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  Lanthanide Elements Homework Help - K-12 Grade Level, College Level Chemistry

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.

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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

4f3

4f4

4f5

4f6

4f7

4f8

4f9

4f10

4f11

4f12

4f13

4f14

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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