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Chapter 7: Problem 97

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. Use the highest oxidation state of each element.

Short Answer

Expert verified
Li鈧侽 is basic, BeO is amphoteric, B鈧侽鈧�, CO鈧�, and N鈧侽鈧� are acidic oxides.

Step by step solution

01

Identify Elements and Oxidation States

The second-period elements from Li to N are Lithium (Li), Beryllium (Be), Boron (B), Carbon (C), and Nitrogen (N). We need to use the highest oxidation state for each element, which corresponds to the group number in many cases: Li (+1), Be (+2), B (+3), C (+4), and N (+5).
02

Write Formulas of the Oxides

Using the highest oxidation states, we determine the formulas of the oxides by balancing the charges between the cations and oxygen. The formulas are: 1. Lithium oxide: Li鈧侽 (Li鈦�, O虏鈦�) 2. Beryllium oxide: BeO (Be虏鈦�, O虏鈦�) 3. Boron oxide: B鈧侽鈧� (B鲁鈦�, O虏鈦�) 4. Carbon dioxide: CO鈧� (C鈦粹伜, O虏鈦�) 5. Dinitrogen pentoxide: N鈧侽鈧� (N鈦碘伜, O虏鈦�).
03

Classify Oxides as Acidic, Basic, or Amphoteric

Classify each oxide based on its nature: 1. Li鈧侽: Basic, as it reacts with water to form a base (LiOH). 2. BeO: Amphoteric, as it can react with both acids and bases. 3. B鈧侽鈧�: Acidic, as it can react with water to form an acid (H鈧傿O鈧�). 4. CO鈧�: Acidic, as it forms carbonic acid (H鈧侰O鈧�) when dissolved in water. 5. N鈧侽鈧�: Acidic, as it forms nitric acid (HNO鈧�) in water.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Elemental Oxidation States
Understanding the concept of oxidation states is crucial. They represent the charge an atom would have if all bonds were ionic. For second-period elements like Lithium (Li), Beryllium (Be), Boron (B), Carbon (C), and Nitrogen (N), the highest oxidation state often correlates with their group number on the periodic table:
  • Li is in Group 1, so it has an oxidation state of +1.
  • Be is in Group 2, thus its oxidation state is +2.
  • B is in Group 13, with an oxidation state of +3.
  • C is in Group 14, giving it an oxidation state of +4.
  • N is in Group 15, resulting in an oxidation state of +5.
This knowledge helps determine the number of electrons involved in forming bonds with oxygen, impacting the chemistry of the compounds they form.
Chemical Formulas
Chemical formulas represent the composition of a compound in terms of the symbols of the elements present and their relative proportions. For oxides of second-period elements, these formulas are determined based on their oxidation states and those of oxygen (which is -2). The goal is to balance the total positive and negative charges. Here are the formulas for the oxides:
  • Lithium oxide: Li鈧侽, where two Li鈦� ions balance one O虏鈦� ion.
  • Beryllium oxide: BeO, where one Be虏鈦� ion balances one O虏鈦� ion.
  • Boron oxide: B鈧侽鈧�, where two B鲁鈦� ions balance three O虏鈦� ions.
  • Carbon dioxide: CO鈧�, where one C鈦粹伜 ion is balanced by two O虏鈦� ions.
  • Dinitrogen pentoxide: N鈧侽鈧�, where two N鈦碘伜 ions balance five O虏鈦� ions.
These formulas provide insight into their molecular composition and potential reactions.
Acidic, Basic, and Amphoteric Oxides
The nature of oxides can be acidic, basic, or amphoteric. This classification depends on how they react with water or other chemicals, forming acids, bases, or both. Let's see how the oxides of second-period elements are classified:
  • Basic Oxide: Li鈧侽 is basic because it reacts with water to form LiOH, a strong base.
  • Amphoteric Oxide: BeO can react with both acids and bases, showcasing its amphoteric nature.
  • Acidic Oxides:
    • B鈧侽鈧� reacts with water to yield boric acid, H鈧傿O鈧�, displaying acidity.
    • CO鈧� reacts with water to form carbonic acid, H鈧侰O鈧�.
    • N鈧侽鈧� dissolves in water to give nitric acid, HNO鈧�.
Understanding these properties helps predict the behavior of these oxides in various chemical reactions.
Second-Period Elements
The second-period elements span from Lithium (Li) to Neon (Ne) on the periodic table. These elements' properties change significantly across the period due to increasing atomic numbers. For oxides, we're primarily interested in elements Li to N:
  • These elements show a diversity of chemical reactions and bonding patterns.
  • Their oxides provide a wide range of acid-base characteristics.
  • The increasing electronegativity across the period influences their oxidative behavior.
Studying these elements helps us understand broader periodic trends and the complex nature of their chemical compounds.
Oxides Classification
Classifying oxides is essential in understanding their chemical behavior and potential applications. Oxides can be categorized broadly into three types based on their acid-base characteristics:
  • Acidic Oxides: These react with water, forming acids. They are typically non-metal oxides, like CO鈧� and N鈧侽鈧�.
  • Basic Oxides: These form bases upon reacting with water. Metal oxides such as Li鈧侽 fall into this category.
  • Amphoteric Oxides: These react with both acids and bases. BeO exemplifies this dual behavior.
This classification is pivotal because it aids chemists in predicting how a particular oxide will react under different chemical conditions. Understanding oxide classification informs everything from environmental science to industrial chemistry.

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Most popular questions from this chapter

The electron configuration of \(\mathrm{C}\) is \(1 s^{2} 2 s^{2} 2 p^{2}\). (a) If each core electron (i.e., the \(1 s\) electrons) were totally effective in shielding the valence electrons (i.e., the \(2 s\) and \(2 p\) electrons) from the nucleus and the valence electrons did not shield one another, what would be the shielding constant \((\sigma)\) and the effective nuclear charge \(\left(Z_{\text {eff }}\right)\) for the \(2 s\) and \(2 p\) electrons? (b) In reality, the shielding constants for the \(2 s\) and \(2 p\) electrons in \(\mathrm{C}\) are slightly different. They are 2.78 and \(2.86,\) respectively. Calculate \(Z_{\text {eff }}\) for these electrons, and explain the differences from the values you determined in part (a).

Arrange the following isoelectronic species in order of increasing ionization energy: \(\mathrm{O}^{2-}, \mathrm{F}^{-}, \mathrm{Na}^{+}, \mathrm{Mg}^{2+}\).

The electron configuration of \(\mathrm{B}\) is \(1 s^{2} 2 s^{2} 2 p^{1}\). (a) If each core electron (i.e., the \(1 s\) electrons) were totally effective in shielding the valence electrons (i.e., the \(2 s\) and \(2 p\) electrons) from the nucleus and the valence electrons did not shield one another, what would be the shielding constant \((\sigma)\) and the effective nuclear charge \(\left(Z_{\text {eff }}\right)\) for the \(2 s\) and \(2 p\) electrons? (b) In reality, the shielding constants for the \(2 s\) and \(2 p\) electrons in \(\mathrm{B}\) are slightly different. They are 2.42 and 2.58 , respectively. Calculate \(Z_{\text {eff }}\) for these electrons, and explain the differences from the values you determined in part (a).

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

Which is the largest atom in the third period of the periodic table?
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