Chemistry: Unit 11 - The p-Block Elements

There are six p-block elements in each period of the periodic table, excluding Helium.

A set of p orbitals can accommodate a maximum of 6 electrons.

Helium (He) does not follow the ns²npx electronic configuration typical of p-block elements.

The inner core electronic configuration significantly influences the physical properties of p-block elements within a group.

The total number of valence electrons determines the maximum oxidation state a p-block element can exhibit.

The number of possible oxidation states increases from left to right across the periodic table for p-block elements.

For heavier elements in groups 13 (boron), 14 (carbon), and 15 (nitrogen), an oxidation state two units less than the group oxidation state becomes progressively more stable.

The general electronic configuration for the first member of group 14 is ns²np².

Non-metals and metalloids exist in the p-block of the periodic table.

The heaviest element in each p-block group tends to exhibit metallic character.

Highly reactive non-metals and metals generally form ionic compounds.

The change from non-metallic to metallic character in the p-block contributes to the diversity in the chemistry of p-block elements.

Non-metals readily form anions because they have higher ionization enthalpies and higher electronegativities than metals.

Non-metals form ionic oxides with highly reactive metals.

For heavier elements in groups 13, 14 and 15, an oxidation state two units less than the group oxidation state is the most stable.

Non-metals form covalent compounds with other non-metals.