For alkaline earth metals [noble gas] ns 2. • Group 1 Elements: Alkali metals. What are the different reactions that occur in the Solvay process? Ca(OH)2 + C02 ———> CaC03 + H20 It includes all the topics given in NCERT class 11 Chemistry text book. S block elements 1. STUDYDUNIYA The Educational Social Network C H E M I S T R Y - I N O R G A N I C - s - B L O C K E L E M E N T S IIT JEE @studyduniya +91 7744994714 MEMBERS OF s- BLOCK ELEMENTS 2. Group II = [Noble gas] ns2 Uses: The alkali metals dissolve in liquid ammonia to give deep blue solution. (ii) Lithium is used to make both primary and secondary batteries. Ionic hydrides are formed when hydrogen reacts with S-block metals, excluding Be and Mg. Quick Revision Notes Chapter 8 The D and F-Block Elements Class 12 Notes Chemistry. Alkaline earth metals and alkali metals are both characterized by the presence of s-electron in the valence shell of their atoms – two and one, respectively. (ii) They have generally low density which increases down the group. Their atomic and ionic sizes increase on moving down the group and ionization enthalpies decrease systematically down the group. 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Except Be and Mg, they have to be stored under liquid paraffin to prevent contact with the atmosphere. Group 1 consists of : lithium, sodium, potassium, rubidium, caesium and francium and collectively known as the alkali metals. 4. (Ca2Si04) dicalcium silicate 26% The first three elements of second period (Li, Be, B) show diagonal similarity with the elements (Mg, Al, Si) of third period. As the atomic sizes increase down the group ionization enthalpies are expected to decrease in the same manner. These notes are aligned with our Channel’s Video Lectures. (ii) Reaction with water: (Ca3Al206) Tricalcium Aluminate 11% 2(CaS04-2H20) ———-> 2(CaS04) . H20 + 3H20 For alkaline earth metals [noble gas] ns2 s-BLOCK ELEMENTS - ALKALINE EARTH METALS ELEMENTS OF GROUP 2 Be - Beryllium Mg - Magnesium Ca - Calcium Sr - Strontium Ba - Barium Ra - Radium (Radioactive) s-block has two groups (1 and 2). • General electronic configuration of Reply. When the excited electron comes back to the ground state, there is emission of radiation in the visible region. Required fields are marked *. Alkali metals react with water to form hydroxide and dihydrogen (i) They are harder than alkali metals. Justify this statement by giving some examples from the oxidation state of these elements. Jan 03, 2021 - Detailed Chapter Notes - S Block elements, Class 11, Chemistry | EduRev Notes is made by best teachers of JEE. For alkali metals [noble gas] ns1 • Ionization Enthalpies But the switch it up on us, and we’re caught off guard by the punchline, and it gets a laugh. Group 1 and group 2 elements combined are known as s-block elements. The hydration enthalpies decreases down the group since the cationic size increases. The alkali metals combine with hydrogen at about 673 K (lithium at 1073 K) to form hydrides. Preparation: Prepared by combining a material rich in CaO with other material such as clay, which contains Si02 along with the oxides of aluminium, iron and magnesium. 8.29. (iii) They impart colour to an oxidising flame. These S-Block Elements Classroom HandWritten Notes Pdf Class Notes is printed with a high-quality printer so that visible quality should be the best. 2. Their reducing power increases down both groups. The blue solutions are paramagnetic while the concentrated solutions are diamagnetic. The s-block is on the left side of the conventional periodic table and is composed of elements from the first two columns, the nonmetals hydrogen and helium and the alkali metals (in group 1) and alkaline earth metals (group 2). The chapter highlights the elements of the first two groups of the periodic table, which are collectively known as the s block elements. S block elements 1)Elements in which the last electron enters the s orbital of their respective outermost shells are called s block elements. • Uses of Alkali Metals Which is less reactive Sodium or potassium? These s-block elements are present in Group 1 and Group 2 of the periodic table and among the most active metals. Electronic Configuration, ns 1, where n represents the valence shell. In plastering and in construction purposes. (iv) Exept BeO, they are basic in nature and react with water to form sparingly soluble hydroxides. (ii) Used as reducing agent. Li+ > Na+ > K+ > Rb+ > Cs+ NCERT Solutions for Class 6, 7, 8, 9, 10, 11 and 12. • Diagonal Relationship Thus alkaline earth metals have more tendency to become hydrate. They have high melting and boiling points. They are much similar to alkali metals but due to small size some differences are there. 1) Elements in which the last electron enters the s orbital are called s-block elements. Reason: Because these elements have only two valence electrons and the magnitude of the force of attraction with the nucleus is quite small. These metals form mono positive and dipositive ions and are extremely reactive. Mg + 2H20 ——-> Mg(OH)2 + H2 (i) Reaction with air: Introduction Group 1 of the periodic table consists of the elements: Lithium, Sodium, Potassium, Rubidium, Caesium and … • Ionization Enthalpy (ii) When it is mixed in adequate quantity of water it forms a plastic hard mass within 15 minutes. • Hydration Enthalpy • Chemical Properties of Alkali Metals (i) It is used in the manufacturing of building material. (iv) BeCl2 has a chain structure in the solid phase as shown below. Practising these Chemistry Revision Notes which contain the similar paper pattern as given by CBSE during last years, will help you to be confident in exams. For this we have included Pdf notes of each Chapter (still updating….). (ii) Used in the surgical bandages for setting the fractured bone or sprain. Be2+ > Mg2+ > Ca2+ > Sr2+ > Ba2+ Not only is this one of the chief elements of the Spanish Inquisition, it’s the foundation principle for most humor. The ionic character of hydrides increases from Li to Cs. Sulphates MO + 2HX ——> MX2 + H20 (iii) Used to detect C02 gas in the laboratory. This document is highly rated by JEE students and has been viewed 20001 times. These elements are called alkali metals because they readily dissolve in water to form … The d -Block elements: The elements lying in the middle of periodic table belonging to groups 3 to 12 are known as d – block elements. (iii) The tendency to form halide hydrates decreases down the group. 2 H20. Alkaline earth metals are characterized by two s-electrons, whereas alkali metals by one s-electron in the valence shell of their atoms. (i) All the alkali metals are silvery white, soft and light metals. Your email address will not be published. The hydration enthalpies of alkaline earth metal ions are larger than those of the alkali metals. (v) Hydroxides of alkaline earth metals are less stable and less basic than alkali metal hydroxides. Properties: These metals except Be combine with hydrogen directly upon heating to form metal hydrides. The alkali metals are strong reducing agents. Ca + 2H20 ————> Ca(OH)2 + H2 (iv) In the manufacture of high quality paper. (iii) Lithium hydride is used as source of hydrogen for meteorological purposes. Group 1 elements are called alkali metals. Reason. Uses: 2M + X2————–> 2MX They are named so because of the alkaline nature of the hydroxides and oxides. (iii) BeO is amphoteric in nature while oxides of other elements are ionic. This can be explained in terms of electrode potentials (E°). M+ (x + y) NH3 ———-> [M (NH3) X]+ + [e (NH3) y]– (i) The sulphates of alkaline earth metals are white solids and quite stable to heat. • General Electronic Configuration of s-Block Elements (i) In rocket propellent It can also prepared by the reaction of a solution of sodium carbonate with calcium chloride. 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