Electrostatic
forces in atoms
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Now there are two types of atoms, non-metals and metals. Non-metals generally have moderate to strong electrostatic forces attracting the outer most electrons(valence electrons) to the nucleus. Metals on the other hand, have very low electrostatic attraction for their outer most electrons and often tend to lose these electrons when reacting with other atoms. | |
Have a look at the atoms on
the left, there are metal (sodium and lithium) atoms and non-metal (fluorine,
helium, oxygen and hydrogen) atoms. |
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Fluorine,
on the other hand has seven electrons in its outer level and each electron
is attracted into the nucleus by a charge of 7+. Even though there are nine
protons in the nucleus the two electrons between the valence electrons and
the nucleus neutralise the effect of two protons. You might wonder, all this talk of attraction between protons and electrons and not one mention of repulsion between electrons and repulsion between protons. Well, there is repulsion between electrons. As electrons move around the nucleus they tend to keep away from one another due to eletrostatic repulsion. In the nucleus where protons are packed in tightly, massive repulsive forces are acting trying to push the protons apart. An even greater force, called the nuclear binding force, holds the nucleus together and prevents it from blowing apart. |
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