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Chapter 8: Problem 5

Consider the following statement: "Because oxygen wants to have a negative two charge, the second electron affinity is more negative than the first." Indicate everything that is correct in this statement. Indicate everything that is incorrect. Correct the incorrect statements and explain.

Short Answer

Expert verified
The corrected statement is: "Because oxygen wants to have a negative two charge, it can attract two additional electrons. However, the second electron affinity is less negative than the first due to increased electron-electron repulsion." Oxygen aims to achieve a stable electron configuration (full octet) by gaining two electrons. The first electron affinity is negative due to energy release, but the second electron affinity is less negative or even positive due to electron-electron repulsion and the need for energy input.

Step by step solution

01

Identify what is correct in the statement

The statement correctly states that oxygen wants to have a negative two charge. This is because oxygen has six valence electrons, and it needs two more electrons to achieve a full octet, which gives it a stable electron configuration like that of noble gases.
02

Identify what is incorrect in the statement

The incorrect part of the statement is that "the second electron affinity is more negative than the first." In reality, the first electron affinity is usually a negative value since energy is released when an electron is added to an atom, but the second electron affinity is typically less negative than the first or even positive. This is because the added electron will experience electron-electron repulsion, which requires energy input.
03

Correct the statement and provide an explanation

The corrected statement should read: "Because oxygen wants to have a negative two charge, it can attract two additional electrons. However, the second electron affinity is less negative than the first due to increased electron-electron repulsion." The explanation for the corrected statement is as follows: Oxygen aims to achieve a stable electron configuration (full octet) by achieving a negative two charge (which implies gaining two electrons). The first electron affinity typically results in a release of energy (negative value) when an electron is added to an atom. However, the second electron affinity will result in a less negative value, or even a positive value, since the added electron will experience electron-electron repulsion. This second electron addition requires energy input, which is why the second electron affinity will not be more negative than the first.

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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. \(\mathrm{Rb}^{+}\)

Use the formal charge arguments to rationalize why \(\mathrm{BF}_{3}\) would not follow the octet rule.

Some of the important properties of ionic compounds are as follows: i. low electrical conductivity as solids and high conductivity in solution or when molten ii. relatively high melting and boiling points iii. brittleness iv. solubility in polar solvents How does the concept of ionic bonding discussed in this chapter account for these properties?

Use the following data to estimate \(\Delta H\) for the reaction \(\mathrm{S}^{-}(g)+\) \(\mathrm{e}^{-} \rightarrow \mathrm{S}^{2-}(g)\). Include an estimate of uncertainty. $$ \begin{array}{|lcccc|} \hline & & \text { Lattice } & & \Delta H_{\text {sub }} \\ & \Delta \boldsymbol{H}_{\mathrm{t}}^{\circ} & \text { Energy } & \text { I.E. of } \mathbf{M} & \text { of M } \\ \hline \mathrm{Na}_{2} \mathrm{~S} & -365 & -2203 & 495 & 109 \\ \mathrm{~K}_{2} \mathrm{~S} & -381 & -2052 & 419 & 90 \\ \mathrm{Rb}_{2} \mathrm{~S} & -361 & -1949 & 409 & 82 \\ \mathrm{Cs}_{2} \mathrm{~S} & -360 & -1850 & 382 & 78 \\ \hline \end{array} $$ $$ \begin{aligned} \mathrm{S}(s) & \longrightarrow \mathrm{S}(g) & \Delta H &=227 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{S}(g)+\mathrm{e}^{-} & \longrightarrow \mathrm{S}^{-}(g) & \Delta H &=-200 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$ Assume that all values are known to \(\pm 1 \mathrm{~kJ} / \mathrm{mol}\).

Write Lewis structures that obey the octet rule for each of the following molecules. a. \(\mathrm{CCl}_{4}\) c. \(\mathrm{SeCl}_{2}\) b. \(\mathrm{NCl}_{3}\) d. \(\mathrm{ICl}\) In each case, the atom listed first is the central atom.
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