Textbook Question
Which is the best electron-dot structure for the thiosulfate ion (S2O3 2-) based on the rules of formal charge? (LO 7.16)(a) (b) (c) (d)
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Ch.7 - Covalent Bonding and Electron-Dot Structures
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 7, Problem 29
Which of the following alkali metal halides has the largest lat-tice energy? Explain.(a) (b) (c)
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Identify the alkali metals and halides involved in each option (a), (b), and (c).
Understand that lattice energy is influenced by the charge of the ions and the distance between them. The greater the charge and the smaller the ionic radii, the stronger the lattice energy.
Recall that in the periodic table, as you move down a group, the ionic radius increases. This means that for alkali metals, the ionic radius increases from Li to Cs.
Similarly, for halides, the ionic radius increases as you move down the group in the periodic table, from F to I.
Compare the alkali metals and halides in each option based on their positions in the periodic table to determine which combination has the smallest ions with the highest charges, as this will likely have the largest lattice energy.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Lattice Energy
Lattice energy is the amount of energy released when gaseous ions combine to form an ionic solid. It is a measure of the strength of the forces between the ions in an ionic compound. Higher lattice energy indicates stronger ionic bonds, which typically results from smaller ionic radii and higher charges on the ions.
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00:49
Lattice Energy
Ionic Size and Charge
The size of the ions involved in the formation of an ionic compound significantly affects lattice energy. Smaller ions can pack more closely together, leading to stronger electrostatic attractions and higher lattice energy. Additionally, the charge of the ions plays a crucial role; ions with higher charges will produce greater lattice energy due to stronger interactions.
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01:53Formal Charge
Trends in Alkali Metal Halides
In alkali metal halides, lattice energy trends can be analyzed based on the alkali metal and halide involved. As you move down the group of alkali metals, the ionic size increases, leading to lower lattice energies. Conversely, halides with higher electronegativity (like fluorine) tend to form compounds with higher lattice energies due to their smaller ionic size compared to other halides.
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Related Practice
Textbook Question
Use formal charge to select which resonance structure makes the largest contribution to the resonance hybrid. (LO 7.16) (a) Structure I (b) Structure II (c) Structure III (d) All structures are equivalent and make the same contri-bution to the resonance hybrid. (I)
(II)
(III)
Textbook Question
What is the best prediction for the carbon–oxygen bond length in the carbonate anion, CO3 2-? (LO 7.14)Data for average carbon-oxygen bond lengths: (a) 143 pm (b) 132 pm(c) 121 pm(d) 118 pm
Textbook Question
Two electrostatic potential maps are shown, one of methyl-lithium (CH3Li) and the other of chloromethane (CH3Cl). Based on their polarity patterns, which do you think is which? (a)
(b)
Textbook Question
The following diagram shows the potential energy of two atoms as a function of internuclear distance. Which bond is the strongest? Which bond is the longest?
Textbook Question
The following diagram shows the potential energy of two atoms as a function of internuclear distance. Match the descriptions with the indicated letter on the plot.(a) Repulsive forces are high between the two atoms. (b) The two atoms neither exert attractive nor repulsive forces on one another.(c) The attractive forces between atoms are maximized, resulting in the lowest energy state.(d) Attractive forces between atoms are present but are not at maximum strength.