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Names: Period: Chemistry Extension: Electrons and the Periodic Table The periodic table is the chemist’ s most basic and, perhaps, most useful tool. We have seen that the periodic table can be used to predict properties of the elements such as boiling point, melting point, and formation of oxides and chlorides, but its usefulness does not end there. An element’s reactivity can be determined by actually combining it with a variety of other substances. but this is not always practical or safe. Since an elemen t’s reactivity is dependent upon the electron arrangements in its atoms, knowing the electro n arrangements is helpful information in predicting reactivity. Specifically, the arrangement or configuration of the outermost or valence electrons is the most important information. In this activity, you will determine the relationship between an element’s position on the periodic table and the element’s valence electron configuration. When you have finished, you should be able to predict an element’s electron structure and, therefore, its reactivity based on the periodic table alone. The valance electron configuration is made up of three pieces of inform ation which each receives its own notation. The first piece of information is energy level or shell, which is noted using whole number integers (1,2,3...). Next are the sublevels represented by one of four letter; s, p, ci, f Finally, an exponent raised to the sublevel letter represents the numbers of electrons contain ed within a given number of orbitals found in that particular sublevel. 1 Example: Lithium (Li): I S 2 LS 1 From the example above, one could determine that an atom of the elemen t Lithium has 2 electrons in the s-sublevel of the first energy level and 1 electron in the s-sublevel of the second energy level. 1. Based upon the definition for valence electrons given in the background information, devise a definition for valence shell. 2. Examine groups 1, 2 and 13-18 on the periodic table and identify two patterns that can be observed regarding the valence electrons and valence shells. 3. Using the patterns identified in question #2, predict the following information for the elements indicated: Cs S a. number corresponding to the valence shell b. sublevel(s) which contain valence electrons c. number of valence electrons 4. Examine the periods on the periodic table and identify two patterns that can be observed regarding the valence electrons and valence shells. 5. Using the patterns identified in question #4, predict the following information for the elements indicated: Mg Sn a. number corresponding to the valence shell b. sublevel(s) which contain valence electrons c. number of valence electrons 6. Complete all empty squares on the periodic table using the same format and infonnation provided for the other elements. 7. When elements react to form ionic compounds, the atoms either lose or gain electrons to form ions with filled valence shells since this is the most stable electron structure. Based on your determination of trends in electron structure on the periodic table, at the top of each group, write the charge for the ions formed from atoms in groups 1, 2, 13, and 16-18. s and it bonds with element Z 1p 2 2 3 3 4 6 8. If element X has an electron arrangement of 2 s what would the formula of the 2p 1s 2 3 6 3 2 , which has an electron arrangement of 5 resulting compound be, in terms of X and Z? (Hint: Figure out the charge of elements X and Z and then write the corresponding formula.) 9. Suggest why the metals in group 1 might be the most reactive metals. +1 IsZ2si +1 1 Is +1 Fr +1 [KrI5s’ +1 [RiiI7s’ Cs ÷i [Arj4s’ Rb K — I2 2 s 2 p3s’ s Na Li [1 - +2 2 [KrJ5s +2 [Rn Ra 751 +2 2 [XeJ(,s Ba Sr +2 2 [ArJ4s Ca +2 2s 2 1s Mg Be 2 — — — — — — 567 8 9 11 — — 12 + +3 +I+3 XJ6s 6 2 p’ TI tKrj5s 5 t p’ In [Ar]4s 4 2 i a 1 2 1s 2 3 6 3 2 p s +3 -4,+2, +4 2p 1s 2 2 s -4,+2, +4 +2,+4 6p 2 [Xe]6s Pb Sn 4p 2 [Arj4s GC÷ , 2 ±4 2p 1s 2 3 6 3 2 s Si C 14 I -3 -3 3 2 ls 2 2 p s 15 -3 - 1 6 2 [Xej6s p Bi 3 5 2 rj5s p Sb 3 4 2 [ArJ4s p As -2 -2 16 +2,+4 [Xejós 6 2 p’ Po -2 1t\14s 4 2 l S S 0 Charges 3 2 1s 2 3 2 p”3s p s P IN anJ I -i ] 6 2 p At [Kuj5s 5 2 p -i The numbers at the bottom of each square represent the electrons and the regions of space they occupy 1 he larger numbers represent the energy level where electrons might be found, while the superscripts represent the number of electrons in that particular energy level. The letter (s or p) represents the sublevel(s) in which the electrons are found. —- 1s 0 Rn Xc o 0 [Aij4s 4 2 p o 2p 1s 2 3 6 3 2 s Ar Ne Ic -iKr [\J4s 4 2 p Fr 1 -i 2p3s 2 s2s 3 p Fl 2s22 F 17 The charge(s) for the ion(s) formed ilom atoms of each element are shown in the upper right corner of each square Some elements have other possible charges in addition to those indicated. 10 +3 2 2 1s 2 p’ s Al B 13 Periodic Table with Electrons 18