Brainscape's Knowledge GenomeTM

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


See full index

Chemistry A Level > 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

What is a transition metal?

A

A d-block element that forms at least one ion with a partially filled d-subshell

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

How many electrons can each orbital hold?

A

2

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

How many orbitals does the S sub-shell have?

A

1

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

How many orbitals does the P sub-shell have?

A

3

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

How many orbitals does the D sub-shell have?

A

5

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

How many orbitals does the F sub-shell have?

A

7

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

Which two d-block elements are not classified as transition metals?

A

Scandium and zinc, scandium only forms a 3+ ion meaning that it loses 2 electrons from the 4s orbital and loses its one electron from the 3d orbital meaning it has no electrons in its d sub-shell. Zinc only forms a 2+ ion, it loses 2 electrons from its 4s orbital leaving it with an complete d sub-shell meaning it doesn’t have a partially complete d sub-shell

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

What is the electronic configuration of chromium?

A

(Ar) 4s1 3d5

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

What is the electronic configuration of copper?

A

(Ar) 4s1 3d10

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

What are the key physical properties of transition metals?

A
  • Lustrous in appearance
  • High density
  • High melting and boiling points
  • When solid, exist as giant metallic lattices containing delocalised electrons which move freely to conduct electricity
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What are the chemical properties of transition metals?

A
  • Form coloured compounds/compounds of transition metals from coloured solutions when dissolved in water
  • Can have different oxidation states
  • Act as catalysts
  • These properties are a results of electron configurations of transition metals and in particular their partially filled d sub-shells
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Why are electrons from the 4s sub-shell l lost before electrons from the 3d sub-shell?

A

The 4s sub-shell is at a lower energy level than the 3d sub-shell

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

What is a disproportionation reaction?

A

Where one species is both oxidised and reduced in the same reaction eg. Cu2O + H2SO4 → Cu + CuSO4 + H2O
In this reaction Cu+(aq) is oxidised to Cu2+(aq) and reduced to Cu(s)

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

What is the colour of compounds in inorganic chemistry linked to?

A

The partially filled d sub-shell, for example, scandium doesn’t have a partially filled d sub-shell so forms a colourless solution when dissolved in water

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

How do transition metals act as catalysts?

A
  • Provide a surface that a reaction can take place on, reactants are absorbed and held in place for the reaction, after the reaction the products are desorbed and the metal remains unchanged
  • Transition metal ions have the ability to change their oxidation states, they then bind to reactants, forming intermediates as part of a chemical pathway, often with a lower activation energy which speeds up the reaction
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Which catalyst is used in the Haber process?

A

An iron catalyst, it increases the rate of reaction and it also decreases the temperature which the reaction takes place due to the lower activation energy of the alternative reaction pathway

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

Which catalyst us used in the contact process?

A

V2O5

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

What is the Haber process?

A

A chemical process that is used to make ammonia from nitrogen and hydrogen. Much of the ammonia produced is used in manufacturing agricultural fertilisers. N2(g) + 3H2(g) → 2NH3(g) (this is an equilibrium reaction)

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

What is the contact process?

A
  • 2SO2(g) + O2(g) → 2SO3(g) (equilibrium reaction)
  • Converts sulfur dioxide to sulfur trioxide. SO3 is used to manufacture H2SO4
  • Sulfuric acid is an important inorganic chemical with many uses such as; production of fertilisers, detergents adhesives and explosives and also used as the electrolyte in car batteries
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What is the catalyst required for the hydrogenation of alkenes?

A
  • Nickel metal, lowers the temperature and pressure needed to carry out the reaction
  • This process is used in the hydrogenation of unsaturated vegetable oils to saturated margarine spreads
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What catalyst is used in the decomposition of hydrogen peroxide?

A
  • Manganese dioxide

- 2H202(aq) → 2H2O(l) + O2(g)

22
Q

What catalyst is used in the production of hydrogen?

A
  • CuSO4

- Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g)

23
Q

What is a coordination number?

A

The number of coordinate bonds to the central metal ion

24
Q

What is a ligand?

A

A molecule or ion with a lone pair that donates this pair f electrons to the central metal ion to form a coordinate bond/dative covalent bond

25
Q

What is a coordinate bond/dative covalent bond?

A

A bond where one atom provides both electrons for the covalent bond. The central metal ion accepts the pair of electrons to form the coordinate bond

26
Q

What is a Lewis base?

A

An electron pair donor (a nucleophile)

27
Q

What is a Lewis acid?

A

An electron pair acceptor (an electrophile)

28
Q

What is the charge of an SCN ligand and a CN ligand?

A

-1

29
Q

What can NH2CH2CH2NH2 or ethane-1,2-diamine be abbreviated to?

A

En, the en ligand has a neutral charge

30
Q

What is the charge of the ethandioate ion (C2O4)?

A

2-

31
Q

What is the charge of the EDTA hexadentate ligand?

A

4-, it has 6 lone pairs of electrons to form coordinate bonds

32
Q

What is the molecular formula of the EDTA4- ion?

