Inorganic Chemistry 3.1 - Transition Metals - Electron Configuration, Oxidation Number Rules, Naming of Complexes Flashcards
The d-block transition metals are metals with an ___ d subshell in at least one of their ___.
incomplete, ions
When the d orbital is filled, moving across the d block of the periodic table, the Aufbau Principle is followed by all elements except ___ and ___.
Chromium (Cr), Copper (Cu)
The 4s subshell has ___er energy than the 3d and so is filled (before/after).
lower, before
However, Cr and Cu both pull a __ electron into the __ subshell, because…
4s, 3d, of the special stability associated with a half full or completely full subshell
Now, when atoms from the first row of the transition elements from ions, electrons in the __ subshell are lost first, not electrons in the __.
4s, 3d
An element is said to be in a particular oxidation state when it has a specific ___ ___.
oxidation number
There are six oxidation number rules:
1. Uncombined elements (eg Noble Gasses, Gold, Silver and Platinum), have an oxidation number of _.
2. Single ions (eg Fe2+) have an oxidation number equal to…
- 0
- The ion’s charge (Eg Fe2+ has an oxidation number of +2)
- In most of its compounds, oxygen has an oxidation number of _.
- In most of its compounds, hydrogen has an oxidation number of _.
- -2
- +1
- The sum of oxidation numbers in a neutral compound must be _.
- The sum of oxidation numbers in a polyatomic ion must be…
- 0
- equal to the ion’s charge
A transition metal can have different ___ ___ in different compounds.
oxidation states
This is because oxidation state differs based on the number of electrons ___ or ___ when it joins/forms a compound.
gained or lost
Compounds of the same ___ ___ in different oxidation states may have different c___.
transition metals, colours
What is the definition of oxidation?
What about reduction?
an increase in oxidation number
a decrease in oxidation number
Changes in oxidation number of transition metal ions can be used to determine if ___ or ___ has occurred.
oxidation, reduction
Compounds containing metals in high oxidation states are often ___ agents.
Compounds containing metals in low oxidation states are often ___ agents.
high: oxidising agents
low: reduction agents
Oxidised metal in compound = ___ agent.
Reduced metal in compound = ___ agent.
oxidising,
reduction
What is a ligand?
a molecule or ion which forms a complex with a transition metal by donating one or more Non-Bonding electron pairs, forming a dative covalent bond
What is a complex?
a central transition metal surrounded by ligand(s)
Depending on the number of electron pairs a ligand donates, it can be classified as:
1: __dentate
2: __dentate
3: __dentate
4: __dentate
5: __dentate
6: __dentate
1: monodentate
2: bidentate
3: tridentate
4: tetradentate
5: pentadentate
6: hexadentate
What is the coordination number of a complex?
the total number of bonds from the ligands to the central transition metal
What is the coordination number of a complex made of a copper ion and two tridentate ligands?
6
The name of which type of ligands change? (meaning it’s different to the molecule/element’s typical name).
anionic (-ve)
-ate becomes…
-ite becomes…
-ide becomes…
For example, Bromide (Br-) becomes…
-ato,
-ito,
-ido.
Bromido
How is Naming neutral ligands different to naming anionic ligands?
the name of anionic ligands’ change
the names of neutral ligands does not
Name them
1. Br-
2. F-
3. O2-
4. OH-
5. CN-
6. (C2O4)2-
7. I-
8. OH2
9. NH3
- Bromido
- Fluorido
- Oxido
- Hydroxido
- Cyanido
- Oxalato
- Iodido
- Aqua
- Ammine
If a complex is neutral, the names of metals…
doesn’t change (literally just its name)
How do the names of metals change in negative complexes?
The names of which two metals change completely when the complex is negative? What do their names change to?
-ate is added.
copper and iron
cuprate and ferrate
What is the difference between the name of a metal in a negative complex versus a neutral complex?
negative has an -ate.
eg nickel - in a negative complex it’s nickelate, but in a neutral complex it’s just nickel
What do the Roman Numerals in brackets at the end represent?
Metal complexes are always within ___ brackets.
The oxidation state of the transition metal (eg ferrate (II) means the iron has a +2 oxidation state)
[Square]
Any additional species that are not a part of the complex (not in the ___ ___), should be included in the name.
If the species is written before the complex (on the left of the square brackets), then put it at the ___. Vice versa
Square brackets, start
A Roman numeral put at the end of a complex’s name, tells you…
the oxidation state of the T metal
Name this complex: [Cu(OH2)6]2-
hexa-aqa-cuprate (II)
Name this complex: (3k+[CoF5])2+
potassium-penta-fluorido-cobaltate (iv) (ate because the complex is negative)
Name this complex: ([Fe(CN-)2(NH3)4]2Cl-)1+
tetra-ammine-di-cyanido-iron-chlorine (v)
Ligand formula are written so the attaching atom comes ___.
first.
ie OH2 - not H2O
Ligand formula and names are always written ____.
alphabetically. (even if the name of the ligand starts with a different letter than its symbol, like aqua being OH2)
Name this complex: [CoCl2 (NH3)4 ]
tetra-ammine-di-chlorido-cobalt (II)
[CoCl2 (NH3)4 ]
tetra-ammine-di-chlorido-cobalt (II)
Notice how the ‘Cl2’ comes before the ‘NH3’, but ‘chlorido’ does not come before ‘___’
ammine
In a complex of a transition metal, the d orbitals are no longer ___.
degenerate
