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Ch.9 - Chemical Bonding I: The Lewis Model
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Not the one you use?Change textbook
All textbooksTro 4th EditionCh.9 - Chemical Bonding I: The Lewis ModelProblem 107c
Chapter 9, Problem 107c

Draw the Lewis structure for each compound. c. H3AsO4

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Identify the total number of valence electrons in the compound. Arsenic (As) has 5 valence electrons, each hydrogen (H) has 1, and each oxygen (O) has 6. Calculate the total valence electrons for H_3AsO_4.
Determine the central atom. Typically, the least electronegative atom that is not hydrogen is the central atom. In this case, arsenic (As) will be the central atom.
Arrange the atoms around the central atom. Place the three hydrogen atoms and four oxygen atoms around the arsenic atom.
Connect the atoms with single bonds initially. Each bond represents a pair of electrons. Connect each hydrogen to an oxygen, and then connect each oxygen to the arsenic atom.
Distribute the remaining electrons to satisfy the octet rule for each atom, starting with the outer atoms (oxygen) and then the central atom (arsenic). Adjust the bonds if necessary to ensure all atoms have a complete octet, considering the possibility of double bonds if needed.

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Key Concepts

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

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 represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting the behavior of molecules in chemical reactions.
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Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in determining how an atom will bond with others. The number of valence electrons influences the atom's reactivity and the types of bonds it can form. For example, in H3AsO4, knowing the valence electrons of hydrogen, arsenic, and oxygen helps in constructing the correct Lewis structure.
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Formal Charge

Formal charge is a concept used to determine the distribution of electrons in a molecule and to assess the stability of a Lewis structure. It is calculated by comparing the number of valence electrons in the free atom to the number of electrons assigned to it in the structure. A Lewis structure with the lowest formal charges on atoms is generally more stable, guiding the correct representation of molecules like H3AsO4.
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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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A compound composed of only carbon and hydrogen is 7.743% hydrogen by mass. Propose a Lewis structure for the compound.

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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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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

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

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