5.3 Transition Metals

Question 1

Define a transition metal

Answer 1

-d-block elements that have an ion with an incomplete d-sub shell

Question 2

Why are scandium and zinc not classed as transition metals?

Answer 2

-because they do not have any ions with partially filled d-orbitals
-scandium only forms Sc+3 ion in which d-orbitals are empty
-zinc forms only Zn2+ ion in which d-orbitals are full

Question 3

When writing electron configurations in what order should you write the 3d and 4s sub shell?

Answer 3

The 4s sub shell has a lower energy than the3d sub shell
This means that the 4s orbital fills before the orbitals in the 3D sub shell

Question 4

What are the two transition metals do not follow the rules for filling sub shells?

Answer 4

Chromium-the five 3d-orbitals and the 4s orbital all contain one electron with no orbital being completely filled.
Copper-the five 3d-orbitals are full but there is only one electron in the 4s-orbital

Question 5

Write out the electron configuration for chromium

Answer 5

1s2 2s2 2p6 3s2 3p6 4s1 3d5

Question 6

Write out the electron configuration for copper

Answer 6

1s2 2s2 2p6 3s2 3p6 4s1 3d10

Question 7

When forming positive ions from transition metals the ___ electrons are lost before the ____ electrons.

Answer 7

4s orbital
3d orbitals
As once the electrons occupy the orbitals the 4s electrons have a higher energy

(FIRST IN FIRST OUT)