Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > Transition Metals > Flashcards

Transition Metals Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

What is the ‘best’ definition of a transition metal?

A

That a translation metal has at least one ion with an incomplete d-subshell (bar Sc and Zn)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What two metals (from the top row of transition metals) are excempt from most transition metal rules ?

A

Zinc and Scandium

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What are the properties of transition metals?

A

They are found in the d-block of the periodic table; they usually have an incomplete d-subshell; each has at least one ion with an incomplete d-subshell; they can produce different valencies ; they can produce coloured compounds; and they can act as catalysts. *all except Sc and Zn.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Which two transition metals fill their 4s and 3D orbitals differently than usual?

A

Cr - 4s^1 3d^5

Cu - 4s^1 3d^10

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Why are copper and chromiums 4s orbitals only 1/2 filled ?

A

There is extra stability in the 3d orbital gained by filling or 1/2 filling it. Simultaneously the 4s orbital is still stable as it is 1/2 full

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Transition metals exist in…

A

Variable oxidation states of differing stability

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Why do transition metals exist in variable oxidation states?

A

They can loose all their electrons from their 4s orbital as well as some or sometimes all of their 3d orbital electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

How can electron configurations be used to explain oxidation states ?

A

They can often show which oxidation state would be more stable for the orbitals in the atom to form.
(With the exception of Cu^2+ kind which form in the place of Cu^+ ions even though the Cu^+ ions are more stable

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What can oxidation numbers keep track of?

A

They can help keep track of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is the assumed oxidation number of oxygen ?

A

2-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is the assumed oxidation number of hydrogen?

A

+1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What are ligands?

A

An atom,molecule or ion that contains at least one lone pair

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What are transition metal complexes ?

A

A metal atom or ion surrounded by ligands with the ligands bound to the metal through co-ordinate covalent bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

How do metals form transition metal complexes ?

A

The metals make use of empty hybrid orbitals, usually involving at least some d-orbital

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What is a dative covalent bond ?

A

When both the electrons making a covalent bond come from the same atom.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Is a dative covalent bond the same as a co-ordinate covalent bond ?

A

Yes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Why are ligands described as dentate?

A

The ligands are considered to bite the metal ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

How can ligands be classified ?

A

By the number of bonds they can make with a central atom or ion.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What is a monodentate ligand ?

A

Ligands that can only form 1 bond with a metal atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What are examples of molecules containing monodentate ligands ?

A

NH3 , Cl^- , CN^- ( a cyanide ion) and H2O

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

How do ligands bond to metal ions ?

A

By donating one or more electron pairs into unfilled metal orbitals

22
Q

What are bidentate ligands ?

A

Ligands that can form 2 bonds with a metal atom/ion

23
Q

What are examples of molecules containing bidentate ligands ?

A

Ethylenediamine

Oxalate ions

24
Q

What are polydentate ligands ?

A

Ligands that can form many bonds with a metal atom or ion

25
Q

What are examples of molecules containing polydentate ligands ?

A

EDTA ions

Triphosphate ions

26
Q

What are coordination numbers ?

A

The number of bonds formed between the metal ion and the ligands in a complex ion

27
Q

What is the normal range of coordination numbers ?

A

2 and 8 bonds

28
Q

What is the most common coordination number ?

A

6

29
Q

What is the second most common coordination number ?

A

4

30
Q

What is the third most common coordination number ?

A

2

31
Q

Do all metals only have one coordination number ?

A

No, many often have multiple coordination numbers

32
Q

What are the rules of naming complexes ?

A

The cation is always named before the anion
The ligands are always named before the metal ion
Always add an ‘o’ to the root name of an anion
Use prefixes to indicate the no. simple ligands
The oxidation state of the central metal ion is designated a Roman numeral in brackets
When more then one type of ligand is present they are named alphabetically
If the complex ion has a negative change add ‘ate’ to the Latin name of the metal

33
Q

What is a cation ?

A

The positive ion in a metal complex

34
Q

What is an anion?

A

The negative ion in a metal complex

35
Q

What is the name of the ligand (H2O) ?

A

Aqua

36
Q

What is the name of the ligand NH3 ?

A

Ammine

37
Q

What is the name of the ligand CO

A

Carbonyl

38
Q

What creates the circumstances that leads to the absorption of some light from the visible spectrum ?

A

Interactions between ligands and electrons occupying the d-orbitals

39
Q

Which compounds / ions are often coloured ?

A

Simple ions and transition metals

Because they absorb light fro maje visible spectrum

40
Q

Why are transition metals coloured?

A

Because they absorb light of certain wavelengths because the d-orbitals in the compounds aren’t degenerate

41
Q

What colour is observed in a metal compound if green light is absorbed ?

A

Red and blue light is transmitted so purple/magenta is seen

42
Q

What colour is seen in transition metal complexes if red light is absorbed ?

A

Green and blue light is transmitted hence a green/blue colour is seen

43
Q

What colour is observed in a metal complex if blue light is absorbed ?

A

Red and green light is transmitted hence yellow is seen ?

44
Q

When does a complex become degenerate?

A

When ligands approached an isolated metal ion and the d -orbitals split

45
Q

Why do the d-orbitals split ?

A

Due to ligands approaching the isolated metal ion causing electro plastic repulsion. Some d orbitals are raised to a higher energy than the other orbitals.

46
Q

What is d-d orbital splitting ?

A

When the d orbitals have different energies and no ñonger become degenerate (symbol 🔼)

47
Q

Do d-orbitals split the same in every molecule ?

A

No, they split differently depending on the shape of the molecule.

48
Q

What does the energy difference between d-orbitals depend on ?

A

The position of the ligands in the spectrochemical series

49
Q

Why do many transition metals act as catalysts?

A

Their ability to exist in a variety of oxidation states

50
Q

How do transition metals work as catalysts?

A

They provide an alternative pathway with a lower activation energy which speeds up the reaction and reverts to its original oxidation state when the reaction has finished

51
Q

How does a transition metal existing in a variety of oxidation states allow it to provide alternative routes for reactions ?

A

The impact essence of unpaired d electrons which allow intermediate complexes to form

52
Q

What are the two different types of catalysis ?

A

Heterogeneous - where the catalyst is in a different state to the reactants
Homogeneous - where the catalyst is in the same state as the reactants

Chemistry (7 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions