If positive, the solution will go milky. With their low first and second ionization energies, the group 2 elements almost exclusively form ionic compounds that contain M2+ ions. NCERT DC Pandey Sunil Batra HC Verma Pradeep Errorless. Lanthanides (Ce-Eu) . Volume 88: Esters with Water - Revised and Updated. JPCRD 2009, 38(2). This is a trend which holds for the whole Group, and applies whichever set of data you choose. When added to water, the first alkaline earth metal, (Beryllium), is totally nonreactive, and doesn't even react with steam. This discussion on What is the solubility order of fluorides for alkaline earth metals? If ... Alkaline Earth Metals." The chemistry of Be2+ is dominated by its behavior as a Lewis acid, forming complexes with Lewis bases that produce an octet of electrons around beryllium. Elemental magnesium also serves as an inexpensive and powerful reductant for the production of a number of metals, including titanium, zirconium, uranium, and even beryllium, as shown in the following equation: $TiCl_{4\;(l)} + 2Mg(s) \rightarrow Ti_{(s)} + 2MgCl_{2\;(s)} \label{11}$. In contrast, the alkaline earth chlorides are readily soluble. The two reactions below show this: Be(OH)2 (s) + H2SO4 (aq) ® BeS4 (aq) + 2H2O(l), Be(OH)2 (s) + 2NaOH(aq) ® Na2Be(OH)4 (aq). C2 to C4 Esters This means it has the properties of both an acid and a base. The solubility of the carbonates and the sulfates decreases rapidly down the group because hydration energies decrease with increasing cation size. The group 2 elements do exhibit some anomalies, however. Consistent with this formulation, reaction of Be2C with water or aqueous acid produces methane: $Be_2C_{(s)} + 4H_2O_{(l)} \rightarrow 2Be(OH)_{2(s)} + CH_{4(g)} \label{Eq8}$. The explanation for the trends in solubility is given in chapter 3.17 enthalpies of solution The pH of an aqueous solution of a hydroxide depends on the extent to which the metal hydroxide can be split to produce independent ions. All alkaline earth metals react vigorously with the halogens (group 17) to form the corresponding halides (MX2). Fundamental, Recent edits by: SarMal, Jen Moreau, Taylor (ScienceAid Editor). Let us discuss the characteristics of the compounds of the alkali earth metals. Solubility of the sulfates; Solubility of the carbonates; Contributors and Attributions; This page discusses the solubility of the hydroxides, sulfates and carbonates of the Group 2 elements—beryllium, magnesium, calcium, strontium and barium—in water. drying agent for removing water from the atmosphere—CaCl, $$\mathrm{CaH_2(s)}+\mathrm{TiO_2(s)}\xrightarrow\Delta$$, $$\mathrm{BeCl_2(s)}+\mathrm{Mg(s)}\xrightarrow\Delta$$, $$\mathrm{BeCl_2(s)}+\mathrm{Mg(s)}\xrightarrow\Delta\mathrm{Be(s)}+ \mathrm{MgCl_2(s)}$$. To be familiar with the reactions, compounds, and complexes of the alkaline earth metals. The values given in parenthesis are in kJ/mol. Except for Be, all the alkaline earth metals react with N2 to form nitrides, and all react with carbon and hydrogen to form carbides and hydrides. Many of the difluorides adopt the fluorite structure, named after calcium fluoride (and also adopted by several metal dioxides such as CeO 2, UO 2, ThO 2, etc. The reactions of the alkaline earth metals with the heavier chalcogens (Y) are similar to those of the alkali metals. The correct order regarding the solubility of alkaline earth metal chlorides in water is . The alkaline earth metals form difluorides that are insoluble. Accessed Jan 11, 2021. https://scienceaid.net/chemistry/fundamental/group2.html. Part 1. Development of an MSE-based chemical model for the solubility of calcium sulphate in mixed chloride–sulphate solutions. The trend in the reactivities of the alkaline earth metals with nitrogen is the opposite of that observed for the alkali metals. Elemental magnesium is the only alkaline earth metal that is produced on a large scale (about 5 × 105 tn per year). Group 2, Alkaline Earth Metals. The most important alkaline earth carbide is calcium carbide (CaC2), which reacts readily with water to produce acetylene. Explain your choice in each case. As expected for compounds with only four valence electrons around the central atom, the beryllium halides are potent Lewis acids. Like the alkali metals, the alkaline earth metals form complexes with neutral cyclic ligands like the crown ethers and cryptands discussed in Section 21.3. Except for the beryllium halides, these compounds are all primarily ionic in nature, containing the