Q Arrange the following solids in order of increasing melting points and account for the order:

step 1 So let's look at the trend in the melting points for the oxides form from the group two metals.

Q Arrange the following solids in order of increasing...

Key Concepts

Cation Size Effect

The size of the cation influences the distance between oppositely charged ions in the lattice. Smaller cations can approach anions more closely, resulting in stronger electrostatic interactions and higher lattice energies. Conversely, larger cations create greater ionic separation, leading to weaker interactions and lower melting points.

Periodic Trends

Periodic trends help explain variations in properties such as melting points among similar compounds. For the alkaline earth metal oxides, as one moves down the group from magnesium to barium, the cation size increases and the corresponding lattice energy decreases, which results in a decrease in melting points.

Ionic Bonding

Ionic bonding is the electrostatic attraction between positively and negatively charged ions. In solids like the alkaline earth metal oxides, the strength of this bonding is a key factor in determining melting points; stronger ionic bonds generally lead to higher melting points because more energy is required to overcome these forces during melting.

Lattice Energy

Lattice energy is the energy released when gaseous ions combine to form an ionic solid. It is directly related to the strength of the ionic bonds within the crystal lattice. A higher lattice energy indicates a more stable crystal structure and typically correlates with a higher melting point, as more energy is needed to break apart the lattice.

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