Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Developing metals (DM) > Flashcards

Developing metals (DM) Flashcards

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

Transition metal definition

A

D-block elements which form one or more stable ions which have incompletely filled d-orbitals

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

In the first row of d-block elements, which elements are not transition metals?

A

Sc and Zn

Sc only forms 1 ion, which has an empty d subshell

Zn only forms 1 ion, which has a full d-subshell

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

Electronic configuration of d-block elements:

A
  • 4s fills before 3d as 4s has a lower energy
  • Cr and Cu are exceptions- an electron in the 4s orbital moves into the 3d as this gives a lower energy
  • Electrons then fill 3d subshells singly before pairing up
  • When ions are formed, the 4s orbital always loses its electrons first
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Determining the iron content using a redox titration:

A
  • Fe (II) ions can be oxidised to Fe (III) ions by potassium manganate (VII) in acidic solution
  • Known volume of Fe (II) solution is titrated with potassium manganate (VII) solution of known concentration
  • Potassium manganate in burette
  • End point is when the first permanent pink colour is observed
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Common oxidation states of iron

A

Fe (II)

Fe (III)

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

Common oxidation sates of copper

A

Cu (I) - unstable

Cu (II)

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

Colour of iron (II) hydroxide

Colour of Iron (III) hydroxide

A

Dark green

Red/orange

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

Colour of aqueous iron (II) ions

Colour of aqueous iron (III) ions

A

Pale green

Yellow

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

Colour of aqueous copper (I) ions

Colour of aqueous copper (II) ions

A

Unstable - no colour

Pale blue

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

Colour of copper (II) hydroxide

Colour of copper (II) ammonia complex

A

Blue

Dark blue

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

Describe what happens when ammonia solution is added to copper (II) hydroxide

A
  • Ammonia = source of OH- ions
  • Pale blue precipitate of copper (II) hydroxide dissolves to give a deep blue solution of a copper ammonia complex ion

PALE BLUE——————DARK BLUE

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

Ligand definition

A

A negatively charged ion or neutral molecule with a LONE PAIR of electrons which it donates to a central TRANSITION METAL ION to form a COORDINATE bond

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

Complex ion definition

A

A transition metal ion or atom surrounded by a number of ligands

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

Ligand substitution definition

+ when it occurs

A

When a ligand is swapped for another ligand

Usually results in a colour change

Occurs if the new complex formed is more stable than the previous complex

Sometimes substitution is only partial

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

Writing complex ions

A

The overall charge of the complex ion is the sum of the charge on the central metal ion + the charges on the ligands

(Fe(H2O)6)^2+

(Fe(H2O)6)^3+

(Cu(H2O)6)^2+

(Cu(NH3)4)^2+

(CuCl4)2-

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

Another word to describe a coordinate bond:

A

Dative

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

Monodentate ligand definition

A

a ligand that attaches to a transition metal through one atom only (eg OH-, H2O)

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

Bidentate ligand definition

A

a ligand with 2 atoms with lone pairs or negative charges, which forms 2 bonds to a metal ion

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

Structure of ethanedioate

How does it act as a ligand?

A

-^OO=C-C=OO^- (see notes)

Bidentate ligand- has 2 atoms with lone pairs which forms 2 coordinate bonds to a metal ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Iron (II) hydroxide and iron (III) hydroxide reaction/colour change with ammonia solution

A

Both do not form complexes with ammonia

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Coordination number definition:

A

the number of coordinate bonds that are formed with the central metal atom

Usual coordination numbers are 4 and 6

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Shape of complex ion and bond angle when coordination number is 6:

A

Octahedral

90 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Shape of complex ion and bond angle when coordination number is 4

A

Tetrahedral - 109.5

OR

Square planar - 90

24
Q

Why shape of complex ion differs when coordination number is 4?

A

Shape either tetrahedral or square planar

Depends on ligands

If ligands are small (eg water or ammonia) 6 can fit around central metal ion

If ligands are larger (eg Cl-) only 4 can fit around central metal ion

25
Q

How ligands lead to colour in transition metal complexes:

A
  • Normally the 3d orbitals of transition metal ions all have the same energy
  • When ligands bond to the ions- orbitals close to the ligands are pushed to slightly higher energy levels
  • As a result- some of the orbitals gain energy which splits the 3d orbitals into 2 different energy levels
  • When visible light absorbed- electrons can be excited to a higher energy level
  • Light is only absorbed if the energy of the light matches the energy gap between the 2 energy states in the atom
  • The frequency of the light absorbed is proportional to the gap between the energy levels (E=hv)
  • The complementary colour is transmitted (the colour we see)
26
Q

Why do transition metal ions of the same element often have different colours in aqueous solutions?