M2+ cation and two X− anions. Legal. It is measured in either, grams or moles per 100g of water. The solubility of other halides decreases with increase in ionic size i.e. Melting and boiling points of elements temperature dependence of mineral 2nd 3rd 4th 5th ion as trend of solubility sulps alkaline earth metals study material Alkaline Earth MetalsWhat Is The Ility Order Of Alkali Metal Chlorides QuoraMelting And Boiling Points Of Elements Periodic TableTemperature Dependence Of Mineral Solubility In Water Part IAlkali And Alkaline Earth… Read More » Higher lattice energies cause the alkaline earth metals to be more reactive than the alkali metals toward group 15 elements. This is due to the fact that the lattice energy decreases down the group due to increase in size of the alkaline earth metals cation whereas the hydration energy of the cation remains almost unchanged. ScienceAid, scienceaid.net/chemistry/fundamental/group2.html Accessed 11 Jan 2021. Books. In contrast, the alkaline earth metals generally have little or no tendency to accept an additional electron because their ns valence orbitals are already full; an added electron would have to occupy one of the vacant np orbitals, which are much higher in energy. Included in these metals are beryllium(Be), magnesium(Mg), strontium(Sr), barium(Ba) and radium(Ra). For each application, choose the most appropriate substance based on the properties and reactivities of the alkaline earth metals and their compounds. Ditto, MgO is referred to oxides possessing extremely low solubility in melts based on alkali metal chlorides and it remains slightly soluble even in the mixtures containing alkaline earth chlorides, especially CaCl2,. They react readily with Lewis bases, such as ethers, to form tetrahedral adducts in which the central beryllium is surrounded by an octet of electrons: $BeCl_{2(s)} + 2(CH_3CH_2)_2O_{(l)} \rightarrow BeCl_2[O(CH_2CH_3)_2]_{2(soln)} \label{Eq4}$. Add 1 mL (about 25 drops or fill the well about 1⁄ 4 inch or 0.5 cm deep) of an alkaline earth metal chloride solution to each well in a horizontal row, as follows (see Figure 1): Which of the indicated alkaline earth metals or their compounds is most appropriate for each application? Given: application and selected alkaline earth metals, Asked for: most appropriate substance for each application. Millions of tons of calcium compounds are used every year. Beryllium differs from its brothers and sisters in Group 2 in that it usually forms covalent bonds, but unlike other covalent molecules, it is soluble in organic solvents and a poor conductor when molten. (2017). The alkaline earth metals are somewhat easier to isolate from their ores, as compared to the alkali metals, because their carbonate and some sulfate and hydroxide salts are insoluble. Hydroxides of the lighter alkaline earth metals are insoluble in water, but their solubility increases as the atomic number of the metal increases. In contrast to the alkali metals, the alkaline earth metals generally have little or no affinity for an added electron. To neutralize excess stomach acid that causes indigestion, would you use BeCO. The reaction in Equation $$\ref{Eq7}$$ is the basis of antacids that contain MCO3, which is used to neutralize excess stomach acid. This tendency is most important for the lightest cation (Be2+) and decreases rapidly with the increasing radius of the metal ion. The solubility of the alkaline earth metal hydroxides in water increases with increase in atomic number down the group. "Group 2, Alkaline Earth Metals." “Quicklime” (CaO), produced by heating CaCO3 (Equation $$\ref{Eq5}$$), is used in the steel industry to remove oxide impurities, make many kinds of glass, and neutralize acidic soil. Hence beryllium oxide is amphoteric. Solubility is the maximum amount a substance will dissolve in a given solvent. Similarly, in the presence of a strong base, beryllium and its salts form the tetrahedral hydroxo complex: [Be(OH)4]2−. Accessed Jan 11, 2021. https://scienceaid.net/chemistry/fundamental/group2.html. Use any tables you need in making your decision, such as Ksp values (Table 17.1), lattice energies (Table 8.1), and band-gap energies. In contrast, beryllium reacts with elemental carbon to form Be2C, which formally contains the C4− ion (although the compound is covalent). For example, Be2+ salts dissolve in water to form acidic solutions that contain the tetrahedral [Be(H2O)4]2+ ion. It is measured in either, grams or moles per 100g of water. Based on the discussion in this section and any relevant information elsewhere in this book, determine which substance is most appropriate for the indicated use. The hydroxides become more soluble as you go down the Group. Even ignoring entropy (to a first approximation we might assume that the entropy change is constant for all the metals), solubility depends on both lattice energy and hydration enthalpy so you can't just look at one trend. Halides of Alkaline Earth Metals Fluorides are insoluble in water. ), which surrounds each metal cation with 8 fluorides. The heavier alkaline earth metals also form complexes, but usually with a coordination number of 6 or higher. Because of their higher positive charge (+2) and smaller ionic radii, the alkaline earth metals have a much greater tendency to form complexes with Lewis bases than do the alkali metals. Some compounds of Mg2+ also have significant covalent character. Of the three metals listed, Ba has the lowest ionization energy and thus releases electrons most readily. Asked for: products and balanced chemical equation. Thus, while the solubility of BaSO 4 is only slightly greater in acidic solution than in water, the solubility … These compounds are volatile, producing vapors that contain the linear X–Be–X molecules predicted by the valence-shell electron-pair repulsion (VSEPR) model. 1. If you have problems with any of the steps in this article, please ask a question for more help, or post in the comments section below. The only other alkaline earth that is widely used as the metal is beryllium, which is extremely toxic. The correct order regarding the solubility of alkaline earth metal chlorides in water is . from Mg 2+ to Ba 2+. Only the lightest element (Be) does not react readily with N2 to form the nitride (M3N2), although finely divided Be will react at high temperatures. As discussed in earlier chapters, CaCl2 is used as “road salt” to lower the freezing point of water on roads in cold temperatures. The alkaline earths possess many of the characteristic properties of metals.Alkaline earths have low electron affinities and low electronegativities.As with the alkali metals, the properties depend on the ease with which electrons are lost.The alkaline earths have two electrons in the outer shell. Thanks to all authors for creating a page that has been read 6,293 times. It is safe to use because it so weakly alkaline. In the reverse of Equation $$\ref{Eq5}$$, the oxides of Ca, Sr, and Ba react with CO2 to regenerate the carbonate. In ScienceAid. The alkaline earth metals have a greater tendency than the alkali metals to form complexes with crown ethers, cryptands, and other Lewis bases. It is measured in either, grams or moles per 100g of water. NCERT P Bahadur IIT-JEE Previous Year Narendra Awasthi MS Chauhan. 22.4: The Alkaline Earth Metals (Group 2), [ "article:topic", "showtoc:no", "license:ccbyncsa", "program:hidden" ], https://chem.libretexts.org/@app/auth/2/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FGeneral_Chemistry%2FBook%253A_Chemistry_(Averill_and_Eldredge)%2F21%253A_Periodic_Trends_and_the_s-Block_Elements%2F22.4%253A_The_Alkaline_Earth_Metals_(Group_2), $\mathrm{BeCl_2(s)}+\mathrm{2K(s)}\xrightarrow\Delta\mathrm{Be(s)}+\mathrm{2KCl(s)} \label{Eq1}$, General Properties of the Alkaline Earth Metals, Reactions and Compounds of the Alkaline Earth Metals, Organometallic Compounds Containing Group 2 Elements, information contact us at info@libretexts.org, status page at https://status.libretexts.org. In contrast to the alkali metals, the heaviest alkaline earth metal (Ba) is the strongest reductant, and the lightest (Be) is the weakest. Reactions in Water. Retrieved Jan 11, 2021, from https://scienceaid.net/chemistry/fundamental/group2.html. Solubilities for the binary systems, salt-H/sub 2/O, of the chlorides of lithium, rubidium, cesium, magnesium, calcium, strontium, and barium from near 0/sup 0/C to the saturated boiling point are reported. Solubility Patterns in the Periodic Table continued 2 216 linn Scientiic nc ll ihts esered 4. Some examples may help you to remember the trend: Magnesium hydroxide appears to be insoluble in water. Other applications of group 2 compounds described in earlier chapters include the medical use of BaSO4 in “barium milkshakes” for identifying digestive problems by x-rays and the use of various alkaline earth compounds to produce the brilliant colors seen in fireworks. "The effects of hydrogen chloride (hcl) concentration and temperature on the solubility and hydration state of the alkali chlorides licl, nacl, and kcl and the alkaline-earth chlorides, mgcl2, and cacl2 were investigated by the Bureau of Mines. When the reactants are present in a 1:1 ratio, the binary chalcogenides (MY) are formed; at lower M:Y ratios, salts containing polychalcogenide ions (Yn2−) are formed. In. Hydroxides of the lighter alkaline earth metals are insoluble in water, but their solubility increases as the atomic number of the metal increases. The group 2 elements almost exclusively form ionic compounds containing M2+ ions. Low solubility of LiF (0.27 g/100 g H2O ) is due to its high lattice energy ( - 1005 KJmol-1) whereas the low solubility of CsI (44g/100g H2O ) is due to smaller hydration energy of the two ions (-670 KJ/mol) . Author has 619 answers and 52.9K answer views The alkaline earth metals are magnesium, calcium, strontium, and beryllium. Pure samples of most of the alkaline earth metals can be obtained by electrolysis of the chlorides or oxides. Write about solubility of fluorides in comparison to chlorides of alkaline earth metals. This means the precipitate barium sulfate has been formed; which, as you can see from the solubility table above, this is insoluble. The solubility of alkaline earth carbonate and sulfates decrease down the group because the hydration energies decrease. JPCRD 2008, 37(4). Also, like the alkali metals, the alkaline earth metals form a wide variety of simple ionic salts with oxoanions, such as carbonate, sulfate, and nitrate. Both elemental Be and BeO, which is a high-temperature ceramic, are used in nuclear reactors, and the windows on all x-ray tubes and sources are made of beryllium foil. Strontium was obtained from strontianite ($$SrCO_3$$) found in a lead mine in the town of Strontian in Scotland. MgO_{(s)} + Fe/Si_{(s)} \rightarrow 2Mg(l) + Ca_2SiO_{4\;(s)} + Fe(s) \label{Eq3}\]. As salt is a sulfate, the solubility differs depending on the type of salt and whether the salt is hydrated or not. Another strange feature is that it is amphoteric. 2.8K views An early source of magnesium was an ore called magnesite ($$MgCO_3$$) from the district of northern Greece called Magnesia. Both lattice enthalpy and hydration enthalpy decreases down the group as the size of the cation increases but lattice enthalpy decreases more rapidly than the hydration enthalpy and hence the solubility increases down the group. On a microscale students add solutions containing lithium, calcium and silver cations to solutions containing fluoride, chloride, bromide and iodide anions, and record which combinations produce an insoluble precipitate. The nitrate salts tend to be soluble, but the carbonates and sulfates of the heavier alkaline earth metals are quite insoluble because of the higher lattice energy due to the doubly charged cation and anion. The carbonates of the alkaline earth metals also react with aqueous acid to give CO2 and H2O: $MCO_{3(s)} + 2H^+_{(aq)} \rightarrow M^{2+}_{(aq)} + CO_{2(g)} + H_2O_{(l)} \label{Eq7}$. If we consider the periodic table, the elements that would fall in the group 2 of the table are usually known as alkali earth metals. Like the alkali metals, the heavier alkaline earth metals are sufficiently electropositive to dissolve in liquid ammonia. Complex formation is most important for the smaller cations (Mg2+ and Ca2+). The alloy in a spark plug electrode must release electrons and promote their flow across the gap between the electrodes at high temperatures. All the alkaline earth carbonates will neutralize an acidic solution by Equation $$\ref{Eq7}$$. Here we shall look at the solubilities of the hydroxides and sulfates of Group 2 metals. Edited by Jamie (ScienceAid Editor), Taylor (ScienceAid Editor), Jen Moreau, SarMal and 1 other. Except for BeO, which has significant covalent character and is therefore amphoteric, all the alkaline earth oxides are basic. When magnesium is reacted with steam, it is even more vigorous, and instead of a hydroxide, an oxide is produced as well as hydrogen gas. Follow the procedure given in Example 3 to predict the products of each reaction and then balance each chemical equation. is done on EduRev Study Group by NEET Students. Unless otherwise noted, LibreTexts content is licensed by CC BY-NC-SA 3.0. The standard electrode potentials of Ca and Sr are not very different from that of Ba, indicating that the opposing trends in ionization energies and hydration energies are of roughly equal importance. In association with Nuffield Foundation. Here we shall look at the solubilities of the hydroxides and sulfates of Group 2 metals. Solubility of the hydroxides. Halides are hygroscopic and have the water of crystallization in their solid state (CaCl 2.6H 2 O). Solubility is the maximum amount a substance will dissolve in a given solvent. Categories : With their half-filled ns orbitals, the alkali metals have a significant affinity for an additional electron. Be → Sr : form only monoxide(MO) Ba : form peroxide BaO2 under pressure; Solubility increases from BeO to BaO BeO,MgO,SrO,BaO → increasing solubility; All oxides are base (BeO is amphoteric) BeO,MgO,SrO,BaO All metal oxides are ionic (except BeO) divalent metal ions are sufficiently polarizing to make peroxide when heated in pure oxygen. The solubility of various metals in fused chlorides, a phenomenon not widely recognized, has been summarized by Corbett (1) and Eastman et al. The beryllium halides, with properties more typical of covalent compounds, have a polymeric halide-bridged structure in the solid state, as shown for BeCl2. Would you like to give back to the community by fixing a spelling mistake? Most commercial aluminum actually contains about 5% magnesium to improve its corrosion resistance and mechanical properties. A small percentage of beryllium dramatically increases the strength of copper or nickel alloys, which are used in nonmagnetic, nonsparking tools (such as wrenches and screwdrivers), camera springs, and electrical contacts. The solutions in the alkali metal chlorides are pseudo‐binary reciprocal ternary mixtures; the more soluble barium and strontium oxides showed small deviations, calcium oxide showed larger deviations while the extremely sparingly‐soluble magnesium oxide showed extensive deviations from ideality. For more information contact us at info@libretexts.org or check out our status page at https://status.libretexts.org. All oxides except BeO react with CO2 to form carbonates, which in turn react with acid to produce CO2 and H2O. The solutions in the alkaline‐earth metal chlorids melts are binary mixtures with no solvate formation; these systems show some from ideality at low mole fractions (x = 0.1 to 0.25) but they are practically ideal at mole fractions from 0.25 to 0.6. Magnesium can be substituted for any Group 2 metal, however. Very quickly we shall go over the trends in properties of Group 2 elements using the below table. B The balanced chemical equation is $CaO_{(s)} + 2HCl_{(g)} → CaCl_{2(aq)} + H_2O_{(l)}$, $$\mathrm{CaH_2(s)}+\mathrm{TiO_2(s)}\xrightarrow\Delta\mathrm{Ti(s)}+\mathrm{CaO(s)}+\mathrm{H_2O(l)}$$. Alkaline earth metals dissolve in liquid ammonia to give solutions that contain two solvated electrons per metal atom. ScienceAid.net. Therefore stability of alkyl metal chlorides follows the order KCl (-428)>CsCl (-424)>RbCl (-423)>NaCl (-400)>LiCl (-398). Solubility is the maximum amount a substance will dissolve in a given solvent. Chemistry. Predict the products of each reaction and then balance each chemical equation. For the same halide ion, the melting point of lithium halides are lower than those of the corresponding sodium halides and thereafter they decrease as we move down the group from Na to … The fluorides of these are soluble in water and their solubility decreases with the increase in atomic numbers. While it's more favourable to solvate Li+, it's also harder to … In this case, however, two solvated electrons are formed per metal atom, and no equilibriums involving metal dimers or metal anions are known. MLA (Modern Language Association) are solved by group of students and teacher of NEET, which is also the largest student community of NEET. Physics. The relative solubility of the metal hydroxides. Heating a barium-containing alloy to high temperatures will cause some ionization to occur, providing the initial step in forming a spark. As an example, the following reaction takes place between magnesium and water, an alkali earth metal hydroxide and hydrogen gas is produced. Beryllium was first obtained by the reduction of its chloride; radium chloride, which is radioactive, was obtained through a series of reactions and separations. The higher lattice energy due to the highly charged M2+ and N3− ions is apparently sufficient to overcome the chemical inertness of the N2 molecule, with its N≡N bond. Its low density (1.74 g/cm3 compared with 7.87 g/cm3 for iron and 2.70 g/cm3 for aluminum) makes it an important component of the lightweight metal alloys used in aircraft frames and aircraft and automobile engine parts (Figure $$\PageIndex{1}$$). Alkaline earth metals fluorides solubility-related constants; Metal M 2+ HE [clarification needed] F − HE [clarification needed] "MF 2 " unit HE MF 2 lattice energies Solubility [clarification needed] Be 2,455 458 3,371 3,526 soluble Mg 1,922 458 2,838 2,978 0.0012 Ca 1,577 458 2,493 2,651 0.0002 Sr 1,415 458 2,331 2,513 0.0008 Ba 1,361 458 To describe how to isolate the alkaline earth metals. $\mathrm{MCO_3(s)}\xrightarrow\Delta\mathrm{MO(s)}+\mathrm{CO_2(g)} \label{Eq5}$. Magnesium sulfate and calcium sulfate (both salts) are considered insoluble unless they are hydrated. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. "Group 2, Alkaline Earth Metals." Evidently more negative value of ∆Hf°, more stable is the compound. For alkaline earth ... tion of the metal in the alkaline earth metal-metal chloride systems proceeds by the formation of polymer ions of the type ++ Mn where n is a number from two to four. Thus they react with water to form the hydroxides—M(OH)2: $MO_{(s)} + H_2O_{(l)} \rightarrow M^{2+}_{(aq)} + 2OH^−_{(aq)} \label{Eq6}$. - The solubility of the alkaline earth metal sulphates is slightly increased by the addition of strong acids. As a component of the alloy in an automotive spark plug electrode, would you use Be, Ca, or Ba? Please help me to understand the solubility trend of group 2 salt trend? When added to water, the first alkaline earth metal (Beryllium) is totally unreacative, and doesn't even react with steam.Then as you move down the group, the reactions become increasingly vigourous.. As an example, the following reaction takes place between magnesium and water, an alkali earth metal hydroxide and hydrogen gas is produced. Recall that beryllium halides behave like Lewis acids by forming adducts with Lewis bases (Equation $$\ref{Eq4}$$). The stability of a compound depends upon its enthalpy of formation, ∆Hf°. All the heavier alkaline earth metals (Mg through Ba) react directly with hydrogen to produce the binary hydrides (MH2). and they dissolve in aqueous acid. … (2). For example, MgO (melting point = 2825°C) is used to coat the heating elements in electric ranges. The chemical test for a sulphate is to add Barium Chloride. Because BeO and MgO are much more inert than the other group 2 oxides, they are used as refractory materials in applications involving high temperatures and mechanical stress. In addition, CaCO3 is a major component of cement and an ingredient in many commercial antacids. Have questions or comments? Properties of the Alkaline Earth Metals . The hydrides of the heavier alkaline earth metals are ionic, but both BeH2 and MgH2 have polymeric structures that reflect significant covalent character. Because BeO and MgO are much more inert than the other group 2 oxides, they are used as refractory materials in applications involving high temperatures and mechanical stress. Each of these elements contains two electrons in their outermost shell. For example, the density of Ca is less than that of Be and Mg, the two lightest members of the group, and Mg has the lowest melting and boiling points. Evidently greater the lattice energy, higher is the melting point of the alkali metals halide and lower is its solubility in water. Grignard reagents can be used to synthesize various organic compounds, such as alcohols, aldehydes, ketones, carboxylic acids, esters, thiols, and amines. Several important properties of the alkaline earth metals are summarized in Table $$\PageIndex{1}$$. Like the alkali metals, the lightest alkaline earth metals (Be and Mg) form the most covalent-like bonds with carbon, and they form the most stable organometallic compounds. Beryllium does not react with hydrogen except at high temperatures (1500°C), although BeH2 can be prepared at lower temperatures by an indirect route. All alkaline earth metals react with the halogens to produce the corresponding halides, with oxygen to form the oxide (except for barium, which forms the peroxide), and with the heavier chalcogens to form chalcogenides or polychalcogenide ions. Because beryllium and its salts are toxic, however, BeCO.

Snappy Trap Lowe's, Caution Child At Play Signnorthern Beaches Council Parking, What Is Exceptional Customer Service In Banking, Mahindra Tractor 575, Pin Lock Keg Tap, Programming Languages List On Resume, Coconut Oil Chocolate, Tamil Panchangam 2020 To 2021 Pdf,