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SME Chemistry Topic 13 Notes
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SME Chemistry Topic 13 Notes
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H e a d t o s a v e m y e x a m s . c o . u k f o r m o r e a w e s o m e r e s o u r c e sPage 1 of 26
© 2 0 1 5 − 2 0 2 3 S a v e M y E x a m s , L t d . · R e v i s i o n N o t e s , T o p i c Q u e s t i o n s , P a s t P a p e r sIB Chemistry DP
13. HL The Periodic Table- Transition Metals
CONTENTS
13.1 Transition Metals
13.1.1 Transition Elements
13.1.2 Variable Oxidation States
13.1.3 Complex Ions
13.1.4 Catalytic & Magnetic Properties
13.1.5 Colour in Transition Metals
13.1.6 Factors A ecting ColourYOUR NOTES H e a d t o s a v e m y e x a m s . c o . u k f o r m o r e a w e s o m e r e s o u r c e s
Page 2 of 26
© 2 0 1 5 − 2 0 2 3 S a v e M y E x a m s , L t d . · R e v i s i o n N o t e s , T o p i c Q u e s t i o n s , P a s t P a p e r sTransition Elements
Transition metals are elements with an incomplete d-subshell or that can form at least one
stable cation with an incomplete d-subshell
This definition distinguishes them from d-block elements, because scandium and zinc do
not fit the definition
Scandium only forms the ion Sc , configuration [Ar] 3d
Zinc only forms the ion Zn , configuration [Ar] 3d
The elements of the first transition series are therefore titanium to copper
The transition elements and the d-block elements
Electron Configuration
The full electronic configuration of the first d-series transition metals is shown in the table
below
Following the Aufbau Principle electrons occupy the lowest energy subshells first
The 4s overlaps with the 3d subshell so the 4s is filled first
Remember that you can abbreviate the first five subshells, 1s-3p, as [Ar] representing the
configuration of argon (known as the argon core)
Table showing the electronic configuration of the first d-series transition elements
13.1 Transition Metals
13.1.1 Transition Elements3+ 0
2+ 10YOUR NOTES H e a d t o s a v e m y e x a m s . c o . u k f o r m o r e a w e s o m e r e s o u r c e s
Page 3 of 26
© 2 0 1 5 − 2 0 2 3 S a v e M y E x a m s , L t d . · R e v i s i o n N o t e s , T o p i c Q u e s t i o n s , P a s t P a p e r s
From your previous studies in chemistry, you should recall there are two exceptions to the
Aufbau Principle in the first row of d-block, chromium and copper
In both cases an electron is promoted from the 4s to the 3d to achieve a half full and full d-
subshell, respectively
Chromium and copper have the following electron configurations, which are di erent to
what you may expect:
Cr is [Ar] 3d 4snot [Ar] 3d 4s
Cu is [Ar] 3d 4snot [Ar] 3d 4s
This is because the [Ar] 3d 4s and [Ar] 3d 4sconfigurations are energetically more
stable and are preferred configurations
When forming cations, remove the 4s electrons first
Worked Example
Writing electronic configuration of transition element ionsState the full electronic
configuration of the manganese(III) ion
Answer
Step 1: Write out the electron configuration of the atom first:
Mn atomic number = 255 1 4 2
10 1 9 2
5 1 10 1 YOUR NOTES
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