2.3.3 properties of transition metals

what is the definition of transition metal

an element with an incomplete d subshell or an element that can form at least one stable cation with an incomplete d subshell

what 2 element are not transition metals and why

scandium because can only forms Sc3+ with configuration of (Ar) 3d0

zinc because forms Zn2+ with configuration 3d10

draw a periodic table. indicate the s p and d blocks

decribe the structure of a transisiton metal

a lattice of positive metal ions surrounded by a sea of delocalised electrons

why can transition metals delocalise d electrons

because 3d and 4s subshells so close

why do transition metals have high melting points

can delocalise d block eletrons so have greater electron density. means the electrostatic forces of attraction between large positive charge of ions and delocalised electrons strenghtened and higher melting point as more energy to overcome

high or lower than group 1 and 2 elements

higher melting points than g1 and g2

why do transition metals have a high electrical conductivity

lots of delocalised electrons which are free to flow and carry a charge when a potential difference applied