A

Transition metal ions have different oxidation states

The energy needed to excite a d electron to the higher energy level depends on the oxidation state of the metal

27
Q

What does the colour of a transition metal complex depend on?

A
  • Number of d-electrons present in the transition metal ion
  • The arrangement of ligands around the ion - this affects the splitting of the d sub-shell
  • The nature of the ligand- different ligands have a different effect on the relative energies of the d orbitals in a particular ion
28
Q

Complementary colours:

A
  • Complementary colours- opposite each other in a colour wheel
  • Mix 2 complementary colours of light = white light
  • The colour of a transition metal solution is the complement of the colour that’s absorbed
  • eg- blue solution- absorbs the red part of the spectrum
29
Q

Colorimetry definition

A

A technique that can be used to find the concentration of a coloured solution

30
Q

Explain how colorimetry can be used to find the concentration of a transition metal ion solution

A
  • Intensity of colour depends on the concentration of the solution
  • The more concentrated the solution, the darker its colour and the more light it absorbs
  • Absorbance of a solution is proportional to its concentration
  • High absorbance reading means a lot of light has been absorbed + sample is very concentrated
31
Q

Describe how to use a colorimeter to measure concentrations of solutions

A

1) Make up a series of standard solutions of the test solution of known concentration
2) Select a filter with the complementary colour to the test solution
3) Zero the colorimeter with a tube of pure solvent
4) Measure the absorbance of the standard solution + plot a calibration curve, showing the concentration (x) against absorbance (y)
5) Measure the absorbance of the test solution and read off the concentration from the calibration curve

32
Q

Describe how to use a visible spectrophotometer to measure concentrations of solutions

A

Uses a beam of light of a single colour (monochromatic light)

1) The beam of monochromatic light is passed through a solution of the complex
2) A detector measures the light intensity before and after it’s passed through the solution- from this can work out absorbance
3) Different complexes absorb different colours- so produce characteristic visible absorption spectra
4) Use calibration curve to convert absorbance data to find concentration data

33
Q

Balancing redox equations rules:

A

Check:

1) Atoms balance
2) Oxidation states balance
3) Charges balance

If oxidising agent contains oxygen- might have to add H+ ions and water to make equation balance

34
Q

Components of an electrochemical cell:

A
  • 2 half-cells joined together
  • Half cell- a metal dipped in a salt solution of the metal’s ion
  • Voltmeter- measures the maximum potential difference between 2 half cells (Ecell)
  • Salt bridge- provides an ionic connection between 2 half cells
35
Q

Ecell definition

A

The potential difference between 2 half cells

36
Q

Electrochemical cells involving metal ion/metal half cells

A

Eg- zinc/copper electrochemical cell

  • Zinc has a more negative electrode potential (more reactive metal). Loses electrons more easily- oxidised
  • Copper has a more positive electrode potential- (less reactive metal)- accepts electrons- reduced
37
Q

What direction do electrons flow in an electrochemical cell?

A

From negative half cell to positive half cell

38
Q

Half cell with more negative electrode potential- metal is………………..

Half cell with more positive electrode potential- metal is………………..

A

Oxidised

Reduced

39
Q

Electrochemical cells involving half-cells based on different oxidation states of the same element in aqueous solution:

A

Eg- Fe 2+, Fe 3+

  • Conversion between these ions occurs on surface of the electrode
  • As neither reactants nor products are solids, something else needs to be the electrode
  • Platinum or graphite used- conducts electricity, inert
40
Q

Standard electrode potential definition:

A

Standard electrode potential of a half cell is the voltage under standard conditions when the half cell is connected to a standard hydrogen electrode

41
Q

What are the standard conditions for measuring the standard electrode potential of a half cell?

