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Chapter 7: Problem 62

Arrange the following oxides in order of increasing acidity: $$ \mathrm{CO}_{2}, \mathrm{CaO}, \mathrm{Al}_{2} \mathrm{O}_{3}, \mathrm{SO}_{3}, \mathrm{SiO}_{2}, \mathrm{P}_{2} \mathrm{O}_{5} \text {. } $$

Short Answer

Expert verified
The oxides in order of increasing acidity are: \(\mathrm{CaO} \lt \mathrm{Al}_{2} \mathrm{O}_{3} \lt \mathrm{SiO}_{2} \lt \mathrm{P}_{2} \mathrm{O}_{5} \lt \mathrm{SO}_{3} \lt \mathrm{CO}_{2}\).

Step by step solution

01

Identify the oxides of metals and non-metals

Identify whether each oxide is a metal or non-metal oxide. Carbon dioxide (CO2) and silicon dioxide (SiO2) are both non-metal oxides. Calcium oxide (CaO) and aluminium oxide (Al2O3) are metal oxides. Sulfur trioxide (SO3) and phosphorus pentoxide (P2O5) are non-metal oxides.
02

List the oxides based on electronegativity

Now we will list the oxides based on the electronegativity of the elements involved: 1. Calcium Oxide (CaO) - Metal Oxide (Electronegativity of Ca = 1.00) 2. Aluminum Oxide (Al2O3) - Metal Oxide (Electronegativity of Al = 1.61) 3. Silicon Dioxide (SiO2) - Non-metal Oxide (Electronegativity of Si = 1.90) 4. Phosphorus Pentoxide (P2O5) - Non-metal Oxide (Electronegativity of P = 2.19) 5. Sulfur Trioxide (SO3) - Non-metal Oxide (Electronegativity of S = 2.58) 6. Carbon Dioxide (CO2) - Non-metal Oxide (Electronegativity of C = 2.55)
03

Arrange the oxides based on acidity

We will now arrange the given oxides in order of increasing acidity by considering the basic nature of metal oxides and the acidic nature of non-metal oxides along with their electronegativities: 1. Calcium Oxide (CaO) - Basic Metal Oxide 2. Aluminum Oxide (Al2O3) - Basic Metal Oxide 3. Silicon Dioxide (SiO2) - Acidic Non-metal Oxide 4. Phosphorus Pentoxide (P2O5) - Acidic Non-metal Oxide 5. Sulfur Trioxide (SO3) - Acidic Non-metal Oxide 6. Carbon Dioxide (CO2) - Acidic Non-metal Oxide The final order of the oxides based on increasing acidity is: $$\mathrm{CaO} \lt \mathrm{Al}_{2} \mathrm{O}_{3} \lt \mathrm{SiO}_{2} \lt \mathrm{P}_{2} \mathrm{O}_{5} \lt \mathrm{SO}_{3} \lt \mathrm{CO}_{2}$$

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Key Concepts

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

Metal Oxides
Metal oxides are compounds formed between metals and oxygen. These are often ionic in nature, meaning they consist of positive and negative ions. Metal oxides typically display basic characteristics. This is because, when these oxides dissolve in water, they form hydroxide ions (OH鈦�). Think about calcium oxide (CaO) and aluminum oxide (Al鈧侽鈧�), for example. When added to water, calcium oxide forms calcium hydroxide, a strong base. Aluminum oxide, on the other hand, is amphoteric, which means it can react both as an acid and as a base.
  • Most metal oxides are basic.
  • They often contain metal cations combined with oxide anions.
  • Can neutralize acids, resulting in salt and water as products.
  • Some metal oxides, like aluminum oxide, can exhibit amphoteric behavior.
Understanding metal oxides' properties helps us predict how they will interact with other substances, particularly acids.
Non-metal Oxides
Non-metal oxides consist of non-metals bonded with oxygen. Unlike metal oxides, they are typically covalent compounds. This means the oxygen atoms share electrons rather than transferring them as in ionic bonds. Non-metal oxides like carbon dioxide (CO鈧�) and sulfur trioxide (SO鈧�) usually display acidic behavior.
Non-metal oxides react with water to form acids. For instance, sulfur trioxide reacts with water to produce sulfuric acid. This makes these oxides important in understanding acid rain.
  • Tend to be acidic in nature.
  • Often form acids when combined with water.
  • Play a role in environmental processes like acid rain formation.
As we explore non-metal oxides, recognizing their inherent acidity can help us understand their impact on both industrial processes and the environment.
Electronegativity
Electronegativity is a measure of how strongly an element attracts electrons in a chemical bond. When thinking about oxides, it helps us predict their acidity or basicity. Generally, higher electronegativity corresponds to a more acidic nature, especially in non-metal oxides.
For example, sulfur in sulfur trioxide (SO鈧�) has a high electronegativity. This makes it strongly acidic. In contrast, calcium in calcium oxide (CaO) has low electronegativity, contributing to its basic nature. Electronegativity trends can often explain why non-metal oxides are more acidic than metal oxides.
  • High electronegativity in non-metals often equals acidic oxides.
  • Lower electronegativity in metals results in more basic oxides.
  • Helps predict reactions and behaviors of chemical compounds.
Understanding electronegativity can simplify anticipations about chemical reactions and compound properties.
Acid-Base Character
The acid-base character of oxides determines whether a compound acts as an acid or a base. This is influenced by the element's position in the periodic table and its electronegativity.
Metal oxides, with their low electronegativity, are generally basic and can neutralize acids. Non-metal oxides, in contrast, are acidic, due to their higher electronegativity and tendency to form acidic solutions when reacting with water.
Aluminum oxide (Al鈧侽鈧�) is intriguing because it's amphoteric. This means it can act as both an acid and a base depending on the conditions, showcasing the diversity of acid-base behavior.
  • Metal oxides: Typically basic, form bases with water.
  • Non-metal oxides: Generally acidic, form acids with water.
  • Some oxides, like aluminum oxide, are amphoteric.
Grasping the acid-base character of oxides helps in predicting their reactions and practical applications in various fields.

