Module 5: Transition Elements V2 Flashcards
1
Q
Define what is meant by a “d-block element”
A
An elements where the highest energy sub-shell is the d sub-shell. ✓
2
Q
Explain what is meant by a “transition element”
A
d-block element that forms a stable ion with a partially filled d sub-shell. ✓
3
Q
What charged ions do d-block elements normally form.
A
+2 ✓
4
Q
Which two elements are d-block elements but are not considered transition elements? Explain why
A
Sc and Zn are not transition elements because they do not form any stable ions with a partially filled d sub-shell. ✓
5
Q
Draw the energy level diagram to show the electron configuration for iron Fe2+
A
Remember, 4s is added/removed before 3d.
6
Q
Write the electron configuration for an atom of Fe and a Fe2+ ion.
State and explain whether iron is a transition element.
A
Fe is a transition element ✓
Its stable ion forms a partially filled d-subshell ✓
7
Q
Write the electron configuration for an atom of Sc and the Sc3+ ion.
State and explain whether scandium is a transition element.
A
Sc is not a transition element ✓
Its stable ion does not form a partially filled d-subshell ✓
8
Q
Write the electron configuration for an atom of Zn and the Zn2+ ion.
State and explain whether zinc is a transition element.
A
Zn is not a transition element ✓
Its stable ion does not form a partially filled d-subshell ✓
9
Q
Write the electron configuration for an atom of Cu and the Cu2+ ion.
State and explain whether copper is a transition element.
A
Cu is a transition element ✓
Its stable ion forms a partially filled d-subshell ✓
10
Q
Write the electron configuration for an atom of Cr and the Cr3+ ion.
State and explain whether chromium is a transition element.
A
Cr is a transition element ✓
Its stable ion forms a partially filled d-subshell ✓
11
Q
State what is meant by the term “homogenous catalyst”
A
Homogeneous catalysts are in the same state as the reactants. ✓
12
Q
Suggest what is meant by the term “heterogenous catalyst”
A
Heterogeneous catalysts are in a different state to the reactants. ✓
13
Q
State four properties of transition metals
A
Variable oxidation state ✓
Catalytic activity ✓
Formation of coloured ions ✓
Formation of complex ions ✓
14
Q
Which statement about elements in the d block of Period 4 of the periodic table is correct?
A
A ✓
15
Q
Which property/properties is/are correct for a transition element?
A The element has atoms with a partially filled d sub-shell.
B The existence of more than one oxidation state in its compounds.
C The formation of coloured ions.
A
B and C ✓
16
Q
What is the reason that zinc is not classified as a transition element?
A Zinc atoms contain a full d-sub-shell.
B There are no zinc ions with an incomplete d-sub-shell.
C Zinc does not form complex ions.
D Zinc ions are colourless.
A
B ✓
17
Q
Explain how transition metals can act as catalyst.
A
Transition metals have a variable oxidation state so they can be oxidised and reduced back to their initial oxidation state (i.e. regenerated). ✓
Reactants bind to transition metals by adsorption to form an intermediate as part of the new chemical pathway. ✓
They provide an alternative pathway for the reaction with a lower activation energy. ✓
18
Q
Give two examples of catalysts, and write the equation for which they catalyse.
A
19
Q
State the colour of a solution containing Fe2+ ions.
A
Green solution
Green has 2 e’s. Same number the charge.
20
Q
State the colour of Fe(OH)2.
A
Green precipitate
Green has 2 e’s. Same number the charge.
21
Q
State the colour of a solution containing Fe3+ ions.
A
Yellow solution
Y3llow
22
Q
State the colour of Fe(OH)3.
A
Brown precipitate
Brown. Those yellow leaves fall to the ground and become brown.
23
Q
State the colour of solid copper.
A
Shiny brown solid.
24
Q
State the colour of a solution containing Cu+ ions.
A
Colourless solution.
25
State the colour of CuI.
White precipitate.
26
State the colour of a solution containing Cu2+ ions.
Pale blue solution.
Or Cu (cuuuuu) rhymes with blueeeeee
| Copper, police, blue.
27
State the colour of a solution containing the following complex.
Deep blue.
