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?
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Ch.22 - The Main Group Elements
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement143
- Ch.2 - Atoms, Molecules & Ions134
- Ch.3 - Mass Relationships in Chemical Reactions149
- Ch.4 - Reactions in Aqueous Solution157
- Ch.5 - Periodicity & Electronic Structure of Atoms92
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory73
- Ch.7 - Covalent Bonding and Electron-Dot Structures47
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure51
- Ch.9 - Thermochemistry: Chemical Energy104
- Ch.10 - Gases: Their Properties & Behavior138
- Ch.11 - Liquids & Phase Changes43
- Ch.12 - Solids and Solid-State Materials56
- Ch.13 - Solutions & Their Properties98
- Ch.14 - Chemical Kinetics79
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Aqueous Equilibria: Acids & Bases94
- Ch.17 - Applications of Aqueous Equilibria125
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium66
- Ch.19 - Electrochemistry130
- Ch.20 - Nuclear Chemistry73
- Ch.21 - Transition Elements and Coordination Chemistry122
- Ch.22 - The Main Group Elements155
- Ch.23 - Organic and Biological Chemistry43
Chapter 22, Problem 22.163a
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–.
Verified step by step guidance1
Step 1: Draw the electron-dot structure for NO. Start by counting the total number of valence electrons. Nitrogen (N) has 5 valence electrons and oxygen (O) has 6 valence electrons, giving a total of 11 valence electrons. Distribute these electrons to satisfy the octet rule as much as possible, keeping in mind that NO is a radical with an unpaired electron.
Step 2: Draw the electron-dot structure for the superoxide ion, O2–. Oxygen has 6 valence electrons, so for O2, you have 12 valence electrons. The extra negative charge adds one more electron, making it 13 electrons in total. Distribute these electrons to form a bond between the two oxygen atoms, and place the extra electron on one of the oxygens.
Step 3: Draw the electron-dot structure for the peroxynitrite ion, ONOO–. Count the total valence electrons: O (6) + N (5) + O (6) + 1 (for the negative charge) = 18 electrons. Arrange these electrons to form bonds between the atoms, ensuring that the octet rule is satisfied for each atom as much as possible.
Step 4: Consider the resonance structures for ONOO–. Since ONOO– can have multiple valid electron-dot structures, draw the possible resonance forms to show the delocalization of electrons.
Step 5: Predict the O–N–O bond angle in ONOO–. Consider the electron pair geometry around the nitrogen atom. Since ONOO– is a bent molecule due to the presence of lone pairs on the nitrogen, the bond angle will be less than 120 degrees, typical for a bent molecular geometry.
Related Practice
Textbook Question
Write a balanced net ionic equation for the reaction of the amphoteric oxide Ga2O3 with:
a. Aqueous sulfuric acid
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Textbook Question
GeCl4 reacts with Cl- to give GeCl62-, but CCl4 does not react with excess Cl-. Explain.
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Textbook Question
Write a balanced net ionic equation for the reaction of the amphoteric oxide ZnO with:
a. Hydrochloric acid
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Textbook Question
The following pictures represent various silicate anions. Write the formula and charge of each anion.
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Textbook Question
What is the hybridization and geometry around carbon atoms in graphene? Explain why graphene is an excellent conductor of electricity.
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