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Chapter 6: Problem 35

Label the following species as molecules or ions. (a) \(\mathrm{NO}_{3}^{-}\) (b) \(\mathrm{NH}_{4}^{+}\) (c) \(\mathrm{NO}_{2}\) (d) \(\mathrm{CH}_{3} \mathrm{CO}_{2}^{-}\)

Short Answer

Expert verified
(a) Ion, (b) Ion, (c) Molecule, (d) Ion.

Step by step solution

01

Identify the Charge

Look at each given species to determine if they have a net electric charge. If the species has a positive or negative charge, it is an ion. Otherwise, it is a molecule.
02

Analyze Species (a)

The species (a) is \( \mathrm{NO}_{3}^{-} \). It has a negative charge (\(-1\)), indicating it is an ion. Specifically, it is called a nitrate ion.
03

Analyze Species (b)

The species (b) is \( \mathrm{NH}_{4}^{+} \). It has a positive charge (\(+1\)), indicating it is an ion. Specifically, it is called an ammonium ion.
04

Analyze Species (c)

The species (c) is \( \mathrm{NO}_{2} \). It has no charge indicated, meaning it is a neutral molecule. Therefore, it is classified simply as nitrogen dioxide, a molecular compound.
05

Analyze Species (d)

The species (d) is \( \mathrm{CH}_{3} \mathrm{CO}_{2}^{-} \). It has a negative charge (\(-1\)), indicating it is an ion. Specifically, it's called an acetate ion.
06

Conclude the Nature of Each Species

Summary: (a) \( \mathrm{NO}_{3}^{-} \) is an ion, (b) \( \mathrm{NH}_{4}^{+} \) is an ion, (c) \( \mathrm{NO}_{2} \) is a molecule, and (d) \( \mathrm{CH}_{3} \mathrm{CO}_{2}^{-} \) is an ion.

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Key Concepts

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

Charge Identification
When trying to identify whether a species is a molecule or an ion, the first step is to look for an electric charge. An ion is defined as a particle that has an overall positive or negative charge due to the loss or gain of electrons. In contrast, a molecule is a neutral particle made up of two or more atoms bonded together without a net charge.

To determine the charge:
  • Check if a species has a superscripted plus ( (+) ) or minus ( (-) ) symbol. This indicates it's an ion.
  • If no charge is present, the species is a molecule.
This simple observation helps classify substances into ions or molecules, which is fundamental in chemistry for understanding how substances interact in a solution.
Nitrate Ion
The nitrate ion is represented by the chemical formula NO_3^- . It's one of the most commonly encountered polyatomic ions in chemistry. The ion carries a (-1) net charge, which is due to the presence of one more electron than protons.

Here are some characteristics of nitrate ions:
  • Consists of one nitrogen atom and three oxygen atoms.
  • The additional electron gives it a negative charge, classifying it as an ion.
  • Widely found in fertilizers and can impact water quality, promoting plant growth.
Overall, recognizing the nitrate ion's pattern and structure is essential for students learning about chemical compounds.
Ammonium Ion
The ammonium ion is expressed as NH_4^+ . Known for its role in many biological processes and industries, it exhibits a positive charge ( +1 ), making it a cation.

Here are some traits and roles of the ammonium ion:
  • Formed when an ammonia molecule ( NH_3 ) gains a hydrogen ion.
  • Commonly found in fertilizers, it supplies plants with nitrogen.
  • Used in water treatment processes to reduce nitrogen oxides.
Understanding its structure and applications helps students appreciate how such ions function in both industry and natural processes.
Acetate Ion
The acetate ion has the chemical formula CH_3CO_2^- , also known as C_2H_3O_2^- . It is a common organic ion with a charge of (-1) , and it's a primary component in many biochemical and industrial processes.

Important points about the acetate ion include:
  • Derived from acetic acid ( CH_3COOH ) by deprotonation.
  • Widely used in the production of synthetic polymers and as a food preservative.
  • Plays a key role in the body's metabolism, as part of the Krebs cycle.
Grasping the concept of the acetate ion is crucial for exploring organic chemistry and its applications in daily life.

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Most popular questions from this chapter

The following ions all have the same number of electrons: \(\mathrm{Ti}^{4+}, \mathrm{Sc}^{3+}, \mathrm{Ca}^{2+}, \mathrm{S}^{2-} .\) Order them according to their expected sizes, and explain your answer. 6.88 Calculate overall energy changes in kilojoules per mole for the formation of \(\mathrm{MgF}(s)\) and \(\mathrm{MgF}_{2}(s)\) from their elements. In light of your answers, which compound is more likely to form in the reaction of magnesium with fluorine, \(\mathrm{MgF}\) or \(\mathrm{MgF}_{2}\) ? The following data are needed: \(E_{\mathrm{ea}}\) for \(\mathrm{F}(\mathrm{g})=-328 \mathrm{~kJ} / \mathrm{mol}\) \(E_{i 1}\) for \(\mathrm{Mg}(g)=+737.7 \mathrm{~kJ} / \mathrm{mol}\) \(E_{i 2}\) for \(\mathrm{Mg}(g)=+1450.7 \mathrm{~kJ} / \mathrm{mol}\) Heat of sublimation for \(\mathrm{Mg}(s)=+147.7 \mathrm{~kJ} / \mathrm{mol}\)Bond dissociation energy for \(\mathrm{F}_{2}(\mathrm{~g})=+158 \mathrm{~kJ} / \mathrm{mol}\) Lattice energy for \(\mathrm{MgF}_{2}(s)=+2952 \mathrm{~kJ} / \mathrm{mol}\) Lattice energy for \(\mathrm{MgF}(s)=930 \mathrm{~kJ} / \mathrm{mol}\) (estimated)

Why is energy usually released when an electron is added to a neutral atom but absorbed when an electron is removed from a neutral atom?

Where on the periodic table would you find the element that has an ion with each of the following electron configurations? Identify each ion. (a) \(3+\) ion: \(1 s^{2} 2 s^{2} 2 p^{6}\) (b) \(3+\) ion: \([\mathrm{Ar}] 3 d^{3}\) (c) \(2+\) ion: \([\mathrm{Kr}] 5 s^{2} 4 d^{10}\) (d) \(1+\) ion: \([\mathrm{Kr}] 4 d^{10}\)

Why does manganese, atomic number 25 , have a less favorable \(E_{\text {ea }}\) than its neighbors on either side?

Why does ionization energy increase regularly across the periodic table from group \(1 \mathrm{~A}\) to group \(8 \mathrm{~A}\), whereas electron affinity increases irregularly from group \(1 \mathrm{~A}\) to group \(7 \mathrm{~A}\) and then falls dramatically for group \(8 \mathrm{~A} ?\)
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