Explain the relationship between the atomic structure and the position of an element on the periodic table.

href="https://upload.wikimedia.org/wikipedia/commons/thumb/f/fe/Periodic_trends.svg/2000px-Periodic_trends.svg.png">Periodic

trends identify relationships between atomic structure and characteristics and
their
position on the periodic table. Below are several periodic trends and a
short explanation of
each:

1. Atomic radii

Atomic radii increase as one moves
down a group. This is because
additional energy levels are being added. 

Atomic radii
decrease as one moves to the right of a period. This is because additional

protons are being added, making the nucleus more positive. This added positive charge
within the
nucleus pulls the electrons inward more- decreasing the size of
the atomic radii. 

2. Electronegativity and ionization
energy

Electronegativity is the
affinity an atom has for
electrons. Ionization energy is the amount of energy needed to remove
an
electron from the outermost orbital from a neutral atom in the gas
phase. 

Both ionization energy and electronegativity
increase as one moves to the right of the
periodic table. This is
also because additional protons are being added, making the nucleus more

positive. The added positive charge results in the electrons being pulled and held on
tighter by
the nucleus. Thus, they are harder to remove. It also results in
the atom having a greater pull
for additional electrons. 

Both ionization energy and electronegativity
increase as one moves
up a group. This is because there are less orbitals, so the electrons are

closer to the positive nucleus. Thus, the atom has a greater pull for more electrons.
The
electrons that are present are held on more tightly.