Transition Metals Flashcards
(27 cards)
Are all D block elements transition metals
No
Transition metal definition
A transition metal is a D-block element that can form at least one stable ion with a partially filled d-sub shell
Why are zinc and scandium not transition metals
The stable ions they form don’t have partially filled d-sub shells Sc3+ has an empty d sub shell and Zn2+ has a full d sub shell
Which two transition metals have irregular filling patterns
Cu and Cr partially filled 4s orbital to have full 3d sub shell or half full 3d sub shell respectively
Where do transition metals lose electrons from first
4s sub shell
3 key properties of transition metals
1.Variable oxidation states
2.Coloured ions in solution
3.Good catalysts
Why do transition metals have variable oxidation states
Electrons sit in 4s and 3d energy levels which are very close
What is a complex ion
Central transition metal ion is surrounded by ligands bonded by dative covalent bonds
What characteristic do ligands share
At least one lone pair
Three classifications of ligands
Monodentate, Bidentate, Polydentate
Two examples of bidentate ligands
Ethanedioate2-
Ethane-1,2-diamine
Multidentate ligand example and how many coordinate bonds
EDTA4- - 6
What’s the coordination number
Number of dative covalent bonds in a complex
[CuCl4]2- shape
Tetrahedral
Cisplatin shape and structure
Z/cis isomer of square planar platinum with 2 ammonia ligands and 2 chloride ligands
What is cisplatin used for
Cancer drug
What is Haem
A multidentate ligand in haemoglobin which bonds to iron with 4 coordinate bonds from haem, 1 from the globin protein and 1 from oxygen which can bond to the top of the complex
What does Haemoglobin deliver to and from the cell
Oxygen to and water from
What happens if carbon monoxide is inhaled
It replaces the water ligand on the Haemoglobin complex and bonds more strongly than water and oxygen so can’t be removed
Do complexes show optical isomerism
Yes esp when using bidentate ligands
Which complexes show E/Z isomerism
Octahedral - opposite is trans and adjacent is cis
Square planar - opposite is trans and adjacent is cis
What is d-orbital splitting
The d-sub shell splits into two energy levels when ligands bond due to electron density in the ligand
Why do transition metals have colours (3)
D-orbital splitting due to ligands results in energy gap
Electrons absorb energy from light and are excited to higher energy orbitals (d-d transition)
This light absorbed is absent from observed light giving it the complimentary colour
What is deltaE
The energy gap between the split d orbitals
