What are the trends in electron configuration across the periodic table?

What are the trends in electron configuration across the periodic table?

Electron configuration trends refer to how the arrangement of electrons in an atom changes across periods and groups in the periodic table. Generally, as you move from left to right across a period, the number of valence electrons increases, affecting chemical properties.

Can you explain how these trends affect reactivity?

Certainly! In general, elements with fewer valence electrons tend to be more reactive. For example, alkali metals in Group 1 have one valence electron and are highly reactive, while noble gases in Group 18 have full valence shells and are mostly inert.

What about the transition metals?

Transition metals have variable electron configurations, which contribute to their unique properties, such as multiple oxidation states and complex ion formation. Their d-orbitals are involved in bonding, influencing their reactivity and color.

How does this relate to periodic trends like electronegativity?

Electron configuration directly influences electronegativity, which is the tendency of an atom to attract electrons. As you move across a period, electronegativity generally increases due to the increasing nuclear charge, which pulls electrons closer.