Trends of the Periodic Table
Atomic Radius:
The atomic radius is one half the distance between
the nuclei of two atoms of the same element
when the atoms are joined. The atomic radius
increases from top to bottom in a group and
decreases from left to right across a period.
the nuclei of two atoms of the same element
when the atoms are joined. The atomic radius
increases from top to bottom in a group and
decreases from left to right across a period.
Ionic Radius:
Ionic radius is the measure of an atom's ion. Just like the atomic radius, ionic radii increases from top to bottom in a group and decreases from left to right across a period. However, ionic radius is different from atomic radius in elements because positive ions are smaller than uncharged atoms and negative ions are larger than their atoms.
Ionization Energy:
Ionization energy is the energy required to remove an electron
from an atom. This energy can be measured when the
element is in its gaseous state. On the periodic table ionization energy decrease from top to bottom in a group and increases
from left to right across a period.
from an atom. This energy can be measured when the
element is in its gaseous state. On the periodic table ionization energy decrease from top to bottom in a group and increases
from left to right across a period.
Electronegativity:
Electronegativity is the ability of an atom of an element to
attract electrons when it is chemically combined with
another element. Noble gases aren’t affected by electronegativity because they do not combine with any other element. Electronegativity generally increases from left to right across periods and decreases from top to bottom in groups on the periodic table.
attract electrons when it is chemically combined with
another element. Noble gases aren’t affected by electronegativity because they do not combine with any other element. Electronegativity generally increases from left to right across periods and decreases from top to bottom in groups on the periodic table.