Atomic structure

An artist's representation of the orbital model of the atom

Atoms 

Atoms are the building blocks of matter. Atoms are the smallest possible particles into which an element can be subdivided, without changing its properties. 

As building blocks, they can be thought of spheres despite the fact that we now know that they are mostly empty space. 

What's wrong with the image?

The image on the left is only an artist's representation of the orbital model of the atom. The centre sphere represents the nucleus while the three outer spheres represent the electrons.  

The three electrons appear to be in the same shell. This is actually  impossible as there can only be two electrons in the innermost shell of an atom. We will see this later on in the course.

Pearson IGCSE

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Sub atomic particles 

Sub atomic particles are the particles found inside atoms. These include protons, neutrons and electrons:

  • protons are particles with a positive charge and a mass of 1(amu) . They are part of the nucleus of an atom. The number of protons is given by the atomic number of an element.
  • neutrons are particles with no charge and a mass of 1(amu) they are also part of the nucleus of an atom.
  • electrons are particles with a charge of -1 and a mass of 1/2000 of an amu, they orbit the nucleus in shells.
A more accurate "orbital model" of an atom

Atoms and isotopes 

This image shows an atom of carbon, we know is is carbon because it has six protons in the nucleus. The atomic number of carbon is 6. 

The number of protons in the nucleus is given by the atomic number - ( also known as the proton number)

the mass number of an atom is the total nube rof proton and neutrons. In this case, the nucleus has six neutrons and the atom therefore, has a mass number of 6 + 6  = 12.

If this nucleus had an extra neutron it would still be a carbon atom but it would be an isotope, called carbon-13.

If it had two extra neutrons it would be the isotope carbon 14

the three isotopes of carbon

Isotopes and relative atomic mass 

All elements can exist as different isotopes, in naturally occuring carbon about 1% of the atoms are carbon 13. Carbon 14 also exists but is unstable. 

In order to calculate the relative mass of the atoms in elements we need to take into account all the masses of the different isotopes. 

We calculate a value called the relative atomic mass.

The relative atomic mass of an element is an average value of the mass of the individual isotopes in a naturally occurring sample of the element.


Task 1:  

​Sub atomic particles : Use the game below make sure you know these three sub-atomic particles. Can you beat 3 seconds??

The mass spectrum of boron

Calculating relative atomic mass (Ar)

The image shown here is a mass spectrum of the element boron. It shows the relative number of isotopes in a naturally occurring sample of the element. 

We  can calculate Ar values using this isotopic abundance data:

For Boron two isotopes exist, Boron 10 and Boron 11. The mass spectrum shows that 20% of boron atoms are Boron -10 and 80% are Boron -11.

The weighted mean is calculated as follows:

The relative atomic mass of boron is a weighted mean of all the isotopes in a naturally sample of the element.
The mass spectrum of Zinc
The mass spectrum of Magnesium
The mass spectrum of Germanium

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 Task 2

  • ​Look at the mass spectra for Zinc, Magnesium and Germanium and try to estimate the relative atomic mass for each element.
  • Use the data on the mass spectra to calculate the relative atomic masses for those three elements
Molecules are particles made up of more than one atom

Molecules 

​A molecule is a particle composed of more than one atoms combined. The atoms are joined by covalent bonds. eg Hydrogen (H2), Water (H2O), Methane (CH4)