28
State the colour of Cu(OH)2.
Blue precipitate
29
State the colour a solution containing the following complex.
Yellow
| Swimming pools, chlorine... why do we use it.
30
State the colour of a solution containing Cr3+ ions.
Violet
31
State the colour a solution containing the following complex.
Purple.
32
State the colour of Cr(OH)3.
Green precipitate.
33
State the colour a solution containing the following.
green.
34
State the colour of a solution containing dichromate ions.
Orange.
35
State the colour of a solution containing chromate ions.
Yellow.
36
State the colour of a solution containing Mn2+ ions.
Pale pink solution.
| Japanese, manganese, cherry blossom trees, yes they're pink.
37
State the colour of Mn(OH)2
Light brown precipitate.
38
State the colour of a solution containing manganate ions.
Purple solution.
39
Iron (II) ions are converted to iron (III) ions using acidified KMnO4 which in turn is converted to Mn2+ ions.
i) what is the colour change and type of reaction for iron?
ii) what is the colour change and type of reaction for manganese?
i) Oxidation ✓ Green to yellow ✓
ii) Reduction ✓ Purple to Pale Pink ✓
40
Ethanol is reacted with acidified dichromate which is converted to a Cr3+ (aq) ion.
i) what is the colour change and type of reaction for chromium?
ii) what is the type of reaction for the alcohol?
i) Reduction ✓ Orange to violet (green) ✓
ii) Oxidation ✓
41
Define what is meant by a "complex ion".
An ion which is bonded to (or surrounded by) ligands. ✓
42
Define what is meant by a "ligand".
a species that donates an electron pair to a metal ion ✓
and forms a dative covalent bond with the metal ion. ✓
43
Define what is meant by a "monodentate ligand".
donates one lone pair of electrons to the central metal ion ✓
forming one dative bond to the metal ion. ✓
44
Define what is meant by a "bidentate ligand".
donates two lone pairs of electrons to the central metal ion ✓
forming two dative bonds to the metal ion. ✓
45
Write the formula, state the name, and draw the structure of the two bidentate ligands you must remember in A-level Chemistry.
46
For the following complex:
1) State the formula of the ligand
2) State whether the ligand is monodentate/ bidentate/ multidentate
3) The formula of the central metal ion
4) The coordination number
5) The formula and shape of the complex ion
47
For the following complex:
1) State the formula of the ligand
2) State whether the ligand is monodentate/ bidentate/ multidentate
3) The formula of the central metal ion
4) The coordination number
5) The formula and shape of the complex ion
48
For the following complex:
1) State the formula of the ligand
2) State whether the ligand is monodentate/ bidentate/ multidentate
3) The formula of the central metal ion
4) The coordination number
5) The formula and shape of the complex ion
49
For the following complex:
1) State the formula and give the structure of the ligand
2) State whether the ligand is monodentate/ bidentate/ multidentate
3) The formula of the central metal ion
4) The coordination number
5) The formula and shape of the complex ion
50
For the following complex:
1) State the formula and give the structure of the ligand
2) State whether the ligand is monodentate/ bidentate/ multidentate
3) The formula of the central metal ion
4) The coordination number
5) The formula and shape of the complex ion
51
For the following complex:
1) Give the structure of the ligand
2) State whether the ligand is monodentate/ bidentate/ multidentate
3) The formula of the central metal ion
4) The coordination number
5) The formula and shape of the complex ion. Use (pic).
52
For the following complex, determine the structure of all ligands.
53
For the following complex, determine the structure of all ligands.
54
For the following complex, determine the structure of all ligands.
55
Draw the structure of the following and state the oxidation state and coordination number for the metal ion and the shape of the complex:
56
Define what is meant by the term "Stereoisomers".
Compounds with the same structural formula ✓
but a different arrangement of atoms in space ✓
57
Define what is meant by the term "Cis-Trans stereoisomerism"
58
Draw the Cis and Trans isomers for the following complex.
59
State whether the following are cis or trans isomers. Also, identify from the list, which complex is drawn incorrectly.
3, bond should go directly to O not H.
60
Define what is meant by the term "optical isomers".
