The Periodic Table

1. The Periodic Table www.assignmentpoint.com

2. Organizing the Elements • Demitri Mendeleeve (Russian – 1869) • Published the 1st periodic table • Based on atomic mass www.assignmentpoint.com

3. The Periodic Law • Modern Periodic Table • Organized according to atomic number Periods = rows 1-7 equal to the principal energy level Groups = columns 1-18 elements have similar properties Law: Properties of elements repeat as you move from Left→ Right across a period www.assignmentpoint.com

4. Period → Group ↓ www.assignmentpoint.com

5. Metallic Character • Approx. 2/3 of the elements are metals • Metallic Properties • Luster • Conductivity • Malleability • Ductility • Tend to lose electrons • Nonmetallic Properties • Dull luster • Poor conductors • Brittle • Tend to gain electrons • Metalloids (semimetals) • Some properties characteristic of metals and other properties characteristic of nonmetals www.assignmentpoint.com

6. Metals and Nonmetals Metalloids H 1 He 2 1 Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 2 Nonmetals Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 3 K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24 Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36 4 METALS Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag 47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 5 Cs 55 Ba 56 He 72 Ta 73 W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At 85 Rn 86 * 6 Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 W 7 La 57 Ce 58 Pr 59 Nd 60 Pm 61 Sm 62 Eu 63 Gd 64 Tb 65 Dy 66 Ho 67 Er 68 Tm 69 Yb 70 Lu 71 Ac 89 Th 90 Pa 91 U 92 Np 93 Pu 94 Am 95 Cm 96 Bk 97 Cf 98 Es 99 Fm 100 Md 101 No 102 Lr 103 www.assignmentpoint.com

7. decreases • Reference Table • Periodic Table • Trends: 1. Across a period, metallic character → Why? More electrons in outer shells Less tendency to lose electrons 2. Down a group, metallic character → Why? Less electrons in outer shells Greater tendency to lose electrons increases www.assignmentpoint.com

8. Metallic Review • Identify each element as a metal, nonmetal or metalloid • Gold - • Silicon - • Sulfur - • Barium - Metal Metalloid Nonmetal Metal www.assignmentpoint.com

9. boron • Which of these sets of elements have similar physical and chemical properties? • oxygen, nitrogen, carbon, • strontium, magnesium, calcium, beryllium • nitrogen, neon, , fluorine • Name 2 elements that have properties similar to those of the element sodium. nickel Any other Group 1 element: Lithium, Potassium, Rubidium, Cesium, Francium www.assignmentpoint.com

10. Nonmetal Metal • Identify each property below as more characteristic of a metal or a nonmetal • Brittle - • Malleable - • Poor conductor of electricity - • Shiny - • Tend to gain electrons - • In which pair of elements are the chemical properties of the elements most similar? • sodium and chlorine • nitrogen and phosphorus • boron and oxygen Nonmetal Metal Nonmetal www.assignmentpoint.com

11. Classifying the Elements Group 1 (1A) • Alkali Metals – • Alkaline Earth Metals – • Halogens – • Noble Gases – • Representative Elements – • Transition Elements – Group 2 (2A) Group 17 (7a) Group 18 (8A) Inert gases Groups 1A – 7A All Group B www.assignmentpoint.com

12. Label your Reference PeriodicTable… 1 18 H 1 He 2 1 2 15 14 13 17 16 Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 2 Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 3 3 4 5 6 11 7 8 10 12 9 K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24 Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36 4 Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag 47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 5 Cs 55 Ba 56 He 72 Ta 73 W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At 85 Rn 86 * 6 Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 W 7 La 57 Ce 58 Pr 59 Nd 60 Pm 61 Sm 62 Eu 63 Gd 64 Tb 65 Dy 66 Ho 67 Er 68 Tm 69 Yb 70 Lu 71 Ac 89 Th 90 Pa 91 U 92 Np 93 Pu 94 Am 95 Cm 96 Bk 97 Cf 98 Es 99 Fm 100 Md 101 No 102 Lr 103 www.assignmentpoint.com

