TRANSITION METALS Flashcards
define what transition metal is
D block elements forming one or more stable ions with incomplete D orbitals
what properties do transition metals have
- variable oxidation states (apart from Sc 3+ and Zn 2+)
- form coloured compounds
- used as catalysts
when is iron used as a catalyst
HABER PROCESS
- making ammonia
- N2 (g) + 3H2 (g) –> 3NH2 (aq)
THIOSULFATE + IODIDE (Fe 3+)
- S2O8(2-) + Fe(2+) –> 2SO4(2-) + Fe(3+)
2Fe(3+) + 2I- –> I2 + 2Fe(2+)
when is nickel used as a catalyst
HYDROGENATION
- margarine manufacture
- CH2CH2 + H2 –> CH3CH3
Ni / 150ºc
when is Cu(2+) used as a catalyst
ZINC + SULFURIC ACID TO MAKE H2
- Zn + H2SO4 –> ZnSO4 + H2
Cu(2+)
when is vanadium oxide used as a catalyst
CONTACT PROCESS ( step 2) - making sulfuric acid
1. S (l) + O2 (g) --> SO2 (g) \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ *2. 2SO2 (g) + O2 (g) 2SO3 (g) V2O5 \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ 3. SO3 (g) + H2SO4 (l) --> H2S2O7 (l) H2S2O7 (l) + H20 (l) --> 2H2SO4 (l)
why are trans. mets. good catalysts
partially filled d orbitals can be used to form bonds w/ ADsorbed reactant which helps reactions take place more easily
define complex ion
a central metal ion co-ordinately bonded to one or more molecule / negative ion
define ligand
a molecule/ion that donates a pair of e- to a central metal ion to form a co-ordinate bond
define co-ordination number
the total number of co-ordinate bonds formed between the central metal ion + any ligands
colour of Cu(2+) solution
pale blue
copper + NaOH (aq)
observation and ionic equation
forms pale blue ppt - Cu(OH)2
Cu(2+) (aq) + 2OH(-) (aq) –> Cu(OH)2 (s)
copper + XS NaOH (aq)
pale blue ppt - CU(OH)2, does NOT dissolve
copper (+NH3) + XS NH3
forms a blue ppt at first - [Cu(OH)2(H2O)4]
but dissolves w/ XS to make a royal blue solution - Cu(NH3)4(H2O)2
NH3 ACTS AS A BASE [Cu(H2O)6](2+) (aq) + 2NH3 (aq) --> [Cu(OH)2(H2O)4] (s) + 2NH4(+)
XS NH3
[Cu(OH)2(H2O)4] (s) + 4NH3 –> Cu(NH3)4(H2O)2 (aq) + 2H2O (l) + 2OH(-) (aq)
copper + HCL
observation and ionic equation
colour of iron (II) solution
pale green - Fe(2+)
iron (II) + NaOH
observation and ionic equation
forms green ppt - Fe(OH)2
Fe(2+) (aq) + 2OH(-) (aq) –> Fe(OH)2 (s)
OXIDISES TO BROWN IN AIR - Fe(OH)3
iron (II) + XS NaOH
green ppt - Fe(OH)2, does NOT dissolve
colour iron (III) solution
pale yellow - Fe(3+)
iron (III) + NaOH
observation and ionic equation
rusty brown ppt - Fe(OH)3
Fe(3+) (aq) + 3OH(-) (aq) –> Fe(OH)3 (s)
iron (III) +XS NaOH
rusty brown ppt - Fe(OH)3, does NOT dissolve