A
  • Concentration of solutions = 1 mol dm-3
  • Temperature = 298 K
  • Pressure = 100 kPa
42
Q

Using a hydrogen electrode half cell to find the standard electrode potential of another metal ion:

A
  • Measure electrode potential of half cell against standard hydrogen electrode
  • Standard hydrogen electrode half-cell has value - 0.00V
  • Means voltage reading will be equal to the standard electrode potential of other half cell
43
Q

Calculating Ecell:

A

Ecell = (more positive electrode potential - more negative electrode potential)

44
Q

Using electrode potentials to predict whether a reaction will happen:

A
  • Write the 2 half equations as reduction
  • Look at electrode potential of each half equation- one with more negative electrode potential- flipped to oxidation
  • Combine half equations + make sure electrons are balanced
45
Q

Techniques and procedures to set up and use electrochemical cells

A

1) Get a strip of each metal being investigated
2) Clean surface of metals using a piece of emery paper + clean grease from electrodes using propanone
3) Place each electrode into a beaker filled with a solution containing ions of that metal
4) Create a salt bridge to link the solutions together (eg soak a piece of filter paper in salt solution + drape it between 2 beakers)
5) Connect electrodes to voltmeter using crocodile clips + wires

46
Q

Despite predicting a reaction will occur through an experiment using electrochemical cells, explain why it may not occur

A
  • Rate of reaction may be so slow that reaction may not appear to happen
  • Too high activation energy- stops a reaction from occuring
  • Prediction could be wrong if conditions not standard
47
Q

Electronic configuration of Chromium (24 electrons)

A

Chromium prefers to have 1 electron in each orbital of the 3d sub-shell and just 1 electron in the 4s sub-shell

Gives it more stability

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

48
Q

Electronic configuration of Copper (29 electrons)

A

Copper prefers to have a full 3d subshell and just 1 electron in the 4s subshell

Gives it more stability

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

49
Q

Characteristics of transition metals:

A
  • Exist in variable oxidation states

- Form coloured ions in solution

50
Q

Equation involved in the formation of rust:

A

Fe2+ + 2e- ———————– Fe

2H2O + O2 + 4e- ————————– 4OH-

As the iron half equation has a more negative electrode potential, the iron is oxidised and oxygen is reduced

Overall: 2H2O + O2 + 2Fe ———- 2Fe 2+ + 4OH-

Fe2+ and OH- ions formed combine to produce precipitate of iron (II) hydroxide

Further oxidised to iron (III) hydroxide

This gradually turns into hydrated iron (III) oxide (rust)

51
Q

Where oxidation and reduction occur when a water droplet causes iron to rust

A

Edges of droplet- oxygen concentration is higher so oxygen is reduced to hydroxide ions (cathode)

Centre of droplet by iron- oxygen concentration is low so iron is oxidised (anode) This is where iron corrodes. Electrons flow away from this site to areas with higher oxygen concentrations

(This explains why corrosion is always greatest at the centre of a water droplet - where oxygen supply is limited)

52
Q

Rusting prevention:

A
  • paint/apply oil- provides barrier between metal + atmospheric oxygen
  • Sacrificial method- involves adding a metal with a more negative electrode potential to prevent rusting. Other metal is oxidised + corrodes first. Release of electrons promotes reduction in iron half cell to ensure iron in solid state always exists

eg- coating of zinc can be sprayed onto object (galvanising) or blocks of zinc can be bolted to the iron

53
Q

Why is iron less likely to rust in alkaline conditions?

A
  • More OH- ions
  • Shifts position of equilibrium of water half equation left to try to reduce number of OH- ions
  • Electrons produced
  • Shifts position of Fe half equation towards Fe(s)
  • Less Fe 2+ so less rust produced
54
Q

Why do transition metals and their compounds make good catalysts?

A
  • Can change oxidation states by gaining or losing electrons within their d-orbitals
  • Means they can transfer electrons to speed up reactions
55
Q

Transition metals and their compounds as hetrogeneous catalysts:

A
  • Catalyst and reactants- different physical states

- Transition metals can use 3d and 4s electrons of the atoms on the catalyst surface to form weak bonds to reactants

56
Q

Transition metals and their compounds as homogeneous catalysts:

A
  • Catalyst and reactants- same physical state

- Change oxidation states by gaining or losing electrons within their d-orbitals

Chemistry (6 decks)

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