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Chapter 11: Problem 3

What types of elements react to form ionic compounds? Give an example of the formation of an ionic compound from its elements.

Short Answer

Expert verified
Ionic compounds are formed between metal and non-metal elements, where metal atoms lose electrons forming cations, and non-metal atoms gain electrons forming anions. These oppositely charged ions are attracted to each other through electrostatic forces, forming an ionic bond. An example is the formation of sodium chloride (NaCl) from sodium (Na) and chlorine (Cl). Sodium loses an electron to become Na+ ion, while chlorine gains an electron to become Cl- ion. The electrostatic attraction between these two ions forms the ionic compound NaCl. \[ Na \rightarrow Na^+ + e^-\] \[ Cl + e^- \rightarrow Cl^-\] \[ Na^+ + Cl^- \rightarrow NaCl \]

Step by step solution

01

1. Identify the types of elements that form ionic compounds

Ionic compounds are formed between metal and non-metal elements. In these compounds, metal atoms lose one or more electrons (forming cations) while non-metal atoms gain one or more electrons (forming anions). The resulting positively charged metal cations and negatively charged non-metal anions are then attracted to each other through electrostatic forces, forming an ionic bond.
02

2. Example of an ionic compound formation

A classic example of the formation of an ionic compound is the reaction between sodium (Na), a metal, and chlorine (Cl), a non-metal, to form sodium chloride (NaCl) or common table salt.
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3. Detailed steps of the formation of sodium chloride (NaCl)

Step 1: Sodium (Na) loses its outermost electron Sodium (Na) has one electron in its outermost shell, and it needs to lose this electron to reach a stable electron configuration. As a result, Na loses one electron and transforms into a sodium ion (Na+) having a charge of +1. \[ Na \rightarrow Na^+ + e^- \] Step 2: Chlorine (Cl) gains an electron Chlorine (Cl) has seven electrons in its outermost shell, and it needs to gain one electron to fill its outermost shell and achieve a stable electron configuration. Chlorine gains the electron lost by sodium and transforms into a chloride ion (Cl-) having a charge of -1. \[ Cl + e^- \rightarrow Cl^- \] Step 3: Formation of the ionic compound sodium chloride (NaCl) After sodium loses an electron and turns into Na+ and chlorine gains an electron to form Cl-, an electrostatic force of attraction exists between the two oppositely charged ions. \[ Na^+ + Cl^- \rightarrow NaCl \] This electrostatic attraction forms an ionic bond and creates the ionic compound sodium chloride (NaCl).

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Key Concepts

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

Understanding Electrostatic Forces in Ionic Compounds
Electrostatic forces play a crucial role in the formation of ionic compounds. These forces arise from the attraction between oppositely charged particles. Imagine a magnet, where the positive side pulls towards the negative side. Similarly, in chemistry, when a positively charged ion (cation) and a negatively charged ion (anion) come close, they attract each other with a strong force.
This force is the reason behind the formation of ionic bonds, which are the glue that holds ionic compounds together. Without electrostatic forces, cations and anions would simply drift apart, and no ionic compound could form.
  • Electrostatic forces are what keep the ions tightly bonded within a compound.
  • This attraction is necessary to maintain the structure of ionic compounds.
It is this attraction that gives ionic compounds like sodium chloride their unique properties, such as high melting and boiling points. By understanding electrostatic forces, we can better grasp how substances form on a microscopic level.
The Role of Cations and Anions
Cations and anions are fundamental components of ionic compounds. Cations are positively charged ions, formed when atoms lose electrons. In contrast, anions are negatively charged ions created when atoms gain electrons. Let's break it down with some key points.
  • Metals typically become cations by losing one or more electrons.
  • Non-metals usually form anions by gaining electrons.
This transfer of electrons leads to the formation of ions with opposite charges. The nature of these ions is essential for explaining the properties of ionic compounds. The strength of the attraction between cations and anions is what facilitates the stability and structure of ionic compounds.
Understanding the behavior of cations and anions helps students visualize how molecular structures are formed and why ionic compounds exhibit the traits they do.
How Sodium Chloride is Formed
The formation of sodium chloride (NaCl) is a classic example of how ionic compounds are created. Sodium (Na) is a metal, while chlorine (Cl) is a non-metal. Here's how they react to form this well-known compound.
  • First, sodium loses an electron from its outer shell, turning into a sodium ion (Na+) with a positive charge:
\[ Na \rightarrow Na^+ + e^- \]
  • Next, chlorine accepts this electron, transforming into a chloride ion (Cl-) with a negative charge:
\[ Cl + e^- \rightarrow Cl^- \] After these ions are formed, the crucial step occurs: sodium's positive ion and chlorine's negative ion attract each other. This electrostatic force securely binds them into a stable ionic compound, sodium chloride:
  • The final reaction gives us NaCl:
\[ Na^+ + Cl^- \rightarrow NaCl \] Sodium chloride's formation illustrates the powerful interactions at play in making an ionic bond, turning two separate elements into a cohesive and incredibly stable compound.

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Most popular questions from this chapter

For each of the following pairs, indicate which is smaller. a. Fe or \(\mathrm{Fe}^{3+}\) b. \(\mathrm{Cl}\) or \(\mathrm{Cl}^{-}\) c. \(A l^{3+}\) or \(\mathrm{Na}^{+}\)

For each of the following molecules or ions, indicate the bond angle expected between the central atom and any two adjacent chlorine atoms. a. \(\mathrm{Cl}_{2} \mathrm{O}\) b. \(\mathrm{NCl}_{3}\) c. \(\mathrm{CCl}_{4}\) d. \(\mathrm{C}_{2} \mathrm{Cl}_{4}\)

For each of the following sets of elements, arrange the elements in order of increasing electronegativity. a.\(\mathrm {Li}\), \(\mathrm{F}\), \(\mathrm{C}\) b. \(\mathrm {I}\), \(\mathrm{Cl}\), \(\mathrm{F}\) c. \(\mathrm {L}\), \(\mathrm{R}\), \(\mathrm{C}\)

On the basis of their electron configurations, predict the formula of the simple binary ionic compound likely to form when the following pairs of elements react with each other. a. sodium, \(\mathrm{Na}\), and selenium, Se b. rubidium, Rb, and fluorine, F c. potassium, \(\mathrm{K}\), and tellurium, Te d. barium, Ba, and selenium, Se e. potassium, \(\mathrm{K}\), and astatine, \(\mathrm{At}\) f. francium, Fr, and chlorine, \(\mathrm{Cl}\)

Describe in general terms the structure of ionic solids such as NaCl. How are the ions packed in the crystal?
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