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Most popular questions from this chapter

(a) If the core electrons were totally effective at screening the valence electrons and the valence electrons provided no screening for each other, what would be the effective nuclear charge acting on the \(3 s\) and \(3 p\) valence electrons in \(\mathrm{P}\) ? (b) Repeat these calculations using Slater's rules. (c) Detailed calculations indicate that the effective nuclear charge is \(5.6+\) for the \(3 s\) electrons and \(4.9+\) for the \(3 p\) electrons. Why are the values for the \(3 s\) and \(3 p\) electrons different? (d) If you remove a single electron from a P atom, which orbital will it come from?

(a) What is the trend in first ionization energies as one proceeds down the group 7A elements? Explain how this trend relates to the variation in atomic radii. (b) What is the trend in first ionization energies as one moves across the fourth period from \(\mathrm{K}\) to \(\mathrm{Kr}\) ? How does this trend compare with the trend in atomic radii?

Write equations that show the process for (a) the first two ionization energies of lead and (b) the fourth ionization energy of zirconium.

We will see in Chapter 12 that semiconductors are materials that conduct electricity better than nonmetals but not as well as metals. The only two elements in the periodic table that are technologically useful semiconductors are silicon and germanium. Integrated circuits in computer chips today are based on silicon. Compound semiconductors are also used in the electronics industry. Examples are gallium arsenide, GaAs; gallium phosphide, GaP; cadmium sulfide, CdS; and cadmium selenide, CdSe. (a) What is the relationship between the compound semiconductors' compositions and the positions of their elements on the periodic table relative to \(\mathrm{Si}\) and \(\mathrm{Ge}\) ? (b) Workers in the semiconductor industry refer to "II-VI" and "III-V" materials, using Roman numerals. Can you identify which compound semiconductors are II-VI and which are III-V? (c) Suggest other compositions of compound semiconductors based on the positions of their elements in the periodic table.

Zinc in its 2+ oxidation state is an essential metal ion for life. \(\mathrm{Zn}^{2+}\) is found bound to many proteins that are involved in biological processes, but unfortunately \(\mathrm{Zn}^{2+}\) is hard to detect by common chemical methods. Therefore, scientists who are interested in studying \(\mathrm{Zn}^{2+}\)-containing proteins frequently substitute \(\mathrm{Cd}^{2+}\) for \(\mathrm{Zn}^{2+}\), since \(\mathrm{Cd}^{2+}\) is easier to detect. (a) On the basis of the properties of the elements and ions discussed in this chapter and their positions in the periodic table, describe the pros and cons of using \(\mathrm{Cd}^{2+}\) as a \(\mathrm{Zn}^{2+}\) substitute. (b) Proteins that speed up (catalyze) chemical reactions are called enzymes. Many enzymes are required for proper metabolic reactions in the body. One problem with using \(\mathrm{Cd}^{2+}\) to replace \(\mathrm{Zn}^{2+}\) in enzymes is that \(\mathrm{Cd}^{2+}\) substitution can decrease or even eliminate enzymatic activity. Can you suggest a different metal ion that might replace \(\mathrm{Zn}^{2+}\) in enzymes instead of \(\mathrm{Cd}^{2+}\) ? Justify your answer.
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