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Advanced higher chemistry > Transition metals > Flashcards

Transition metals Flashcards

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1
Q

What is a d block transition metals

A

A metal which for at least one of its ions has an incomplete d sub shell.

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2
Q

Difference in orbital filling rules for transition metals

A

For copper and chromium (number 4 and 9) having a half filled or filled 3d sub shell is more stable than a 4s sub shell, so the last electron goes into the 3d sub shell.

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3
Q

Difference in ions formed in transition metals

A

In transition metals the 4s electrons are lost before the 3d electrons .

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4
Q

Oxidation number rules

A

Uncombined elements have ON =0
Ions of single atoms have ON equal to charge
Oxygen has ON = -2 in compounds
In its compounds hydrogen has ON=+1
Compounds ON =0
Polyatomic ions ON= charge

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5
Q

Oxidation state

A

The oxidation number in Roman numerals

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6
Q

Oxidation number or state of individual ion in compound

A

Calculate oxidation number of other ion,
make it equal to the individual ion
Take away or add charge.

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7
Q

Oxidation effect on oxidation number

A

Increase

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8
Q

Reduction effect on oxidation number

A

Decrease

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9
Q

Transition metals oxidation states

A

Have variable oxidation states with different stability

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10
Q

High oxidation states

A

Oxidising agents

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11
Q

Low oxidation states

A

Reducing agents.

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12
Q

Transition metal complex definition

A

A central metal atom or ion surrounded by ligands which have formed dative covalent bonds with the metal.

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13
Q

Ligand’s definition

A

Molecules or negative ions with non bonding electrons which they donate to the unfilled d sub shell

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14
Q

Common ligands ( negative ions)

A

Cl-
CN-
OH-

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15
Q

Common ligands (molecules)

A

H2O, NH3

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16
Q

Process of ligand forming covalent bond

A

The ligands non bonded electron pair will donate both electrons to the metal ions orbital and form a dative covalent bond.

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17
Q

Dative covalent bond

A

A covalent bond formed by a ligand donating a non bonded electron pair.

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18
Q

Dative bond properties

A

Identical to other covalent bonds after formed.

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19
Q

Types of ligand

A

Monodentate
Bidentate
Hexadentate

20
Q

Monodentate ligand

A

A ligand which donates one set of non bonded electrons

21
Q

Bidentate ligand

A

A ligand which donates two sets of non bonded electrons

22
Q

Hexadentate ligand

A

A ligand which donates 6 non bonded electron pairs

23
Q

Monodentate examples

A

OH2
NH3
CN-
OH-
F-
Cl-

24
Q

Bidentate examples

A

O2C2O2 2- oxalato
1,2-diaminoethane

25
Q

Hexadentate examples

A

EDTA

26
Q

Co-ordination number

A

The number of bonds between a ligand and a metal.
(Count)

27
Q

Iupac rules

A

The rules for naming metal complexes

28
Q

Metal complexes definition

A

A metal atom or ion bonded to ligands

29
Q

Rules for IUPAC formula

A

[metal ligandA ligandB]
Ligands are ordered alphabetically based on element which donates non bonded electron pair.

30
Q

Rules for IUPAC naming

A

Ligands are named alphabetically followed by
metal and oxidation state
Suffix e is now o
Water is aqua, ammonia is ammine and carbon monoxide is carbonyl
If negative oxidation state the metals suffix is -ate and iron is ferrite and copper is cuprate.

31
Q

How are metal complexes coloured

A

A metal complexes ligands will cause 3d orbital splitting which will allow electrons to be promoted from the lower 3d orbital to the higher 3d orbitals, this will allow the metal complex to absorb visible wavelengths of light and reflect complimentary wavelengths of light.

32
Q

Higher energy 3d orbitals

A

dx2-y2 and dz2

33
Q

Lower energy 3d orbitals

A

dxy, dxz, dyz

34
Q

Order of ligands from strong to weak

A

CN-, NH3, OH2 OH- F- Cl- Br- I-

35
Q

Strong field ligands

A

Ligands that cause a large energy gap between the upper and lower 3d orbitals, meaning more energy is needed for the d-d orbital transition.

36
Q

Weak field ligands

A

Ligands that cause a small energy gap between the upper and lower 3d orbitals meaning less energy is needed for the d-d orbital transition.

37
Q

What region of light do strong field ligands absorb

A

Ultraviolet light.

38
Q

Uv wavelengths of light

A

200 to 400nm

39
Q

Visible wavelengths of light

A

400 to 700nm

40
Q

What are typical catalysts

A

Transition metals

41
Q

Types of catalysts

A

Homogenous and heterogenous

42
Q

Homogenous catalyst

A

A catalyst which is in the same state as the reactants.

43
Q

Heterogenous catalyst

A

A catalyst which id in a different state to the reactants.

44
Q

How do heterogenous catalysts work

A

Reactant molecules approach the surface of the catalyst.
Due to the unfilled d orbitals in the catalyst the reactants form activated complexes and bond with the catalyst - this is known as adsorption .
The bonds between reactant molecules rearrange.
Product molecules will leave the surface of the catalyst.

45
Q

How do homogenous catalysts work

A

Homogenous catalysts change the oxidation state to make a reactant molecule more reactive and react faster.

46
Q

Absorption definition

A

Where reactant molecules collide with the surface of a heterogenous catalyst and stick to it

47
Q

How does absorption on heterogenous catalysts work

A

The presence of unfilled d orbitals allows the molecules to form activated complexes between the reactant and catalyst.

Advanced higher chemistry (8 decks)

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