Bonding and Structure Grade 10

Bonding & Structure

K Warne

SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY

For FULL presentation click HERE >> www.warnescience.net

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.





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



Click to edit Master text styles Second level

Third level Fourth level

Fifth level



O x

xxx

xx

O x

x

xx

xx

O x

xxx

xx

O x

x

xx

xx

O xx

xx

xx

Ox

xx

x xx

O O

“Dot Cross Diagrams” - Lewis & Couper Notation

Lewis Diagrams

Couper Notation

Chemical Formulae

…………

Name:Oxygen



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Third level Fourth level

Fifth level



Cl

Covalent Molecules

H2, O2, F2, Cl2, Br2, N2, HCl, H2O, NH3, CH4

CO2, NH4+,

CL

H X





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





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





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.









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-





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





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





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.

+ + + + + + +

+ + + + + + +

+ + + + + + +

+ + + + + + +

-

- -

-

-

-

- -

- -

-

-

-

-

-

-

-

-

-

-

-

-

-

-

-

-

-

-

-

-





Explaining Metal Properties

Property Explanation

Malleable

Ductile

Conductors of

electricity

Shiny (Luster)





Bonding Summary

Covalent

Ionic

•

•

•

Metallic

•

•

H xH•

Cl-Na+

Properties•

•

•

•

•

Properties

•

•

•

•

•

Properties•

•

•

•

• .

H-H

Eg



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



Phases of Matter

PLASMA+

++

++

+

There are FOUR states or phases of matter.

1

2

3

4









Molecular structure

Network Molecular Ionic Metallic

Particles

Bonds

Structure

Properties

Example





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Education

Bonding and Structure Grade 10