Introduction of Lanthanide
The Lanthanide or lanthanoid (IUPAC nomenclature) series consists of the 15 metallic chemical elements with atomic numbers 57 to 71, from lanthanum till lutetium.
These 15 lanthanide elements, together with the chemically alike elements scandium and yttrium, are often together called as the rare earth elements.
The easy chemical symbol Ln is used in common discussions of lanthanide chemistry to refer to any of the lanthanides. All of the lanthanides except one are f-block elements, resulting in filling of the 4f electron shell; lutetium, a d-block element, is also generally taken to be a lanthanide because of its chemical similarities with the other 14 elements. All lanthanide elements create trivalent cations Ln3+, whose chemistry is determined by the ionic radius which decreases progressively from lanthanum to lutetium.
The lanthanide elements are group of elements with atomic number increasing from 57 i.e. lanthanum) to 71 i.e. lutetium. They are called as lanthanide because the lighter elements in the series are chemically equivalent to lanthanum. Strictly saying both lutetium and lanthanum have been labeled as group 3 elements as they both possess a single valence electron in the d shell. However, both elements are frequently involved in any common discussion of the chemistry of the lanthanide elements.
Chemical element
La
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
Atomic number
57
58
59
60
61
62
63
64
65
66
67
68
69
70
71
Density (g/cm3)
6.162
6.770
6.77
7.01
7.26
7.52
5.244
7.90
8.23
8.540
8.79
9.066
9.32
6.90
9.841
Melting point (°C)
920
795
935
1024
1042
1072
826
1312
1356
1407
1461
1529
1545
824
1652
Atomic electron configuration*
5d1
4f15d1
4f3
4f4
4f5
4f6
4f7
4f75d1
4f9
4f10
4f11
4f12
4f13
4f14
4f145d1
Ln3+ electron configuration*]
4f0
4f1
4f2
4f8
Ln3+ radius (pm)
103
102
99
98.3
97
95.8
94.7
93.8
92.3
91.2
90.1
89
88
86.8
86.1
Common Properties of the Lanthanides
1. Silvery-white metals that discolor when expose to air forming oxides.
2. Comparatively soft metals. Hardness increases fairly with higher atomic number.
3. Moving from left to right diagonally the period (increasing atomic number), the radius of every Lanthanide 3+ ion gradually decreases. This is known as 'lanthanide contraction'.
4. High boiling points and melting points.
5. highly reactive.
6. React with water to form hydrogen (H2), gradually in cold or rapidly upon heating. Lanthanides generally bind to water.
7. React with H+ (dilute acid) to liberate H2 (rapidly at room temperature).
8. React in an exothermic reaction with H2.
9. Be on fire easily in air.
10. They are highly strong reducing agents.
11. Their compounds are commonly ionic.
12. At elevated temperatures, many rare earths catch fire and burn vigorously.
13. Most of the rare earth compounds are strongly paramagnetic.
14. Various rare earth compounds fluoresce strongly in ultraviolet light.
15. Lanthanide ions tend to be pale, resulting in weak, narrow, forbidden f x f optical transitions.
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