Textbook Question
If hydrogen were used as a fuel, it could be burned according to this reaction: H2(g) + 1/2 O2(g) → H2O(g) Which fuel yields more energy per mole?
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Ch.9 - Chemical Bonding I: The Lewis Model
Chapter 9, Problem 107a
Draw the Lewis structure for each compound. a. Cl2O7 (no Cl–Cl bond)
Verified step by step guidance1
Step 1: Count the total number of valence electrons. Chlorine (Cl) has 7 valence electrons and oxygen (O) has 6 valence electrons. Calculate the total for Cl2O7.
Step 2: Determine the central atom. In Cl2O7, chlorine atoms are typically central, with oxygen atoms surrounding them.
Step 3: Arrange the atoms. Place the two chlorine atoms in the center and connect each to three oxygen atoms, ensuring no Cl-Cl bond is formed.
Step 4: Distribute the electrons. Start by placing single bonds between the Cl and O atoms, then distribute the remaining electrons to satisfy the octet rule for each atom, starting with the outer atoms.
Step 5: Check for formal charges and resonance. Adjust the structure by forming double bonds if necessary to minimize formal charges, ensuring the most stable structure.
Related Practice
Textbook Question
If hydrogen were used as a fuel, it could be burned according to this reaction: H2(g) + 1/2 O2(g) → H2O(g) Which fuel yields more energy per gram?
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Textbook Question
Calculate ΔHrxn for the combustion of octane (C8H18), a component of gasoline, by using average bond energies and then calculate it using enthalpies of formation from Appendix IIB. What is the percent difference between your results? Which result would you expect to be more accurate?
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Textbook Question
Draw the Lewis structure for each compound. b. H3PO3 (two OH bonds)
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Textbook Question
Draw the Lewis structure for each compound. c. H3AsO4
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Textbook Question
The azide ion, N3-, is a symmetrical ion, all of whose contributing resonance structures have formal charges. Draw three important contributing structures for this ion.
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