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The s-block elements consist of the elements in which the outermost electrons enter into the s-orbital. These elements are divided into two categories i.e, alkali metals or group 1 elements and alkaline earth metals or group 2 elements. Their oxides and hydroxides are alkaline in nature. The general electronic configuration of these elements is ns1 and ns2 respectively. The first element of these groups i.e, lithium and beryllium show deviation in their properties from their respective group and they resemble the second element of the following group. This is known as the diagonal relationship.
These elements have a large number of applications in our daily life such as washing Soda, it is also known as sodium carbonate. It is used for various purposes such as water softening, manufacture of glass, paper, paints, etc.
Limestone is also one of the important compounds of the s-block element. It is used to neutralize the acidic soils. It has various other applications as well such as, for making cement, in glassmaking industry and in construction works, etc.
There are also various other applications of s-block elements. In this article, you will get every important information regarding this chapter like important topics, how to prepare for this chapter and important books for preparation.
Important Topics
(i) Electronic configuration: The alkali metals or group 1 elements have the valence shell electronic configuration is ns1. The table given below describes the electronic configuration of the alkali metals.
Element | Symbol | Electronic configuration |
Lithium | Li | [He] 2s1 |
Sodium | Na | [Ne] 3s1 |
Potassium | K | [Ar] 4s1 |
Rubidium | Rb | [Kr] 5s1 |
Caesium | Cs | [Xe] 6s1 |
Francium | Fr | [Rn] 7s1 |
(ii) Atomic and ionic radii: Alkali metal atoms have the largest sizes in their respective periods. This atomic size decreases as we move along the period and increases as we move down the group.
(iii) Ionization Enthalpy: The ionization enthalpy of the alkali metal atoms are low as compared to other atoms in their respective periods. This is because of the larger size of these atoms. As we move down the group, the ionization enthalpy further decreases because of the larger size of the atoms.
(iv) Chemical Properties
Anomalous Properties of Lithium
The deviation of the behaviour of lithium from its respective elements is because of two factors:
(i) The exceptionally small size of the atom
(ii) High polarising power
Because of these above two factors, lithium has some point of differences between other alkali metals and some similarities with magnesium.
(i) Differences between Lithium and other alkali metals
(ii) Similarities between Lithium and Magnesium
The similarity between lithium and magnesium is also known as the diagonal relationship with magnesium. This similarity of lithium and magnesium arises because of their similar sizes.
Some Important Compounds of Sodium
There are some important compounds of sodium from industrial basis. Their production and uses are discussed below.
(i) Sodium Carbonate
(ii) Sodium Chloride
(iii) Sodium Hydroxide
(iv) Sodium Hydrogencarbonate
Element | Symbol | Electronic configuration |
Beryllium | Be | [He] 2s2 |
Magnesium | Mg | [Ne] 3s2 |
Calcium | Ca | [Ar] 4s2 |
Strontium | Sr | [Kr] 5s2 |
Barium | Ba | [Xe] 6s2 |
Radium | Ra | [Rn] 7s2 |
(ii) Atomic and ionic radii: Alkaline earth metal atoms have larger sizes than other metal atoms in their respective periods but smaller than the alkali metals. This atomic size decreases as we move along the period and increases as we move down the group.
(iii) Ionization Enthalpy: The ionization enthalpy of the alkali metal atoms are low as compared to other atoms in their respective periods but higher than the alkali metal atoms. As we move down the group, the ionization enthalpy further decreases because of the larger size of the atoms.
(iv) Chemical Properties
Aluminum and Beryllium both have oxide film on their surface thus are not easily attacked by acids.
Both aluminum hydroxide and beryllium hydroxide react with alkali to form beryllate and aluminate ions
Some Important Compounds of Calcium
(i) Calcium Oxide or Quick Lime(CaO)
(ii) Calcium Hydroxide (Slaked lime), Ca(OH)2
(iii) Calcium Carbonate, CaCO3
(iv) Calcium Sulphate (Plaster of Paris), CaSO4·H2O
This chapter is a part of inorganic chemistry. It is completely theory-based and very easy to learn, no need to memorize any formula.
Before reading this chapter, first, you must have the basic knowledge of chapter - periodic classification of elements.
You must also learn why there are some elements like Boron and Carbon show anomalous behaviour with respect to other elements in their group.
Rest this complete chapter is very simple, just be regular and be consistent in your numerical practice.
First, you must finish the class XI textbook and solve each and every example and unsolved question given in it. Then for advanced level preparation like JEE and NEET, you must follow O.P. Tandon or Solomons and Fryhle. You must definitely solve the previous year papers. Meanwhile, in the preparation, you must continuously give the mock tests for the depth of knowledge. Our platform will help you to provide with the variety of questions for deeper knowledge with the help of videos, articles and mock tests.
Chapters No. |
Chapters Name |
Chapter 1 |
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Chapter 2 |
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Chapter 3 |
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Chapter 4 |
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Chapter 5 |
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Chapter 6 |
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Chapter 7 |
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Chapter 8 |
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Chapter 9 |
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Chapter 10 |
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Chapter 11 |
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Chapter 12 |
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Chapter 13 |
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Chapter 15 |
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Chapter 16 |
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Chapter 17 |
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Chapter 18 |
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Chapter 19 |
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Chapter 20 |
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Chapter 21 |
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Chapter 22 |
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Chapter 23 |
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Chapter 24 |
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Chapter 25 |
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Chapter 26 |
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Chapter 27 |
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Chapter 28 |
The number and type of bonds between two carbon atoms in calcium carbide are
one sigma, one pi
one sigma, two pi
two sigma, one pi
two sigma, two pi
Among the properties reducing
oxidising
complexing, the set of properties shown by
ion towards metal species is
Beryllium and aluminium exhibit many properties which are similar. But, the two elements differ in
exhibiting maximum covalency in compounds
forming polymeric hydrides
forming covalent halides
exhibiting amphoteric nature in their oxides.