4s 3d 4s 3d Ni 1! 1 11 l1l (Ar)3dº4s? 4s 3d 4s 3d Zn 1 11 11 I iL I1 (Ar]3d104s? 3d Shown above are actual electron configurations for the indicated atoms. Which of these is not the configuration predicted by theory? Explain why the metal has that particular configuration. Please type your answer below.

Using partial orbital diagrams explain why arsenic can acquire charges of 3- and 3+ but not 2+

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

19. Based on the information given below, give the group, period, block, and identity of each element described. (Hint: See Sample Problem B.) a. [He]2s² b. [Ne]3s¹ c. [Kr]5s² d. [Ar]4s² e. [Ar]3d³4s¹ Without looking at the periodic table, write the expected outer electron configuration for each of the following elements. (Hint: See Sample Problem C.) a. Group 7, fourth period b. Group 3, fifth period

The first ionization energy shows an overall increase from left to right across a period as shown in the diagram below for 2nd period elements. 2nd period 2100 1700 S 1300 900 A. 500 A Li Be B C NO F Ne a) Define the first ionization energy a) Why the first ionization energy of boron (B) is less than that of beryllium (Be) and why the first ionization energy of oxygen (O) is less than that of nitrogen (N)? Explain 1st ionization energy /kJ mol

5) Why does copper (Cu) easily lose and electron from its s subshell instead of its d shell when forming a Cu ion? What does this have to do with the stability of the atom? Explain the difference between electron affinity and first ionization energy. Why does ionization energy for an atom increase for each additional e

jlpa

x |H|V R E S You will use the known periodic trends to compare properties for elements indicate with letters in this periodic table. Consider their relative positions for these questions. Your answers will be letters as indicated above, not the actual element symbol they would coordinate to. (Do not use a real periodic to answer this question.) ● Which alkali metal would be expected to have the lowest first ionization energy? BI H O N> T D LIQ A 0

Each metal has a different energy at which it ejects electrons. At lower energy, electrons are not emitted True or False?

Molecules can be paramagnetic or diamagnetic. Which of the following is INCORRECT? a. Mercury: diamagnetic b. Cesium: paramagnetic c. Krypton: diamagnetic d. Zinc: paramagnetic Given the following ionization energies (kJ/mol) of a certain element, predict which group does it belong. IE, = 418.81 IE2 = 3051.35 IE3 = 4419.30 IE, = 5878.00 a. Group 1 b. Group 2 c. Group 3 d. Group 4