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Chapter 3

Classification of Elements and Periodicity in Properties

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Classification of elements and periodicity in properties is a crucial topic in chemistry covered in class 11 CBSE. The topic provides a deep understanding of concepts involved in the periodicity of the element. In this article, you will find most concepts pertaining to NCERT Solutions for Class 11 chemistry, their elements, properties, as well as formulae. 

Classification of elements and periodicity in properties is an important chapter; therefore, the students are advised to go through it thoroughly to develop a robust understanding of various concepts, which will help you score higher grades in class 11. 

We have tailored our Classification of Elements and Periodicity in Properties NCERT Solutions chapter to meet our student's needs, which will further help them crack entrance examinations. This chapter has been prepared by our subject experts, where many aspects of periodicity are discussed wisely. This data follows a step-by-step procedure to help extract chapter 3 notes to solve the previous year's question papers.

To help students be thorough about each concept regarding chemistry chapter 3 class 11  Classification of Elements and Periodicity in Properties, all of the core principles are elaborated in easy-to-understand language, which will answer every query of your NCERT Textbook.

Topics covered in this Chapter- Contents table

Sr. No. 

Topics 

1

Classification of Elements and Periodicity in Properties (Introduction) 

2 

Why do we Need to Classify Elements? 

3 

Genesis of Periodic Classification 

4 

Modern Periodic Law and the present form of the Periodic Table 

5 

Nomenclature of Elements with Atomic Numbers > 100 

6 

Electronic Configurations of Elements and the Periodic Table 

7

Electronic Configurations and Types of Elements: s-, p-, d-, f – Blocks 

8 

Periodic Trends in Properties of Elements H2: Classification of Elements and Periodicity in Properties 

Classification of Elements and Periodicity in Properties: Introduction

In the early 1800s, Johann Wolfgang Dalereiner was the first scientist who attempted to formulate the classification of elements or periodicity in properties. During one of his experiments in 1829, he pointed out that elements with similar properties formed a group three, which he later termed as "Triads." some triads he classified are: 

  • Chlorine, Bromine, and Iodine 
  • Sulfur, Selenium, and Tellurium
  • Calcium, Strontium, and Barium 
  • Lithium, Sodium, and Potassium 

For CBSE students, chapter 11 Classification of Elements and Periodicity in Properties serves as an introduction to elements, their classification, and periodicity in properties. In this chapter, we have summarised the various aspects of elements, the need to classify elements, and other important topics that will help students obtain a better understanding of this concept and gain higher marks. 

Let's have a look at the topics below to obtain a better understanding of these topics.

Why do we need to classify elements? 

There could be various reasons why there's a need to classify elements. Below, we have listed some of them: 

  • Classification of elements promotes a clearer understanding of the properties of elements and their respective compounds. 
  • Depending on the positioning of elements in the periodic table, the properties of the elements and their compounds can be easily predicted. 
  • Once the elements are classified in the periodic table, it becomes easier to study, compare, and differentiate their properties and compounds from the various groups. 

Note- One should be aware of the fact that there are seven periods in the modern periodic table. It usually holds metals on the right-hand side and non-metals on the left side of the table, along with eighteen groups. These elements have similar chemical behaviour.

  1. Law of Triad: Johann Wolfgang Dalereiner noticed that elements with similar properties formed groups of three, which he later termed "Triads." These groups were known as Dalereiner's Triad, and this generation was known as the Law of Triad. 

2. Telluric Screw: Another attempt made for the classification of elements was by Chancourtois. He arranged the atoms in the increasing weight order and developed a cylindrical table to showcase the occurrence of properties.

3. Newland’s Law of Octave: In 1865, John Alexander introduced the law of Octave, where he arranged the atoms in the increasing weight order and pointed out that the property of the first element is similar to that of the 8th one.

4. Lothar Meyer Arrangement: Lothar Meyer developed a graphical representation of atomic volume and atomic weight of elements. In this process, he noticed that the elements whose properties were similar to each other occupied the same position on the graph.

5. Mendeleev Periodic Law: In 1869, the Russian chemist Dimitri Mendeleev began to develop the periodic table. He noted if the atoms are arranged in the increasing weight order, atoms with same properties are repeated at regular intervals forming a V.

It was developed after the introduction of the Mendeleev Periodic Law in 1869.

Earlier scientists were confused regarding the internal structure of an atom. However, after advancement in quantum theory, it unfolded that the atomic number is the base of a chemical element. 

