Question

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

Short answer

Based on the analysis of electronegativity differences, we predict the following oxides to be ionic or molecular: \( SnO_{2} \) - Molecular \( Al_{2}O_{3} \) - Ionic \( CO_{2} \) - Molecular \( Li_{2}O \) - Ionic \( Fe_{2}O_{3} \) - Ionic \( H_{2}O \) - Molecular

Step-by-step solution

Determine the electronegativity values of each element

First, we need to find the electronegativity values of each element. We can use a periodic table or look up these values online.

Calculate the electronegativity difference between the elements in each compound

Next, we'll calculate the electronegativity difference for each compound by subtracting the smaller electronegativity value from the larger one. For example, for SnO2: Electronegativity of Sn: 1.96 Electronegativity of O: 3.44 Difference: 3.44 - 1.96 = 1.48 We'll repeat this process for each compound.

Determine if each compound is ionic or molecular based on electronegativity difference

Using our calculations, we'll determine if each compound is ionic or molecular based on the electronegativity difference. If the difference is 1.7 or greater, the compound is ionic. If the difference is less than 1.7, the compound is molecular. Here's what we've found based on these guidelines: \( SnO_{2} \) Electronegativity difference: 1.48 Verdict: Molecular \( Al_{2}O_{3} \) Electronegativity difference: 2.01 Verdict: Ionic \( CO_{2} \) Electronegativity difference: 0.89 Verdict: Molecular \( Li_{2}O \) Electronegativity difference: 2.30 Verdict: Ionic \( Fe_{2}O_{3} \) Electronegativity difference: 1.75 Verdict: Ionic \( H_2O \) Electronegativity difference: 1.24 Verdict: Molecular

Summary

Based on our analysis of electronegativity differences, we predict the following oxides to be ionic or molecular: \( SnO_{2} \) - Molecular \( Al_{2}O_{3} \) - Ionic \( CO_{2} \) - Molecular \( Li_{2}O \) - Ionic \( Fe_{2}O_{3} \) - Ionic \( H_{2}O \) - Molecular

Key concepts

Ionic and Molecular Compounds

Understanding the distinction between ionic and molecular compounds is pivotal for grasping foundational chemistry concepts. An ionic compound forms when there is a complete transfer of electrons from one atom to another, leading to the formation of oppositely charged ions. Typically, these compounds consist of a metal and a non-metal, such as sodium chloride ((SnO_{2}) is molecular, not ionic.

For instance, when considering aluminum oxide (CO_{2}) demonstrates a lower electronegativity difference (0.89), indicating that the attraction between the carbon and oxygen atoms does not result in electron transfer but in sharing, which categorizes (Li_{2}O) ensuring a strong electrostatic attraction and establishing it as an ionic compound.

In essence, to classify a compound as ionic or molecular, one must look not only at the electronegativity difference but also at the types of atoms involved and their bonding tendencies.

The Periodic Table

The periodic table is an organized arrangement of all known elements, providing a wealth of information at a glance. Elements are ordered by increasing atomic number and arranged into rows called periods and columns known as groups or families, which share common characteristics. One vital piece of information the periodic table provides is electronegativity, which is crucial for predicting the type of bond that forms between atoms.

To solve our textbook exercise, the periodic table acts as a map to find each element's electronegativity. Elements such as fluorine, found on the upper right of the table, exhibit high electronegativity, while those like lithium, located lower left, show lower values. This variation is what underpins our understanding of why some compounds, like (SnO_{2}) or Al_{2}O_{3}) and lithium oxide ((H_{2}O), fall on the molecular side, as the differences in electronegativity in these pairings are not drastic enough to cause full electron transfer.

Chemical Bonding

Chemical bonding is the process that enables atoms to join together to form compounds. Bonds result from attractions between atoms trying to reach a more stable energy state. Generally, bonds can be classified into three main types: ionic, covalent (molecular), and metallic.

Ionic bonds, as seen in lithium oxide ((H_{2}O), electrons are shared between atoms, leading to the formation of a molecule. The guidelines in our exercise use the electronegativity difference to determine the bond type because it implies how strongly an atom can attract and hold onto electrons. A larger difference often signals ionic bonding, as is the case for Al_{2}O_{3}), stoichiometry, and molecular geometry also play roles.