Predict whether each of the following oxides is ionic or molecular: SnO₂, Al₂O₃, CO₂, Li₂O, Fe₂O₃, H₂O.

Verified step by step guidance

1. Identify the type of elements involved in each oxide. Metals typically form ionic oxides, while nonmetals form molecular oxides.
2. For SnO_2, Sn is a metal, so SnO_2 is likely ionic.
3. For Al_2O_3, Al is a metal, so Al_2O_3 is likely ionic.
4. For CO_2, C is a nonmetal, so CO_2 is likely molecular.
5. For Li_2O, Li is a metal, so Li_2O is likely ionic.

Key Concepts

Ionic vs. Molecular Compounds

Ionic compounds are formed when electrons are transferred from one atom to another, typically between metals and nonmetals, resulting in charged ions that attract each other. In contrast, molecular compounds consist of atoms that share electrons through covalent bonds, usually between nonmetals. Understanding the nature of the bonding helps in predicting whether a compound is ionic or molecular.

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a bond. When the difference in electronegativity between two atoms is large (generally greater than 1.7), the bond is likely ionic, while a smaller difference indicates a covalent bond. This concept is crucial for determining the type of bonding in oxides.

Metallic and Nonmetallic Oxides

Oxides can be classified based on the nature of the elements involved. Metallic oxides, formed from metals and oxygen, tend to be ionic, while nonmetallic oxides, formed from nonmetals and oxygen, are usually molecular. Recognizing the type of elements in the oxide helps in predicting its bonding characteristics.