3d-block Transition Metal Advanced A Level
Inorganic Chemistry:
Appendix 10 Extended
3d–block data table -
A collection of data
sets on the properties of the 3d–block metals including the 1st series
of transition metals
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INDEX of advanced revision notes on 3d block
and transition metal chemistry
All my advanced UK A level
(~US grades 11-12 honors)
inorganic
chemistry notes
GCSE level (~US grade 9-10)
basic Transition Metal Chemistry Revision Notes
Appendix 10
Extended DATA TABLE Extended SUMMARY FOR 3d BLOCK
& TRANSITION METALS
|
Group number |
3 |
4 |
5 |
6 |
7 |
8 |
9 |
10 |
11 |
12 |
|
Z
and symbol |
21
Sc |
22
Ti |
23
V |
24
Cr |
25
Mn |
26
Fe |
27
Co |
28
Ni |
29
Cu |
30
Zn |
|
property\name |
scandium |
titanium |
vanadium |
chromium |
manganese |
iron |
cobalt |
nickel |
copper |
zinc |
|
melting
pt./oC |
1541 |
1668 |
1910 |
1857 |
1246 |
1538 |
1495 |
1455 |
1083 |
420 |
|
boiling
pt./oC |
2836 |
3287 |
3380 |
2672 |
1962 |
2861 |
2870 |
2730 |
2567 |
907 |
|
density/gcm–3 |
2.99 |
4.54 |
6.11 |
7.19 |
7.33 |
7.87 |
8.90 |
8.90 |
8.92 |
7.13 |
|
1st
IE/kJmol–1 |
631 |
658 |
650 |
653 |
717 |
759 |
760 |
737 |
745 |
906 |
|
2nd
IE/kJmol–1 |
1235 |
1310 |
1414 |
1592 |
1509 |
1561 |
1646 |
1753 |
1958 |
1733 |
|
3rd
IE/kJmol–1 |
2389 |
2652 |
2828 |
2987 |
3248 |
2957 |
3232 |
3393 |
3554 |
3832 |
|
4th
IE/kJmol–1 |
7089 |
4175 |
4507 |
4740 |
4940 |
5290 |
4950 |
5300 |
5326 |
5730 |
|
5th
IE/kJmol–1 |
8844 |
9573 |
6294 |
6690 |
6990 |
7240 |
7670 |
7280 |
7709 |
7970 |
| Z and symbol |
21 Sc |
22 Ti |
23 V |
24 Cr |
25 Mn |
26 Fe |
27 Co |
28 Ni |
29 Cu |
30 Zn |
|
atomic
radius/pm |
161 |
145 |
132 |
125 |
124 |
124 |
125 |
125 |
128 |
133 |
|
M2+
ionic radius/pm |
na |
90 |
88 |
84 |
80 |
76 |
74 |
72 |
69 |
74 |
|
Relative polarising power M2+ ion |
na |
2.2 |
2.3 |
2.4 |
2.5 |
2.6 |
2.7 |
2.8 |
2.9 |
2.7 |
|
M3+
ionic radius/pm |
81 |
76 |
74 |
69 |
66 |
64 |
63 |
62 |
na |
na |
|
Relative polarising power M3+ ion |
3.7 |
3.9 |
4.1 |
4.3 |
4.5 |
4.7 |
4.8 |
4.8 |
na |
na |
|
M4+
ionic radius/pm |
na |
68 |
60 |
56 |
54 |
na |
na |
na |
na |
na |
|
Relative polarising power M4+ ion |
na |
5.9 |
6.7 |
7.1 |
7.4 |
na |
na |
na |
na |
na |
|
Z and symbol |
21 Sc |
22 Ti |
23 V |
24 Cr |
25 Mn |
26 Fe |
27 Co |
28 Ni |
29 Cu |
30 Zn |
|
oxidation
states,
less common/stable |
+3
only |
+2,+3,+4 |
+2,+3,+4,+5 |
+2,+3,+6 |
+2,+3,+4,+6,+7 |
+2,+3 |
+2,+3 |
+2,+3 |
+1,+2 |
+2
only |
|
simplified electron
configuration |
2,8,9,2 |
2,8,10,2 |
2,8,11,2 |
2,8,13,1 |
2,8,13,2 |
2,8,14,2 |
2,8,15,2 |
2,8,16,2 |
2,8,18,1 |
2,8,18,2 |
|
outer electrons |
3d14s2 |
3d24s2 |
3d34s2 |
3d54s1 |
3d54s2 |
3d64s2 |
3d74s2 |
3d84s2 |
3d104s1 |
3d104s2 |
|
Electrode
pot'l M(s)/M2+(aq) |
na |
–1.63V |
–1.18V |
–0.90V |
–1.18V |
–0.44V |
–0.28V |
–0.26V |
+0.34V |
–0.76V |
|
Electrode
pot'l M(s)/M3+(aq) |
–2.03V |
–1.21V |
–0.85V |
–0.74V |
–0.28V |
–0.04V |
+0.40 |
na |
na |
na |
|
Electrode
pot'l M2+(aq)/M3+(aq) |
na |
–0.37V |
–0.26V |
–0.42V |
+1.52V |
+0.77V |
+1.87V |
na |
na |
na |
|
Electronegativity |
1.36 |
1.54 |
1.63 |
1.66 |
1.55 |
1.83 |
1.88 |
1.91 |
1.90 |
1.65 |
|
Z
and symbol |
21
Sc |
22
Ti |
23
V |
24
Cr |
25
Mn |
26
Fe |
27
Co |
28
Ni |
29
Cu |
30
Zn |
|
Group number |
3 |
4 |
5 |
6 |
7 |
8 |
9 |
10 |
11 |
12 |
3d block data notes:
Atomic and ionic radii are
quoted in pm (1 picometre, 10–12 m), 1000 pm = 1 nm (1 nanometre
= 10–9 m)
na means 'not applicable' or 'not available'.
