1. Aliens Activity Nautilus shell has a repeating pattern. Look carefully at the drawings of the ‘aliens’. Organize all the aliens into a meaningful pattern. Aliens LabAliens Lab Cards Cards

2. How to Organize Elements…

3. How to Organize… Baseball Cards: year, team, player, card number, value ($). Elements: when they were discovered, family, reactivity, state of matter, metal vs. non-metal, atomic mass, atomic number. alphabetically, mass, value, density, solid or liquid or gas Which way is CORRECT to organize the elements? Is it possible to organize the elements correctly in more than one way?

4. Li 3 H1H1 He 2 C6C6 N7N7 O8O8 F9F9 Ne 10 Na 11 B5B5 Be 4 H1H1 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 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 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 Cs 55 Ba 56 Hf 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 Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 Mg 12 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 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 La 57 Ac 89 1 2 3 4 5 6 7   P A6A6 H1H1 S 16 e The Human Element Interactive Periodic Table

5. Dutch Periodic Table 106 107 108 109 110 111 112 113 114 115 116 117 118 Strong, Journal of Chemical Education, Sept. 1989, page 743

6. Stowe’s Periodic Table

7. Benfey’s Periodic Table

8. Periodic Table 1 2 3 4 5 6 7 Li 3 He 2 C6C6 N7N7 O8O8 F9F9 Ne 10 Na 11 B5B5 Be 4 H1H1 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 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 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 Cs 55 Ba 56 Hf 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 Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 Mg 12 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 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 La 57 Ac 89 1 2 3 4 5 6 7 1A 2A Alkali metals Alkali earth metals Transition metals Boron group Nonmetals Noble gases 3B 5B6B7B 8B 1B2B 3A4A5A6A7A 8A 4B Lanthanoid Series 6 7 Actinoid Series C Solid Br Liquid H Gas

9. Periodic Table "...if all the elements be arranged in order of their atomic weights a periodic repetition of properties is obtained." - Mendeleyev Chemists use the properties of elements to sort them into groups. What kinds of properties do elements have?

10. Mendeleev’s Periodic Table Russian scientist Mendeleev arranged elements in his periodic table in order of increasing atomic Mass. What is the difference between atomic number and atomic mass?

11. Dmitri Mendeléev

12. Mendeleev’s Periodic Table Period 1 Group I IIIIIIVVVIVIIVIII H = 1 2 Li = 7Be= 9.4B = 11C = 12N = 14O = 16F = 19 3 Na = 23Mg = 24Al = 27.3Si = 28P = 31S = 32C = 35.5 4 K = 39Ca = 40? = 44Ti = 48V = 51Cr = 52Mn = 55 Fe =56, Co = 59, Ni = 59 5 Cu = 63Zn = 65? = 68? = 72As = 75Se = 78Br = 80 6 Rb = 85Sr = 87? Yt = 88Zr = 90Nb = 94Mo = 96? = 100 Ru= 104, Rh = 104, Pd = 106 7 Ag = 108Cd = 112In = 113Sn = 118Sb = 122Te = 125J = 127 8 Cs = 133Ba = 137?Di = 138?Ce = 140 9 10 ?Er = 178?La = 180Ta = 182W = 184 Os = 195, Ir = 197, Pt = 198 11 Au = 199Hg = 200Tl = 204Pb = 207Bi = 208 12 Th = 231U = 240

13. Elements Properties are Predicted PropertyMendeleev’s Predictions in 1871Observed Properties Molar Mass Oxide formula Density of oxide Solubility of oxide Scandium (Discovered in 1877) 44 g M 2 O 3 3.5 g / ml Dissolves in acids 43.7 g Sc 2 O 3 3.86 g / ml Dissolves in acids Molar mass Density of metal Melting temperature Oxide formula Solubility of oxide Gallium (Discovered in 1875) 68 g 6.0 g / ml Low M 2 O 3 Dissolves in ammonia solution 69.4 g 5.96 g / ml 30 0 C Ga 2 O 3 Dissolves in ammonia Molar mass Density of metal Color of metal Melting temperature Oxide formula Density of oxide Chloride formula Density of chloride Boiling temperature of chloride Germanium (Discovered in 1886) 72 g 5.5 g / ml Dark gray High MO 2 4.7 g / ml MCl 4 1.9 g / ml Below 100 o C 71.9 g 5.47 g / ml Grayish, white 900 0 C GeO 2 4.70 g / ml GeCl 4 1.89 g / ml 86 0 C O’Connor Davis, MacNab, McClellan, CHEMISTRY Experiments and Principles 1982, page 119,

14. Modern Periodic Table In the Modern Periodic table, elements are arranged in order of increasing atomic number. (not mass like Mendeleev proposed. But the pattern of properties within a period repeats this is called the periodic law Periodic Law states: When elements are arranged in order of increasing atomic number there is a periodic repetition of their physical and chemical properties.

