Question

What are the formulas (including charges) for (a) cyanide ion, (b) ammonium ion, (c) nitrate ion, (d) sulfite ion, (e) chlorate ion, and (f) sulfate ion?

Short answer

The formulas for the ions are: (a) Cyanide ion: CN-, (b) Ammonium ion: NH4+, (c) Nitrate ion: NO3-, (d) Sulfite ion: SO3^2-, (e) Chlorate ion: ClO3-, (f) Sulfate ion: SO4^2-.

Step-by-step solution

Identify the Cyanide Ion

The cyanide ion is composed of one carbon atom triple-bonded to a nitrogen atom. It carries a negative charge. The formula for the cyanide ion is CN-.

Identify the Ammonium Ion

The ammonium ion is formed by a nitrogen atom covalently bonded to four hydrogen atoms. It carries a positive charge. The formula for the ammonium ion is NH4+.

Identify the Nitrate Ion

The nitrate ion is made of one nitrogen atom bonded to three oxygen atoms in a trigonal planar arrangement with one of the bonds being a coordinate covalent bond. It carries a negative charge. The formula for the nitrate ion is NO3-.

Identify the Sulfite Ion

The sulfite ion consists of one sulfur atom surrounded by three oxygen atoms in a trigonal pyramidal shape. It has a charge of 2-. The formula for the sulfite ion is SO3^2-.

Identify the Chlorate Ion

The chlorate ion has one chlorine atom covalently bonded to three oxygen atoms. It carries a negative charge. The formula for the chlorate ion is ClO3-.

Identify the Sulfate Ion

The sulfate ion is composed of one sulfur atom bonded to four oxygen atoms in a tetrahedral arrangement. It carries a 2- charge. The formula for the sulfate ion is SO4^2-.

Key concepts

Cyanide Ion Formula

The cyanide ion, a formidable compound often mentioned in the context of poisons, features a simple yet distinct chemical structure. Its formula is represented as CN-. Comprising a single carbon atom (C) and a nitrogen atom (N), these two are linked by a robust triple bond, signaling a strong union. The ion carries a charge of -1, indicating an extra electron that imparts the overall negative charge. This ion plays a critical role in organic chemistry and biochemical processes, although it must be handled with care due to its toxicity.

Ammonium Ion Formula

The ammonium ion is a fundamental component in the realm of chemistry, particularly inorganic chemistry and environmental systems. It presents itself with the formula NH4+. This polyatomic ion is formed when a nitrogen atom (N) coalesces with four hydrogen atoms (H), creating a positively charged entity. The positive charge arises from an additional proton, making the ammonium ion a friendly carrier of positive charge in numerous chemical reactions, fertilizers, and even in biological contexts. Its ubiquity in the nitrogen cycle makes it a cornerstone of ecological studies.

Nitrate Ion Structure

The structure of the nitrate ion, NO3-, is a compelling showcase of molecular geometry. The nitrogen (N) at the center, bonded to three oxygen atoms (O), forms a trigonal planar structure. This arrangement provides the ion with resonance stabilization as the electrons are delocalized among the oxygen atoms, conferring the charge of -1 to the ion. The nitrate ion is a key player in numerous substances, ranging from agricultural fertilizers to explosives, owing to its ability to donate and accept electrons with ease. The comprehensive understanding of its structure is vital for students studying reactions involving nitrates.

Sulfite Ion Charge

When delving into the sulfite ion, one encounters the chemical symbol SO3^2-, hinting at its charge of -2. This ion is composed of a central sulfur atom (S) encircled by three oxygen atoms (O) in a slightly pyramidal shape due to the lone pair of electrons on the sulfur. The charge is particularly important in redox reactions and when predicting the outcomes of chemical combinations involving this ion. In industrial settings, sulfites find their utilization as preservatives and in the papermaking process, among many applications.

Chlorate Ion Composition

The chlorate ion, with its composition denoted as ClO3-, is a fascinating combination of one chlorine atom (Cl) and three oxygen atoms (O). It carries a charge of -1, and in its free state, it contributes significantly to reactions as an oxidizing agent. The chlorate ion is essential not only in laboratories but also in the manufacture of safety matches and explosives. Its reactive nature makes it a topic of interest in chemical kinetics and thermodynamics.

Sulfate Ion Configuration

Understanding the sulfate ion encompasses recognizing its tetrahedral configuration, symbolized by SO4^2-. The ion's foundation lies in a sulfur atom (S) at its core, orbited by four oxygen atoms (O) symmetrically positioned. This sulfate ion claims a -2 charge due to the presence of two excess electrons. It is widely distributed in nature, playing pivotal roles in numerous biological and geological phenomena. From the formation of gypsum deposits to its prevalence in sea spray, the sulfate ion's configuration is a critical concept in multiple branches of science, including environmental chemistry and geology.