Textbook Question
List three ways in which the properties of boron differ from those of the other group 3A elements.
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 22.163a
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.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Electron-Dot Structures
Electron-dot structures, also known as Lewis structures, represent the valence electrons of atoms within a molecule. They illustrate how electrons are shared or transferred between atoms, helping to visualize molecular bonding and geometry. For nitric oxide (NO), the structure shows a double bond between nitrogen and oxygen, while the superoxide ion (O2–) has an unpaired electron, indicating its radical nature. Understanding these structures is essential for predicting molecular behavior and reactivity.
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Lewis Dot Structures: Ions
Bond Angles and Molecular Geometry
Bond angles are the angles formed between adjacent bonds in a molecule, which are influenced by the arrangement of electron pairs around a central atom. The molecular geometry of ONOO– can be predicted using VSEPR (Valence Shell Electron Pair Repulsion) theory, which states that electron pairs will arrange themselves to minimize repulsion. In ONOO–, the presence of resonance structures and lone pairs will affect the O–N–O bond angle, which is crucial for understanding the molecule's reactivity and interactions.
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Reactivity of Nitric Oxide and Superoxide
Nitric oxide (NO) and superoxide (O2–) are both reactive species that play significant roles in biological systems. NO is a signaling molecule involved in various physiological processes, while O2– is a reactive oxygen species that can cause oxidative stress. Their interaction to form peroxynitrite (ONOO–) is a critical reaction that can lead to further biological effects, including cellular damage. Understanding the reactivity of these species is essential for grasping their physiological implications and the chemistry behind their interactions.
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Related Practice
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?
Textbook Question
a. Why is the SO3 molecule trigonal planar but the SO32– ion is trigonal pyramidal?
Textbook Question
Which compound in each of the following pairs is more covalent?
(a) PCl3 or AlF3
Textbook Question
Write a balanced net ionic equation for the reaction of the amphoteric oxide Ga2O3 with:
a. Aqueous sulfuric acid
Textbook Question
Which element in each of the following pairs has more nonmetallic character?
(a) Se or Te