Lithium shows diagonal relationship with

Diagonal Relationship of Lithium with Magnesium The main points of similarity : (1) Both have almost similar electronegativities. (2) Both Li and Mg are quite hard. They are harder and lighter than other elements in their respective groups. (3) Both LiOH and Mg(OH) 2 are weak bases. (4) Both form ionic nitrides when heated in atmosphere of Nitrogen. 6 Li + N 2 → 2 Li 3N 3 Mg + N 2 → 2 Mg 3N 2 (5) The hydroxides of both lithium and magnesium decompose upon heating. 2 LiOH → Li 2O + H 2O Mg(OH) 2 → MgO + H 2O (6) Both lithium and magnesium combine with oxygen to form monooxide while other members of their respective groups form peroxide and superoxide. 4 Li + O 2 → 2 Li 2O 2 Mg + O 2 → 2 MgO The Li 2O and MgO thus formed do not combine with excess O 2 to form peroxide and superoxide. (7) The carbonates of these metals decompose on heating to the corresponding oxides with the evolution of carbon dioxide. Li 2CO 3 → Li 2O + CO 2 MgCO 3 → MgO + CO 2 (8) Both Lithium and magnesium do not form solid bicarbonates. (9) Both Lithium and magnesium nitrate decompose on heating producing nitrogen dioxide. 4 LiNO 3 → 2 Li 2O + 4 NO 2 + O 2 2 Mg(NO 3) 2 → MgO + 4 NO 2 + O 2 (10) The hydroxides, carbonate, oxalates, phosphates and fluorides of both Lithium and magnesium are sparingly soluble in water. (11) Because of the covalent character, LiCl and MgCl 2 are soluble in ethanol. (12) Both Lithium perchlorate and magnesium perchlorate are highly soluble in ethanol. (13) LiCl and MgCl 2 ar...

• Chemistry • Physical Chemistry • Diagonal Relationship Diagonal Relationship Stop what you are doing and think about everything that you know about the periodic table. You have probably learned that atomic radius of elements decreases across a period and increases down a group, and also that ionization energy and electronegativity tend to increase across a period and up a group. You might also remember that elements in the same group… Diagonal Relationship • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • Stop what you are doing and think about everything that you know about the You might also remember that elements in the same group have a vertical relationship and show...

An element’s chemical properties are closely associated with the atoms in terms of size. A diagonal relationship exists between specific pairings of diagonally adjacent nodes in the second and third periods of the atomic numbers. These pairings share several common features. For example, in the periodic table of elements, the diagonal relationship of lithium and magnesium is opposite in the second and third periods, and they have many similar properties. Definition of a Diagonal Relationship In the periodic table, some elements have a diagonal relationship. These elements lie diagonally adjacent to one another in the periodic table’s second and third rows from the first 20 elements. The properties of diagonal elements are frequently identical, as seen when moving down the group and from left to right. It is evident among the lighter ones. Thus, the pairs that exhibit a diagonal relationship are as follows: • Lithium (Li) from group IA with Magnesium (Mg) from group IIA • Beryllium (Be) from group IIA with aluminium (Al) from group IIIA • Boron (B) from group IIIA with silicon (Si) from group IVA • Carbon (C) from group IVA with phosphorus (P) from group VA Cause of Lithium-Magnesium Diagonal Relationship Magnesium and lithium have a diagonal relationship. • Despite its small size, lithium is distinct from all other alkali metals yet similar to magnesium due to its similar size. The equal size of the ions results in the formation of the diagonal relationship of lithium with...

\( \newcommand\) No headers A Diagonal Relationship is said to exist between certain pairs of diagonally adjacent elements in the second and third periods of the periodic table. These pairs (Li & Mg, Be & Al, B & Si etc.) exhibit similar properties; for example, Boron and Silicon are both semiconductors, form halides that are hydrolyzed in water and have acidic oxides. Such a relationship occurs because crossing and descending the periodic table have opposing effects. On crossing a period of the periodic table, the size of the atoms decreases, and on descending a group the size of the atoms increases. Similarly, on moving along the period the elements become progressively more covalent, less reducing and more electronegative, whereas on descending the group the elements become more ionic, more basic and less electronegative. Thus, on both descending a group and crossing by one element the changes cancel each other out, and elements with similar properties which have similar chemistry are often found - the atomic size, electronegativity, properties of compounds (and so forth) of the diagonal members are similar.

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In diagonal relationship is said to exist between certain pairs of diagonally adjacent The organization of elements on the periodic table into horizontal rows and vertical columns makes certain relationships more apparent ( Similarly, on moving rightward a period, the elements become progressively more [ clarification needed], less basic and more and crossing a group by one element, the changes "cancel" each other out, and elements with similar properties which have similar chemistry are often found – the atomic size [ clarification needed], electronegativity, properties of compounds (and so forth) of the diagonal members are similar. It is found that the chemistry of a The reasons for the existence of diagonal relationships are not fully understood, but + is a small cation with a +1 charge and Mg 2+ is somewhat larger with a +2 charge, so the ionic potential of each of the two ions is roughly the same. It was revealed by an examination that the charge density of lithium is much closer to that of magnesium than to those of the other alkali metals. • When combined with oxygen under standard conditions, Li and Mg form only normal oxides whereas Na forms • Li is the only 3N. • Lithium carbonate, phosphate and fluoride are sparingly soluble in water. The corresponding group 2 salts are insoluble. (Think lattice and solvation energies). • Both Li and Mg form covalent 2 (cf. • Chlorides of both Li and Mg are 2·6H 2O) separates out from hydrated crystal LiCl·2H 2O. • Further diag...

S – Block Elements (Alkali & Alkaline Earth Metals) : Notes and Study Materials -pdf S – Block Elements (Alkali & Alkaline Earth Metals) NEET and AIIMS Special S – Block Elements (Alkali & Alkaline Earth Metals) Refresher Course S – Block Elements (Alkali & Alkaline Earth Metals) : Master File S – Block Elements (Alkali & Alkaline Earth Metals) : Quick Revision Notes S – Block Elements (Alkali & Alkaline Earth Metals) : Brain Map About this unit Group I and group 2 elements:General introduction, electronic configuration, occurrence, anomalous properties of the first element of each group, diagonal relationship, trends in the variation of properties (such as ionization enthalpy, atomic and ionic radii), trends in chemical reactivity with oxygen, water, hydrogen and halogens; uses.Preparation and Properties of Some important Compounds:Sodium carbonate, sodium chloride, sodium hydroxide and sodium hydrogencarbonate, biological importance of sodium and potassium.Industrial use of lime and limestone, biological importance of Mg and Ca. All alkali metals and their salts impart characteristic colours to the flame because of the bonding of the outermost electron.The outer electrons of these atoms are excited to higher energy levels. On returning to the original state they give out visible light of characteristic wavelength. This gives a characteristic colour to the flame. • All the alkali metals when heated with oxygen form different types of oxides for example, lithium forms lith...