Transition Metals Flashcards

Unit 1

1
Q

five properties of transition metals:

A

*have atoms/ions with an incomplete d-subshell
*can form complexes
*have variable oxidation states
*show catalytic ability
*form coloured ions

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2
Q

what is the definition of a transition metal?

A

a metal that, in at least one of its stable ions, has a partially filled d-subshell

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3
Q

what is the oxidation number of a free, uncombined atom?

A

0

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4
Q

what is the oxidation number of an ion of a single atom?

A

the same as its charge

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5
Q

in it’s compounds, Fluorine always has the same oxidation number. What is it?

A

-1

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6
Q

what must the algebraic sum of the oxidation number always be equal to?

A

0 or the charge of the ion

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7
Q

what is happening when there is an increase in the oxidation number?

A

oxidation

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8
Q

what is happening when there is a decrease in the oxidation number?

A

reduction

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9
Q

what do compounds containing metals in high oxidation states tend to be?

A

oxidising agents

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10
Q

what do compounds containing metals in low oxidation states tend to be?

A

reducing agents

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11
Q

what are two examples of oxidising agents?

A

acidified permanganate and acidified dichromate

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12
Q

what can be observed as oxidation state changes?

A

colour change

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13
Q

what other term can be used to refer to metal complexes?

A

co-ordination compounds

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14
Q

what are the molecules or ions which surround central metal atom/ion called?

A

ligands

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15
Q

what do ligands contain in order to form a co-ordinate bond?

A

(at least one) lone pair of electrons

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16
Q

what type of bond is a co-ordinate bond?

A

a dative covalent bond

17
Q

how is the dative covalent bond formed?

A

the ligand donates the lone pair of electrons into an empty orbital in the transition metal atom/ion.

18
Q

what is meant by a monodentate ligand?

A

ligands that form one co-ordinate bond to the metal atom/ion.

19
Q

what is meant by a bidentate ligand?

A

ligands that form two co-ordinate bonds to the metal atom/ion.

20
Q

what type of ligands bind in haemoglobin?

A

quadridentate ligands

21
Q

what is an example of a hexadentate ligand?

22
Q

what is meant by the co-ordination number?

A

the total number of co-ordinate bonds from the ligand to the central metal atom/ion.

23
Q

why are ligands referred to as Lewis bases?

A

they donate electrons

24
Q

why are the metals, in turn, referred as Lewis acids?

A

they accept the electrons

25
what is a homogenous catalyst?
a catalyst that is in the same state as the reactants
26
what is a heterogenous catalyst?
a catalyst that is in a different state to the reactants
27
how does the size of the energy gap between the two sets of d orbitals vary?
*the transition metal ion *the oxidation state of the transition metal *the type of ligand
28
what determines the colour of the metal complex?
the size of the split
29
what shows the ability of ligands to cause splitting?
the spectrochemical series
30
what can be determined based on absorbance of visible light?
The concentration of transition metals in solution (the higher the concentration of ions, the greater the absorbance)
31
what is the process which heterogenous catalysts work trough called?
chemisorption
32
how can transition metals act as catalysts?
they have unfilled d-orbitals
33