9. Explain why the electrons depicted in the diagram below are placed as far apart as possible. . • Si • Use the diagr

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9. Explain why the electrons depicted in the diagram below are placed as far apart as possible. . • Si •
Use the diagram below to answer questions 10 to 12. H He 13 4 17 B 19 10 Li Be | В IC IN o Ne e և : Ե 11 12 13 14 15 16 18 Na Si IP IS Ar 19 Mg 20 Ca 21 22 23 24 26 127 28 29 30 AI 31 Ga 32 33 34 25 Mn 35 K SC Ti V Cr Fe Co Ni Cu Zn Ge As Se Br Kr 37 39 41 42 43 44 145 46 47 49 SO 52 153 40 Zr 48 cd 51 Sb 54 Xe Rb Sr Y Nb Mo TC Ru Rh Pd Ag In Sn Te 155 56 57 72 73 74 75 76 77 TO 79 B0 181 82 B3 14 CS Ba La HE Ta W Re Os Pt Au Rn Hg 112 87 99 ווין 80 Ra 104 RE 118 105 Db lir 109 Mt 106 Sg 107 Bh 100 Hs ITI IPb Ві Ро At 113 114 115 116 Uut Uuq Uup Uuh* 110 Ds Fr [Ac Rg Cn Uuo 10. Define the following terms. a. atomic radius C. electronegativity b. electron affinity d. ionization energy 11. For each term in question 10, describe how the values of this property change a. down a group b. from left to right across a period 12. The colour codes in this periodic table divide elements into categories that highlight their unique chemical properties. Name the category highlighted by each colour below and describe the properties of the elements in this category. a. yellow c. brown b. purple
13. Write a caption to explain what is occurring in the following diagram. Na Na a:-( l'a. :-(M$ 17 1933: O Mg:0:- :O: 14. Describe the octet rule and explain why certain elements do not follow this rule. 15. Draw Lewis diagrams for the following ionic compounds containing transition metals. a. Fe2O3 b. FeCl2
16. Which statement best describes a covalent bond? a. A bond that involves an uneven distribution of electrons. b. The electrostatic attraction between positively charged electrons and negatively charged nuclei. c. The attractive electrostatic force between a negative ion and a positive ion. d. The attraction between atoms that results from the sharing of electrons. e. none of the above 17. Compare and contrast the concepts of lone pair and bonding pair.