces between the layers
• layers slide over each other – so you can write
with graphite and it is a lubricant
Diamond Graphite
Properties:
• Strong/ hard/brittle – high m. & bpts.
• Electrical insulator (electrons held in
bonds) in all phases – no ions.
• insoluble
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Phases of Matter
PLASMA+
++
++
+
There are FOUR states or phases of matter.
1
2
3
4
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Molecular structure
Network Molecular Ionic Metallic
Particles
Bonds
Structure
Properties
Example
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Hi -
This is a SAMPLE presentation only.
My FULL presentations, which contain a lot more more slides and other resources, are freely
available on my resource sharing website:
www.warnescience.net(click on link or logo)
Have a look and enjoy!
WarneScience