교과서 질문
Write Lewis structures for each molecule or ion. Use expanded octets as necessary. a. PF5
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Ch.10 - Chemical Bonding I: The Lewis Model
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving117
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds128
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions84
- Ch.6 - Gases112
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements86
- Ch.10 - Chemical Bonding I: The Lewis Model91
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials48
- Ch.14 - Solutions93
- Ch.15 - Chemical Kinetics114
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases137
- Ch.18 - Aqueous Ionic Equilibrium154
- Ch.19 - Free Energy & Thermodynamics91
- Ch.20 - Electrochemistry105
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry141
10장, 문제 74
Write the Lewis structure for each molecule (octet rule not followed). a. BBr3 b. NO c. ClO2
검증된 단계별 안내1
1. Identify the central atom in each molecule. For BBr3, it's Boron (B); for NO, it's Nitrogen (N); and for ClO2, it's Chlorine (Cl).
2. Count the total number of valence electrons for each molecule. For BBr3, Boron has 3 valence electrons and each Bromine has 7, so the total is 3 + 3*7 = 24. For NO, Nitrogen has 5 valence electrons and Oxygen has 6, so the total is 5 + 6 = 11. For ClO2, Chlorine has 7 valence electrons and each Oxygen has 6, so the total is 7 + 2*6 = 19.
3. Draw a skeleton structure for each molecule, connecting the atoms with single bonds. This uses up 2 electrons for each bond. For BBr3, connect Boron to each Bromine atom. For NO, connect Nitrogen to Oxygen. For ClO2, connect Chlorine to each Oxygen atom.
4. Distribute the remaining electrons as lone pairs on the outer atoms first, then the central atom, until all electrons are used up or until each atom (except Hydrogen) has an octet. For BBr3, each Bromine atom gets 3 lone pairs. For NO, Oxygen gets 2 lone pairs and Nitrogen gets 1 lone pair. For ClO2, each Oxygen atom gets 3 lone pairs and Chlorine gets 1 lone pair.
5. If any atoms lack an octet after step 4, and there are no more electrons to distribute, consider forming double or triple bonds until each atom has an octet. For NO, form a double bond between Nitrogen and Oxygen. For ClO2, form a double bond between Chlorine and one of the Oxygen atoms. Note that in these cases, the octet rule is not followed for all atoms.
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주요 개념
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Lewis Structures
Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent valence electrons and lines to indicate bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting reactivity.
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가이드 코스
04:28
Lewis Dot Structures: Ions
Octet Rule
The octet rule is a chemical rule of thumb that states atoms tend to bond in such a way that they each have eight electrons in their valence shell, achieving a stable electron configuration similar to that of noble gases. However, some molecules, like BBr3 and NO, do not follow this rule, which is crucial for understanding their bonding and structure.
추천 영상:
가이드 코스
01:36Octet Rule
Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is influenced by the number of bonds and lone pairs around the central atom, which can affect the molecule's reactivity and properties. Understanding molecular geometry is important for predicting how molecules will interact in chemical reactions.
추천 영상:
가이드 코스
01:33Molecular Geometry with Two Electron Groups