Periodic Table Trends

Periodic Table Trends

1. Atomic Radius

   • The atomic is defined as half the distance between two nucleus of two adjacent atoms, sometimes found in a net.
   • This is a Periodic Trend
     • This happens because as the elements get closer to fill their outer shell, the attraction becomes stronger.
       • Helium has the smallest atomic radius.

2. Ionic Radius

   • When an atom losses an electron it becomes a cation, this means the radius becomes smaller. When the atom gains electrons and becomes an anion, the radius gets larger; this is the ionic radius.
   • Ions
     • Ions are atoms or molecules that have charge, this happens when the amount of protons is not equal to the amount of electrons.

3. This are properties that follow an exponential pattern throughout the periodic table

4. Ionization Energy

   • Energy required to remove an electron from its atom.
     • Usually this acts as a sequence when the first electron is removed with the first ionization energy and the second electron with the second ionization energy.
       • This sequence has an increase going from 1st to 2nd, this is because, of the influential factors, the closer the electron is to the nucleus the more energy is required to remove it.
     • Units: KJ/Mol
   • This is Periodic Trend
     • This is because the attraction on the electrons is lower because it harder to reach electrons farther away.
       • Factors: Nuclear Charge, Electron shield/Screening, Distance.

5. Electron Affinity

   • This is the energy an atom gives away when the electron is added and it forms an anion.
     • Some atoms have the affinity to sustain an extra electron and some others don't due to the flowing factors.
       • Factors: Nuclear Charge, Electron shield/Screening, Distance.
     • Units: -KJ/Mol
   • This is partially a periodic trend
     • Even though there are some exceptions there is a slight increase in Electron Affinity while going through a period.

6. Electronegativity

   • Electronegativity is the power of atom in a molecule to attract electrons to itself.
     • Bonds with the same or similar electronegativities are called Non-polar covalent bonds, when the difference is lager that 0.5 its defined as a Polar bond. When the difference is larger that 1.7 is a Ionic bond.
   • This is a periodic trend
     • The tendency is periodical because an element that has its outer shell less full doesn't have the energy required to bond other electrons that a more full shell would be able to maintain.

7. Metallic nature

   • Metallic properties: Shine, Density, Solid, Maleable, Conductors.
   • This is a periodic trend

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