Intro 

When using the periodic table you will notice that it is arranged in a specific way. When using the table you will notice three different trends such as ionization energy, atomic radius, and electronegativity 

The 3 Trends

     Ionization Energy: This is the measurable energy derived from the removal or addition of electrons to a molecule. This increases as you go further right on the periodic table. And from top to bottom it decreases.

One example of ionization energy is Hydrogen, which is 1,312. Another example is Francium, which is 380. Francium has a lower ionization level than Hydrogen because it decreases from top to bottom. The ionization energy levels increase from left to right. 

Electronegativity: This is the ability of atoms to attract electrons. From top to bottom it decreases and left to right it increases.

For example, in the periodic table in the far left corner, an element is most likely to lose electrons. Aluminum has an electronegativity of 1.61 and chlorine has 3.16. This is because electronegativity increases from left to right and decreases from top to bottom. One important thing is that noble gases do not have any electronegativity.