Arrangement

• The periodic table is arranged into columns and periods

• This sequence of the periodic table has metals and non-metals segregated

Periodic Trends

• The groups are arranged in a similar pattern because they have the same properties due to the similar number of valance electrons, in one group every atom will have the same valance electron

• Each group to the right, the number of valance electrons increase

• The atomic mass and atomic number increases when going to the right side of the groups

  

• The atomic radius increases when it goes to down and left

• Ions with the same electron configuration will have their radii decreased as the atomic number increases

• This is because more protons create a greater positive charge in the nucleus, which attracts the electrons more strongly

• The ionization energy increase from up and right of the periodic table, ionization energy is the minimum energy to pull a electron from a radius

• ↓ down a group: Increases (more shells).

• → across a period: Decreases (stronger nuclear pull).

Electromagnetic Force

• ↓ down a group: Decreases.

• → across a period: Increases.

• Most electronegative = Fluorine.

Metallic Character

• ↓ down a group: Increases.

• → across a period: Decreases.

• Metals on left, nonmetals on right.

Electron Affinity

• Electron affinity talks about the tendency of the atom to gain a electron

• Electron affinity increases to top and right of the periodic table