Very Short Question and Answers - Properties of Ionic Compounds

Ionic compounds are held together by strong electrostatic forces of attraction, also known as ionic bonds, between oppositely charged ions.

Ionic compounds have high melting and boiling points because of the strong electrostatic forces of attraction between their oppositely charged ions, which require a large amount of heat energy to break.

Examples include sodium chloride (NaCl) with a melting point of about 800°C and magnesium oxide (MgO) with a melting point of about 2852°C.

Ionic compounds dissolve well in water because water is a polar solvent that can surround and separate the positive and negative ions, pulling them into solution.

Sodium chloride (NaCl) and potassium nitrate (KNO₃) are highly soluble in water.

Ionic compounds generally do not dissolve in non-polar solvents such as kerosene or petrol.

In the solid state, ionic compounds do NOT conduct electricity because their ions are fixed in place and cannot move.

Molten NaCl conducts electricity because the ions are free to move and can carry electric current.

The melting point of NaCl is about 800°C and the boiling point is 1413°C.

Barium sulfate (BaSO₄) is an example of an ionic compound that is sparingly soluble in water.

In aqueous solution, the ions are free to move and carry electric current, but in solid form, the ions are fixed and cannot move, so no electricity is conducted.

Ionic compounds conduct electricity in molten (liquid) state and when dissolved in water (aqueous solution).

Sodium chloride (NaCl) and copper(II) sulfate (CuSO₄) are used in electrolysis.

Water is called a polar solvent because its molecules have partial positive and negative charges that help separate and stabilize ions.

NaCl would not dissolve in petrol because petrol is a non-polar solvent and cannot separate the positive and negative ions of NaCl.

Ionic compounds generally have high melting and boiling points, are soluble in water, and conduct electricity in molten or solution state; covalent compounds usually have lower melting/boiling points, are less soluble in water, and do not conduct electricity.

The strong electrostatic attraction between the ions makes ionic compounds form solid, crystalline structures at room temperature.

Free ions act as charge carriers, allowing the flow of electric current in molten or aqueous ionic compounds.

Molten aluminium oxide (Al₂O₃) is used for extraction of aluminium; its ability to conduct electricity in molten state is utilized.

Ionic compounds have high melting and boiling points, are generally soluble in water but not in non-polar solvents, and conduct electricity in molten or aqueous state but not in solid state.