Chapter 24 Flashcards
What are transition metals?
Elements with an incomplete d-subshell that can form at least one stable ion with an incomplete d-subshell.
What two elements aren’t transition elements?
Scandium and Zinc.
Scandium only forms the ion Sc3+, configuration [Ar] 3d0
Zinc only forms the ion Zn2+, configuration [Ar] 3d10
What fills or loses electrons first? 3d or 4s?
4s
When writing them which is first 3d or 4s?
3d, 4s is always at the end.
What is the electron configuration of Chromium?
Cr is [Ar] 3d5 4s1 not [Ar] 3d4 4s2
this is because its energetically more stable.
What is the electron configuration of Copper?
Cu is [Ar] 3d10 4s1 not [Ar] 3d9 4s2
this is because its energetically more stable.
What are some general properties of transition elements?
-Variable oxidation states
-Form complex ions
-Form coloured compounds
-Behave as catalysts
What is a complex ion?
A molecule or ion, consisting of a central metal atom or ion, with a number of molecules or ions surrounding it
What is a ligand?
A ligand is a molecule or ion that forms a co-ordinate bond with a transition metal by donating a pair of electrons to the bond.
A molecule or ion surrounding the central metal atom or ion.
What colour is Cr3+
Green
What colour is Cr 6+
Orange/yellow
What colour is Mn2+
Pink
What colour is Cu2+
Blue
Why are transition metals good catalysts? How do they work?
Since transition elements can have variable oxidation states, they make excellent catalysts.
During catalysis, the transition element can change to various oxidation states by gaining electrons or donating electrons from reagents within the reaction.
Substances can also be adsorbed onto their surface and activated in the process.
Examples of how transition metals are used as catalysts in industrial processes:
1- Haber process to manufacture ammonia. Catalysed by finely divided iron catalyst.
2- Contact process, producing sulphur triode. Catalysed by vanadium oxide (V2O5)
3- catalytic decomposition of hydrogen peroxide uses manganese (V1) oxide as the catalyst.