Textbook Question
The following pictures represent structures of the hydrides of four second-row elements:
(1)
(2)
(3)
(4)
(a) Which compound has the highest melting point?
Ch.22 - The Main Group Elements
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Chapter 22, Problem 22.41a
Which compound in each of the following pairs is more covalent?
(a) PCl3 or AlF3
Verified step by step guidance1
Identify the types of bonds present in each compound. PCl₃ and AlF₃ both have polar covalent bonds, but the degree of covalency can differ.
Consider the electronegativity difference between the atoms in each compound. A smaller difference in electronegativity generally indicates a more covalent character.
For PCl₃, compare the electronegativity of phosphorus (P) and chlorine (Cl).
For AlF₃, compare the electronegativity of aluminum (Al) and fluorine (F).
Determine which compound has a smaller electronegativity difference, indicating a more covalent character.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Covalent Bonding
Covalent bonding occurs when two atoms share electrons to achieve a full outer shell, typically between nonmetals. The degree of covalency can vary based on the electronegativity of the atoms involved; the greater the difference in electronegativity, the more ionic the bond becomes. In this context, understanding how covalent bonds form helps in comparing the compounds.
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Chemical Bonds
Electronegativity
Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a bond. Elements with similar electronegativities tend to form more covalent bonds, while a large difference indicates a more ionic character. By comparing the electronegativities of phosphorus, chlorine, aluminum, and fluorine, one can determine which compound is more covalent.
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02:10Electronegativity Trends
Molecular Structure and Geometry
The molecular structure and geometry of a compound influence its bonding characteristics. For example, PCl3 has a trigonal pyramidal shape, while AlF3 has a more ionic lattice structure. Understanding these geometrical arrangements helps in predicting the nature of the bonds and the overall covalency of the compounds in question.
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Related Practice
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a. Why is the SO3 molecule trigonal planar but the SO32– ion is trigonal pyramidal?
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An important physiological reaction of nitric oxide (NO) is its interaction with the superoxide ion (O2–) to form the peroxynitrite ion (ONOO–).
a. Write electron-dot structures for NO, O2–, and ONOO–, and predict the O–N–O bond angle in ONOO–.
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