A

[NCH2CH2N(CH2COO)4]4-

33
Q

What is the shape of a complex with a coordination number of 6?

A

Octahedral with bond angle of 90º

34
Q

What is the shape of a complex containing 4 chloride ligands?

A

Tetrahedral bond angle 109.5º

35
Q

What shape are complexes containing nickel and platinum that have a coordination number of 4?

A

Square planar with bond angle 90º

36
Q

What is a cis-trans isomer in transition metal chemistry?

A
  • Where there are 4 monodentate ligands and two other monodentate ligands, the 2 other monodentate ligands are on opposite sides of the molecule in a trans isomer and at 90º in the cis isomer
  • This also works with 2 bidentate ligands and 2 monodentate ligands, with the monodentate ligands on opposite sides in the trans isomer and
37
Q

What is optical isomerism?

A

Where there are there are 3 bidentate ligands or two bidentate ligands and two monodentate ligands. Two molecules are formed that are mirror images of each other

38
Q

What is cis-platin’s main function?

A

Cis-platin [PtCl2(NH3)2] is used in the treatment of cancer cells, it binds to the DNA of the cancer cells which prevents the DNA from replicating and therefore the cell from dividing

39
Q

Why have alternative drugs to cis-platin been developed?

A

Cis-platin is a very effective drug but it has many nasty side effects, a new drug called carboplatin was developed that treats ovarian cancer, it has a lower dose and fewer side effects

40
Q

What happens when ammonia is added to a solution of aqueous copper(II) ions?

A
  • The solution of Cu2+ (aq) ions contains [Cu(H2O)6]2+ which have a characteristic pale blue colour
  • When NH3 (aq) is added a pale blue gelatinous precipitate of Cu(OH)2 is formed
  • When excess NH3 (aq) is added, the pale blue precipitate dissolves and a deep blue solution is formed containing [Cu(NH3)4(H2O)2]2+ ions
41
Q

What is the equation for the reaction between excess ammonia and aqueous solution of copper(II) ions?

A

[Cu(H2O)6]2+(aq) (pale blue solution) + 4NH3 (aq) ⇌ [Cu(NH3)4(H2O)2]2+(aq) (deep blue solution) + 4H2O(l)

42
Q

What is the equation for the formation of the precipitate of Cu(OH)2 when ammonia is added to a solution of aqueous copper(II) ions?

A

[Cu(H2O)6]2+(aq) + 2NH3 (aq) → Cu(OH)2(H2O)4 + 2NH4+ (aq)

43
Q

What happens when a hydrochloric acid is added to a solution of copper(II) ions?

A

The pale blue solution of copper (II) ions initially turns green on addition of HCl (aq), before eventually turning yellow, it turns green because the [CuCl4]2- ions have a yellow colour and the [Cu(H2O)6]2+ ions have a pale blue colour. The solution is initially a mixture of these two ions meaning that the solution is green

44
Q

What is the equation for the reaction between aqueous copper(II) ions and hydrochloric acid?

A

[Cu(H2O)6]2+(aq) + 4Cl-(aq) ⇌ [CuCl4]2-(aq) + 6H2O(l)

45
Q

Why does the [CuCl4]2- complex ion only have 4 ligands?

A

The chloride ligands are larger and have stronger repulsions than the water ligands so less chloride ions can fit around the same central metal ion. The [CuCl4]2- complex ion has a tetrahedral shape with a bond angle of 109.5º

46
Q

What happens when aqueous ammonia is added to a solution of aqueous chromium(III) ions?

A

A green precipitate is formed that dissolves to form a purple solution when excess ammonia is added

47
Q

What is the equation for the reaction between chromium(III) and ammonia to form a green precipitate?

A

[Cr(H2O)6]3+(aq) + 3NH3(aq) → Cr(OH)3(H2O)3 + 3NH4+(aq)

48
Q

What is the equation of the reaction to form the purple solution of [Cr(NH3)6]3+(aq)?

A

Cr(OH)3(H2O)3 + 6NH3(aq) ⇌ [Cr(NH3)6]3+(aq) + 3OH-(aq) + 3H2O(l)

49
Q

What gives blood its red colour?

A

When the Fe2+ in the haem group is bound to oxygen, the haem group is red in colour

50
Q

Why is carbon monoxide so dangerous?

A
  • It binds to the Fe2+ central ion instead of oxygen as haemoglobin has a higher affinity for CO than O2
  • Once CO has bound to the central ion, the change is irreversible meaning that the haemoglobin molecule can no longer carry oxygen around the body
  • This means that CO causes you to suffocate as you can’t intake any oxygen
51
Q

When [Mn(H2O)6]2+ (aq) is reacted with 2OH-(aq), Mn(OH)2(H2O)4 and 2H2O(l) is produced, what is the equation for the oxidation of the manganese complex, the manganese complex can be simplified to Mn(OH)2?

A

4Mn(OH)2 + O2 → 2Mn2O3 (manganese oxidation number = +3) + 4H2O

Chemistry A Level (15 decks)

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