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MAGNESiUM (Mg)

A typical metal with atomic number 12.
Period: 3
Group: IIA
Atomic weight: 24
Protons: 12
Neutrons: 12 (frequent isotope Mg-24)
Electrons: 12 or 10 if constant oxidation degree is +2
Electron configuration: 2, 8, 2
(+12) ) ) )
      2 8 2 (Free metal)

(+12) ) )
      2 8 (Cation)
Electron formula:
1s2 2s2 2p6 3s2
Electronegativity: 1.2

Gray metal
Melting point 650*С
Boiling point 1105*С
Hexagonic crystall lattice
Clark 19 kg/tonn
Sea water 0,13 %

Well-Known Substances:
Carnallite MgCl₂ • KCl • 6H₂O
Bishofite MgCl₂ • 6H₂O
Kieserite MgSO₄ • H₂O
Epsomite MgSO₄ • 7H₂O
Kainite KCl • MgSO₄ • 3H₂O
Magnesite MgCO3
Dolomite CaCO3 x MgCO3
Brucite Mg(OH)2

Mg production: USA 43%; CIS 26%; Norway 17%

<sub>Reactive metal covered by MgO

Typical reactions:</sub>

Magnesium preparation:
MgCl2 => (electrolysis) Mg + Cl2
MgO + C => Mg + CO

2MgO + CaO + Si = CaSiO₃ + 2Mg

CaCO₃·MgCO₃ = CaO + MgO + 2CO<sub>2

Mg + 2H2O => Mg(OH)2 + H2

Mg + 2HCl => MgCl2 + H2

2Mg + O2 => 2MgO

3Mg + N2 => Mg3N2

2Mg + CO2 => 2MgO + C

Significance:</sub>

MgH2 - capacious accumulator of hydrogen
MgO - refractory material
Mg(ClO4)2 (anhydrone) - profound reclamation of gases in labs
MgF2 - used in optics as synthetic monocrystalls
MgBr2 - used as electrolyte for chemical backup power source
Also Mg is used in medicine, warfare, photographing, accumulators

CALCiUM (Ca)
A typical alkaline earth metal with atomic number 20.
Period: 4
Group: IIA
Atomic weight: 40
Protons: 20
Neutrons: 20 (frequent isotope Ca-40 (96.97%))
Electrons: 20 or 18 if constant oxidation degree is +2
Electron configuration: 2, 8, 8, 2
(+20) ) ) ) )
      2 8 8 2 (Free metal)

(+20) ) ) )
      2 8 8 (Cation)
Electron formula:
1s2 2s2 2p6 3s2 3p6 4s2
Electronegativity: 1.0

Soft gray metal
Melting point 1112K
Boiling point 1757K
Cubic face-centred crystall lattice
3.38% of Earth crust (5th place)
Sea water 400 mg/l

Well-Known Substances:
Ca[Al₂Si₂O₈] (anorthite)
CaCO3 (calcite)
CaSO4 (anhydrite)
CaSO4 x 0.5 H2O (alabaster)
CaSO4 x 2H2O (gypsum)
CaF2 (fluorite)
Ca₅(PO₄)₃(F,Cl,OH) (apatites)
MgCO3 x CaCO3 (dolomite)
385 minerals (4th place)
Ca₅(PO₄)₃OH (hydroxyapatite)
3Ca₃(PO₄)₂·Са(OH)<sub>2

Reactive metal
=> Recommend to save it in kerosene or liquid paraffin (react with air/water/CO2 quickly)

Typical reactions:

4CaO + 2Al => CaAl2O4 + 3Ca (Preparation of Ca)

Ca + 2H2O => Ca(OH)2 + H2
2Ca + O2 => 2CaO
Ca + Br2 => CaBr2
Ca + H2 => CaH2
Ca + 6B => CaB6
3Ca + N2 => Ca3N2
Ca + 2C => CaC2
6Ca + P4 => 2Ca3P2
2Ca + Si => Ca2Si
CaH2 + 2H2O => Ca(OH)2 + 2H2
Ca3N2 + 6H2O => 3Ca(OH)2 + 2NH3
CaCO3 + H2O + CO2 <=> Ca(HCO3)2

Significance:

Reduct metals from their oxides (3Ca + Al2O3 => 3CaO + 2Al)
Ca x Pb (accumulator batteries)</sub>
Destroying the air in electrovacuum devices
Metallothermy
Ca-48 - radioactive isotope used in nuclear physics
Used in medicine and toothpaste

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