Brainscape's Knowledge GenomeTM

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


See full index

y1 mchem s2 > Inorganic: Transition Metals > Flashcards

Inorganic: Transition Metals Flashcards

1
Q

Definition of transition metal?

A

One which has a partially filled d (or f) electron sub shell in any common oxidation state

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

Properties of transition metals?

A

Lustre
Malleable & ductile
High MPts/ BPts

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

What group has elements with +1 ions

A

Alkali metals

Li, Na, K, Rb, Cs

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

What group has elements with +2 ions?

A

Group 2

Be, Mg, Ca, Sr, Ba

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

Which element can display every oxidation state from -2 to +7?

A

Manganese

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

Colour arises from movement in which electron subshell

A

d subshell

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

What is a paramagnetic compound

A

Compounds with unpaired electrons

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

Uses/ Applications of transition metals?

A 
Construction 
Medical 
Electronics
Colour
Catalysis 
Medicine
Biology
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Quantum number n =

A

Principal quantum number

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

The principal quantum number n defines what

A

The electron shell

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

The quantum number l =

A

Angular quantum number

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

The angular quantum number defines what

A

The orbital shape

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

The quantum number ml=

A

Magnetic quantum number

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

The magnetic quantum number defines what

A

The orientation

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

The quantum number ms =

A

Spin quantum number

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

The spin quantum number defines what

A

The spin

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

S orbitals have the angular momentum number of

A

0

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

P orbitals have the angular momentum of

A

1

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

D orbitals have the angular momentum number of

A

2

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

S orbitals have how many electrons?

A

2

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

P orbitals have how many electrons?

A

6

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

d orbitals have how many electrons?

A

10

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

[Ar] - is what

A

Argon - 18th electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Atomic radii … over a period

A

Decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Definition of nuclear charge

A

The effective nuclear charge (Z*) is the positive charge “felt” by the outer electrons. It is equal to the total change in the nucleus (Z) minus the effect of shielding (or screening of the charge by electrons in lower energy shells

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Equation for nuclear charge

A

Z* = Z-S

Z* = ENC
Z   = atomic number 
S   = shielding
27
Q

4s orbital and 3d orbital values

A 
4s = 0
3d = 0.35
28
Q

Why are groups 5&6 so close in terms of nuclear charge?

A

Due to the lananthanide contraction, they all have really poor shielding

29
Q

Definition of complex

A

Formed when a number of ions or molecules combine with a central metal ion to form an entity, in which the number of atoms attached directly to the central metal ion exceeds the formal oxidation state of this ion

30
Q

Low oxidation states properties

A

Lattice structures

Arrays if oxide or halide ions

TM ions regularly arranged in octahedral or tetrahedral holes in the lattice

Electrically neutral

Oxidation states up to +3

31
Q

High oxidation states

A

More covalent

Often molecular

Oxidation states above +3

32
Q

Metal ions is placed where in the ligand formula

A

To the left

33
Q

Ligands bond to metal centres by …

A

Donation one or more electron pairs in order to form bonds

34
Q

Both the electrons are donated from one of the atoms into an empty atomic orbital, forming a which type of bond?

A

Dative covalent bond

35
Q

complex name and number of ligands for di

A

BIS and 2

36
Q

complex name and number of ligands for tri

A

TRIS and 3

37
Q

complex name and number of ligands for tetra

A

TETRAKIS and 4

38
Q

complex name and number of ligands for penta

A

PENTAKIS and 5

39
Q

On traversing the 3d elements (Sc to Zn) the +2 oxidation state becomes less stable and lower oxidation states come more stable

True or false?

A

False

+2 Oxidation states become more stable and higher oxidation states become less stable

40
Q

Coordination geometry in transition elements is defined by what?

A

Number of ligands

41
Q

Most 3d elements have which coordination number?

A

4-6

42
Q

Longer atoms at the beginning of the period can have a coordination number of 7 or 8, why?

A

Bigger molecules

43
Q

Ligands with coordination number 2

A

Linear - 180°

44
Q

Ligands with coordination number 3

A

Trigonal planar - 120°

45
Q

Ligands with coordination number 4

A

Tetrahedral - 109.5°
Or
Square planar - 90°

46
Q

Ligands with coordination number 5

A 
Trigonal bipyramidal, 
equatorial - 120°
Axial - 90°
Or
Square pyramidal - 90°
47
Q

Ligands with coordination number 6

A

Octahedral - 90°

48
Q

The axial angle on trigonal bipyramidal ligand?

A

90°

49
Q

The equatorial angle on trigonal bipyramidal ligand?

A

120°

50
Q

Ionisation isomers are isomers of a … which differ in the …

A

Anion which is coordinated to the metal atom

51
Q

Hydrate Isomers are … which differ in the placement of

A

Water molecules in the complex

52
Q

Coordination isomers are isomers consisting of complex … & complex … which differ

A

Cations and ions

In the distribution of the ligand between metal ions

53
Q

Linkage isomers are … which differ in the atom of ..

A

The ligand which is bonded to the metal centre, this requires a ligand which has more than one potential donor atom

54
Q

Optical isomers are compounds which are …

A

Non superimposable mirror images of one another

55
Q

Early translation elements

Good at oxidation? Y/N
Form higher oxidation states? Y/N
Less stable lower oxidation states? Y/N

A

Very susceptible
Yes they form higher oxidation states
Lower oxidation states are less stable

56
Q

Later translation elements

Good at oxidation? Y/N
Form higher oxidation states? Y/N
Less stable lower oxidation states? Y/N

A

Harder to oxidise
Form generally lower oxidation states
Higher oxidation states are less stable

57
Q

Why is extraction of Titanium from ores difficult?

A

It is very electrophilic making it harder to reduce

Very oxophillic so hard to remove oxygen

58
Q

Why is the Kroll process run under inert gas?

A

To prevent oxygen being present in the reaction

59
Q

Reduction of TiCl4

What is used as the reducing agent?

A

Magnesium

60
Q

TiCl4 had which formal oxidation state?

A

+4

61
Q

Solvolyis reactions require a reactant which has what?

A

An acidic hydrogen atom

62
Q

Titanium chlorides are used as catalysts in the formation of which compounds?

A

Alkenens and polymers

63
Q

Process of removing iron from its ores

A

Coke burned in air

Co2 produced at base

Reduced by excess coke to give CO

CO is the reducing agent that reduces the iron oxides

The the top (coolest) iron 3* is reduces to iron 2 (FeO)
FeO then reduces in the hottest part to form Fe liquid

y1 mchem s2 (3 decks)

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