Basics of transition metals Flashcards
Where are transition metals found in the periodic table?
D block
Which two elements in period 4 dont count as transition metals?
Zinc
Scandium
What is the definition of a transition metal?
A metal that can form one or more stable ions with an incomplete sub-shell
Why does the 4s sub shell fill up before the 3d?
It has lower energy
What are the two exceptions to the filling of electron shells?
Chromium
Copper
How does chromium fill up?
It prefers to have one electron in each orbital of the 3d sub shell and just one in the 4s sub shell as this gives more stability
How does copper fill up?
It prefers to have a full 3d sub level and just one electron in the 4s sub-level as it is then more stable
Do transition metals form positive or negative ions?
Positive
When transition metals form ions, which electrons are removed first?
The 4s electrons and then the 3d electrons
Why aren’t zinc and scandium transition metals?
They stable ions don’t form incomplete d-subshells
How doesn’t the stable ion of scandium have an incomplete d sub shell
The stable ion is Sc3+
The electron configuration of Sc is [Ar]3d1 4s2 so if it lost three it would end up as just [Ar]
How doesn’t the stable ion of zinc have an incomplete d sub shell?
The stable ion is Zn2+
The electron configuration of Zn is [Ar]3d104s2 so if it lost two electrons it would end up as [Ar]3d10
What chemical properties of transition metals make them different to other metals?
- They can form complex ions
- They form coloured ions
- They are good catalysts
- They can exist in variable oxidation states
What colour is the aqueous ion of Ti²⁺?
Violet
What colour is the aqueous ion of Ti³⁺?
Purple
