S-Block Elements - Notes, Overview, Formula, Books, FAQs

The periodic table is divided into 4 blocks, i.e., s-block, p-block, d-block, and f-block. Out of all these blocks, the elements of the s-block form the foundation of chemistry. The s-block elements are divided into two categories, i.e., alkali metals or group 1 elements and alkaline earth metals or group 2 elements. The elements of the s-block have high reactivity and low ionisation energy. These elements are important for both biological and industrial processes. These metals are everywhere around us, from the sodium in the salt we use in our food, to lithium in batteries, to calcium in our bones and teeth. The oxides and hydroxides of s-block elements are alkaline. The general electronic configuration of these elements is ns1 and ns2, respectively.

This Story also Contains

1. Notes for S-block Elements
2. Important Topics
3. Overview Of The Chapter - s-block Elements
4. Group 2 Elements: Alkaline Earth Metals
5. Diagonal Relationship Between Beryllium and Aluminium:
6. How To Prepare For p-Block Elements?
7. Uses Of S-block Elements
8. Prescribed Books

In this article, we cover the concept of the S-block elements. which is a very important chapter from the board exam point of view and also for the JEE Mains Exam, NEET Exam, and many other entrance exams like SRMJEE, BITSAT, WBJEE, BCECE, and more

These elements have a large number of applications in our daily life, such as washing Soda, which is also known as Sodium Carbonate . It is used for various purposes such as water softening and the manufacture of glass, paper, paints, etc.

Limestone is also one of the important compounds of the s-block elements. It is used to neutralize the acidic soils. It has various other applications as well, such as for making cement, in the glassmaking industry,y and in construction works, etc.

There are also various other applications of s-block elements. In this article, you will get all the important information regarding this chapter, like important topics, how to prepare for this chapter, and important books for preparation.

Notes for S-block Elements

Important Topics

Group 1 Element- Alkali Metal:

Alkali metals have an electron configuration of ns1, where n is the period number. These elements are well-known for having unique chemical and physical characteristics as well as strong reactivity in the Periodic Table

Anomalous Properties of Lithium:

Lithium, the third element in the periodic table and the lightest metal, is unique among alkali metals. The Anomalous Behaviour Of Lithium is due to the exceptionally small size of its atom and ion and high polarising power.

Alkali Metal Halide:

Alkali Metal Halides are basic compounds made up of alkali metals from Group 1 of the periodic table (such as lithium, sodium, and potassium) and halogens from Group 17 (such as fluorine, chlorine, and bromine).

Some Important Compounds Of Sodium:

• Sodium Chloride And Sodium Hydroxide: Sodium chloride (NaCl), commonly known by the names table salt, rock salt, sea salt, or common salt, is a white, crystalline, hygroscopic solid with a melting point of 1081K and a boiling point of 1713K. Sodium hydroxide (NaOH), or caustic soda, is another crucial chemical with a variety of industrial and laboratory uses. It is created by heating a solution of ferric oxide and sodium carbonate to create sodium ferrite, which is subsequently hydrolyzed to form NaOH
• Sodium Carbonate And Sodium Bicarbonate: Sodium bicarbonate, also referred to as baking soda, it is a white, crystalline solid, mostly produced by the Solvay Process. Sodium bicarbonate(NaHCO₃)is the result of the reaction between carbon dioxide and a saturated solution of sodium carbonate.

Group 2 Elements: Alkaline Earth Metals

Alkaline Earth Metals are shiny, silvery-white in color, and high density similar to alkali metals. As they are more metallic (i.e. the bonding is stronger), their melting points and boiling points tend to be higher than those of alkali metals. These elements have two electrons in the s-orbital of the valence shell. Their general electronic configuration may be represented as [noble gas]ns2

Anomalous Behaviour of Beryllium:

Berylium differs from the rest of the alkaline earth metals on account of its small atomic size, high electronegativity, and a slight difference in electronic configuration. The different behavior of beryllium is called Anomalous Behaviour Of Beryllium.

Structure Of Beryllium Chloride:

The Structure Of Beryllium Chloride is a polymeric chain structure. Every beryllium atom is tetrahedrally linked to four chlorine atoms, while every chlorine atom connects two beryllium atoms.

Some Important Compounds Of Calcium:

• Calcium Oxide (quick Lime) And Calcium Hydroxide (slaked Lime): Calcium oxide is a white, caustic, alkaline, crystalline solid at room temperature. It is prepared by the thermal decomposition of calcium carbonate (limestone). Calcium Hydroxide is also known as slaked lime. It is prepared by the reaction of lime with water.
• Calcium Carbonate And Calcium Sulphate(plaster Of Paris): Calcium carbonate, CaCO₃ is obtained in most rocks, primarily as the minerals calcite and aragonite. It forms the principal constituents of pearls, shells of marine organisms, and eggshells. Calcium sulphate, CaSO₄ occurs in a number of hydrated forms; the most well-known are gypsum, CaSO₄·2H₂O, and plaster of Paris, CaSO₄·0.5H₂O.

Diagonal Relationship Between Beryllium And Aluminium:

Several aspects of beryllium and aluminum are the same, such as being amphoteric, the formation of covalent compounds, and resistance to acid attacks. Also, beryllium and aluminum combine to form some covalent compounds with certain elements. This similarity between these two is called the Diagonal Relationship Between Beryllium And Aluminium.

Also Read,

• Preparation Properties and Uses Baking Soda
• Baking Soda Washing Soda Plaster of Paris
• Caustic Soda Preparation Properties and Uses
• Na₂CO3
• Sodium Sulfate
• Potassium Hydroxide
• Sodium Oxide

Overview Of The Chapter - s-block Elements

The s-block elements are those in which the outermost electrons exist in the s-orbital. Alkali and alkaline earth metals are respectively the members of group 1 and group 2 elements. In this chapter, there are various important properties that you need to learn, such as electronic configuration, ionization enthalpy, hydration enthalpy, chemical properties, etc.

