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IB CHEMISTRY HL > Periodicity HL > Flashcards

Periodicity HL Flashcards

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1
Q

What is a transition element

A

an element with an incomplete d sub-level or can form positive ions with an incomplete d sub-level

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2
Q

What element is not actually a transition element and why

A

Zinc: it has a complete d sub-level as an atom and ion
Sc: it has no d sub-level as an ion

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3
Q

What is the electron configuration for Cu

A

4s1 3d10

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4
Q

What is the electron configuration for Cr

A

4s1 3d5

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5
Q

List physical properties of transition metals

A
  • malleable and ductile
  • good electrical and heat conductor
  • high tensile strength
  • high melting + boiling points
  • show magnetic properties
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6
Q

List chemical properties of transition metals

A
  • variable oxidation states
  • formation of complex ions
  • coloured compounds
  • catalytic behaviour
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7
Q

Why do transition metals have variable oxidation states

A

the 3d and 4s orbitals close in energy which results in a small difference in ionisation energy (there is still a gradual increase in successive ionisation). Transition elements can lose varying number of electrons with the same relative ease

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8
Q

What is a complex ion

A

transition metal ions can form complexes which consist of a central metal ion and ligands

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9
Q

What are ligands

A

molecules or ions with a lone pair of electrons (or more) that form coordinate covalent bonds with a central metal ion

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10
Q

Properties/features of ligands

A
  • they have a lone pair of electron
  • they can be Lewis bases
  • they have a negative charge
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11
Q

What is a co-ordination number

A

the number of co-ordinate bonds

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12
Q

Name a couple of common ligands

A

H2O, OH-, CN-, NH3, Cl-

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13
Q

What is a bidentate ligand

A
  • they form 2 co-ordinate bonds with the central atom
  • each ligand contains 2 atoms with lone pairs
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14
Q

What is a polydentate ligand

A
  • they form more than 2 co-ordinate bonds with the central atom
  • each ligand contains more than 2 atoms with lone pairs
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15
Q

What is an example of a polydentate ligand

A

EDTA

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16
Q

What are coordination compounds

A

they are made up of complex ion and counter ions which balance the charge of the complex ion

17
Q

What is a co-ordinate bond

A

a covalent bond in which both electrons come from the same atom

18
Q

What is a catalyst

A

a substance that provides an alternative pathway with a lower activation energy

19
Q

What are the 2 types of catalysts

A

homogenous and heterogeneous

20
Q

Why are transition metals good catalysts

A

their ability to form variable oxidation states means they can accept electrons easily

21
Q

What is a heterogeneous catalyst

A

a catalyst that is in the same phase (physical state) as its reactants

22
Q

What is a homogenous catalyst

A

a catalyst that is in a different phase (physical state) from its reactants

23
Q

List examples of heterogeneous catalysts

A
  • Fe (Haber process)
  • Ni (hydrogenation of margarine)
  • Pd & Pt (catalytic converter)
  • V2O5 (Contact process)
  • MnO2 (decomposition of H2O2)
24
Q

List examples of homogenous catalysts

A
  • Fe (heamoglobin)
  • Co (vitamin B12)
25
Q

What does paramagnetic mean

A

substances that have unpaired electrons

26
Q

What does diamagnetic mean

A

substances that have no unpaired electrons

27
Q

What does ferromagnetic mean

A

only occurs with Fe, Co, Ni: the attraction to a magnetic field is so much stronger in these metals because a large number of unpaired electrons line up in regions called domains

28
Q

Why do transition metal compounds appear coloured

A

they absorb energy corresponding to certain parts of the electromagnetic spectrum and the complementary colour will be transmitted (ex: orange light being absorbed corresponds to blue light being transmitted)

29
Q

Describe the Crytsal Field Theory

A
  • As the ligand approaches the metal to form a complex ion the lone pairs of electrons on the ligand will repel the d orbital causing the five d orbitals to split: 3 to lower energy and two to higher energy
  • The energy gap between the two levels correspond to the wavelength of visible light
  • Electrons can transition from the lower to a higher set of d orbitals by absorbing certain wavelengths of light.
30
Q

What are the factors that affect the colour of transition metal compound

A
  • the size and types of ligands
  • the nuclear charge and identity of the metal ion
  • the oxidation state of the metal
  • the shape of the complex
31
Q

How does the nuclear charge affect the colour of the transition metal compound

A

The greater the charge density; the more strongly the ligand interacts with the metal ion causing greater splitting of the d-orbitals. As a result, a different colour of light is absorbed by the complex solution and a different complementary colour is observed.

32
Q

How does the oxidation state affect the colour of the transition metal compound

A

When the same metal is in a higher oxidation state that will also create a stronger interaction with the ligands

33
Q

The spectrochemical series

A

the higher up the ligan on the spectrochemical series, the greater their ability to separate the d-orbitals, the shorter the waevelegnth absorbed

IB CHEMISTRY HL (2 decks)

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