Use the data table for the first eight ionization energies of a particular element shown below to predict and explain which element you would expect to show this trend in successive ionization energ Ionization Number 1st 2nd 3rd 4th 5th 6th 7th 8th 1. I and III 2. II and III 3. I and IV 4. II and IV Ionization Energy (kJ/mol) 04 1,314 3,388 5,300 7,469 10,990 13,327 71,330 I.Fluorine II.Oxygen Because III.core electrons are more strongly attracted to the nucleus than valence electrons. IV.valence electrons release more energy when they are removed from the atom. 84,078

Use the data table for the first eight ionization energies of a particular element shown below to predict and explain which element you would expect to show this trend in successive ionization energ Ionization Number 1st 2nd 3rd 4th 5th 6th 7th 8th 1. I and III 2. II and III 3. I and IV 4. II and IV Ionization Energy (kJ/mol) 04 1,314 3,388 5,300 7,469 10,990 13,327 71,330 I.Fluorine II.Oxygen Because III.core electrons are more strongly attracted to the nucleus than valence electrons. IV.valence electrons release more energy when they are removed from the atom. 84,078

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Two sets of ionizations are shown in the tables below. Complete the tables by ordering each set of ionizations by increasing amount of energy required. In other words, for each set choose "1" next to the ionization that would require the least energy, "2" next to the ionization that would require the next least energy, and so on. F-> F+ + e- Ca-> Ca+ + e- He-> He+ + e- ------------------ Ra-> Ra+ + e- Xe-> Xe+ + e- He-> He+ + e-
Two sets of ionizations are shown in the tables below. Complete the tables by ordering each set of ionizations by increasing amount of energy required. In other words, for each set choose "1" next to the ionization that would require the least energy, "2" next to the ionization that would require the next least energy, and so on. He-> He+ + e- Fr-> Fr+ + e- Na-> Na+ + e- ---------------- Na-> Na+ + e- F->F+ + e- Fr-> Fr+ + e-
Arrange the following set of elements in order of increasing first ionization energies. Ne N Li B C O
Which one of these ions is not isoelectronic with Ar? A. S²- B. Ca2+ C. Fe2+ D. CH E. K+
11. How do the core charges for H, Li, and Na compare to each other? Based on this answer and their respective ionization energies, which species has the valence shell with the largest radius? Which has the valence shell with the smallest radius? 12. Can you deduce a trend in ionization energy as you move from left to right across a period (row)? Can you deduce a trend in core charge as you move from left to right across a period (row)? Explain.
Examine the following set of ionization energy values for a certain element. How many valence electrons does an atom of the neutral element possess? Ionization step Ionization Energy (kJ/mol) Ei1 1012 Ei2 1903 Ei3 2912 Ei4 4956 Ei5 6273 Ei6 22233 Ei7 25997 Enter the answer numerically as an integer.
5. Explain, using Coulomb's law, the general trend in second and successive ionization energies across a period for main group Element Na 496 4560 Mg 738 1450 7730 Core electrons elements. Al 578 1820 2750 11,600 SI 786 1580 3230 4360 16,100 1012 1900 2910 4960 6270 22,200 1000 2250 3360 4560 7010 8500 27,100 CI 1251 2300 3820 5160 6540 9460 11,000 Ar 1521 2670 3930 5770 7240 8780 12,000
MISSED THIS? Read Section 9.7 (Pages 371 - 379). Part A Consider the following set of successive ionization energies: To which third-period element do these ionization values belong? IE = 578 kJ/mol Express your answer as an element symbol. IE2 = 1, 820 kJ/mol IES = 2, 750 kJ/mol 11, 600 kJ/mol IE4 Submit Request Answer
11. The first five ionization energies of an element in period 3 is shown in the graph below. Predict the element and explain why there is a large jump in energy between the 3rd and 4th ionization. Your explanation should reference the attractive forces within an atom and include an energy orbital diagram. IE5 IE4 IE3 IE, IE, Energy (kJ/mol)
MISSED THIS? Read Section 9.7 (Page). Consider the following set of successive ionization energies: IE₁ 578 kJ/mol IE2 = 1, 820 kJ/mol IE3 = 2, 750 kJ/mol IE4 11,600 kJ/mol = = Part A To which third-period element do these ionization values belong? Express your answer as an element symbol. Submit Request Answer
Arrange strontium, cesium, iodine, and lead in order of increasing atomic size using general periodic table trends. Cs < Sr < Pb < I I < Sr < Pb < Cs Sr < Cs < I < Pb Sr < I < Cs < Pb
Using the data in the tables and Coulomb's law, calculate the energy change for this reaction (per formula unit of CaS). Ca(g) + S(g) → CaS(g) Ionization energy Atom Mg Ca Electron affinity Atom O S Ionic radius Ion Mg²+ Ca²+ 0²- S²2- I₁ (aJ) 1.23 0.980 EA₁ (aJ) -0.234 -0.332 I₂ (aJ) 2.41 1.90 EA₂ (aJ) +1.30 +0.980 Radius (pm) 72 100. 140. 184 ▲Erxn = 6.76 Incorrect aJ