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Chapter 3: Problem 1

What are the two types of ions?

Short Answer

Expert verified
The two types of ions are cations and anions.

Step by step solution

01

Understanding Ions

An ion is an atom or molecule that has gained or lost one or more electrons, giving it a net positive or negative charge.
02

Define Cations

Cations are ions that have lost one or more electrons, resulting in a positive charge. This happens because the loss of electrons means there are more protons than electrons in the atom or molecule.
03

Define Anions

Anions are ions that have gained one or more electrons, leading to a negative charge. Gaining extra electrons means there are more electrons than protons in the atom or molecule.

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Key Concepts

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

Cations
In the world of chemistry, cations are a type of ion that have a positive charge. This positive charge occurs because cations have lost one or more electrons. Losing electrons increases the proton count relative to the number of electrons, which results in a net positive charge overall.
In general:
  • Cations are formed when an atom or molecule loses electrons.
  • This loss means there are more protons than electrons.
  • Cations are positively charged.
For example, when a sodium atom (\[ \text{Na} \]) loses an electron, it becomes a sodium cation:\[ \text{Na}^{+} \]
This process is typical in metals, where elements tend to form cations by losing electrons. Remember, the fundamental idea here is the balance between protons and electrons. When balance is lost due to electron loss, a positive charge remains.
Anions
Anions are ions that carry a negative charge. This happens when an atom or molecule gains one or more electrons. Adding electrons increases the electron count over the proton count, giving the ion a net negative charge.
Characteristics of anions include:
  • Anions are formed from electron gain.
  • The increased electron count means there are more electrons than protons.
  • Anions are negatively charged.
For example, a chlorine atom (\[ \text{Cl} \]) can gain an electron to form a chloride anion:\[ \text{Cl}^{-} \]
This is often seen in nonmetals. By gaining electrons, these atoms achieve a negative charge. The take-home point here is that the gain of electrons shifts the balance towards a negative charge.
Electron Gain and Loss
The process of electron gain or loss is central to the formation of ions and determines whether those ions are cations or anions. When we speak of electron gain and loss:
  • Electron loss leads to the formation of cations, which are positively charged.
  • Electron gain leads to the formation of anions, which are negatively charged.
Atoms naturally strive for stability, often achieved by having full outer electron shells. Due to this, atoms will either lose or gain electrons in a bid to reach such states. Metals usually lose electrons due to their lower electronegativity, creating cations. Conversely, nonmetals with higher electronegativity gain electrons to form anions.
This gaining or losing of electrons is thus a fundamental characteristic driving chemical reactions and interactions.

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Most popular questions from this chapter

Write the chemical formula for the ionic compound formed by each pair of ions. a. \(\mathrm{Cr}^{3+}\) and \(\mathrm{O}^{2-}\) b. \(\mathrm{Cr}^{2+}\) and \(\mathrm{O}^{2-}\) c. \(\mathrm{Pb}^{2+}\) and \(\mathrm{Cl}^{-}\) d. \(\mathrm{Pb}^{4+}\) and \(\mathrm{Cl}^{-}\)

Name the ionic compound formed by each pair of ions. a. \(\mathrm{Na}^{+}\) and \(\mathrm{N}^{3-}\) b. \(\mathrm{Mg}^{2+}\) and \(\mathrm{N}^{3-}\) c. \(\mathrm{Al}^{3+}\) and \(\mathrm{S}^{2-}\)

Write the chemical formula for the ionic compound formed by each pair of ions. a. \(\mathrm{Mg}^{2+}\) and \(\mathrm{I}^{-}\) b. \(\mathrm{Na}^{+}\) and \(\mathrm{O}^{2-}\)

Write the chemical formula for the ionic compound formed by each pair of ions. a. \(\mathrm{K}^{+}\) and \(\mathrm{Cl}^{-}\) b. \(\mathrm{Mg}^{2+}\) and \(\mathrm{Cl}^{-}\) c. \(\mathrm{Mg}^{2+}\) and \(\mathrm{Se}^{2-}\)

Write the chemical formula for the ionic compound formed by each pair of ions. a. \(\mathrm{Na}^{+}\) and \(\mathrm{Br}^{-}\) b. \(\mathrm{Mg}^{2+}\) and \(\mathrm{Br}^{-}\) c. \(\mathrm{Mg}^{2+}\) and \(\mathrm{S}^{2-}\)
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