Transition Metals

Question 1

Properties of transition metals

Answer 1

-hard solids with high mps and bps
-can act as catalysts and form coloured ions and compounds
-form ions with different oxidation numbers and ions are it’s incompletely filled d subshells

Question 2

Definition of a transition metal

Answer 2

D block elements that can form at least one stable ion with an incomplete subshell

Question 3

Why do transition metals have variable oxidation states

Answer 3

Because the 4s and 3d orbitals are very close in energy levels meaning it is possible for electrons to be lost from both orbitals relatively easily and remaining electrons can form stable configs

Question 4

Where are electrons removed from when ions formed

Answer 4

Initially removed from 4s subshell then 3d

Question 5

What stable ion does scandium form

Answer 5

Sc3+

Question 6

What ion does zinc form

Answer 6

Zn2+

Question 7

What are the two exceptions to the 4s subshell rule and why

Answer 7

Copper and chromium as half filled (chromium) and completely filled (copper) 3d subshell is more stable

Question 8

Why are scandium and zinc not transition metals

Answer 8

-transition metals form an ion with an incomplete d subshell
-Sc3+ has electronic config of 1s2 2s2 2p6 3s2 3p6 so d sub shell empty
-Zn2+ has electronic config 1s2 2s2 2p6 3s2 3p6 3d10 do has full d sub shell

Question 9

Why can transition metals show variable oxidation numbers in terms of IEs

Answer 9

Only gradual increase in successive ionisation energies