Question

Predict whether each of the following oxides is ionic or molecular: \(\operatorname{Sn} \mathrm{O}_{2}, \mathrm{Al}_{2} \mathrm{O}_{3}, \mathrm{CO}_{2}, \mathrm{Li}_{2} \mathrm{O}, \mathrm{Fe}_{2} \mathrm{O}_{3}, \mathrm{H}_{2} \mathrm{O} .\)

Short answer

Based on the analysis of each oxide, the predictions are as follows: - \( \operatorname{SnO}_{2} \): Ionic - \( \mathrm{Al}_{2} \mathrm{O}_{3} \): Ionic - \( \mathrm{CO}_{2} \): Molecular - \( \mathrm{Li}_{2} \mathrm{O} \): Ionic - \( \mathrm{Fe}_{2} \mathrm{O}_{3} \): Ionic - \( \mathrm{H}_{2} \mathrm{O} \): Molecular

Step-by-step solution

SnO2

Sn (Tin) is a metal and O (Oxygen) is a non-metal, we should expect this to be an ionic compound.

Al2O3

Al (Aluminum) is a metal and O (Oxygen) is a non-metal, we should expect this to be an ionic compound.

CO2

C (Carbon) and O (Oxygen) are both non-metals, we should expect this to be a molecular compound with covalent bonds.

Li2O

Li (Lithium) is a metal and O (Oxygen) is a non-metal, we should expect this to be an ionic compound.

Fe2O3

Fe (Iron) is a metal and O (Oxygen) is a non-metal, we should expect this to be an ionic compound.

H2O

H (Hydrogen) and O (Oxygen) are both non-metals, we should expect this to be a molecular compound with covalent bonds. In summary, according to the analysis, the following are the predictions for each oxide: - SnO2: Ionic - Al2O3: Ionic - CO2: Molecular - Li2O: Ionic - Fe2O3: Ionic - H2O: Molecular

Key concepts

Chemical Bonding

Chemical bonding is the force that holds atoms together in compounds, and it comes in various types, primarily ionic and covalent bonds. In ionic bonding, atoms transfer electrons to achieve a full outer electron shell, leading to the formation of positively charged ions (cations) and negatively charged ions (anions). This electron transfer typically occurs between metallic and nonmetallic elements, such as in lithium oxide (Li_2O), where lithium (Li) donates electrons to oxygen (O). On the other hand, a covalent bond forms when two nonmetallic elements share electrons, as is the case with carbon dioxide (CO_2), where carbon and oxygen share electrons in a molecular compound.

Understanding the difference between these types of bonds is crucial for predicting the properties of a compound. For instance, ionic compounds typically have higher melting and boiling points and conduct electricity when dissolved in water or melted, while covalent compounds can be gases, liquids, or solids at room temperature, with lower melting points compared to ionic compounds and poor conductivity.

Metallic and Nonmetallic Elements

The distinction between metallic and nonmetallic elements is one of the most fundamental concepts in chemistry and plays a key role in the classification of compounds. Metals, found on the left side of the periodic table, readily lose electrons to form positive ions. Nonmetals, on the right side, tend to gain electrons to form negative ions.

In the exercise, we encounter a variety of elements: tin (Sn), aluminum (Al), lithium (Li), and iron (Fe) are classified as metals and tend to form cations, while carbon (C), hydrogen (H), and oxygen (O) are nonmetals and likely to form anions or share electrons in covalent bonds. Compounds made from metals and nonmetals like (Al_2O_3 and SnO_2) are typically ionic, whereas compounds composed entirely of nonmetals, such as water (H_2O) and carbon dioxide (CO_2), are molecular with covalent bonds.

Compound Classification

Classifying compounds as either ionic or molecular determines how we predict their behavior and properties. Ionic compounds are usually formed between metallic and nonmetallic elements where there is a transfer of electrons. This transfer leads to the formation of ions that are held together by the electrostatic attraction between oppositely charged particles. In our exercise, when predicting the nature of oxides like (Fe_2O_3 and Li_2O), the involvement of a metal indicates the compound is ionic.

Molecular compounds, however, result from the covalent bonding between nonmetallic elements and involve the sharing of electrons between atoms. These shared electrons result in the stable outer electron shells for each atom within the molecule. The oxides formed in this manner, such as CO_2 and H_2O, exhibit molecular characteristics.

Moreover, the classification of compounds guides us in understanding their physical states under normal conditions, reactivity, solubility, electrical conductivity, and other key properties that are essential for practical applications in daily life and various industries.