To bring clarity in thoughts, the Mendeleev Periodic Law was modified, known as the Modern Periodic Table, also the present form of the periodic table, which is widely accepted, including horizontal rows known as periods and the vertical columns are called groups.

Nomenclature of Elements with Atomic Numbers > 100
The modern periodic table has around 118 elements.

Atomic number

Name 

Symbol

IUPAC Name

IUPAC Symbol

101

Unnilunium

Unu

Mendelevium

Md

102

Ununbium

Unb

Nobelium

No

103

Ununtrium

Unt

Lawrencium

Lr

104

Unnilquadium

Unq

Rutherfordium

Rf

105

Unnilpentium

Unp

Dubnium

Db

106

Unnilhexium

Unh

Seaborgium

Sg

107

Unnilseptium

Uns

Bohrium

Bh

108

Unniloctium

Uno

Hassnium

Hs

109

Unnilennium

Une

Meitnerium

Mt

110

Ununnilium

Uun

Darmstadtium

Ds

111

Unununium

Uuu

Roentgenium

Rg

112

Ununbium

Uub

Copernicium

Cp

113

Ununtrium

Uut

   

114

Ununquadium

Uuq

   

115

Ununpentium

Uup

   

116

Ununhexium

Uuh

   

117

Ununseptium

Uus

   

118

Ununoctium

Uuo

   

119

Ununennium

Uue

   

120

Unbinilium

Ubn

   

121

Unbiunium

Ubu

   

130

Untrinilium

Utu

   

140

Ununnilium

Uqn

   

150

Unpentnilium

Upn

   

160

Unhexnilium

Uhn

   

170

Unseptnilium

Usn

   

180

Ununnilium

Uon

   

190

Ununnilium

Uen

   

200

Binilnnium

Bnn

   

201

Binilunium

Bnu

   

201

Binibium

Bnb

   

300

Trinilnilium

Tnn

   

400

Quadnilnilium

Qnn

   

500

Pentnilnilium

Pnn

   

900

Enilnilium

Enn

   

 

