Textbook Question
Using the shorthand notation of Figure 22.9, draw the structure of the silicate anion in:
(a) K4SiO4 (b) Ag10Si4O13
What is the relationship between the charge on the anion and the number of terminal O atoms?
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 22.23a
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?
Verified step by step guidance1
Identify the second-row elements in the periodic table, which are lithium (Li), beryllium (Be), boron (B), carbon (C), nitrogen (N), oxygen (O), and fluorine (F).
Determine the hydrides of these elements: LiH, BeH2, BH3, CH4, NH3, H2O, and HF.
Consider the types of intermolecular forces present in each hydride: London dispersion forces, dipole-dipole interactions, and hydrogen bonding.
Recognize that hydrogen bonding is the strongest intermolecular force and occurs in NH3, H2O, and HF.
Compare the strength of hydrogen bonding in NH3, H2O, and HF, noting that HF typically has the strongest hydrogen bonds due to the high electronegativity of fluorine.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Hydride Structures
Hydrides are compounds formed between hydrogen and other elements. The structure of a hydride can significantly influence its physical properties, including melting point. For second-row elements, the type of bonding (ionic, covalent, or metallic) and molecular geometry play crucial roles in determining the stability and melting point of the hydride.
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01:00
Metallic Hydrides
Melting Point Trends
The melting point of a compound is influenced by the strength of the intermolecular forces present. Generally, ionic compounds have higher melting points due to strong electrostatic forces, while covalent compounds may vary based on molecular size and polarity. Understanding these trends helps predict which hydride will have the highest melting point among the given options.
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04:29Boiling Point and Melting Point
Periodic Trends
Periodic trends refer to the predictable patterns in the properties of elements as you move across or down the periodic table. For second-row elements, factors such as electronegativity, atomic size, and the type of bonding can affect the properties of their hydrides. Recognizing these trends is essential for comparing the melting points of different hydrides.
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00:38Periodic Trends
Related Practice
Textbook Question
What is the hybridization and geometry around carbon atoms in graphene? Explain why graphene is an excellent conductor of electricity.
Textbook Question
List three ways in which the properties of boron differ from those of the other group 3A elements.
Textbook Question
a. Why is the SO3 molecule trigonal planar but the SO32– ion is trigonal pyramidal?
Textbook Question
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–.
Textbook Question
Which compound in each of the following pairs is more covalent?
(a) PCl3 or AlF3