The Atom and Periodic Table

1. The Atom and Periodic Table Chemistry: Unit 7

2. Atomic Model Scientists John Dalton 1803 John Dalton (Wikipedia.org)

3. Dalton’s Atomic Theory All matter is made up of tiny, unbreakable particles called atoms (Democritus proposed this in 460-370 BC) Atoms of the same element are identical, but they are different from atoms of other elements. Chemical reactions occur when atoms are separated, joined, or rearranged

4. Successes and Problems Verified theories and experiments by Democritus and Lavoisier (law of conservation of matter) and Proust (law of definite proportions). We know today that atoms are made of smaller particles and can be split, and there can be isotopes of the same element.

5. Atomic Model Scientists (cont.) Joseph John Thomson 1897 Found rays bent toward a positively charged plate and away from a negatively charged plate. Determined cathode rays are made up of negatively charged particles referred to as electrons.

6. JJ’s Successes (additions to jigsaw activity) Scientists were able to use JJ Thompson’s cathode ray tube to discover protons. (Rutherford; these had to balance the charge from the electrons) The amount of charge on an electron and proton is equal but opposite, but the mass of a proton is much greater that that of an electron.

7. Thompson Again! He also discovered that Neon consisted of atoms of two different masses. Later, these were called isotopes: atoms of an element that are chemically alike but differ in mass (# of neutrons). Scientists were then able to discover the neutron (1930s): a neutrally charged particle of equal mass to a proton.

8. Atomic Model Scientists (cont.) Ernest Rutherford 1911 Discovered the positively charged nucleus through gold foil experiment. Ernest Rutherford (Nobelprize.org)

9. Rutherford’s Gold Foil Experiment http://wps.prenhall.com/wps/media/objects/602/616516/Media_Assets/Chapter02/Text_Images/FG02_05.JPG

10. Atomic Model Scientists (cont.) Niels Bohr 1913 Niels Bohr (The University of New York)

11. Bohr Continued Rutherford’s atomic model did not explain the chemical properties of elements A description of the behavior of electrons was needed Bohr described fixed energy levels an electron can possess. In order to move up an energy level, energy must be absorbed and vice versa but energy is released The more energy an e- has, the further from the nucleus it is

12. Bohr concluded A quantum of energy is the amount of energy needed to move an e- from one level to the next The higher the energy level, the less energy it takes to move from that level to the next This idea failed to explain more complex elements… this is where Shrodinger comes in

13. Erwin Schroedinger(quantum mechanical model) Electrons are not stuck in a “planetary orbit,” or exact path, around the nucleus. Instead, they’re spherical regions, of space around the nucleus in which electrons are most likely to be found. You can’t determine the exact location of an e- Called “electron clouds” A region of space in which there is a high probability of finding an electron

14. Atomic Structure Atoms are made up of three subatomic particles: Subatomic = smaller than an atom Yes, substantial + In nucleus Yes, substantial none In nucleus Outside nucleus No, negligible -

15. Elements Substances made of only one type of atom Identified by atomic number (protons!!!) Can not be broken down into simpler substances

16. Element Symbols Shorthand name of the element Most are based on the Latin name Ex: Gold = Au The symbol is either: One capital letter -ex: Carbon = C Two letters…one capitol, one lower case -ex: Krypton = Kr

17. Determining Composition of atoms Number of neutrons = mass number – atomic number # of protons = atomic number If neutral atom… # protons = # electrons Charge is positive? That # fewer electrons than protons Charge is negative? That # more electrons than protons

18. Is a tool to organize the elements The Periodic Table of Elements…

19. By 1860, scientists had discovered 60 elements They noticed some elements had similar properties. They also noticed differences between the elements. Periodic Table Development

20. Atomic Model Scientists (cont.) Dmitri Mendeleev (Wikipedia.org) • Dmitri Mendeleev • 1869 • Developed a Periodic Table based on atomic mass

21. Dmitri Mendeleev (Wikipedia.org) Dmitri Mendeleev • 1869 • Developed a Periodic Table based on atomic mass • He left blank spaces

