Question

Order the following compounds according to the increasing ionic character of their bonds: \(\mathrm{NH}_{3}, \mathrm{NCl}_{3}, \mathrm{Na}_{3} \mathrm{~N}, \mathrm{NO}_{2}\)

Short answer

Order: \( \mathrm{NH}_3 < \mathrm{NO}_2 < \mathrm{NCl}_3 < \mathrm{Na}_3 \mathrm{N} \).

Step-by-step solution

Identify Bond Types

Examine each compound to determine the type of bond it contains. 1. \( \mathrm{NH}_3 \): Contains covalent bonds (non-metal to non-metal).2. \( \mathrm{NCl}_3 \): Contains covalent bonds (non-metal to non-metal).3. \( \mathrm{Na}_3 \mathrm{N} \): Contains ionic bonds (metal to non-metal).4. \( \mathrm{NO}_2 \): Contains covalent bonds (non-metal to non-metal).

Compare Electronegativity Differences

The ionic character of a bond generally increases with a larger difference in electronegativity between the two bonding atoms.1. \( \mathrm{NH}_3 \): \( \mathrm{N} - \mathrm{H} \) electronegativity difference is small.2. \( \mathrm{NCl}_3 \): \( \mathrm{N} - \mathrm{Cl} \) electronegativity difference is moderate.3. \( \mathrm{Na}_3 \mathrm{N} \): \( \mathrm{Na} - \mathrm{N} \) has a large electronegativity difference.4. \( \mathrm{NO}_2 \): \( \mathrm{N} - \mathrm{O} \) electronegativity difference is similar to \( \mathrm{N} - \mathrm{Cl} \).

Rank Compounds by Ionic Character

Based on the electronegativity differences, we can rank the compounds according to increasing ionic character:1. \( \mathrm{NH}_3 \) (Smallest ionic character)2. \( \mathrm{NO}_2 \) 3. \( \mathrm{NCl}_3 \) 4. \( \mathrm{Na}_3 \mathrm{N} \) (Greatest ionic character)

Key concepts

Electronegativity

Electronegativity is a crucial concept when understanding chemical bonds. It refers to the ability of an atom to attract the electron pair in a chemical bond toward itself. Different elements have different electronegativities, and this difference helps determine the type of bond that will form between them.
For instance:

• Elements with higher electronegativity, like fluorine, have a greater tendency to pull electrons toward themselves.
• Elements with lower electronegativity, such as sodium, are less effective at attracting electrons.

A larger electronegativity difference between two atoms leads to a stronger attraction. This often means that the bond is more likely to have a higher ionic character, as electrons are transferred rather than shared.
In chemistry, electronegativities are often compared using Pauling's scale. Understanding this helps predict how a substance may behave chemically and what type of bond it is likely to form.

Types of Chemical Bonds

Chemical bonds are forces that hold atoms together in compounds. The primary types of bonds are ionic, covalent, and metallic, each with distinct characteristics:

• Ionic Bonds: Formed when one atom donates electrons to another, resulting in positive and negative ions that attract each other. Commonly occur between a metal and a non-metal, like in NaCl (salt).
• Covalent Bonds: Involve the sharing of electron pairs between atoms. These bonds usually occur between non-metal atoms, like in the oxygen molecule (O extsubscript{2}).
• Metallic Bonds: Found in metals where atoms share a "sea" of electrons that move freely throughout the structure. This type of bonding explains the conductivity and malleability of metals.

Each bond type has its unique properties and influences the chemical and physical nature of the compounds they form. Ionic and covalent bonds stand out as they are most commonly compared, especially when assessing the ionic character of a compound.

Covalent vs Ionic Bonds

When distinguishing between covalent and ionic bonds, it's important to consider the nature of electron interactions between the atoms. Covalent bonds are characterized by the sharing of electron pairs. This type of bonding usually occurs between nonmetals, like in the molecule NH extsubscript{3} (ammonia). These bonds can be polar or nonpolar, depending on the electronegativity difference.
On the other hand:

• Ionic bonds are formed when electrons are transferred from one atom to another, usually between metals and nonmetals. They result in the formation of ions that are held together by electrostatic attraction, as seen in Na extsubscript{3}N.
• The greater the difference in electronegativity between the bonding atoms, the more ionic the bond is.

Comparatively, covalent bonds tend to have lower electronegativity differences, exhibiting less ionic character. Understanding these differences helps in predicting the behavior and properties of compounds, as seen in ordering compounds by their ionic character, like the original exercise you encountered. This knowledge aids in various applications from predicting solubility to reaction tendencies in chemical processes.