Question

Compare the oxyanions sulfate and sulfite.

Short answer

The main differences between the oxyanions sulfate (\(SO_4^{2-}\)) and sulfite (\(SO_3^{2-}\)) are the number of oxygen atoms and their molecular structures. Sulfate has four oxygen atoms in a tetrahedral structure, while sulfite has three oxygen atoms in a trigonal pyramidal structure. Both oxyanions have a central sulfur atom and a -2 charge.

Step-by-step solution

1. Chemical Formulas

To compare sulfate and sulfite, we must first identify their respective chemical formulas. Sulfate has the chemical formula \(SO_4^{2-}\), and sulfite has the chemical formula \(SO_3^{2-}\).

2. Number of Oxygen Atoms

The next step is to compare the number of oxygen atoms in each oxyanion. In sulfate, there are four oxygen atoms, while in sulfite, there are only three oxygen atoms.

3. Structures

Now, we will look at the structures of these oxyanions. Both sulfate and sulfite have a central sulfur atom, which is surrounded by oxygen atoms. In the case of sulfate, the central sulfur atom has double bonds with each of the four oxygen atoms, resulting in a tetrahedral structure. On the other hand, the sulfite ion has a trigonal pyramidal structure in which the central sulfur atom is bonded to three oxygen atoms, with one of the oxygen atoms forming a double bond, while the other two oxygen atoms have single bonds.

4. Charge

Finally, we will compare the charges of these oxyanions. Both sulfate and sulfite ions have a negative 2 charge, indicated as \(SO_4^{2-}\) and \(SO_3^{2-}\), respectively. In summary, the main differences between sulfate and sulfite ions are the number of oxygen atoms and their molecular structures. Both oxyanions have a central sulfur atom and a -2 charge, but the sulfate ion has four oxygen atoms in a tetrahedral structure, while the sulfite ion has three oxygen atoms in a trigonal pyramidal structure.

Key concepts

Chemical Formulas

Understanding chemical formulas is crucial in identifying and comparing different compounds, including oxyanions. The chemical formula provides us a shorthand representation of the elements present in a compound and their respective quantities. For example, in the exercise comparing sulfate (\(SO_4^{2-}\)) and sulfite (\(SO_3^{2-}\)), we can easily deduce that both contain sulfur (S) and oxygen (O), but differ in their oxygen content. These formulas form the foundation of our comparison, and without them, we wouldn’t be able to discuss the more complex concepts of structure and charge.

Number of Oxygen Atoms

The number of oxygen atoms in an oxyanion directly impacts its properties and name. Sulfate and sulfite are differentiated by the suffixes '-ate' and '-ite' respectively, indicating a difference in oxygen content. As noted in the solution, sulfate contains one more oxygen atom (four in total) compared to sulfite (three oxygen atoms). This distinction is not trivial, as it often results in observable differences in reactivity, acidity, and other chemical behaviors. Understanding how to count and interpret oxygen atoms in oxyanions is a fundamental skill in the study of inorganic chemistry.

Molecular Structures

While formulas tell us what is in a compound, molecular structures reveal 'how' those atoms are arranged. Considering oxyanions, their structures define shape, bond angles, and the type of bonding between atoms—critical factors in predicting physical and chemical properties. Sulfate ('tetrahedral') and sulfite ('trigonal pyramidal') differ in shape due to the difference in their number of oxygen atoms. Visualizing these three-dimensional shapes can be quite challenging but is extremely helpful for students to understand concepts such as bond lengths, angles, and the spatial arrangement of atoms in a molecule.

Polyatomic Ions Charges

The charge of a polyatomic ion is a key attribute that affects how it interacts with other ions to form ionic compounds. Sulfate and sulfite both carry a -2 charge, which reflects the balance between the positively charged protons in the sulfur nucleus and the negatively charged electrons shared with oxygen atoms. The similarity in charge plays a crucial role in how these oxyanions can replace one another in reactions or form salts with metal cations. Grasping the importance of these charges helps students predict the formulas of resultant compounds when these ions participate in chemical reactions.