22. Dmitri Mendeleev • Realized chemical + physical properties of elements repeated in an orderly way. • Periodicity- the tendency to recur at regular intervals

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

24. Printable Periodic Tables Click on the element symbol to download the PDF file. Click Here All of the following tables are in Acrobat PDF format. To view and print these files, you will need to install the free Adobe Acrobat Reader program on your computer. The program can be downloaded from the Adobe Website. http://www.sciencegeek.net/index.html

25. Groups of Elements 1A 8A 1A 5A Nitrogen group Alkali metals H 1 2A 6A He 2 Alkaline earth metals Oxygen group 1 1 2A 7A 3A 4A 5A 6A 7A Halogens Transition metals 3A 8A Noble gases Boron group Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 2 2 4A Carbon group Hydrogen Inner transition metals Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 3 3 8B 3B 4B 5B 6B 7B 1B 2B 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 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 5 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 * * 6 6 Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 W W 7 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 W

26. Groups of Elements H 1 He 2 1 1 IA IIA IIIB IVB VB VIB VIIB VIIIB IB IIB IIIA IVA VA VIA VIIA VIIIA 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 Alkali metals Halogens 2 2 Other non-metals Alkaline earth metals Lanthanides Transition metals Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 Other metals Actinides 3 3 Noble gases 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 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 5 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 * * 6 6 Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 W W 7 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 W

27. Wikipedia Printable Periodic Table Elements listed Alphabetically

28. Periodic Table 8A Alkali metals 1A Alkaline earth metals He 2 H 1 Transition metals 1 1 3A 4A 5A 6A 7A 2A Boron group B 5 C 6 N 7 O 8 F 9 Ne 10 Li 3 Be 4 Nonmetals 2 2 Noble gases Si 14 P 15 S 16 Cl 17 Ar 18 Na 11 Mg 12 Al 13 3 3 8B 3B 4B 5B 6B 7B 1B 2B As 33 Se 34 Br 35 Kr 36 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 4 4 Te 52 I 53 Xe 54 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 5 5 At 85 Rn 86 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 6 6 Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 7 7 Lanthanoid Series 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 6 Solid C Actinoid Series Liquid Br 7 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 Gas H

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

30. Chinese Periodic Table http://www.limestone.on.ca/ibuild/davies/chinesept.html

31. Stowe’s Periodic Table

32. Benfrey’s Periodic Table

33. developed by Mohd Abubakr, Hyderabad, India

34. How to Organize Elements… Periodic Table Designs

35. 1894-1918 Ancient Times H He Midd. -1700 1923-1961 1965- 1735-1843 1843-1886 Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Rf Db Sg Bh Hs Mt Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Discovering the Periodic Table Journal of Chemical Education, Sept. 1989

36. Columns and Rows Called “groups” or “families” Called “periods”

37. Periods • An atom can have up to 7 energy levels of electrons. • An element’s period (row) tells us the number of …? • For example, a sodium (Na) atom has ____ electron orbitals? • Fluorine (F) has ____ electron orbitals?

38. Groups/ Families • An element’s family (aka group) tells us ...? • The outer 2 shells of the Group B elements are considered valence electron orbits. We will be able to ignore Group B for now. • For example Sodium (Na) has ____ valence electrons • Fluorine (F) has ____ valence electrons

39. Alkali Metals • Group 1A • Only one valence electron • VERY reactive!!!! • Hydrogen is NOT included

40. Group 2A Two valence electrons Not as reactive as the alkali metals Named because of where they are found on Earth Alkaline Earth Metals

41. Transition Metals • Found in the middle of the table • In the “B Groups” • Can change their number of valence electrons Bottom Rows are also known as the Rare Earth Metals!!!

