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Chapter 8: Problem 14

Does a Lewis structure tell which electrons come from which atoms? Explain.

Short Answer

Expert verified
A Lewis structure does not indicate which electrons come from which atoms. It is a graphical representation that focuses on showing the distribution of valence electrons and the arrangement of atoms in a molecule, rather than identifying the origin of the electrons.

Step by step solution

01

Understand Lewis structures

A Lewis structure is a simplified, graphical representation of a molecule's chemical bonding. It is used to show how the valence electrons (the electrons in an atom's outermost shell) are distributed among the atoms in a molecule. The main elements of a Lewis structure are atoms' symbols, bonds (lines), and lone pairs (dots). One pair of shared electrons between two atoms is called a single bond (represented by a single line), two pairs will form a double bond (represented by two lines), and three pairs form a triple bond (represented by three lines).
02

Determine electrons' origin in Lewis structures

In a Lewis structure, the electrons involved in the bonding are represented by dots or lines connecting the atoms. However, once they are shared between the atoms to form bonds, it becomes impossible to distinguish which electrons come from which atoms. The purpose of a Lewis structure is to show the distribution of valence electrons and the arrangement of atoms in a molecule, rather than identifying the origin of the electrons.
03

Conclusion

A Lewis structure does not tell which electrons come from which atoms. It is a simplified representation of a molecule's chemical bonding that shows electron distribution among the atoms, but it does not differentiate the electrons based on their origin.

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Most popular questions from this chapter

Give the formula of a negative ion that would have the same number of electrons as each of the following positive ions. a. \(\mathrm{Na}^{+}\) c. \(\mathrm{Al}^{3+}\) b. \(\mathrm{Ca}^{2+}\) d. \(\mathrm{Rb}^{+}\)

Some plant fertilizer compounds are \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}, \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}, \mathrm{~K}_{2} \mathrm{O}\), \(\mathrm{P}_{2} \mathrm{O}_{5}\), and \(\mathrm{KCl}\). Which of these compounds contain both ionic and covalent bonds?

Use the following standard enthalpies of formation to estimate the \(\mathrm{N}-\mathrm{H}\) bond energy in ammonia: \(\mathrm{N}(\mathrm{g}), 472.7 \mathrm{~kJ} / \mathrm{mol} ; \mathrm{H}(\mathrm{g})\), \(216.0 \mathrm{~kJ} / \mathrm{mol} ; \mathrm{NH}_{3}(g),-46.1 \mathrm{~kJ} / \mathrm{mol}\). Compare your value to the one in Table \(8.4\).

Consider the following reaction: $$ \mathrm{A}_{2}+\mathrm{B}_{2} \longrightarrow 2 \mathrm{AB} \quad \Delta H=-285 \mathrm{~kJ} $$ The bond energy for \(\mathrm{A}_{2}\) is one-half the amount of the \(\mathrm{AB}\) bond energy. The bond energy of \(\mathrm{B}_{2}=432 \mathrm{~kJ} / \mathrm{mol}\). What is the bond energy of \(\mathrm{A}_{2}\) ?

Consider the following bond lengths: \(\begin{array}{lllll}\mathrm{C}-\mathrm{O} & 143 \mathrm{pm} & \mathrm{C}=\mathrm{O} & 123 \mathrm{pm} & \mathrm{C} \equiv \mathrm{O} & 109 \mathrm{pm}\end{array}\) In the \(\mathrm{CO}_{3}^{2-}\) ion, all three \(\mathrm{C}-\mathrm{O}\) bonds have identical bond lengths of \(136 \mathrm{pm}\). Why?
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