When moving across a period from left to right in the periodic table, several trends can be observed:
-
Increasing Atomic Number: The atomic number increases as you move from left to right due to the addition of protons in the nucleus.
-
Decreasing Atomic Radius: Generally, the atomic radius decreases from left to right. This is because the increasing positive charge in the nucleus pulls the electrons closer to the nucleus, resulting in a smaller atomic size.
-
Increasing Electronegativity: Electronegativity typically increases across a period. This means that atoms are more capable of attracting and holding onto electrons when they are located further to the right.
-
Increasing Ionization Energy: Ionization energy, which is the energy required to remove an electron from an atom, generally increases across a period. This is due to the increased nuclear charge, which holds the electrons more tightly.
-
Increasing Electron Affinity: Electron affinity, which is the energy change that occurs when an atom gains an electron, typically becomes more negative (indicating a more exothermic process) as you move from left to right.
These trends are largely due to the increasing nuclear charge and the effective nuclear charge experienced by the valence electrons. However, there can be exceptions to these trends based on specific elements and their electron configurations.
6 answers