Textbook Question
Ethanol is a possible fuel. Use average bond energies to calculate ΔHrxn for the combustion of ethanol. CH3CH2OH(g) + 3 O2(g) → 2 CO2(g) + 3 H2O(g)
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Ch.9 - Chemical Bonding I: The Lewis Model
Chapter 9, Problem 85
Write an appropriate Lewis structure for each compound. Make certain to distinguish between ionic and molecular compounds. a. BI3 c. HCFO b. K2S d. PBr3
Verified step by step guidance1
Step 1: Identify the type of compound (ionic or molecular) for each given formula. BI3, HCFO, and PBr3 are molecular compounds, while K2S is an ionic compound.
Step 2: For molecular compounds (BI3, HCFO, PBr3), determine the total number of valence electrons by adding the valence electrons of each atom in the molecule.
Step 3: Draw the skeletal structure for each molecular compound, placing the least electronegative atom in the center (except hydrogen, which is always terminal). Connect the atoms with single bonds.
Step 4: Distribute the remaining valence electrons around the atoms to satisfy the octet rule (or duet for hydrogen), starting with the outer atoms and then moving to the central atom if needed.
Step 5: For the ionic compound K2S, represent the transfer of electrons from the metal (K) to the non-metal (S), forming K+ and S2- ions. Show the resulting ionic structure with brackets and charges.
Related Practice
Open Question
Hydrogen, a potential future fuel, can be produced from carbon (from coal) and steam by this reaction: C(s) + 2 H2O(g) -> H2(g) + CO2(g). Use average bond energies to calculate ΔHrxn for the reaction.
Textbook Question
In the Chemistry and the Environment box on free radicals in this chapter, we discussed the importance of the hydroxyl radical in reacting with and eliminating many atmospheric pollutants. However, the hydroxyl radical does not clean up everything. For example, chlorofluorocarbons—which destroy stratospheric ozone—are not attacked by the hydroxyl radical. Consider the hypothetical reaction by which the hydroxyl radical might react with a chlorofluorocarbon: OH(g) + CF2Cl2(g) → HOF(g) + CFCl2(g) Use bond energies to explain why this reaction is improbable. (The C–F bond energy is 552 kJ/mol.)
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Textbook Question
Write an appropriate Lewis structure for each compound. Make certain to distinguish between ionic and molecular compounds. b. ClF5
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Textbook Question
Each compound contains both ionic and covalent bonds. Write ionic Lewis structures for each, including the covalent structure for the ion in brackets. Write resonance structures if necessary. a. BaCO3
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Open Question
Does each compound contain both ionic and covalent bonds? Write ionic Lewis structures for each of them, including the covalent structure for the ion in brackets. Write resonance structures if necessary for the following: b. NH4Cl, d. Sr(CN)2, a. RbIO2, c. KOH.