Inorganic Chemistry 3.1 - Transition Metals - Electron Configuration, Oxidation Number Rules, Naming of Complexes

Question 1

The d-block transition metals are metals with an ___ d subshell in at least one of their ___.

Answer 1

incomplete, ions

Question 2

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 ___.

Answer 2

Chromium (Cr), Copper (Cu)

Question 3

The 4s subshell has ___er energy than the 3d and so is filled (before/after).

Answer 3

lower, before

Question 4

However, Cr and Cu both pull a __ electron into the __ subshell, because…

Answer 4

4s, 3d, of the special stability associated with a half full or completely full subshell

Question 5

Now, when atoms from the first row of the transition elements from ions, electrons in the __ subshell are lost first, not electrons in the __.

Answer 5

4s, 3d

Question 6

An element is said to be in a particular oxidation state when it has a specific ___ ___.

Answer 6

oxidation number

Question 7

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…

Answer 7

1. 0
2. The ion’s charge (Eg Fe2+ has an oxidation number of +2)

Question 8

3. In most of its compounds, oxygen has an oxidation number of _.
4. In most of its compounds, hydrogen has an oxidation number of _.

Answer 8

3. -2
4. +1

Question 9

5. The sum of oxidation numbers in a neutral compound must be _.
6. The sum of oxidation numbers in a polyatomic ion must be…

Answer 9

5. 0
6. equal to the ion’s charge

Question 10

A transition metal can have different ___ ___ in different compounds.

Answer 10

oxidation states

Question 11

This is because oxidation state differs based on the number of electrons ___ or ___ when it joins/forms a compound.

Answer 11

gained or lost

Question 12

Compounds of the same ___ ___ in different oxidation states may have different c___.

Answer 12

transition metals, colours

Question 13

What is the definition of oxidation?
What about reduction?

Answer 13

an increase in oxidation number
a decrease in oxidation number

Question 14

Changes in oxidation number of transition metal ions can be used to determine if ___ or ___ has occurred.

Answer 14

oxidation, reduction

Question 15

Compounds containing metals in high oxidation states are often ___ agents.
Compounds containing metals in low oxidation states are often ___ agents.

Answer 15

high: oxidising agents
low: reduction agents

Question 16

Oxidised metal in compound = ___ agent.
Reduced metal in compound = ___ agent.

Answer 16

oxidising,
reduction

Question 17

What is a ligand?

Answer 17

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

Question 18

What is a complex?

Answer 18

a central transition metal surrounded by ligand(s)

Question 19

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

Answer 19

1: monodentate
2: bidentate
3: tridentate
4: tetradentate
5: pentadentate
6: hexadentate

Question 20

What is the coordination number of a complex?

Answer 20

the total number of bonds from the ligands to the central transition metal

Question 21

What is the coordination number of a complex made of a copper ion and two tridentate ligands?

Answer 21

6

Question 22

The name of which type of ligands change? (meaning it’s different to the molecule/element’s typical name).

Answer 22

anionic (-ve)

Question 23

-ate becomes…
-ite becomes…
-ide becomes…
For example, Bromide (Br-) becomes…

Answer 23

-ato,
-ito,
-ido.
Bromido

Question 24

How is Naming neutral ligands different to naming anionic ligands?

Answer 24

the name of anionic ligands’ change
the names of neutral ligands does not

Question 25

Name them 1. Br- 2. F- 3. O2- 4. OH- 5. CN- 6. (C2O4)2- 7. I- 8. OH2 9. NH3

Answer 25

1. Bromido 2. Fluorido 3. Oxido 4. Hydroxido 5. Cyanido 6. Oxalato 7. Iodido 8. Aqua 9. Ammine

Question 26

If a complex is neutral, the names of metals...

Answer 26

doesn't change (literally just its name)

Question 27

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?

Answer 27

-ate is added. copper and iron cuprate and ferrate

Question 28

What is the difference between the name of a metal in a negative complex versus a neutral complex?

Answer 28

negative has an -ate. eg nickel - in a negative complex it's nickelate, but in a neutral complex it's just nickel

Question 29

What do the Roman Numerals in brackets at the end represent? Metal complexes are always within ___ brackets.

Answer 29

The oxidation state of the transition metal (eg ferrate (II) means the iron has a +2 oxidation state) [Square]

Question 30

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

Answer 30

Square brackets, start

Question 31

A Roman numeral put at the end of a complex's name, tells you...

Answer 31

the oxidation state of the T metal

Question 32

Name this complex: [Cu(OH2)6]2-

Answer 32

hexa-aqa-cuprate (II)

Question 33

Name this complex: (3k+[CoF5])2+

Answer 33

potassium-penta-fluorido-cobaltate (iv) (ate because the complex *is* negative)

Question 34

Name this complex: ([Fe(CN-)2(NH3)4]2Cl-)1+

Answer 34

tetra-ammine-di-cyanido-iron-chlorine (v)

Question 35

Ligand formula are written so the attaching atom comes ___.

Answer 35

first. ie OH2 - not H2O

Question 36

Ligand formula and names are always written ____.

Answer 36

alphabetically. (even if the name of the ligand starts with a different letter than its symbol, like aqua being OH2)

Question 37

Name this complex: [CoCl2 (NH3)4 ]

Answer 37

tetra-ammine-di-chlorido-cobalt (II)

Question 38

[CoCl2 (NH3)4 ] tetra-ammine-di-chlorido-cobalt (II) Notice how the 'Cl2' comes before the 'NH3', but 'chlorido' does not come before '___'

Answer 38

ammine

Question 39

In a complex of a transition metal, the d orbitals are no longer ___.

Answer 39

degenerate