Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > Transition Metals > Flashcards

Transition Metals Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

Define transition metals

A

Elements that contain an incomplete d-subshell of electrons as either an atom or an ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Properties of transition metals

A

Form complexes
These complexes tend to be coloured
Variable oxidation states
Can act as catalysts

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Define ligand

A

Molecule/ion that forms a coordinate bond to a metal by donating a pair of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Define Lewis base

A

Electron pair donator

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Define Lewis acid

A

Electron pair acceptor

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Define complex

A

Metal atom surrounded by ligands

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Define coordination number

A

The number of coordinate bonds around a metal ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

How many coordinate bonds does copper normally have

A

6

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What are the three types of ligand

A

Unidentate
Bidentate
Multidentate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Define unidentate

A

Forms 1 coordinate bond per molecule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Examples of unidentate ligands

A

NH3, H2O, Cl-, CN-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Define bidentate

A

Forms 2 coordinate bonds per molecule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Examples of bidentate ligands

A

1,2-diaminoethane, ethandioate ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Define multidentate ligands

A

Forms multiple coordinate bonds per molecule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Examples of multidentate ligands

A

EDTA and polyphyrin

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Which shape had the most ligand complexes

A

Octahedral

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Which shape usually contains Cl- ligands

A

Tetrahedral

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What metal ions are usually in square planar shapes

A

Pt2+ and Ni2+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What shape is cis-platin

A

Square planar

20
Q

What shape are complexes with a Ag+ metal ion

A

Linear

21
Q

Which type of ligands can have geometric isomerism

A

Unidentate ligands

22
Q

Which type of ligand can display optical isomerism

A

Bidentate ligands

23
Q

What changes the ease at which metals are oxidised

A

The pH of the solution and the nature of the ligands attached

24
Q

What do Alkaline conditions cause in a ligand complex

A

Hydrolysis of the ligand
This results in a complex with an increasingly negative charge
This causes easier oxidation as the ion is negative

25
Q

What does acidic conditions cause in a ligand complex

A

Prevents hydrolysis from taking place and the H+ ions provide electrons that reduce the complex ion

26
Q

Is Zn an oxidising or reducing agent

A

Reducing

27
Q

In a potassium manganite titration what properties must the acid have

A

Be strong, many H+
Not an oxidising agent (could react with the sample)
Not be a reducing agent (could react with MnO4- ions)

28
Q

Why can’t you use HCl in potassium manganate titrations

A

oxidised to Cl- by MnO4

29
Q

why can’t you use HNO3 in potassium manganate titrations

A

it is an oxidising agent

30
Q

why can’t you use concentrated H2SO4 in potassium manganate titrations

A

it could be an oxidising agent

31
Q

why does potassium manganate act as its own indicator

A

the pink colour intensifies due to an excess of Mn2+ once all of the Fe2+ have reacted

32
Q

what is the colour change for a potassium dichromate titration

A

orange to blue/green

33
Q

why is sodium diphenylaminesulphonate used in potassium dichromate titrations

A

to give a clearer end point, colourless to purple

34
Q

steps for redox titration calculations

A

write the half equations for the oxidising agent and reducing agent
combine equations
calculate the number of mols of the oxidising agent (MnO4 or CrO7)
calculate the number of mols of reducing agents
calculate the number of mols in the original solution
determine the concentration of the original solution or percentage of reducing agent

35
Q

the two commonly used oxidising agents when completing a redox titration with Fe2+

A

potassium dichromate and potassium manganate

36
Q

the two equations which find number of mols

A

n=cv

mols=mass/Mr

37
Q

define heterogeneous catalyst

A

a catalyst in a different phase from the reactants

38
Q

define homogeneous catalyst

A

a catalyst in the same phase as the reactants

39
Q

what makes a good catalyst

A

good adsorption or reactant molecules and the good desorption of products

40
Q

how does adsorption of a reactant onto a metal surface speed up a reactant

A

weakening bonds within the reactant molecule, reducing the Eact
causing a reactant molecule to break up onto more reactant molecules, lowering the Eact
holding a reactant in a particular position, increasing the chance of a collision in a favourable position
giving a higher concentration of a reactant on the catalyst surface increasing the chance of a favourable collision with another reactant

41
Q

how is a catalyst poisoned

A

the active sites are blocked

42
Q

how does homogeneous catalysis proceed

A

via a catalyst

43
Q

when does autocatalysis occur

A

when one of the products catalyses the reaction

44
Q

what is the acidity of solutions of metal ions decided by

A

charge of the metal ion

size of the metal ion

45
Q

why does charge of the metal ion affect pH

A

larger charge=greater dissociation=lower pH

46
Q

why does size of the metal ion affect pH

A

greater ionic charge to size ratio = greater dissociation = lower pH

47
Q

is the pH of a solution of M3+ ions or Mn2+ ions lower pH

A

Mn3+ ions

Chemistry (24 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions