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Вы можете ознакомиться и скачать презентацию на тему Alkaline earth metals. Доклад-сообщение содержит 10 слайдов. Презентации для любого класса можно скачать бесплатно. Если материал и наш сайт презентаций Mypresentation Вам понравились – поделитесь им с друзьями с помощью социальных кнопок и добавьте в закладки в своем браузере.

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OCCURRENCE Since the group 2A elements are relatively active metals, they occur in compounds in nature. Magnesium, Mg The principal useful ores o f magnesium are dolomite (CaCO3 · MgCO3 a double salt), carnallite, (KCl · MgCl2 · 6H2O) and epsom salt (MgSO4 · 7H2O) which is found in mineral water.

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Calcium, Ca Calcium, Ca Calcium compounds are widely distributed in nature, occurring as limestone or marble (CaCO3), gypsum (CaSO4 · 2H2O) and fluorite (CaF2). Salts of sulfate, silicate and phosphate are also found in the earth‘s crust.

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Reactions 1) All alkaline earth metals, except beryllium, react with H2 gas in hot medium to produce hydrides, like alkali metals. M(s) + H2(g) ⎯⎯heat→ MH2(s) (M : alkaline earth metals) Mg(s) + H2(g) ⎯heat⎯→ MgH2(s) Ca(s) + H2(g) ⎯heat⎯→ CaH2(s)

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2) Ca, Sr and Ba react with water, like alkali metals, at room temperature to produce metal hydroxides and hydrogen gas. 2) Ca, Sr and Ba react with water, like alkali metals, at room temperature to produce metal hydroxides and hydrogen gas. Ca(s) + 2H2O(l) → Ca(OH)2(aq) + H2(g) Magnesium metal reacts slowly with boiling water. The reaction of beryllium with water is very difficult. Mg(s) + 2H2O(l) ⎯→ Mg(OH)2(s) + H2(g) Be(s) + 2H2O(l) ⎯→ Be(OH)2(s) + H2(g)

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3. They form oxides as a result of their reactions with oxygen, in MO formula 2M(s) + O2(g) ⎯→ 2MO(s) 2Mg(s) + O2(g) ⎯→ 2MgO(s)

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4. All alkaline earth metals give direct reactions with halogens to produce metal halides. M(s) + X2(g) ⎯→ MX2(s) Ca(s) + Cl2(g) ⎯→ CaCl2(s) Mg(s) + Cl2(g) ⎯→ MgCl2(s)

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5. The reactions of the group 2A elements with acids like HCl and H2SO4, produce salts and H2 gas. 5. The reactions of the group 2A elements with acids like HCl and H2SO4, produce salts and H2 gas. Ca(s) + 2HCl(aq) ⎯→ CaCl2(s) + H2(g) While magnesium reacts with dilute H2SO4 by giving H2 gas, it reacts with hot and concentrated H2SO4 by producing SO2 gas. Mg(s) + H2SO4(dil.) → MgSO4(s) + H2(g) Mg(s) + 2H2SO4(aq)(conc.) → MgSO4(aq) + . SO2(g)+2H20(l)