Textbook Question
Arrange the following oxides in order of increasing covalent character: B2O3, BeO, CO2, Li2O, N2O5.
Ch.22 - The Main Group Elements
Chapter 22, Problem 125
Arrange the following oxides in order of increasing ionic character: SiO2, K2O, P4O10, Ga2O3, GeO2.
Verified step by step guidance1
Step 1: Understand the concept of ionic character. Ionic character refers to the degree to which a bond between two atoms is ionic. The greater the difference in electronegativity between the two atoms, the more ionic the bond is.
Step 2: Identify the elements involved in each oxide and their positions in the periodic table. This will help determine the electronegativity differences. For example, K (potassium) is a metal, while O (oxygen) is a non-metal, suggesting a high ionic character for K2O.
Step 3: Compare the electronegativity differences for each oxide. Generally, the larger the difference in electronegativity between the metal and oxygen, the more ionic the compound. Use a periodic table to find the electronegativity values.
Step 4: Consider the nature of the elements. Metals tend to form more ionic compounds with oxygen, while non-metals form more covalent compounds. For instance, SiO2 and P4O10 are more covalent because Si and P are non-metals.
Step 5: Arrange the oxides in order of increasing ionic character based on the analysis of electronegativity differences and the nature of the elements involved. Start with the most covalent and end with the most ionic.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Ionic Character
Ionic character refers to the degree to which a bond between two atoms has ionic characteristics, as opposed to covalent characteristics. It is influenced by the difference in electronegativity between the bonded atoms; larger differences typically indicate higher ionic character. This concept is crucial for understanding how to classify compounds based on their bonding nature.
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Electronegativity
Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. The Pauling scale is commonly used to quantify electronegativity values, with higher values indicating a stronger attraction for electrons. Understanding electronegativity helps predict the type of bond (ionic or covalent) that will form between different elements.
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Oxide Classification
Oxides can be classified based on their properties and the elements involved. Metal oxides, such as K2O, typically exhibit higher ionic character due to the presence of metals with low electronegativity, while non-metal oxides, like SiO2 and P4O10, often have more covalent character. Recognizing these classifications aids in arranging oxides by their ionic character.
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