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Презентация на тему Ionization Energy

Ionization EnergyThe amount of energy required to completely remove an electron from a gaseous atom.An atom's 'desire' to grab another atom's electrons. Removing one electron makes a +1 ion.The energy required is called the first ionization
Ionization Energy12.1.1	 Explain how evidence from first ionization energies 	across periods accounts Ionization EnergyThe amount of energy required to completely remove an electron from Ionization EnergyThe second and third ionization energies can be represented as follows: X+ Group trendsIonization energy decreases down the group. Going from Be to Mg, IE decreases because:Mg outer electron is in Notice any trends? Any surprises? General trend: Increasing I.E. as we go across a periodLook at the Why is there a fall from Mg to Al?  Al has configuration Why is there a fall from P to S?  This can be Driving ForceFull Energy Levels are very low energy.Noble Gases have full energy 2nd Ionization EnergyFor elements that reach a filled or half filled sublevel 3rd IEUsing the same logic s2p1 atoms have an low 3rd IE.Atoms
Слайды презентации

Слайд 2 Ionization Energy
The amount of energy required to completely

Ionization EnergyThe amount of energy required to completely remove an electron

remove an electron from a gaseous atom.
An atom's 'desire'

to grab another atom's electrons.
Removing one electron makes a +1 ion.
The energy required is called the first ionization energy.
X(g) + energy →X+ + e-

Слайд 3 Ionization Energy
The second and third ionization energies can

Ionization EnergyThe second and third ionization energies can be represented as

be represented as follows:
 X+ (g) + energy? X2+ (g)

+ e-
X2+ (g) + energy? X3+ (g) + e-
More energy required to remove 2nd electron, and still more energy required to remove 3rd electron

Слайд 4 Group trends
Ionization energy decreases down the group.

Group trendsIonization energy decreases down the group.

Слайд 5
Going from Be to Mg, IE decreases because:
Mg

Going from Be to Mg, IE decreases because:Mg outer electron is

outer electron is in the 3s sub-shell rather than

the 2s. This is higher in energy
The 3s electron is further from the nucleus and shielded by the inner electrons
So the 3s electron is more easily removed
A similar decrease occurs in every group in the periodic table.


Слайд 6 Notice any trends? Any surprises?

Notice any trends? Any surprises?

Слайд 7 General trend: Increasing I.E. as we go across

General trend: Increasing I.E. as we go across a periodLook at

a period
Look at the peak at Mg and the

plateau between P and S. Can you explain why?

Слайд 8 Why is there a fall from Mg to

Why is there a fall from Mg to Al?  Al has

Al?
 Al has configuration 1s2 2s2 2p6 3s2 3p1, its

outer electron is in a p sublevel
 Mg has electronic configuration 1s22s22p63s2.
 The p level is higher in energy and with Mg the s sub level is full – this gives it a slight stability advantage

Слайд 9 Why is there a fall from P to

Why is there a fall from P to S?  This can

S?

 This can be explained in terms of electron

pairing.
 As the p sublevel fills up, electrons fill up the vacant sub levels and are unpaired.
This configuration is more energetically stable than S as all the electrons are unpaired. It requires more energy to pair up the electrons in S so it has a lower Ionisation energy.
There is some repulsion between the paired electrons which lessens their attraction to the nucleus.
 It becomes easier to remove!

Слайд 10 Driving Force
Full Energy Levels are very low energy.
Noble

Driving ForceFull Energy Levels are very low energy.Noble Gases have full

Gases have full energy levels.
Atoms behave in ways to

achieve noble gas configuration.

Слайд 11 2nd Ionization Energy
For elements that reach a filled

2nd Ionization EnergyFor elements that reach a filled or half filled

or half filled sublevel by removing 2 electrons 2nd

IE is lower than expected.
Makes it easier to achieve a full outer shell
True for s2
Alkaline earth metals form +2 ions.

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