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Chapter 4: Problem 69

Positive ions are called __________, whereas negative ions are called _________.

Short Answer

Expert verified
Positive ions are called cations, whereas negative ions are called anions.

Step by step solution

01

Recognize Positive Ions

Positive ions are atoms or molecules that have lost one or more electrons, resulting in a net positive charge. These ions are also known as cations. #Step 2: Understanding Negative Ions#
02

Recognize Negative Ions

Negative ions are atoms or molecules that have gained one or more electrons, resulting in a net negative charge. These ions are also known as anions. #Step 3: Filling in the Blanks#
03

Complete the sentence

Now that we know the terms for positive and negative ions, we can fill in the blanks: Positive ions are called cations, whereas negative ions are called anions.

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Key Concepts

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

Cations
Cations are ions with a net positive charge. This happens when an atom or molecule loses one or more of its electrons. Electrons are negatively charged, so losing them results in a net positive charge.
Here鈥檚 why cations form:
  • Atoms seek stability. By shedding electrons, they often reach a more stable, lower energy state.
  • Many metals lose electrons to become positive ions. For example, when a sodium atom (Na) loses an electron, it becomes a sodium cation (\( \text{Na}^+ \)).
Cations have crucial roles in chemistry and biology. For instance, the sodium cation helps transmit nerve signals in our bodies.
To identify a cation, look for a plus sign (\( ^+ \)) after the chemical symbol, indicating a positive charge.
Anions
Anions are ions with a net negative charge because they have gained extra electrons. Electrons have a negative charge, so gaining them makes the overall charge of the particle negative.
The formation of anions typically occurs in the following scenarios:
  • Non-metal elements tend to gain electrons to become more stable, much like reaching a complete outer electron shell.
  • Chlorine, for example, gains an electron to form a chloride anion (\( \text{Cl}^- \)). This anion is significant in forming common table salt when combined with sodium cations.
Anions are vital in creating compounds, especially salts and other ionic compounds. These compounds are formed by the attraction between oppositely charged cations and anions.
To spot an anion, look for a negative sign (\( ^- \)) after the chemical symbol, which points to a gained electron resulting in a negative charge.
Charge of Ions
The charge of ions plays a vital role in understanding chemical reactions and compounds' formation. When atoms gain or lose electrons, they no longer remain neutral and acquire charges as ions.
Here's how the charge of an ion is determined:
  • Cations form by losing electrons and carry a positive charge. The charge's magnitude corresponds to the number of electrons lost. For instance, if an atom loses two electrons, it will have a \( 2^+ \) charge.
  • Anions form by gaining electrons and bear a negative charge. Similarly, the number of gained electrons determines the charge's magnitude. If an atom gains three electrons, its charge will be \( 3^- \).
Understanding ionic charge is fundamental for predicting the behavior of ionic compounds in reactions, such as reactivity and solubility.
When you examine ions in chemical equations, note the charge. It guides you in balancing equations and deducing the chemical reactions' outcomes.

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Most popular questions from this chapter

How many electrons are contained in each of the following ions? a. \(\mathrm{Fe}^{2+}\) b. \(C a^{2+}\) c. \(C O^{2+}\) d. \(C O^{3+}\) e. \(S^{2-}\) f. \(C I^{-}\) g. \(\mathrm{Cr}^{3+}\) h. \(\mathrm{K}^{+}\)

For each of the following elements, give the chemical symbol and atomic number. a. astatine b. xenon c. radium d. strontium e. lead f. selenium g. argon h. cesium

Why are the elements of Group 8 referred to as the noble or inert gas elements?

Write the atomic symbol \((^{A}_{z} X)\) for each of the isotopes described below. a. \(Z=6,\) number of neutrons \(=7\). b. the isotope of carbon with a mass number of 13. c. \(Z=6, A=13\) d. \(Z=19, A=44\) e. the isotope of calcium with a mass number of 41 f. the isotope with 19 protons and 16 neutrons

Write the number and name (if any) of the group (family) to which each of the following elements belongs. a. cesium b. Ra c. Rn d. chlorine e. strontium f. \(\mathrm{Xe}\) g. \(\mathrm{Rb}\)
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