For each pair, determine which compound has bonds with greater ionic character: (a) \(\mathrm{PH}_{3}\) or \(\mathrm{NH}_{3}\); (b) \(\mathrm{SO}_{2}\) or \(\mathrm{NO}_{2}\); (c) \(\mathrm{SF}_{6}\) or \(\mathrm{IF}_{5}\).

Short Answer

Expert verified
Greater ionic character is found in NH3, NO2, and IF5 for the respective comparisons.

Step by step solution

01

Understanding Ionic Character

The ionic character of a bond in a molecule is determined by the difference in electronegativity between the atoms forming the bond. The greater the difference in electronegativity, the more ionic the character of the bond is.
02

Comparing Ionic Character in PH3 and NH3

To compare the ionic character of bonds in abla(PH_3) and abla(NH_3), look at the electronegativity of phosphorus (P) and nitrogen (N). Nitrogen is more electronegative than phosphorus, so the bonds in abla(NH_3) will have a greater ionic character since the difference in electronegativity between N and H is greater than between P and H.
03

Comparing Ionic Character in SO2 and NO2

Analyze the electronegativity difference between sulfur (S) and oxygen (O), and between nitrogen (N) and oxygen (O). Oxygen is more electronegative than sulfur and nitrogen, but since the difference in electronegativity between N and O is greater than between S and O, abla(NO_2) has bonds with greater ionic character.
04

Comparing Ionic Character in SF6 and IF5

Consider the differences in electronegativity between sulfur (S) and fluorine (F), and between iodine (I) and fluorine (F). Fluorine is more electronegative than both sulfur and iodine. Iodine is less electronegative than sulfur, so the bonds in abla(IF_5) have greater ionic character due to the larger difference in electronegativity between I and F than between S and F.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with Vaia!

Key Concepts

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

Electronegativity
Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. When atoms with different electronegativities form a bond, the bonding electrons are not shared equally. The more electronegative atom will attract the electrons more strongly, creating a dipole with a partial-negative charge on the more electronegative atom and a partial-positive charge on the less electronegative atom.

This difference in charge distribution is what gives rise to the concept of ionic character in a bond. Ionic character increases as the difference in electronegativity between two bonding atoms increases. On the periodic table, electronegativity typically increases as you move from left to right across a period and decreases as you move down a group. Hence, elements like fluorine, oxygen, and nitrogen are among the most electronegative elements, and as such, bonds involving these elements often have a significant ionic character.
Chemical Bonding
Chemical bonding is the process where atoms come together to form molecules through the sharing or transfer of electrons. The nature of chemical bonds can be broadly classified into three main types: ionic, covalent, and metallic bonds.

An ionic bond is formed when there is a complete transfer of one or more electrons from a less electronegative atom to a more electronegative atom, resulting in ions that are held together by electrostatic forces. Conversely, a covalent bond is the result of the sharing of electrons between two atoms; if the sharing is unequal due to differing electronegativities, the bond displays some ionic character. When solving problems on chemical bonding, one must consider both the type of bond and the difference in electronegativity to ascertain the overall ionic or covalent nature of a compound.

In practical terms, if students find the concepts difficult, they should try visualizing the molecular interactions and how electron distribution affects them. This can help in comprehending why certain compounds, even with covalent bonds, can exhibit notable ionic characteristics.
Molecular Structure
Molecular structure refers to the three-dimensional arrangement of atoms within a molecule. The spatial configuration of a molecule can influence its physical and chemical properties, including reactivity, color, and magnetism. Molecular geometry can be predicted using VSEPR theory (Valence Shell Electron Pair Repulsion theory), which is based on the idea that electron groups around a central atom will arrange themselves to minimize repulsion.

The shape of a molecule affects its dipole moment and, by extension, its ionic character. For instance, molecules with asymmetrical distributions of charge due to uneven electron distribution and molecular geometry will have high ionic character. Understanding molecular geometry aids in visualizing how the vector sum of individual bond polarities results in the overall polarity of the molecule, which is crucial for predicting molecular behavior during chemical reactions.

By grasping the connection between molecular structure and polarity, students can better determine the properties of compounds and predict their behavior in various environments. This illustration of concept correlation enhances the understanding and identification of molecular characteristics in study and real-world contexts.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

See all solutions

Recommended explanations on Chemistry Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free