13. Classifying Review • Which of the following are symbols for representative elements Na, Mg, , Cl? • Which of these metals is not a transition metal? • Aluminum • Silver • Iron • Zirconium Fe, Ni www.assignmentpoint.com

14. Atomic Radius • Atoms are roughly spherical • Sphere size can be determined using the radius • Problem: Edges of orbitals are fuzzy and difficult to measure… Solution: Atomic Radii – half the distance between the nuclei of identical atoms that are bonded together www.assignmentpoint.com

15. decreases • Reference Table: • Table S • Trends: 1. Across a period, the atomic radius → Why? Nuclei have larger positive charges Electrons are pulled in closer 2. Down a group, the atomic radius → Why? Greater number of energy shells Valence electrons are further away from the nucleus increases www.assignmentpoint.com

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17. Atomic Radius Review • Which element in each pair has a larger atomic radius? • & lithium • & bromine • carbon & • & neon • Arrange these elements in order of decreasing atomic size: sulfur, chlorine, aluminum, and sodium. Sodium → Aluminum → Sulfur → Chlorine sodium calcium germanium fluorine www.assignmentpoint.com

18. Ionization Energy • What is an ion? • An electrically charged atom • Atoms may either gain or lose electrons • Loss of electrons = (+) charge → • Gain of electrons = (-) charge → • Ionization energy= cation anion the amount of energy required to remove the most loosely bound electron A + energy A+ + e- www.assignmentpoint.com

19. increases • Reference Table • Table S • Trends: 1. Across a period, the ionization energy → Why? Electrons are held closer to the nucleus Electrons are more difficult to remove 2. Down a group, the ionization energy → Why? Electrons are further away from the nucleus Electrons are easier to remove Relate Back: decreases What type of relationship exists between ionization energy and atomic radii? Inverse www.assignmentpoint.com

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21. Ionization Review • Which element in each pair has a greater ionization energy? • lithium, • magnesium, • cesium, • Arrange the following groups in order of increasing ionization energy • Be, Mg, Sr • Bi, Cs, Ba • Na, Al, S boron strontium aluminum Be → Mg → Sr Bi → Ba → Cs Na → Al → S www.assignmentpoint.com

22. Ionic Size • Cations from when atoms loosee- The cation is smaller • Anions from when atoms gain e- The anion is larger www.assignmentpoint.com

23. decreases • Reference Table • No true table • Trends: 1. Across a period, ionic size → Why? When e- are lost, the attraction between the remaining e- increases e- are drawn closer to the nucleus 2. Down a group, ionic size → Why? Increased atomic radius e- are further away from the nucleus increases www.assignmentpoint.com

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25. Ion Size Review • Which particle has the larger radius in each atom/ion pair? • Na, • S, • I, • Al, • The ions Na+ and Mg2+ each have 10e-. Which ion would you expect to have a smaller ionic radius? Mg2+ atomic radius is smaller & e- are pulled in closer Na+ S2- I- Al3+ www.assignmentpoint.com

26. Electronegativity • A measure of the ability of an atom to attract a pair of electrons when bonded to another atom • Ability to ‘pull’ electrons from another atom Electrons pulled closer: Electrons pulled away: www.assignmentpoint.com

27. increases • Reference Table • Table S • Trends: 1. Across a period, the electronegativity → Why? Atoms are very close to a stable octet ‘Pull’ electrons from other atoms 2. Down a group, the electronegativity → Why? Top atoms have few electrons, and hold them tightly Bottom atoms have numerous electrons and little desire to acquire more decreases www.assignmentpoint.com

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29. Electronegativity Review • Which element in each pair has a higher electronegativity value? • Cl, • C, • Mg, • As, • Which element in each pair has a greater attraction for electrons? • Ca or • O or • S F N Ne Ca O F or K www.assignmentpoint.com

30. Summary Periodic Property Variation across a Period Variation down a Group Metallic Character Decreases Increases Atomic Radius Decreases Increases Ionization Energy Increases Decreases Decreases Ion Size Increases Electronegativity Increases Decreases www.assignmentpoint.com