chemistry - unit 1.3 Flashcards

1
Q

What are the d-block transition metals?

A

Metals with an incomplete d subshell in at least one of their ions.

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2
Q

What does the filling of the d-orbitals follow?

A

The aufbau principle, with the exception of chromium and copper atoms.

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3
Q

What are these exceptions due to?

A

The special stability associated with the d subshell being half-filled or completely filled.

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4
Q

When atoms from the first row of the transition elements form ions, which electrons are lost first?

A

The 4s electrons that are lost first rather than the 3d electrons.

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5
Q

When is an element said to be in a particular oxidation state?

A

When it has a specific oxidation number.

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6
Q

What do uncombined elements have an oxidation number of?

A

0

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7
Q

What do ions containing single atoms have an oxidation number of?

A

The same as the charge on the ion.

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8
Q

In most of its compounds, what does oxygen have an oxidation number of?

A

-2

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9
Q

In most of its compounds, what does hydrogen have an oxidation number of?

A

+1

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10
Q

What must the sum of all the oxidation numbers of all the atoms in a neutral
compound add up to?

A

0

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11
Q

What must the sum of all the oxidation numbers of all the atoms in a polyatomic ion equal?

A

The charge on the ion.

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12
Q

What can a transition metal have?

A

Different oxidation states in its compounds.

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13
Q

What may compounds of the same transition metal in different oxidation states have?

A

Different colours.

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14
Q

What can oxidation be defined as?

A

An increase in oxidation number.

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15
Q

What can reduction be defined as?

A

A decrease in oxidation number.

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16
Q

What can be used to determine whether oxidation or reduction has occurred.

A

Changes in oxidation number of transition metal ions.

17
Q

What are compounds containing metals in high oxidation states often?

A

Oxidising agents, whereas compounds with metals in low oxidation states are often reducing agents.

18
Q

What are ligands?

A

They may be negative ions or molecules with non-bonding pairs of electrons that they donate to the central metal atom or ion, forming dative covalent bonds.

19
Q

What can ligands be classified as?

A

Monodentate, bidentate, up to hexadentate.

20
Q

How can you deduce the ligand classification?

A

From a formula or structure of the ligand or complex.

21
Q

What is known as the coordination number?

A

The total number of bonds from the ligands to the central transition metal.

22
Q

In a complex of a transition metal, what are the d-orbitals?

A

No longer degenerate.

23
Q

When does splitting of d-orbitals to higher and lower energies occur?

A

When the electrons present in approaching ligands cause the electrons in the orbitals lying along the axes to be repelled.

24
Q

What do you call ligands that cause a large different in energy between subsets of d-orbitals?

A

Strong field ligands.

25
Q

What do weak field ligands cause?

A

A small energy difference.

26
Q

What is the spectrochemical series?

A

Ligands placed in an order of their ability to split d-orbitals.

27
Q

What can the colours of many transition metal complexes be explained in terms of?

A

d-d transitions.

28
Q

When is light absorbed?

A

When electrons in a lower energy d-orbital are promoted to a d-orbital of higher energy.

29
Q

When do electrons transition to higher energy levels?

A

When energy corresponding to the ultraviolet or visible regions of the electromagnetic spectrum is absorbed.

30
Q

What light of one colour is absorbed, what will be observed?

A

The complementary colour.

31
Q

What can transition metals and their compounds act as?

A

Catalysts.

32
Q

What are heterogeneous reactants in?

A

A different state to the reactants.

33
Q

How can heterogeneous catalysis be explained in terms of?

A

The formation of activated complexes and the adsorption of reactive molecules onto active sites.

34
Q

What is thought to allow activated complexes to form?

A

The presence of unpaired d-electrons or unfilled d-orbitals.

35
Q

What can heterogenous catalysts provide?

A

Reaction pathways with lower activation energies compared to the uncatalysed reaction.

36
Q

What are homogeneous catalysts in?

A

The same state as the reactants.

37
Q

How can homogeneous catalysis be explained in terms of?

A

Changing oxidation states with the formation of intermediate complexes.