A metal with an incomplete d sub-level in one or more oxidation states
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Name two metals that are not transition metals and why?
Scandium - no d electrons; Zinc - full d sub level
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Name some properties of transition metals
Shiny, conduct heat and electricity, form complex ions with ligands, variable oxidation states, catalytic properties, magnetic properties, coloured compounds
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True/ false: The 3d and 4s sub levels are similar in energy
True
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Which electrons are lost first in transition metals?
4s electrons
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What oxidation state do all transition metals have?
+2
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Why can some transition metals go up to the 3+ and 4+ oxidation state?
The ionisation energies are such that they can lose up to two d electrons
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Give examples of two metals that can get into the 3+ or 4+ oxidation states?
Fe3+ and Mn4+
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How is the M4+ ion found in these higher oxidation states? Why?
Covalently bonded or as an oxyanion because the metal ion is not as free at higher oxidation states
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Which process is iron used as a catalyst?
Haber process
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Which process is manganese (IV) oxide used as a catalyst?
Breakdown of hydrogen peroxide
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Which process is vanadium (V) oxide used as a catalyst?
Contact process
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Which process is Nickel used as a catalyst?
Hydrogenation reaction
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What is the contact process?
Making sulfuric acid from sulfur dioxide and oxygen
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What is hydrogenation?
Converting unsaturated fatty acids into saturated fatty acids
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Name two metals used in catalytic converters in cars
Palladium and platinum
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Which transition metal is found in vitamin B12?
Cobalt
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Which transition metal is found in haem?
Iron
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In general, which transition metals are magnetic?
The ones that contain unpaired electrons
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What is ferromagnetism?
Permanent magnetism
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Give examples of metals with ferromagnetism
Cobalt and nickel
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What causes ferromagnetism?
When the unpaired electrons align parallel to each other
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What is an application of ferromagnetism?
Compasses that align with the Earth's magnetic field to point North
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What is paramagnetism?
The slight magnetic attraction present when a magnetic field or electric field is applied to the metal
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How does paramagnetism work?
Spinning unpaired electrons causes a magnetic field and this reinforces the magnetic field
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The more unpaired electrons...
The more paramagnetic the complex is
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How many unpaired electrons must a diamagnetic metal have?
None! - They are all paired
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If the ligands are low in the spectrochemical series when split...
D orbitals only split by small amount - electrons can occupy all d orbitals giving four units of paramagnetism
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If the ligands are high in the spectrochemical series...
Larger splitting so only the lower d orbitals will be occupied so no unpaired electrons - diamagnetic
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Name a substance that can be paramagnetic or diamagnetic
Iron (II) complex ions- ([Ar] 3d6)
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Name three ligands that are neutral
Water, carbonyl, ammonia
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Name three ligands with a 1- charge
Chlorine, bromine, carbon nitride
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Other cards in this set
Card 2
Front
Name two metals that are not transition metals and why?
Back
Scandium - no d electrons; Zinc - full d sub level
Card 3
Front
Name some properties of transition metals
Back
Card 4
Front
True/ false: The 3d and 4s sub levels are similar in energy
Back
Card 5
Front
Which electrons are lost first in transition metals?
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