Write the half equation for:
1. Oxidation of potassium to form potassium ion
2. Oxidation of lithium to form lithium ion
3. Oxidation of francium to form francium ion
4. Oxidation of calcium to form calcium ion
5. Oxidation of barium to form barium ion
6. Oxidation of magnesium to form magnesium ion
7. Oxidation of aluminium to form aluminium ion
8. Reduction of bromine to form bromide ion
9. Reduction of iodine to form iodide ion
10. Reduction of chlorine to form chloride ion
11. Reduction of oxygen to oxide ion
12. Reduction of sulphur to form sulphide ion
13. Reduction of nitrogen to form a nitride ion
14. Oxidation of a chloride ion to form chlorine molecule
15. Oxidation of bromide ion to form bromine molecule
16. Oxidation of oxide ion to form oxygen molecule
17. Reduction of a sodium ion to form a sodium atom
18. Reduction of a calcium ion to form a calcium atom
19. Reduction of a magnesium ion to form a magnesium atom
20. Reduction of an aluminium ion to form an aluminium atom
Ps:si lo haceis doy 300ptos + es muy urgente
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Group 2A (or IIA) of the periodic table are the alkaline earth metals: beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra). They are harder and less reactive than the alkali metals of Group 1A. The name comes from the fact that the oxides of these metals produced basic solutions when dissolved in water, and they remained solids at the temperatures available to the ancient alchemists. Like the Group 1A elements, the alkaline earth metals are too reactive to be found in nature in their elemental form.
The alkaline earth metals have two valence electrons in their highest-energy orbitals (ns2). They are smaller than the alkali metals of the same period, and therefore have higher ionization energies. In most cases, the alkaline earth metals are ionized to form a 2+ charge.
The alkaline earth metals have much higher melting points than the alkali metals: beryllium melts at 1287ºC, magnesium at 649ºC, calcium at 839ºC, strontium at 768ºC, barium at 727ºC, and radium at 700ºC. They are harder metals than the Group 1A elements, but are soft and lightweight compared to many of the transition metals.
Salts of the Group 2A metals are less soluble in water than those of Group 1A because of the higher charge densities on the 2+ cations; nevertheless, many Group 2A salts are at least moderately soluble. Some Group 2A salts bond strongly to water molecules, and crystallize as hydrates; among these are Epsom salt, MgSO4·7H2O, and gypsum, CaSO4·2H2O.
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