Chemistry – Atoms, elements and compounds - Ions and ionic bonds | e-Consult
Atoms, elements and compounds - Ions and ionic bonds (1 questions)
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Ionic compounds, such as sodium chloride (NaCl), have significantly higher melting and boiling points compared to most covalent compounds. This is due to the strong electrostatic forces between the positively charged ions (cations) and the negatively charged ions (anions) in the ionic lattice.
Explanation:
- Strong Electrostatic Forces: The attraction between oppositely charged ions is a powerful force. These forces extend throughout the entire crystal lattice.
- Energy Required to Overcome Forces: To melt or boil an ionic compound, a large amount of energy is required to overcome these strong electrostatic forces and disrupt the ionic lattice.
- Large Number of Ions: Ionic compounds consist of a vast number of ions packed closely together in a regular arrangement. This contributes to the overall strength of the lattice.
The higher the charge on the ions and the smaller the ionic radii, the stronger the electrostatic forces and the higher the melting and boiling points will be. For example, magnesium oxide (MgO) has a higher melting point than sodium chloride (NaCl) because magnesium ion (Mg2+) has a higher charge and smaller radius than sodium ion (Na+).