15. Physical Chemical Properties: What’s the difference? Physical Properties : a quality or condition of a substance that can be observed or measured without changing the substance’s composition Examples : State of matter (solid, liquid, gas), Color, Melting point, Boiling Point Chemical Properties: the qualities and conditions that allow a substance to undergo change. Examples: any change that creates a new substance

16. Introduction to the Periodic Table Elements are arranged in seven horizontal rows, in order of increasing atomic number from left to right and from top to bottom. Rows are called periods and are numbered from 1 to 7. Elements with similar chemical properties form vertical columns, called groups, which are numbered from 1 to 18. Groups 1, 2, and 13 through 18 are the main group elements. Groups 3 through 12 are in the middle of the periodic table and are the transition elements. The two rows of 14 elements at the bottom of the periodic are the lanthanides and actinides. Copyright 2007 Pearson Benjamin Cummings. All rights reserved.

17. Major families in the periodic table Group 1 (except for hydrogen) – Alkali Metals Most reactive group of metals Flammable in air and water Form ions with +1 charge Low Melting Point and Boiling Point (MP of Li = 181º C, Na = 98º C) Soft (Na can be cut with a knife) Has one outer (valance) electron

18. Major families in the periodic table Group 2 – Alkali Earth Metals Reactive, but less so than alkali metals React in air and water (show Ca reacting in water) Form ions with +2 charge Low MP and BP, but higher than alkali metals (MP of Ba= 302º C, Mg = 649ºC Soft, but harder than alkali metals Has two outer / valance electrons

19. Major families in the periodic table Groups 3-12: (Outer) transition metals Note: These are general properties and may vary from transition metal to transition metal! There are many exceptions to each of these rules! Stable and unreactive. Hard High MP and BP (Fe = 1535º C, Ti = 1660º C). Form ions with various positive charges (usually include +2 and several others) Used for high strength/hardness applications, electrical wiring, jewelry

20. Major families in the periodic table Lanthanides – the inner transition metals Also called the rare earth metals, because they’re rare. Usually intermediate in reactivity between alkaline earth metals and transition metals. High MP and BP Used in light bulbs and TV screens as phosphors.

21. Major families in the periodic table Actinides (more inner transition metals) Many have high densities Most are radioactive and manmade Melting points vary, but usually higher than alkaline earth metals. Reactivity varies greatly Used for nuclear power/weapons, radiation therapy, fire alarms.

22. Major families in the periodic table Metalloids The bonding in metalloids is between that of metals and nonmetals, so metalloids have properties of both. Some metalloids are shiny (silicon), some are not (gallium) Metalloids tend to be brittle, as are nonmetals. Metalloids tend to have high MP and BP like metals. Metalloids tend to have high density, like metals. Metalloids are semiconductors of electricity – somewhere between metals and nonmetals. This makes them good for manufacturing computer chips.

23. Major families in the periodic table Non-Metals Bonds between the atoms, cause each of the properties below. Again, these are g eneral properties and may not be true for all nonmetals. Brittle Poor conductors of heat and electricity Low density Low MP and BP (many are gases)!

24. Group 17: Halogens The most highly reactive nonmetals. Highly volatile – F and Cl are gases, Br is a volatile liquid, and I is an easily sublimed solid. Strong oxidizers – they readily pull electrons from other atoms. Diatomic – form molecules with formula of X 2 Form ions with -1 charge Used in water treatment and chemical production – Cl 2 was used as a chemical weapon in World War I.

25. Major families in the periodic table Group 18: Noble Gases Highly unreactive Used to provide the atmosphere in situations where you don’t want chemical reactions to occur (light bulbs, glove boxes, etc).

26. Major families in the periodic table Hydrogen – “The Weirdo” Has properties unlike any other element Diatomic – H 2 Can form either a +1 or -1 charge Relatively unreactive unless energy is added (under most conditions) – it can form explosive mixtures with oxygen (as it did in the Hindenburg explosion)

27. First &Most important Periodic Pattern: Number of Valance Electrons 1 1 3 4 5 6 7 2435 8 7 6