Electronic Configurations of Elements and the Periodic Table

NUMBER

ELEMENT

ELECTRON CONFIGURATION

1

Hydrogen

1s1

2

Helium

1s2

3

Lithium

[He]2s1

4

Beryllium

[He]2s2

5

Boron

[He]2s22p1

6

Carbon

[He]2s22p2

7

Nitrogen

[He]2s22p3

8

Oxygen

[He]2s22p4

9

Fluorine

[He]2s22p5

10

Neon

[He]2s22p6

11

Sodium

[Ne]3s1

12

Magnesium

[Ne]3s2

13

Aluminum

[Ne]3s23p1

14

Silicon

[Ne]3s23p2

15

Phosphorus

[Ne]3s23p3

16

Sulfur

[Ne]3s23p4

17

Chlorine

[Ne]3s23p5

18

Argon

[Ne]3s23p6

19

Potassium

[Ar]4s1

20

Calcium

[Ar]4s2

21

Scandium

[Ar]3d14s2

22

Titanium

[Ar]3d24s2

23

Vanadium

[Ar]3d34s2

24

Chromium

[Ar]3d54s1

25

Manganese

[Ar]3d54s2

26

Iron

[Ar]3d64s2

27

Cobalt

[Ar]3d74s2

28

Nickel

[Ar]3d84s2

29

Copper

[Ar]3d104s1

30

Zinc

[Ar]3d104s2

31

Gallium

[Ar]3d104s24p1

32

Germanium

[Ar]3d104s24p2

33

Arsenic

[Ar]3d104s24p3

34

Selenium

[Ar]3d104s24p4

35

Bromine

[Ar]3d104s24p5

36

Krypton

[Ar]3d104s24p6

37

Rubidium

[Kr]5s1

38

Strontium

[Kr]5s2

39

Yttrium

[Kr]4d15s2

40

Zirconium

[Kr]4d25s2

41

Niobium

[Kr]4d45s1

42

Molybdenum

[Kr]4d55s1

43

Technetium

[Kr]4d55s2

44

Ruthenium

[Kr]4d75s1

45

Rhodium

[Kr]4d85s1

46

Palladium

[Kr]4d10

47

Silver

[Kr]4d105s1

48

Cadmium

[Kr]4d105s2

49

Indium

[Kr]4d105s25p1

50

Tin

[Kr]4d105s25p2

51

Antimony

[Kr]4d105s25p3

52

Tellurium

[Kr]4d105s25p4

53

Iodine

[Kr]4d105s25p5

54

Xenon

[Kr]4d105s25p6

55

Cesium

[Xe]6s1

56

Barium

[Xe]6s2

57

Lanthanum

[Xe]5d16s2

58

Cerium

[Xe]4f15d16s2

59

Praseodymium

[Xe]4f36s2

60

Neodymium

[Xe]4f46s2

61

Promethium

[Xe]4f56s2

62

Samarium

[Xe]4f66s2

63

Europium

[Xe]4f76s2

64

Gadolinium

[Xe]4f75d16s2

65

Terbium

[Xe]4f96s2

66

Dysprosium

[Xe]4f106s2

67

Holmium

[Xe]4f116s2

68

Erbium

[Xe]4f126s2

69

Thulium

[Xe]4f136s2

70

Ytterbium

[Xe]4f146s2

71

Lutetium

[Xe]4f145d16s2

72

Hafnium

[Xe]4f145d26s2

73

Tantalum

[Xe]4f145d36s2

74

Tungsten

[Xe]4f145d46s2

75

Rhenium

[Xe]4f145d56s2

76

Osmium

[Xe]4f145d66s2

77

Iridium

[Xe]4f145d76s2

78

Platinum

[Xe]4f145d96s1

79

Gold

[Xe]4f145d106s1

80

Mercury

[Xe]4f145d106s2

81

Thallium

[Xe]4f145d106s26p1

82

Lead

[Xe]4f145d106s26p2

83

Bismuth

[Xe]4f145d106s26p3

84

Polonium

[Xe]4f145d106s26p4

85

Astatine

[Xe]4f145d106s26p5

86

Radon

[Xe]4f145d106s26p6

87

Francium

[Rn]7s1

88

Radium

[Rn]7s2

89

Actinium

[Rn]6d17s2

90

Thorium

[Rn]6d27s2

91

Protactinium

[Rn]5f26d17s2

92

Uranium

[Rn]5f36d17s2

93

Neptunium

[Rn]5f46d17s2

94

Plutonium

[Rn]5f67s2

95

Americium

[Rn]5f77s2

96

Curium

[Rn]5f76d17s2

97

Berkelium

[Rn]5f97s2

98

Californium

[Rn]5f107s2

99

Einsteinium

[Rn]5f117s2

100

Fermium

[Rn]5f127s2

101

Mendelevium

[Rn]5f137s2

102

Nobelium

[Rn]5f147s2

103

Lawrencium

[Rn]5f147s27p1

104

Rutherfordium

[Rn]5f146d27s2

105

Dubnium

*[Rn]5f146d37s2

106

Seaborgium

*[Rn]5f146d47s2

107

Bohrium

*[Rn]5f146d57s2

108

Hassium

*[Rn]5f146d67s2

109

Meitnerium

*[Rn]5f146d77s2

110

Darmstadtium

*[Rn]5f146d97s1

111

Roentgenium

*[Rn]5f146d107s1

112

Copernium

*[Rn]5f146d107s2

113

Nihonium

*[Rn]5f146d107s27p1

114

Flerovium

*[Rn]5f146d107s27p2

115

Moscovium

*[Rn]5f146d107s27p3

116

Livermorium

*[Rn]5f146d107s27p4

117

Tennessine

*[Rn]5f146d107s27p5

118

Oganesson

*[Rn]5f146d107s27p6

Electronic Configurations and Types of Elements: s-, p-, d-, f – Blocks 
These are elements in the long-form in the modern periodic table.

  • General electronic configuration of sodium is 1s22s22p63s1 .
  • The electronic configuration of carbon (p-) is 1s22s22p2.

Similarly, the d and f-block elements have the same properties.

Periodic Trends in Properties of Elements 

Periodic tables have specific properties. The periodic trends explain these properties of elements. These trends are ionic radius, atomic radius, chemical reactions, electronegativity, electron affinity, ionization energy, and metallic character. 

1. What are the properties and classification of elements?

The properties are the base on which the elements are mainly classified. One primary element classification is metalloids, metals, and nonmetals. Elements that have similar chemical properties are grouped known as “families.”

2. What is periodicity in properties Class 11? 

When the properties of an element keep on repeating at regular intervals, it is known as the periodicity in properties. In case the elements are placed in the increasing atomic number order in the periodic table, then the chances of elements with repeating properties increases.

3. What are the critical benefits of Class 11 Chemistry Chapter 3 Classification of Elements and Periodicity in Properties?

To predict the behaviour of the element, even if it’s newly introduced, a thorough understanding of class 11 classification of elements and periodicity in properties chapter plays a significant role.

 

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