Group 1 elements: Alkali metals

(i) Electronic Configuration: The alkali metals or group 1 elements have the valence shell electronic configuration of ns¹. The table given below describes the electronic configuration of the alkali metals.

(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 is 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

• Reactivity towards air: Alkali metals react too fast with oxygen and form oxides. Lithium, being the smallest element, forms monoxide, sodium forms peroxide, and other large metals form superoxides.
  $\begin{aligned} & 4 \mathrm{Li}+\mathrm{O}_2 \rightarrow 2 \mathrm{Li}_2 \mathrm{O} \\ & 2 \mathrm{Na}+\mathrm{O}_2 \rightarrow \mathrm{Na}_2 \mathrm{O}_2 \\ & \mathrm{~K}+\mathrm{O}_2 \rightarrow \mathrm{KO}_2\end{aligned}$ All these metals in their oxides have the oxidation number equal to +1.
• Reactivity towards water: Alkali metals react with water to form hydroxides and dihydrogen.$2 \mathrm{Na}+2 \mathrm{H}_2 \mathrm{O} \rightarrow 2 \mathrm{NaOH}+\mathrm{H}_2$
• Reactivity towards dihydrogen: Alkali metals react with dihydrogen and form hydrides.$2 \mathrm{Na}+\mathrm{H}_2 \rightarrow 2 \mathrm{NaH}$
• Reactivity towards halogens: Alkali metals react too fast with halogen elements to form alkali halides.$2 \mathrm{Na}+\mathrm{Cl}_2 \rightarrow 2 \mathrm{NaCl}$
• Alkali metals with ammonia: These metals dissolve in liquid ammonia giving the deep blue solution.$M+(x+y) NH_3 \rightarrow\left[M\left(NH_3\right)_x\right]^{+}+\left[e\left(NH_3\right)_y\right]^{-}$

Anomalous Properties Of Lithium

The deviation of the behavior 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 two factors, lithium has some points of difference from other alkali metals and some similarities with magnesium.

(i) Differences Between Lithium And Other Alkali Metals

• Lithium is harder, and its melting point and boiling point are also higher than other alkali metals.
• Lithium is less reactive than other alkali metals.
• Lithium does not form solid hydrogen carbonate, unlike other alkali metals.
• Lithium does not form ethynide on reaction with ethyne, unlike other alkali metals.
• Lithium nitrate on heating gives lithium oxide but other alkali metal nitrates produce metal nitrite.
• Fluorides and oxides of lithium are less soluble in water than those of 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 between lithium and magnesium arises because of their similar sizes.

• Lithium and Magnesium, both are harder and lighter than their respective group elements.
• Their oxides and hydroxides are less soluble.
• Both oxides of lithium and magnesium do not combine with excess oxygen.
• The chlorides of both lithium and magnesium are soluble in ethanol.
• Both form nitride in reaction to nitrogen, known as lithium nitride and magnesium nitride.

Some Important Compounds Of Sodium

There are some important compounds of sodium from an industrial basis. Their production and uses are discussed below.
(i) Sodium Carbonate
(ii) Sodium Chloride
(iii) Sodium Hydroxide
(iv) Sodium hydrogen carbonate

Group 2 Elements: Alkaline Earth Metals

(i) Electronic configuration: The alkaline earth metals or group 2 elements have the valence shell electronic configuration of ns². The table given below describes the electronic configuration of the alkali metals.

(ii) Atomic and Ionic radii: Alkaline earth metal atoms have larger sizes than other metal atoms in their respective periods but are 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 is 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

• Reactivity towards air and water: Beryllium and magnesium are usually inert as they are covered with an oxide film on their surface. But the powdered beryllium burns in air and forms beryllium oxide. Other heavier elements of this group readily react with air and form oxides.
• Reactivity towards halogens: All alkaline earth metals combine with halogen to form halides.$\mathrm{Mg}+\mathrm{Cl}_2 \rightarrow \mathrm{MgCl}_2$
• Reactivity towards hydrogen: Except beryllium, all other alkaline earth metals combine with hydrogen to form their hydrides.
• Reactivity towards acids: The alkaline earth metals react with acids and liberate hydrogen.$\mathrm{Mg}+2 \mathrm{HCl} \rightarrow \mathrm{MgCl}_2+\mathrm{H}_2$
• Alkaline earth metals with ammonia: These metals dissolve in liquid ammonia and give a blue-black solution.$M+(x+y) NH_3 \rightarrow\left[M\left(N H_3\right)_x\right]^{2+}+2\left[e\left(N_3\right)_y\right]^{-}$

Diagonal Relationship Between Beryllium and Aluminium:

• Aluminum and Beryllium both have oxide film on their surface and thus are not easily attacked by acids.

• Both aluminum hydroxide and beryllium hydroxide react with alkali to form beryllate and aluminate ions

• Both aluminum and beryllium react with chlorine and form polymeric chlorides. These chlorides are soluble in organic solvents.
• Aluminum and Beryllium ions, both have a strong tendency to form complexes.

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

How To Prepare For p-Block Elements?

• 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 the chapter - periodic classification of elements.

• You must also learn why there are some elements like Boron and Carbon show anomalous behavior 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.

Uses Of S-block Elements

S-block elements have a large number of uses in our daily lives s-block elements form various compounds or salts that are helpful in our daily lives.

• They are used for the manufacture of various paper, soap, artificial silk, and glass.
• s-block elements are used in petroleum refining and for mercerizing cotton
• Alkaline earth metals are used in the production of medicines such as antacids and medicines used in cancer treatments.

Prescribed Books

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's papers.

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