Transition Metals

Define transition elements.
D-block elements that form at least 1 stable ion with incomplete d-subshells.
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Which elements in the d-block are not transition elements?
Scandium 3+ - empty d-subshell. Zinc 2+ - full d-subshell.
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Which transition elements do not follow the electron configuration rules?
Chromium - 4s1, 3d5 and copper - 4s2 3d10.
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Give three properties of transition metal elements.
Variable oxidation states, formation of coloured ions and catalytic behaviour.
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Give an examples of two different transition metals that form coloured ions and why they form them.
Transition metal form coloured compounds because they have variable oxidation states. Mn2+= pink, Mn7+= purple, Fe2+= green, Fe3+= brown.
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Explain the catalytic behaviour of transition elements.
By providing a reaction site to absorb, reacts and desorb or by easily transferring electrons due to the many oxidation states so can provide and accept electrons to form intermediates that provide alternate routes with lower Ea.
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Give examples of transition metals used as catalysts.
Fe(s) in Haber process, V2O5(s) in contact process and Ni(s) in hydrogenation of alkenes.
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What are the advantages and disadvantages of catalysts in industry?
Improve profits so save energy and time. They are toxic so need careful disposal.
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Other cards in this set

Card 2

Front

Which elements in the d-block are not transition elements?

Back

Scandium 3+ - empty d-subshell. Zinc 2+ - full d-subshell.

Card 3

Front

Which transition elements do not follow the electron configuration rules?

Back

Preview of the front of card 3

Card 4

Front

Give three properties of transition metal elements.

Back

Preview of the front of card 4

Card 5

Front

Give an examples of two different transition metals that form coloured ions and why they form them.

Back

Preview of the front of card 5
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