A compound composed of only carbon and chlorine is 85.5% chlorine by mass. Propose a Lewis structure for the compound.

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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.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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.

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.

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.

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Transition Metals Valence Electrons

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Textbook Question

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.

Textbook Question

Calculate the heat of atomization (see previous problem) of C₂H₃Cl, using the average bond energies in Table 9.3.

Textbook Question

A compound composed of only carbon and hydrogen is 7.743% hydrogen by mass. Propose a Lewis structure for the compound.