42. Halogens • Group 7A • Seven valence electrons • VERY reactive!!!!

43. Noble Gases • Group 8A • 8 valence electrons—outer energy level is full • Very UNREACTIVE—what do they need to be 

44. Metalloids Metals and Nonmetals H 1 He 2 1 Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 Nonmetals 2 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 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 * 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

45. Diatomic Elements H2 He Ne Li O2 F2 N2 Be B C Ar S Al P Na Si Cl2 S Mg Sc Ca Mn Co Cu Se K Ti Cr Fe Ni Zn Ga As Br2 V Ge Kr Y Sr Tc Rh Ag Te Rb Zr Mo Ru Pd Cd In Sb Nb Sn Xe I2 Tl La Ba Re Ir Au Po At Cs Hf W Os Pt Hg Tl Bi Ta Pb Rn Fr Ra Ac Nd Pr Gd Dy Er Ce Pm Eu Tb Ho Tm Yb Sm Lu U Pa Cm Cf Fm Th Np Am Bk Es Md No Pu Lr

46. Alkali Metals, Group 1 H He Ne Li O F N Be B C Ar S Al P Na Si Cl Mg Sc Ca Mn Co Cu Se K Ti Cr Fe Ni Zn Ga As Br V Ge Kr Y Sr Tc Rh Ag Te Rb Zr Mo Ru Pd Cd In Sb Nb Sn Xe I La Ba Re Ir Au Po At Cs Hf W Os Pt Hg Tl Bi Ta Pb Rn Fr Ra Ac Nd Pr Gd Dy Er Ce Pm Eu Tb Ho Tm Yb Sm Lu U Pa Cm Cf Fm Th Np Am Bk Es Md No Pu Lr

47. Alkaline Earth Metals, Group 2 H He Ne Li O F N Be B C Ar S Al P Na Si Cl Mg Sc Ca Mn Co Cu Se K Ti Cr Fe Ni Zn Ga As Br V Ge Kr Y Sr Tc Rh Ag Te Rb Zr Mo Ru Pd Cd In Sb Nb Sn Xe I La Ba Re Ir Au Po At Cs Hf W Os Pt Hg Tl Bi Ta Pb Rn Fr Ra Ac Nd Pr Gd Dy Er Ce Pm Eu Tb Ho Tm Yb Sm Lu U Pa Cm Cf Fm Th Np Am Bk Es Md No Pu Lr

48. Halogens, Group 17 H He Ne Li O F N Be B C Ar S Al P Na Si Cl Mg Sc Ca Mn Co Cu Se K Ti Cr Fe Ni Zn Ga As Br V Ge Kr Y Sr Tc Rh Ag Te Rb Zr Mo Ru Pd Cd In Sb Nb Sn Xe I La Ba Re Ir Au Po At Cs Hf W Os Pt Hg Tl Bi Ta Pb Rn Fr Ra Ac Nd Pr Gd Dy Er Ce Pm Eu Tb Ho Tm Yb Sm Lu U Pa Cm Cf Fm Th Np Am Bk Es Md No Pu Lr

49. Noble Gases, Group 18 H He Ne Li O F N Be B C Ar S Al P Na Si Cl Mg Sc Ca Mn Co Cu Se K Ti Cr Fe Ni Zn Ga As Br V Ge Kr Y Sr Tc Rh Ag Te Rb Zr Mo Ru Pd Cd In Sb Nb Sn Xe I La Ba Re Ir Au Po At Cs Hf W Os Pt Hg Tl Bi Ta Pb Rn Fr Ra Ac Nd Pr Gd Dy Er Ce Pm Eu Tb Ho Tm Yb Sm Lu U Pa Cm Cf Fm Th Np Am Bk Es Md No Pu Lr

50. Chalcogens, Group 16 H He Ne Li O F N Be B C Ar S Al P Na Si Cl Mg Sc Ca Mn Co Cu Se K Ti Cr Fe Ni Zn Ga As Br V Ge Kr Y Sr Tc Rh Ag Te Rb Zr Mo Ru Pd Cd In Sb Nb Sn Xe I La Ba Re Ir Au Po At Cs Hf W Os Pt Hg Tl Bi Ta Pb Rn Fr Ra Ac Nd Pr Gd Dy Er Ce Pm Eu Tb Ho Tm Yb Sm Lu U Pa Cm Cf Fm Th Np Am Bk Es Md No Pu Lr