Domanda del libro di testo
Calculate the heat of atomization (see previous problem) of C2H3Cl, using the average bond energies in Table 10.3.
Ch.10 - Chemical Bonding I: The Lewis Model
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
Non è quello che usi tu?Cambia libro di testoScegli un libro di testo diverso
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
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Non è quello che usi tu?Cambia libro di testo
Capitolo 10, Problema 114
A compound composed of only carbon and chlorine is 85.5% chlorine by mass. Propose a Lewis structure for the compound.
Guida verificata passo dopo passo1
Determine the mass percentage of carbon in the compound by subtracting the mass percentage of chlorine from 100%. This gives you the mass percentage of carbon.
Assume a sample size of 100 grams to simplify calculations. This assumption means that the mass of chlorine in the compound is 85.5 grams and the mass of carbon is the remainder.
Convert the mass of each element to moles by using their respective molar masses. The molar mass of chlorine (Cl) is approximately 35.5 g/mol, and the molar mass of carbon (C) is approximately 12.0 g/mol.
Calculate the simplest whole number ratio of moles of carbon to moles of chlorine in the compound. This ratio will help in determining the empirical formula of the compound.
Use the empirical formula to propose a Lewis structure. Remember that carbon typically forms four bonds in neutral compounds, and chlorine usually forms one bond. Arrange the atoms to satisfy these bonding preferences and to achieve a neutral overall charge.
Risposta video verificata per un problema simile:
Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Concetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
Empirical Formula
The empirical formula represents the simplest whole-number ratio of elements in a compound. In this case, knowing that the compound is 85.5% chlorine by mass allows us to determine the ratio of carbon to chlorine, which is essential for proposing a Lewis structure.
Video consigliato:
Percorso guidato
02:26
Empirical vs Molecular Formula
Lewis Structures
Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons. They help visualize how atoms are connected and the distribution of electrons, which is crucial for understanding the compound's chemical behavior and stability.
Video consigliato:
Percorso guidato
04:28Lewis Dot Structures: Ions
Valence Electrons
Valence electrons are the outermost electrons of an atom and are involved in forming bonds. Knowing the number of valence electrons for carbon and chlorine is vital for accurately drawing the Lewis structure, as it determines how atoms will bond and share electrons.
Video consigliato:
Percorso guidato
02:12Transition Metals Valence Electrons
Pratica correlata
Domanda del libro di testo
A compound composed of only carbon and hydrogen is 7.743% hydrogen by mass. Propose a Lewis structure for the compound.
995
views
Domanda del libro di testo
The heat of atomization is the heat required to convert a molecule in the gas phase into its constituent atoms in the gas phase. The heat of atomization is used to calculate average bond energies. Without using any tabulated bond energies, calculate the average C–Cl bond energy from the following data: the heat of atomization of CH4 is 1660 kJ/mol, and the heat of atomization of CH2Cl2 is 1495 kJ/mol.
1987
views
1
rank