periodic patterns of melting points, electrical conductivity, IE

metallic bonding from Na to Al is getting stronger

Na donates 1 electron, while Al donates 3 electrons

Na to Al have strong giant covalent structure

more delocalized electrons in Al compared to Na

increasing charge on the metal ions in the giant metallic lattice

giant molecular structure

giant ionic structure

strong covalent bond (each Si connects to 4 other Si atoms)

Silicon is semimetal or metalloid

has no delocalized electrons

silicon is a very good electrical conductor

silicon is able to conduct electricity when it is doped with other element

P4, S8, Cl2 and argon are all non metal, with relatively small molecules

they have giant covalent structure

the covalent bond is strong but they have weak instanteneous dipole - induced dipole

energy needed to remove one mole of electron from its outermost shell in its gaseous state

energy needed to remove one mole of electron from its outermost shell in its liquid state

energy needed to remove one mole of electron from its outermost shell in its solid state

presence of p orbital in B (2s² 2p¹) or Al (3s² 3p¹)

p orbital is slightly further from nucleus

weaker force of attraction in B or Al

spin spin paired repulsion in p orbital

presence of p orbital in B (2s² 2p¹) or Al (3s² 3p¹)

spin spin paired repulsion in p orbital in O or S