Compare the electron affinity of fluorine to the ionization en- ergy of sodium. Does the process of an electron being "pulled" from the sodium atom to the fluorine atom have a negative or a positive AE? Why is NaF a stable compound? Does the overall formation of NaF have a negative or a positive AE? How can this be?

Compare the electron affinity of fluorine to the ionization en- ergy of sodium. Does the process of an electron being "pulled" from the sodium atom to the fluorine atom have a negative or a positive AE? Why is NaF a stable compound? Does the overall formation of NaF have a negative or a positive AE? How can this be?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter8: Bonding: General Concepts

Section: Chapter Questions

Problem 64E: Compare the electron affinity of fluorine to the ionization energy of sodium. Does the process of an...

See similar textbooks

Similar questions

Compare the electron affinity of fluorine to the ionization energy of sodium. Does the process of an electron being pulled from the sodium atom to the fluorine atom have a negative or a positive E? Why is NaF a stable compound? Does the overall formation of NaF have a negative or a positive E? How can this be?
Which of the following atoms contains only three valence electrons: Li, B, N, F, Ne?
Mat type of bond is likely to form between one element with low ionization energy and another element with high electron affinity? Explain your answer.
The lattice energy of an ionic solid such as NaCl is the enthalpy change H for the process in which the solid changes to ions. For example, NaCl(s)Na+(g)+Cl(g)H=786kJ/mol Assume that the ionization energy and electron a affinity are H values for the processes defined by those terms. The ionization energy of Na is 496 kJ/mol. Use this, the electron affinity from Table 8.4, and the lattice energy of NaCl to calculate H for the following process: Na(g)+Cl(g)NaCl(s)
Write the electron configuration for each of the following ions: (a) As3 (b) I (c) Be2+ (d) Cd2+ (e) O2 (f) Ga3+ (g) Li+ (h) N3 (j) Sn2+ (j) Co2+ (k) Fe2+ (1) As3+
Give three ions that are isoelectronic with neon. Place these ions in order of increasing size.
Which of the following statements is correct and provides the best explanation when removing the first two electrons from calcium? Energy is released when either electron comes off because calcium is a metal and not very electronegative. It takes less energy to remove the second electron from calcium compared with the first because calcium wants to have eight electrons in its outer shell (and thus have a noble gas configuration. It takes less energy to remove the first electron compared with the second because it is in a higher energy level than the second electron. Electrons cannot be removed from calcium because it is a metal and only wants to gain electrons to become more stable. It takes more energy to remove the second electron compared with the first because the nucleus binds the electrons more tightly as each electron is removed.
Fluoride ion, F, has no unpaired electrons. Vanadium forms four binary fluoridesVF2, VF3, VF4, and VF5. Assume that all four are ionic compounds. (a) Which fluoride is diamagnetic? (b) Which fluoride has the greatest attraction to a magnetic field? (c) Which fluoride has two unpaired electrons per vanadium?
In the chemical process called electron transfer, an electron istransferred from one atom or molecule to another. A simpleelectron transfer reaction isA(g) + A(g)---->A+(g) + A-(g) In terms of the ionization energy and electron affinity ofatom A, what is the energy change for this reaction? For arepresentative nonmetal such as chlorine, is this process exothermic?For a representative metal such as sodium, is thisprocess exothermic?
18 - for Cl, Cl + and Cl- ions;Cl- is the largest number of electronsII. Stripping electrons from the Cl + ion is most difficultIII. Neutral Cl atom and Cl- ions have equal radiiWhich of his judgments are correct? A) Only IIIB) I, IIC) I, IIID) I onlyE) I, II, III