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3.7 Ionisation energy and the periodic table (page 53)
T his year we will go a bit further with these configurations. Last year, we used the Rutherford model, combined with the Bohr one (energy levels), but these year we need to investigate a bit more to really know what happens in the outer layers of the atoms.

If you remember, we had some layers that we completed using simple rules. This can only be done up to the 3rd period and only with the representative elements. We had 7 energy levels, exactly the same as the periods in the periodic table.

Now, we face the concepts applied after the chemistry quantum mechanical model. According to this, the 7 energy levels, are splitted in more, depending on the characteristics of the atoms (number of electrons that should be allocated). This is explained in terms of energy and following the quantym mechanical equation (Schrödinger equation), that has to be with the concept of orbital and the "dellocation" of the electrons in the outer layers.

Electrons are not spinning and moving around the nucleus in very defined orbits, they are not exactly located. We can only know a place in which there is high probability of finding an electron, and this was called an orbital.

They are defined by a mathematical equation, can be drawn and there are 4 general type with different shapes and orientation depending on the combination of solutions to the equations.

For the equations, there are four quantic numbers: n, l, ml and ms. They can be expressed by numbers following some rules and each electron in each atom is defined by these four numbers, that give us some useful information about the energy it has, the shape of the orbital it is in, the orientation in that precise orbital and the spinning direction.

This year, we won´t work with the quantic numbers, but we have to learn how to organise the electrons in the different orbitals following 3 very simple rules. This will serve us to order the electrons in the orbitals, to know the electronic configuration of any atom or ion and to relate this to the place they have in the periodic table.

Just for you to know in advance, here you have the Moeller´s diagram, that we use to order the atoms in the atomic orbitals. Yo need to learn to construct it and to use it to have any electronic configuration.

It is based on the energy of the orbitals. WE WILL ALWAYS START LOCATING ELECTRONS FROM THE LESS ENERGETIC LEVEL (n=1) TO THE MOST ENERGETIC ONE (n=7) FOLLOWING THE DIAGRAM.

You can notice that some levels are mixed (we locate 4s before 3d). This is because, they have different total energy depending on the addition of main energy level (n) and secondary energy level (l).

The letters s, p, d and f, refer to the type of orbital (shape, orientation)

The number refers to the main energy level that is related to the size of the orbital. 1s is smaller than 2s (for example)

1. Electrons are "dellocated" in orbitals in the outer shell of the atoms.

2. There are some rules to order the electrons in the different orbitals.

3. These order is called "electronic configuration"

4. To produce an "electronic configuration" we need the atom or ion to know the number of electrons we need to order, and we have to follow the Moeller´s diagram.

5. If we are witty, we will relate the electronic configuration with the place of atoms in the periodic table.

HOW TO PRODUCE AN ELECTRONIC CONFIGURATION:

Silicon (Si, Silicio) has 14 electrons that we have to distribute into the different orbital following the Aufbau principle (Moeller´s diagram)

According to another rule: s type holds 2 electrons, p type holds 6 electrons, d type holds 10 electrons and f type holds 14 electrons. (This is related to the quantic numbers of each electron in an atom)

SOME EXAMPLES OF ELECTRONIC CONFIGURATIONS:

Now I leave you here the link to a page in which you can find a lot of information related to this part of the chemistry and a direct link to a video explaining how to produce an electronic configuration.

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Electronic configurations - Física y Química. Physics and Chemistry. THE SITE TO LEARN AND INVESTIGATE. IES ISAAC NEWTON. MADRID.

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3.7 Ionisation energy and the periodic table (page 53) T his year we will go a bit further with these configurations. Last year, we used the Rutherford model, combined with the Bohr one (energy levels), but these year we need to investigate a bit more to really know what happens in the outer layers of the atoms. If you remember, we had some layers that we completed using simple rules.

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Bohr atomic model