Predict whether each of the following oxides is ionic or molecular: SnO2, Al2 O3, CO2, Li2 O, Fe

step 1 So the trend we're looking at here is that compounds made up of a metal and a non -metal will te

Predict whether each of the following oxides is ionic or...

Predict whether each of the following oxides is ionic or molecular: $\mathrm{SnO}_{2}, \mathrm{Al}_{2} \mathrm{O}_{3}, \mathrm{CO}_{2}, \mathrm{Li}_{2} \mathrm{O}, \mathrm{Fe}_{2} \mathrm{O}_{3}, \mathrm{H}_{2} \mathrm{O} .$ Explain the reasons
for your choices.

Key Concepts

Role of Metal and Nonmetal Characters

The classification of elements as metals or nonmetals plays a significant role in the type of oxide that forms. Metals, which readily lose electrons, tend to form ionic oxides because they react with oxygen (a nonmetal) by transferring electrons to it. In contrast, oxides formed by nonmetals typically involve covalent bonding, where electrons are shared between the oxygen and the nonmetal atom, leading to discrete molecular entities.

Ionic Bonding

Ionic bonding involves the complete transfer of electrons from one atom (usually a metal) to another (usually a nonmetal), forming cations and anions. These oppositely charged ions attract each other and arrange themselves in a regular, repeating lattice. This type of bonding is characterized by high melting points, brittle solids, and conductivity when molten or dissolved in water.

Covalent Bonding

Covalent bonding occurs when atoms share pairs of electrons to achieve a full outer shell, typically occurring between nonmetals or between atoms with similar electronegativities. In covalent compounds, discrete molecules are formed, and these substances often have lower melting and boiling points compared to ionic compounds, as the forces between molecules are generally weaker than the ionic bonds within a lattice.

Electronegativity Difference

The electronegativity difference between atoms is a key predictor in determining the type of bond. A large difference usually results in ionic bonding due to the pronounced electron transfer between atoms, whereas a smaller electronegativity difference often leads to covalent bonding, where electrons are shared more equally between atoms.

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