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Chapter 8: Problem 90

Write the formulas and names of the oxides of the second-period elements (Li to \(\mathrm{N}\) ). Identify the oxides as acidic, basic, or amphoteric.

Short Answer

Expert verified
The oxides of second-period elements from Lithium (Li) to Nitrogen (N) are: Lithium Oxide (\(Li_2O\)), Beryllium Oxide (\(BeO\)), Boron Oxide (\(B_2O_3\)), Carbon Dioxide (\(CO_2\)), and Nitrogen Dioxide (\(NO_2\)). Lithium Oxide and Beryllium Oxide are basic oxides, Boron Oxide is amphoteric, and Carbon Dioxide and Nitrogen Dioxide are acidic oxides.

Step by step solution

01

List the Second Period Elements

Second period elements from the periodic table include: Lithium (Li), Beryllium (Be), Boron (B), Carbon (C), Nitrogen (N), Oxygen (O), Fluorine (F) and Neon (Ne). For this task, we are concerned with Lithium (Li) to Nitrogen (N).
02

Write their Oxides

Each element forms an oxide when reacted with oxygen. The oxides are as follows: Lithium Oxide (\(Li_2O\)), Beryllium Oxide (\(BeO\)), Boron Oxide (also known as Boron Trioxide - \(B_2O_3\)), Carbon Oxide (also known as Carbon Dioxide - \(CO_2\)), and Nitrogen Oxide (also known as Nitrogen Dioxide - \(NO_2\)).
03

Identify their Types

The oxides are classified as acidic, basic, or amphoteric based on their acid-base properties. Lithium Oxide (\(Li_2O\)) and Beryllium Oxide (\(BeO\)) are basic oxides since they react with acids to form salts and water. Boron Oxide (\(B_2O_3\)) is amphoteric because it shows both acidic and basic characteristics. Carbon Dioxide (\(CO_2\)) and Nitrogen Dioxide (\(NO_2\)) are acidic oxides, they can react with bases to produce salts and water.

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Most popular questions from this chapter

What is the most important relationship among elements in the same group in the periodic table?

Indicate whether these elements exist as atomic species, molecular species, or extensive three dimensional structures in their most stable state at \(25^{\circ} \mathrm{C}\) and \(1 \mathrm{~atm},\) and write the molecular or empirical formula for the elements: phosphorus, iodine, magnesium, neon, arsenic, sulfur, carbon, selenium, and oxygen.

Explain why, for isoelectronic ions, the anions are larger than the cations.

Write formulas and give names for the binary hydrogen compounds of the second- period elements (Li to F). Describe the changes in physical and chemical properties of these compounds as we move across the period from left to right.

Define ionic radius. How does the size change when an atom is converted to (a) an anion and (b) a cation?
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