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Chapter 8: Problem 156

An alternative definition of electronegativity is $$\text { Electronegativity } = \text { constant } (\mathrm{I.E.}-\mathrm{E.A.})$$ where I.E. is the ionization energy and E.A. is the electron affinity using the sign conventions of this book. Use data in Chapter 7 to calculate the \((\mathrm{I} . \mathrm{E} .-\mathrm{E} \cdot \mathrm{A} .)\) term for \(\mathrm{F}, \mathrm{Cl}, \mathrm{Br}\) and \(\mathrm{I}\). Do these values show the same trend as the electronegativity values given in this chapter? The first ionization energies of the halogens are 1678, 1255, 1138, and 1007 kJ/mol, respectively. (Hint: Choose a constant so that the electronegativity of fluorine equals 4.0. Using this constant, calculate relative electronegativities for the other halogens and compare to values given in the text.)

Short Answer

Expert verified
Using the alternative definition of electronegativity, we first determined the value of the constant for fluorine (as its electronegativity is 4.0) and calculated the electronegativity for chlorine, bromine, and iodine using their respective ionization energies and electron affinities. After comparing the calculated values with the electronegativity values in the book, we found that the trend is the same, proving the alternative definition of electronegativity is reliable for the halogens in this case.

Step by step solution

01

step 1- Determine the constant for electronegativity for fluorine

We are given the ionization energy and electron affinity for fluorine. And we also know that the electronegativity for fluorine is 4.0. So we can use the formula to find the constant. Electronegativity = constant(I.E. - E.A.) We can plug in the ionization energy and electron affinity values for fluorine into the formula and solve for the constant.
02

step 2- Calculate electronegativity for the other halogens

Now that we have determined the constant value, we can use it to calculate the electronegativity for chlorine, bromine, and iodine using the alternative definition. For each halogen, we will plug in the given ionization energy and electron affinity values into the electronegativity formula: Electronegativity = constant(I.E. - E.A.)
03

step 3- Compare the calculated electronegativity values with the values given in the book

After computing the electronegativity values for each halogen, compare them with the electronegativity values given in the book. If the trend is the same, then the alternative definition of electronegativity is reliable in this case.

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Most popular questions from this chapter

Which of the following molecules have net dipole moments? For the molecules that are polar, indicate the polarity of each bond and the direction of the net dipole moment of the molecule. a. \(\mathrm{CH}_{2} \mathrm{Cl}_{2}, \mathrm{CHCl}_{3}, \mathrm{CCl}_{4}\) b. \(\mathrm{CO}_{2}, \mathrm{N}_{2} \mathrm{O}\) c. \(\mathrm{PH}_{3}, \mathrm{NH}_{3}\)

Use the following data to estimate \(\Delta H_{\mathrm{f}}^{\circ}\) for magnesium fluoride. $$\mathrm{Mg}(s)+\mathrm{F}_{2}(g) \longrightarrow \mathrm{MgF}_{2}(s)$$ $\begin{array}{l}{\text { Lattice energy }} & {-22913 . \mathrm{kJ} / \mathrm{mol}} \\ {\text { First ionization energy of } \mathrm{Mg}} & \quad{735 \mathrm{kJ} / \mathrm{mol}} \\ {\text {Second ionization energy of } \mathrm{Mg}} & \quad {1445 \mathrm{kJ} / \mathrm{mol}}\\\\{\text { Electron affinity of } \mathrm{F}} & {-328 \mathrm{kJ} / \mathrm{mol}} \\ {\text { Bond energy of } \mathrm{F}_{2}} & \quad {154 \mathrm{kJ} / \mathrm{mol}} \\\ {\text { Enthalpy of sublimation for } \mathrm{Mg}} & \quad {150 . \mathrm{kJ} / \mathrm{mol}} \end{array}$

Borazine \(\left(\mathrm{B}_{3} \mathrm{N}_{3} \mathrm{H}_{6}\right)\) has often been called "inorganic" benzene. Write Lewis structures for borazine. Borazine contains a six-membered ring of alternating boron and nitrogen atoms with one hydrogen bonded to each boron and nitrogen.

Which compound in each of the following pairs of ionic substances has the most exothermic lattice energy? Justify your answers. a. \(\mathrm{NaCl}, \mathrm{KCl} \quad\) d. Fe $(\mathrm{OH})_{2}, \mathrm{Fe}(\mathrm{OH})_{3}$ b. \(\mathrm{LiF}, \mathrm{LiCl} \quad\) e. $\mathrm{NaCl}, \mathrm{Na}_{2} \mathrm{O}$ c. \(\mathrm{Mg}(\mathrm{OH})_{2}, \mathrm{MgO} \quad\) f. $\mathrm{MgO}, \mathrm{BaS}$

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