Ionizing energy is how much energy is required to remove one mole of electrons from the ground state of one mole of the gaseous atom. Basically, the energy required to remove an electron from an atom.
As you can see the graph isn't smooth but it shows a lot of important data. All noble gases which have a full outer shell takes a lot of energy to remove an electron while it is easy for all the alkali metals. It also shows the existence of main energy levels and shows hints of sub-levels.
12.1.2 Explain how successive ionization energy data is related to the electron configuration of an atom
From this graph we could tell that there are certainly 2, 8, 8. But in between there are some anomalies which are explained by the existence of p orbitals.
12.1.3 State the relative energy levels of s, p, d and f orbitals in a single energy level.
http://www.youtube.com/watch?v=BP5nhnLSSu4 is a funny video I found which explains this concept.
s is closest to the nucleus, then p, then d and finally f.
Note: you should be able to tell from the image that 4s actually has a lower energy level than 3d which is the reason why we have transition metals. Similar to 6s and 4f.
The lines show the order of energy. However the number shows the energy level they are in.
12.1.4 State the maximum number of orbitals in a given energy level.
s sub-levels can hold a maximum of 2 electrons
p sub-level can hold a maximum of 6 electrons
d sub-level can hold a maximum of 10 electrons
f sub-level can hold a maximum of 14 electrons.
This shows how the common misconception of 2, 8, 8, 2 electron shells as it is really 1s, 2s 2p, 3s 3p, 4s.
This is how the modern day periodic table is shaped.
12.1.5 Draw the shapes of an s orbital and the shapes of the px, py and pz orbitals.
Simply learn how to draw the first 4 orbitals. The rest is just used to frighten you, they are the shapes of the d and f orbitals.
12.1.6 Apply the Aufbau principle, Hund's rule and Pauli exclusion principle to write electron configurations for atoms and ions up to Z = 54
Aufbau principle states that electrons are placed into orbitals of lowest energies first. Boxes can be used to represent the atomic orbitals with single-headed arrows to represent the spinning electrons.
Hund's rule states that we place them in separate orbitals because this configuration minimizes the mutual repulsion between them.
Pauli Exclusion Principle states that no more than two electrons can occupy any one orbital and if two electrons are in the same orbital they must spin in opposite directions.
Atoms
This is carbon's electron configuration compared with oxygen and hydrogen.
This is how you draw the electron configuration. There is another method which you write out the configuration by stating all the electrons in each orbital.
Note that you have to know the anomalies to the pattern which is 24 chromium and 29 copper. You only have to learn up to 54. You can also use the short hand form which is putting the noble gas before.
Ions
It is very simple, the electrons of the ion is how many electrons are in the atom and the charge of the ion.
Just in case anyone doesn't know, you remove the electrons in the same order as you add electrons. However, remember that you remove the electrons in s orbital before the d orbitals.
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