Stereoisomers that are non-superimposable mirror images ✓
61
Draw the structures of the optical isomers present in the following complex.
62
Draw all isomers present in the following complex.
63
Define what is meant by a "ligand substitution" reaction and state the order of ligand binding strength for water, ammonia and chloride.
One ligand replaces another on the transition metal ion because it binds more strongly. ✓
64
When excess HCl is added to copper(II) ions, a ligand substitution reaction occurs. Give the equation for this reaction, including the shape and colour of any complexes.
## Footnote
Yes, a reversible arrow is needed.
65
When excess ammonia solution is added to copper (II) ions, a ligand substitution reaction occurs. Give the equation for this reaction, including the shape and colour of any complexes.
## Footnote
Yes, a reversible arrow is needed.
66
When excess ammonia solution is added to chromium (III) ions, a ligand substitution reaction occurs. Give the equation for this reaction, including the shape and colour of any complexes.
## Footnote
Yes, a reversible arrow is needed.
67
For the ligand substitution reactions of Cu and Cr, explain why an excess of HCl or ammonia solution is required.
To shift the position of the equilibrium to the right ✓
68
When excess HCl is added to a solution of copper (II) ions, a ligand substitution reaction takes place.
State and explain the expected change in appearance if water is added to the mixture.
69
Explain using ligand substitutions how blood transports oxygen around the body.
70
State the use of cis-platin
Anti-cancer drug. ✓
71
Explain using ligand substitutions why carbon monoxide is toxic.
72
A student adds ammonia solution (or sodium hydroxide solution) is added dropwise to a testube containg Iron(II) ions. The student continues to add ammonia solution (or sodium hydroxide solution) until in excess.
Predict what the student would observe, state the name of the reaction and write an equation for the reaction taking place.
Dropwise: Green precipitate forms. ✓
Excess: No visible change. ✓
Reaction: Precipitation. ✓
## Footnote
Green (2 e's for 2+)
73
A student adds ammonia solution (or sodium hydroxide solution) is added dropwise to a testube containg Iron(III) ions. The student continues to add ammonia solution (or sodium hydroxide solution) until in excess.
Predict what the student would observe, state the name of the reaction and write an equation for the reaction taking place.
Dropwise: Orange-brown precipitate forms. ✓
Excess: No visible change. ✓
Reaction: Precipitation. ✓
## Footnote
Y3LLOW
74
A student adds ammonia solution (or sodium hydroxide solution) is added dropwise to a testube containg Manganese(II) ions. The student continues to add ammonia solution (or sodium hydroxide solution) until in excess.
Predict what the student would observe, state the name of the reaction and write an equation for the reaction taking place.
Dropwise: light brown precipitate forms. ✓
Excess: No visible change. ✓
Reaction: Precipitation. ✓
75
A student adds a few drops of ammonia solution (or sodium hydroxide solution) to a testube containg Copper (II) ions.
Predict what the student would observe, state the name of the reaction and write an equation for the reaction taking place.
Dropwise: blue precipitate forms. ✓
Reaction: Precipitation. ✓
76
A student adds excess ammonia solution to a testube containg copper (II) ions.
Predict what the student would observe, state the name of the reaction and write an equation for the reaction taking place.
Deep blue solution. ✓
Ligand substitution. ✓
77
A student adds a few drops of ammonia solution (or sodium hydroxide solution) to a testube containg chromium (III) ions.
Predict what the student would observe, state the name of the reaction and write an equation for the reaction taking place.
Dropwise: grey-green precipitate forms. ✓
Reaction: Precipitation. ✓
78
A student adds excess ammonia solution to a testube containg chromium (III) ions.
Predict what the student would observe, state the name of the reaction and write an equation for the reaction taking place.
Purple solution ✓
Reaction: Ligand substituion. ✓
79
A student adds excess sodium hydroxide solution to a testube containg chromium (III) ions.
Predict what the student would observe and write an equation for the reaction taking place.
Green solution forms.✓
80
Chemist has a solution of Fe ions. How can they figure out which ion is present?
81
Sodium hydroxide is slowly added to a solution containing copper (II) ions. A student records the observation and then adds excess sodium hydroxide before recording final observations. Identify the compounds present, the type of reaction taking place and any observations at each stage.
