Explain the formation of Magnesium Chloride ($ ext{MgCl}2$) by the transfer of electrons. State two general physical pr

Question

Explain the formation of Magnesium Chloride ($	ext{MgCl}2$) by the transfer of electrons. State two general physical properties of ionic compounds.

Accepted Answer

Formation of Magnesium Chloride ($	ext{MgCl}2$): Magnesium atom: Atomic number = 12 Electronic configuration = 2, 8, 2 To achieve a stable octet, it loses 2 valence electrons to form a magnesium cation ($	ext{Mg}^{2+}$): $$	ext{Mg} ightarrow 	ext{Mg}^{2+} + 2e^-$$ Chlorine atom: Atomic number = 17 Electronic configuration = 2, 8, 7 It needs 1 electron to complete its octet and form a chloride anion ($	ext{Cl}^-$): $$	ext{Cl} + e^- ightarrow 	ext{Cl}^-$$ Electron Transfer Process: One magnesium atom transfers its 2 valence electrons to two individual chlorine atoms (1 electron to each chlorine atom). $$	ext{Mg} + 2\cdot\ddot{	ext{Cl}}: ightarrow 	ext{Mg}^{2+} \left :\ddot{	ext{Cl}}:ight^-2$$ The strong electrostatic force of attraction holds the oppositely charged ions ($	ext{Mg}^{2+}$ and $	ext{Cl}^-$) together, forming the ionic compound $	ext{MgCl}2$. Properties of Ionic Compounds: High Melting and Boiling Points: They have strong inter-ionic electrostatic forces of attraction, requiring a significant amount of heat energy to break the ionic bonds. Electrical Conductivity: They conduct electricity in the molten state or when dissolved in water because free ions are available to move, but they do not conduct electricity in the solid state.

Metals and Non-metals

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