The
electronegativity values
are from the Pauling scale.
Redox potentials
See Appendix 11
Some 3d–block compounds, complexes, oxidation states
& electrode potentials
Ionic radii relate to the
'isolated' theoretical ion, NOT the hydrated aqueous ion.
Polarizing power is a measure of
the ions charge density (electric field effect) which has important chemical consequences e.g.
(i)
the bonding nature of metals with non–metals
e.g. relative ionic or a covalent character of the bonds in a MCln
molecule/ionic lattice,
(ii) and the
acidity of the hydrated
aqueous ion [M(H2O)6]n+(aq)
which is capable of donating protons.
The ion charge divided by the
ionic radius of the 'isolated ion' is a 'reasonable' number scale for easy comparison
of polarising power, and in the tables I've multiplied the
charge/radius by 100 to make a suitable scale.
Obviously, the larger the charge,
or the smaller the volume or radius, the greater the charge density or
polarising power, this in turn leads to more covalent character in the
e.g. chloride and increased acidity of the hexa–aqua–ion [M(H2O)6]n+(aq).
that is with increase in the n+ value.
Note that as the oxidation state
of the transition metal increases,
i.e.
increase in charge if an
ionic compound, the greater the polarising power of the cation, which
increases the covalent character of the compound, exemplified by
comparing iron(II) and iron(III) compounds or complex ions
e.g. FeCl2 is
essentially an ionic compound and FeCl3 covalent in
character,
The greater the polarising
power of the central metal ion, the greater the acidity of the hexaaqua
ion
e.g. [Fe(H2O)6]3+
is more acidic than [Fe(H2O)6]2+
Going from iron(II) to iron(III)
involves an increases in cationic positive charge and decrease in radius
of the 'isolated' central metal ion.
The decrease in radius is bound to
result from the same nuclear charge of 26+ 'pulling in' 24 and 23
electrons respectively,
i.e. less electron density in the same quantum
level, less space occupied.
For more details see
Transition Metals Appendix 1 Acidity of
hexaaqua–ions
Relative polarising power of
Groups 1–3 ions for comparison with the 3d block
ions above:
|
Group
of the Periodic Table |
Metal ion and ionic charge |
ionic radius/pm |
relative polarizing power
= 100 x charge / radius |
|
1 |
Na+ |
98 |
1.0 |
|
2 |
Mg2+ |
78 |
2.6 |
|
3 |
Al3+ |
60 |
5.0 |
|
1 |
K+ |
133 |
0.75 |
|
2 |
Ca2+ |
106 |
1.9 |
Note the substantial increase
in polarizing power of the cations across Period 3 from sodium to
aluminium as the ion charge increases and the ionic radius decreases.
From the data from Groups and 1 and 2 you can see the polarising power
of similarly charged cation decreases down a group as the ionic radius
increases.
|
INORGANIC Part
10 3d block TRANSITION METALS sub–index:
10.1–10.2
Introduction to 3d–block Transition Metal
chemistry
10.3
Chemistry of Scandium
* 10.4
Chemistry of Titanium
10.5
Chemistry of Vanadium
* 10.6
Chemistry of Chromium
10.7
Chemistry of Manganese
* 10.8
Chemistry of Iron
10.9
Chemistry of Cobalt
* 10.10
Chemistry of Nickel
10.11
Chemistry of Copper
* 10.12
Chemistry of Zinc
10.13
Selected chemistry of other Transition Metals e.g. Ag and Pt
Appendix 1.
Hydrated salts, acidity of
hexa–aqua ions
Appendix 2. Complexes
and ligands
Appendix 3. Complexes and isomerism
Appendix 4.
Electron configuration and colour theory
Appendix 5.
Redox
equations, feasibility of reaction, Eø
calculations
Appendix 6.
Catalysis - types and
effectiveness
Appendix 7.
Redox
equations - construction and balancing
Appendix 8. Stability
constants
of complexes and entropy
changes
Appendix 9. Colorimetric analysis
and determining a complex ion formula
Appendix 10 3d block
– extended data table
Appendix 11
3d–block transition metal complexes, oxidation states
& electrode potentials
Appendix 12
Hydroxide complex precipitate 'pictures',
formulae and equations
Advanced
Level Inorganic Chemistry Periodic Table Index: Part 1
Periodic Table history
* Part 2
Electron configurations, spectroscopy,
hydrogen spectrum,
ionisation energies *
Part 3
Period 1 survey H to He *
Part 4
Period 2 survey Li to Ne * Part
5 Period 3 survey Na to Ar *
Part 6
Period 4 survey K to Kr and important trends down a
group *
Part 7
s–block Groups 1/2 Alkali Metals/Alkaline Earth Metals *
Part 8
p–block Groups 3/13 to 0/18 *
Part 9
Group 7/17 The Halogens *
Part 10
3d block elements & Transition Metal Series
*
Part 11
Group & Series data & periodicity plots * All
11 Parts have
their own sub–indexes near the top of the pages
|
Periodic
Table - Transition Metal Chemistry - Doc
Brown's Chemistry. Revising
Advanced Level Inorganic Chemistry Periodic Table
Revision Notes.
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