Final answer:
The electron configuration pattern in the periodic table relates to the trends in atomic properties such as atomic radii, electronegativity, and ionization energy. Atomic radii generally decrease across a row and increase down a group. Electronegativity generally increases across a row and from bottom to top, while ionization energy generally increases across a row and decreases down a group.
Step-by-step explanation:
The electron configuration pattern in the periodic table relates to the general trends in atomic properties such as atomic radii, electronegativity, and ionization energy.
a. Atomic radii (size): The atomic radius generally decreases along each row (from left to right) and increases down each group (from top to bottom) in the periodic table. This is because the number of protons in the nucleus increases across a row, leading to a stronger attractive force, while the addition of more energy levels down a group increases the atomic size.
b. Electronegativity: Electronegativity generally increases from left to right and from bottom to top in the periodic table. This trend is due to the increase in effective nuclear charge (number of protons minus shielding electrons), which attracts electrons more strongly.
c. Ionization energy: Ionization energy generally increases from left to right and decreases from top to bottom in the periodic table. This is because it becomes harder to remove an electron from a smaller, more tightly held orbital as you move across a period, while moving down a group allows for easier removal of electrons from larger, higher energy orbitals.