CL 24- transition metals Flashcards
electron configuration of Cr
1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁵
electron configuration of Cu
1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d¹⁰
transition metal
definition
- a d-block element that has an ion with an incomplete d-sub-shell
colours of Cu²⁺ and Mn²⁺
blue and pale pink
two examples of transition-metal elements that form compounds with more than one oxidation state
- Fe²⁺ / Fe³⁺
- Mn²⁺ / MnO₄⁻
- Cu²⁺ / Cu⁺
ligand
definition
- a species that can donate one or more lone pairs to form dative covalent bonds to a central metal ion forming a complex ion
monodentate ligand examples
- only form one dative covalent bond
- H₂O
- NH₃
- OH⁻
- Cl⁻
bidentate ligand examples
- forms two dative covalent bonds
- ethane-1,2-diamine
complex ion
definition
- a central transition metal bonded to one or more electron donating species (ligands) by dative covalent bonds, from the ligand to the metal
coordination number
definition
- the no. of dative covalent bonds between the ligands and the central metal ion
octahedral complex ion
reasoning for shape, example of complex ion
- element connected to central metal ion in period 2, so there is room for 6 dative covalent bonds
- e.g. H₂O, NH₃
- [Cr (H₂O) ₆] ³⁺
tetrahedral complex ion
reasoning for shape, example of complex ion
- element connected to central metal ion in period 3, larger donor atoms so there is only room for 4 dative covalent bonds
- Cl
- [Cu (Cl) ₄] ²⁻
square planar complex ion
reasoning for shape, example of complex ion
- an exception to the rule, only with Pt and Ni
- 4 ligands attached
- [Pt (Cl) ₂ (NH₃)₂ ]
linear complex ions
- only Ag with 2 donor atoms
cis-trans isomerism (only) in complex ions
when does it occur
- in an octahedral complex, monodentate ligands - 4 of one, and 2 another
- square planar complex, monodentate ligands- 2 of each
optical isomerism (only) in complex ions
- octahedral complex
- 3 bidentate ligands
optical and cis-trans isomerism in complex ions
- octahedral complex
- 2 bidentate ligands and 2 monodentate ligands
- 3 different isomers- trans isomer doesn’t have optical isomerism
cis-platin
idk if you need to know this
- [Pt (Cl)₂ (NH₃) ₂ ]
- attacks tumours, and in many cases it works to shrink the tumour, but it has many unpleasant side effects and can lead to kidney damage
ligand substitution reactions for adding NH₃ to Cu²⁺ (in water)
first precipitation reaction, then ligand substitution with excess NH₃
- [Cu (H₂O)₆ ] ₍ₐ₎+ 2NH₃ ₍ₐ₎ –> [Cu (OH)₂ (H₂O)₄ ] ₍ₛ₎ +2NH₄⁺₍ₐ₎
- pale blue solution to pale blue precipitate (initially)
- [Cu (H₂O)₆ ] ₍ₐ₎ + 4NH₃ ₍ₐ₎ –> [Cu (NH₃)₄ (H₂O)₂ ] ²⁺₍ₐ₎ + 4H₂O₍ₗ₎
- pale blue solution to dark blue solution
ligand substitution reactions for adding HCl to Cu²⁺ (in water)
- [Cu (H₂O)₆ ] + 4Cl⁻ –> [CuCl₄]²⁻ + 6H₂O
- pale blue solution to yellow solution
ligand substitution reactions for adding with NH₃ with Cr³⁺
first precipitation reaction, then ligand substitution with excess NH₃
- [Cr (H₂O)₆ ] ³⁺ + 3NH₃ –> [Cr (H₂O)₃ (OH)₃ ] + 3NH₄⁺
- violet solution to grey precipitate
- [Cr (H₂O)₆ ] ³⁺ + 6NH₃ –> [Cr (NH₃) ₆ ] ³⁺ + 6H₂O
- violet solution to purple solution
importance of iron in haemoglobin
- Fe has 4 dative bonds with N atoms on haem, and 1 dative bond to the protein globin
- this leaves 1 space for carrying O₂ or CO
- O₂ reversibly binds to the Fe ion; however if O₂ levels are low, water is susbtituted instead
- if CO is present, this will bind over to O₂ as it binds more strongly than oxygen, and binds irreversibly
- if conc of carboxyhaemoglobin becomes too high, O₂ transport is prevented, leading to death
precipitation reaction with NaOH/NH₃
Cu²⁺
- Cu²⁺ + 2OH⁻ –> Cu (OH)₂
- blue solution to blue precipitate
- Cu also reacts with excess NH₃ (ligand substitution reaction)
precipitation reaction with NaOH/NH₃
Fe²⁺
- Fe²⁺ + 2OH⁻ –> Fe (OH) ₂
- pale green solution to green precipitate