s-block Elements

Sodium

Created byVinay Arya

Last updated 11/2021

English

What you'll learn

The students will have a clear vision about the Alkaline earth metals.
They will know about Alkali Metals.
The learners will become confident in concepts of block elements, periodic table and metals.
The learners will know about metals like sodium, potassium.

Course content

1 section • 22 lectures • 4h 22m total length

Contents of s - block Elements15:05
Explore s-block elements, including alkali metals and alkaline earth metals, their properties, extraction methods, and key compounds like oxides, hydroxides, carbonates, and sulfates.
Diagonal relationships12:15
Explore diagonal relationships in s-block elements. Observe how lithium with magnesium, beryllium with aluminium, boron with silicon illustrate these patterns, and note the first elements' anomalous behavior.
Physical Properties of Alkali Metals13:54
Examine the physical properties and trends of alkali metals in the s-block. Learn about softness, low ionization energy, +1 oxidation state, melting point, flame coloration, and hydration behavior.
Chemical Properties of Alkali Metals15:33
Explore the chemical properties of alkali metals, including reactions with oxygen, water, and acids, and the formation of oxides, hydrates, peroxides, superoxides, and complex salts.
General characteristic of the compounds of the alkali metals13:08
Explore the general characteristics of alkali metal compounds, including oxides, hydroxides, peroxides, and superoxides; study their water reactions, salt formation, solubility, hydration energy, and covalent character.
Salts of oxoacids9:55
Explore how s-block elements form salts of oxoacids with alkaline metals, including carbonates and bicarbonates of carbonic, sulfuric, phosphoric, nitric, and nitrous acids, and note lithium’s anomalous properties.
Extraction of Lithium9:56
Learn lithium extraction from spodumene ore into lithium chloride. Electrolyze lithium chloride at high temperature via acid treatment or fusion routes to yield lithium metal and chlorine gas.
Properties of Lithium15:10
Explore the physical and chemical properties of lithium, its reactions with oxygen, water, and nitrogen forming lithium nitride, and its uses in alloys and lithium chloride and lithium carbonate.
Properties of Sodium11:12
Explore the chemical properties of sodium, detailing its air and moisture reactivity, storage in kerosene, and reactions forming sodium hydroxide, oxide, peroxide, and salts with chlorine, sulfur, and phosphorus.
Sodium Peroxide10:05
Explore sodium peroxide, the oxide of sodium, its preparation by heating sodium metal with rock salt, and its properties, including hydrolysis yielding hydrogen peroxide and differences from sodium oxide.
Sodium Carbonate (Washing soda)10:36
Explore the production of washing soda, or sodium carbonate, via the Solvay ammonia-soda process. Outline brine treatment, ammonia absorption, carbonation, filtration, and uses in washing, softening hard water, and glass.
Potassium carbonate8:37
Prepare potassium carbonate (K2CO3) by absorbing CO2 into a potassium chloride solution with magnesium carbonate, then filter and heat at 140 °C or treat with magnesium oxide, highlighting alkaline nature.
Alkaline Earth Metals14:59
Explore the alkaline earth metals—beryllium, magnesium, calcium, strontium, barium, and radium—group two of the periodic table, their +2 oxidation state, high melting points, higher density, and characteristic flame colors.
Reactivity and Electrode potential12:49
Explore the reactivity and electrode potential of alkaline earth metals, why their reactivity increases down the group, and how ionization energy and standard electrode potentials govern their behavior.
Chemical Properties of Group – II elements11:57
Examine the chemical properties of group 2 elements, detailing reactions with water and oxygen, formation of hydroxides and oxides, and the trend of increasing reactivity down the group.
General characteristics of compounds of the Alkaline9:29
Explore the general characteristics of alkaline earth compounds, including oxides and hydroxides, trends in basicity and solubility down the group, and the amphoteric behavior of beryllium.
Sulphates8:49
Explore the sulfates of the alkaline earth metals, formed from metals and their oxides, hydroxides, or carbonates with sulfuric acid, and note solubility trends from beryllium to barium.
Anomalous Behaviour of Beryllium12:06
Explore the anomalous behaviour of beryllium in the s-block, highlighting its small size, high polarizing power, high electronegativity and ionization energy, and diagonal relationship with aluminium.
Properties of Magnesium12:15
explores the physical and chemical properties of magnesium, its reactions with air, water, and acids, and its uses in alloys, fireworks, and milk of magnesia.
Oxides of Magnesium and Calcium.13:02
Explore the oxides of magnesium and calcium, including magnesia and quick lime, their preparation by heating minerals, their alkaline reactions with water, and carbon dioxide driven carbonate formation.
Calcium Carbonate12:00
Explore the preparation, properties, and uses of calcium carbonate from natural minerals such as marble and limestone, and its reaction with carbon dioxide to form calcium bicarbonate.
Industrial uses of lime and Limestone9:12
Explore the industrial uses of lime and limestone, including calcium carbonate in building materials and cement, steel refining, glass, water softening, and cement manufacture.

Requirements

The learner should be aware of Elements.

Description

The elements in the long form of the periodic table has been divided into four blocks, namely s, p, d & f blocks. The elements

of group I & II receive their last electron in s-orbital. So they are called as s – block elements.

The metals Lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs) and francium (Fr) which have one electron in

their outermost shell belongs to group I and are called alkali metals as they react with water to form hydroxides which are

strong bases or alkalies.

The elements of group II are Beryllium (Be), Magnesium (Mg), Calcium (Ca),Strontium (Sr), barium (Ba) and radium (Ra) which

have two electrons in their outermost shell. All these elements are also metallic in nature and are commonly known as alkaline

earth metals with the exception of beryllium. Because of their low density, alkali metals and alkaline earth metals are called

lighter metals. Both alkali and alkaline earth metals are highly reactive and hence do not occur in free state but found in

combined state. Whereas alkali metals mostly occur as halides, oxides, silicates, borates and nitrates, alkaline earth metals

mainly occur as silicates, carbonates, sulphates and phosphates. Some alkali & alkaline earth metals occur abundantly in

nature. Calcium is the fifth, magnesium is the sixth, sodium is seventh and potassium is eight barium is the fourteenth and

strontium is the fifteenth most abundant element by weight in the earth’s crust. Sodium and magnesium are also present in

sea water brine wells and few salt lakes.

Anomalous behaviour of first element

The first element of a group differs considerably from the rest of the elements of the same group. This anomalous behaviour is due to

(i) Smaller size of their atoms

(ii) Their higher ionization energies

(iii) Their higher electronegativities

(iv) Absence of vacant d – orbitals in their valence shell

(v) High polarizing power of its cation.

Who this course is for:

Beginners and eleventh standard students.