• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

The group II elements are beryllium, magnesium, calcium, strontium, barium andRadium. The appearances of the Group II elements are all metals with a shiny, silvery-white colour.

Extracts from this document...

Introduction

Group II Elements The group II elements are beryllium, magnesium, calcium, strontium, barium and Radium. The appearances of the Group II elements are all metals with a shiny, silvery-white colour. The alkaline earth metals are high in the reactivity series of metals, but not as high as the alkali metals of Group 1. Reactivity of Group II elements increases down the group. This can be explained by the increase in ease at losing two outer electrons as the elements descend the group. The loss of electrons becomes easier due to the decreasing ionisation energy required. Ionisation energy decreases due to extra shielding from inner shells and increase in distance from the nucleus. ...read more.

Middle

These electrons are relatively easy to remove, but removing the third electron is much more difficult, as it is close to the nucleus and in a filled quantum shell. This results in the formation of M2+. The ionisation energies reflect this electron arrangement. The first two ionisation energies are relatively low, and the third very much higher. Reaction with oxygen All group II elements react in air to form an oxide layer which dulls the surface of the metal. Barium is so reactive it is stored under oil.The reactivity increases down the group, and they all forming a white oxide. 2Mg(s) + O2(g) 2MgO(s) Reaction with water Reactivity increases down the group. ...read more.

Conclusion

They are prepared easily by reaction of the metal, metal oxide or metal carbonate with an acid. Magnesium, magnesium oxide or magnesium carbonate all dissolve in hydrochloric acid, to form colourless solutions containing (aq) magnesium chloride, MgCl2(aq). This white crystalline compound may be obtained by partial evaporation of the solution. The reaction of magnesium with hydrochloric acid is that the magnesium ribbon dissolves rapidly in cold dilute hydrochloric acid with rapid evolution of hydrogen gas. Mg(s) + 2HC(aq) MgCL2(aq) + H2(g) Chalk and lime Chalk is made from the sedimentary remains of marine invertebrates, chemically they are composed of calcium carbonate CaCO3. Limestone and chalk are used in large quantities to manufacture quick lime (calcium oxide) and cement. Strong heating of calcium carbonate produces calcium oxide, CaO(s) + CO2(g) Calcium oxide reacts vigorously with water to produce calcium hydroxide Ca(Oh)2. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Aqueous Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related GCSE Aqueous Chemistry essays

  1. The Group VII elements - Halogens

    The likelihood is that, at any instant, the charge distribution of an atom will not be symmetrical. If electrons are thought of as " charge clouds", wherein the electrons are in constant motion, then it is entirely plausible that, at any instant, there will be more electrons in one area than in another.

  2. The Rates of Reaction of Metals with Acid.

    Take the measuring cylinder and measure out 50cm3 of 2 mole HCl. 3) With the 50 cm3, place it into a conical flask and put into the water bath. 4) Place the other thermometer into the conical flask. 5)

  1. How much Iron (II) in 100 grams of Spinach Oleracea?

    Place the conical flask on a white tile. 7) While swirling the conical flask, titrate the Potassium Manganate (VII) (aq) into the conical flask containing Iron (II) Ammonium Sulphate (aq) and Sulphuric Acid (aq) until the first trace of a pink colour appears.

  2. Transition metals

    It is also very malleable and ductile. Copper is easily mixed with other metals to form alloys such as bronze and brass. Bronze is an alloy of tin and copper, and brass is an alloy of zinc and copper. Copper is also resistant to corrosion (it does not rust very easily).

  1. An Essay on theComparison and Contrast between Group 1 and Group 2 Elements

    When we weighed the crucible the again with the residue the weight of sodium carbonate was fairly the same at 31.7212g and calcium carbonate decreased to 29.6521 which meant that no carbon dioxide from the sodium carbonate was given off it still remained in the within the compound this is

  2. Investigating the Chemistry of Group 1 and 2 Elements

    A light precipitate (semi-transparent) or a heavy precipitate (opaque) partially indicates the amount of carbon dioxide released. The exact quantity of carbon dioxide released cannot be given using this test, however it is possible to say that the darker (more opaque/ heavier)

  1. metal extraction and reactivity

    * Si is then added and the mixture is heated in the absence of air. * The FeO is converted into FeSiO3 and run off * The Cu2S is then reduced reduced to Cu by heating in a controlled amount of air.

  2. Observation exercise on the compounds of the s-block elements

    Observation Inference Adding the solution of barium chloride to solution X does not create any visible signs of reaction. Adding dilute hydrochloric acid, also, does not appear to have any effect on the solution. The combination of BaCl2 and HCl is used as a test for both sulphate and carbonate ions.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work