82
A student adds ammonia dropwise to a transition metal ion to give a green precipitate. Excess ammonia is next added and the precipitate dissolves. Identify the compounds present and any observations at each stage.
83
Write an ionic equation with state symbols for the reaction between Mn2+ (aq) and NH3 (aq). Include any colour changes.
84
A student adds NaOH to an unknown transition metal solution and a brown precipitate is produced. The brown precipitate undergoes reduction with iodide ions to give a green coloured precipitate. Identify the transition metal ion in the unknown solution. Explain your answer.
85
A student adds ammonia dropwise to a transition metal ion to give a precipitate. The precipitate dissolves on addition of sodium hydroxide. Identify the transition metal complex present at each stage and any colours that would be seen.
86
A chemist adds ammonia dropwise and then in excess to a transition metal ions solution. Initially, a precipitate is seen which then dissolves to give a deep blue coloured solution. The student next adds distilled water to the deep blue solution and observes further changes. For each stage, write an equation for the reaction taking place, the type of reaction and colour changes involved. Explain why further observations were made when water was added to the deep blue solution.
87
88
89
The white solid copper (I) oxide reacts with hot dilute sulfuric acid in a disproportionation reaction to form a blue solution containing a shiny brown solid. Write an equation for this reaction and explain why it is disproportionation.
90
91
A student wants to test for the presence of halide, carbonate and sulfate ions. In which order should they do the tests. Explain your answer.
92
93
A and B are compounds of two different transition elements.
Two students carry out test-tube tests on aqueous solutions of A and B. They then analyse the results to identity A and B.The observations of Student 1’s tests are shown.
Analyse the results and answer the following.
Identify A and B and write their formulae.
Construct ionic equations for the formation of the products C–G from the relevant ions present in A(aq) and B(aq).
What was the purpose of adding HNO3 (aq) first in Test 2 and Test 3?
94
A and B are compounds of two different transition elements.
Two students carry out test-tube tests on aqueous solutions of A and B. They then analyse the results to identity A and B.The observations of Student 1’s tests are shown.
Analyse the results and answer the following.
Identify A and B and write their formulae.
Construct ionic equations for the formation of the products C–G from the relevant ions present in A(aq) and B(aq).
Student 2 accidentally used HCl (aq) instead of HNO3 (aq) for both Test 2 and Test 3. What different observations would Student 2 obtain? Explain your reasoning.
95
A and B are compounds of two different transition elements.
Two students carry out test-tube tests on aqueous solutions of A and B. They then analyse the results to identity A and B.The observations of Student 1’s tests are shown.
Analyse the results and answer the following.
Identify A and B and write their formulae.
Construct ionic equations for the formation of the products C–G from the relevant ions present in A(aq) and B(aq).
How could the procedure be modified to be certain of the conclusions from Test 3?
96
This question looks at the chemistry of transition elements.
Explain what is meant by the terms transition element, complex ion and ligand.
Discuss, with examples, equations and observations, the typical reactions of transition elements.
In your answer you should make clear how any observations provide evidence for the type of reaction discussed.
97
B and C are compounds of two different transition elements. A student carries out test tube reactions on aqueous solutions of B and C. The observations of the student’s tests are shown below. Identify compounds B-G giving equations to support your answer.
98
Complete the following diagram by adding in the missing formulae of compounds.
What type of reaction is reaction 1 and 2?
Reaction 1: Ligand subtitution.
Reaction 2: Redox.
99
B and C. ✓
100
A. ✓
101
3 ✓
102
Which property/properties is/are correct for a transition element?
A The element has atoms with a partially filled d sub-shell.
B The existence of more than one oxidation state in its compounds.
C The formation of coloured ions.
B and C. ✓
103
A ✓
104
A ✓
105
A and B ✓
106
D. ✓
107
D. ✓
108
B and C. ✓
109
What is the reason that zinc is not classified as a transition element?
A Zinc atoms contain a full d-sub-shell.
B There are no zinc ions with an incomplete d-sub-shell.
C Zinc does not form complex ions.
D Zinc ions are colourless.
B. ✓
110
111
112
