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Chapter 2: Problem 43

What is an ionic compound? How is electrical neutrality maintained in an ionic compound?

Short Answer

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An ionic compound is formed by the electrostatic attraction between positively and negatively-charged ions, which are formed when metals transfer electrons to non-metals. Electrical neutrality in an ionic compound is maintained by the balance of the positive and negative charges of the ions. For instance, in the ionic compound Sodium Chloride (\(NaCl\)), each Sodium ion (\(Na^{+}\)) is balanced by a Chloride ion (\(Cl^{-}\)), resulting in a neutral compound.

Step by step solution

01

Defining Ionic Compounds

Ionic compounds occur when metals donate one or more electrons to non-metals. During this interaction, atoms gain or lose electrons and become ions. The metal becomes a positively charged cation, and the non-metal becomes a negatively charged anion. The strong electrostatic force between these opposite charges forms the ionic bond, resulting in an ionic compound, such as Sodium Chloride (\(NaCl\)).
02

Explaining Electrical Neutrality in Ionic Compounds

Electrical neutrality in ionic compounds is maintained by the balance of the positive and negative charges of the ions. In Sodium Chloride (\(NaCl\)), for example, each sodium atom (\(Na\)) loses one electron and becomes a positively-charged sodium ion (\(Na^{+}\)). Each chlorine atom (\(Cl\)) gains this electron, becoming a negatively-charged chloride ion (\(Cl^{-}\)). The resulting ionic compound, \(NaCl\), is electrically neutral because the number of positive charges is equal to the number of negative charges.
03

Summary

In summary, ionic compounds are made up of positively and negatively-charged ions held together by strong electrostatic forces. Electrical neutrality is maintained in these compounds because the total positive charge from the metal ions equals the total negative charge from the non-metal ions. The result is a neutral compound.

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Key Concepts

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

Electrical Neutrality
Ionic compounds consist of ions that carry charges. These charges need to balance each other out, so the compound remains electrically neutral. This happens because the positive charge of all cations generally equals the total negative charge of all anions in the compound.
For instance, in a sodium chloride ( NaCl ext{) )} compound:
  • Sodium ( Na ext{) )} loses one electron to become Na^{+} ext{. )} This is a positive ion or cation.
  • Chlorine ( Cl ext{) )} gains one electron to become Cl^{-} ext{. )} This is a negative ion or anion.
Together, Na^{+} ext{)} and Cl^{-} ext{)} form a compound that has no overall charge. Hence, the ionic compound maintains electrical neutrality by the equal number of positive and negative charges.
Cation and Anion
Cations and anions are crucial parts of ionic compounds. Cations are positively charged ions formed by metals that have lost electrons. Anions are negatively charged ions formed by non-metals that have gained electrons.
This change happens during an exchange process:
  • The metal atom becomes a cation when it loses one or more electrons. This positive ion seeks a negative ion to bond with.
  • The non-metal atom turns into an anion when it gains one or more electrons. This negative ion is naturally attracted to positive ions.
Strong chemical bonds result from these interactions. They lead to the formation of stable ionic compounds, which combine cations and anions usually in such proportions that the total charge becomes zero.
Electrostatic Force
Electrostatic force plays a significant role in holding ionic compounds together. It is the attractive force between opposite charges 鈥� cations and anions. This force is very strong, leading to the formation of ionic bonds.
How does it work?
  • When a cation and an anion come close, the electrostatic attraction pulls them together.
  • This force stabilizes the newly formed ionic compound and gives it its structure, often crystallized.
Thanks to electrostatic forces, ionic compounds have high melting and boiling points because a lot of energy is needed to overcome these forces and separate the ions.
Electron Transfer
Electron transfer is central to the formation of ionic compounds. It involves the movement of electrons from one atom to another.
Here鈥檚 a step-wise process:
  • Metal atoms want to lose electrons and achieve a stable electron configuration. They become cations when they lose electrons.
  • Non-metal atoms want to gain electrons to fill their outer electron shell. They become anions upon gaining electrons.
Through electron transfer, metallic elements donate electrons while non-metallic elements accept them, leading to the creation of distinct positive and negative ions. These ions combine to form ionic compounds, driven by internal forces seeking equilibrium.

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Most popular questions from this chapter

Give the number of protons and electrons in each of the following common ions: \(\mathrm{K}^{+}, \mathrm{Mg}^{2+}, \mathrm{Fe}^{3+}, \mathrm{Br}^{-}\) \(\mathrm{Mn}^{2+}, \mathrm{C}^{4-}, \mathrm{Cu}^{2+}\)

What are allotropes? Give an example. How are allotropes different from isotopes?

In Section 2.1 it was pointed out that mass and energy are alternate aspects of a single entity called mass-energy. The relationship between these two physical quantities is Einstein's famous equation, \(E=m c^{2},\) where \(E\) is energy, \(m\) is mass, and \(c\) is the speed of light. In a combustion experiment, it was found that \(12.096 \mathrm{~g}\) of hydrogen molecules combined with \(96.000 \mathrm{~g}\) of oxygen molecules to form water and released \(1.715 \times 10^{3} \mathrm{~kJ}\) of heat. Calculate the corresponding mass change in this process and comment on whether the law of conservation of mass holds for ordinary chemical processes. (Hint: The Einstein equation can be used to calculate the change in mass as a result of the change in energy. \(1 \mathrm{~J}=1 \mathrm{~kg} \mathrm{~m}^{2} / \mathrm{s}^{2}\) and \(\left.c=3.00 \times 10^{8} \mathrm{~m} / \mathrm{s} .\right)\)

State two differences between a metal and a nonmetal.

Of the 118 elements known, only two are liquids at room temperature \(\left(25^{\circ} \mathrm{C}\right) .\) What are they? (Hint: One element is a familiar metal and the other element is in Group 7A.)
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