THE PERIODIC TABLE

History Mid 1800’s – 70 known elements Dmitri Mendeleev - 1st to arrange elements systematically & logically Column by increasing atomic mass Arranged columns by similar properties Left blanks (no known element with right mass and properties)

Mendeleev’s Periodic Table Ti = 50 Zr = 90 ? = 180 V = 51 Nb = 94 Ta = 182 Cr = 52 Mo = 96 W = 186 Mn = 55 Rh = 104.4 Pt = 197.4 Fe = 56 Ru = 104.4 Ir = 198 Ni = Co = 59 Pl = 106.6 Os = 199 H = 1 Cu = 63.4 Ag = 108 Hg = 200 Be = 9.4 Mg = 24 Zn = 65.4 Cd = 112 B = 11 Al = 27.4 ? = 68 Ur = 116 Au = 197? C = 12 Si = 28 ? = 70 Sn = 118 N = 14 P = 31 As = 75 Sb = 122 Bi = 210 O = 16 S = 32 Se = 79.4 Te = 128? F = 19 Cl = 35.5 Br = 80 I = 127 Li = 7 Na = 23 K = 39 Rb = 85.4 Cs = 133 Tl = 204 Ca = 40 Sr =87.6 Ba = 137 Pb = 207 ? = 45 Ce = 92 ?Er = 56 La = 94 ?Yt = 60 Di = 95 ?In = 75.6 Th = 118?

History cont’d. 1913 – Henry Moseley (British physicist) determined the atomic numbers of the elements Periodic Table was rearranged according to atomic numbers. Current arrangement

Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 3 1 H 2A 3A 4A 5A 6A 7A 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 11 Na 12 Mg 3B 4B 5B 6B 7B 8B 1B 2B 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 19 K 20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo 43 Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 55 Cs 56 Ba 57 La 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 85 At 86 Rn 87 Fr 88 Ra 89 Ac 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 111 112 114 116 118 Lanthanide Series 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu Actinide Series 90 Th 91 Pa 92 U 93 Np 94 Pu 95 Am 96Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr

The Periodic Law Elements have a periodic repetition of their physical and chemical properties when arranged by increasing atomic number.

Types of Elements Metals

Metals (characteristics due to the sea of free moving electrons) Lustrous (shiny) appearance Malleable & ductile Conduct heat & electricity Tend lose e- to form cations Located on left side of table Generally solids at room temperature Mercury – liquid React with acids (some)

Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 3 1 H 2A 3A 4A 5A 6A 7A 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 11 Na 12 Mg 3B 4B 5B 6B 7B 8B 1B 2B 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 19 K 20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo 43 Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 55 Cs 56 Ba 57 La 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 85 At 86 Rn 87 Fr 88 Ra 89 Ac 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 111 112 114 116 118 Lanthanide Series 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu Actinide Series 90 Th 91 Pa 92 U 93 Np 94 Pu 95 Am 96Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr

Types of Elements Metals Nonmetals

Nonmetals Dull appearance Brittle Poor conductors of heat & electricity Tend to gain e- to form anions Located on right side of table Hydrogen on the left Many are gases at room temperature Do not react with acids

Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 3 1 H 2A 3A 4A 5A 6A 7A 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 11 Na 12 Mg 3B 4B 5B 6B 7B 8B 1B 2B 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 19 K 20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo 43 Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 55 Cs 56 Ba 57 La 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 85 At 86 Rn 87 Fr 88 Ra 89 Ac 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 111 112 114 116 118 Lanthanide Series 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu Actinide Series 90 Th 91 Pa 92 U 93 Np 94 Pu 95 Am 96Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr

Types of Elements Metals Nonmetals Metalloids

Metalloids Lie between metals and nonmetals on the table (stair-step) Have properties of both metals and non metals Mainly solids at room temperature

Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 3 1 H 2A 3A 4A 5A 6A 7A 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 11 Na 12 Mg 3B 4B 5B 6B 7B 8B 1B 2B 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 19 K 20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo 43 Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 55 Cs 56 Ba 57 La 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 85 At 86 Rn 87 Fr 88 Ra 89 Ac 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 111 112 114 116 118 Lanthanide Series 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu Actinide Series 90 Th 91 Pa 92 U 93 Np 94 Pu 95 Am 96Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr

Symbol Colors Natural state at room temperature Black – solids Red – gases Blue (green) – liquids White – man made elements

Table Organization Rows – periods (1-7)

1 Lanthanide Series Actinide Series H 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 11 Na 12 Mg 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 19 K 20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo 43 Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 55 Cs 56 Ba 57 La 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 85 At 86 Rn 87 Fr 88 Ra 89 Ac 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 111 112 114 116 118 Lanthanide Series 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu Actinide Series 90 Th 91 Pa 92 U 93 Np 94 Pu 95 Am 96Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr

Table Organization Rows – periods (1-7) Columns – groups or families 1A – 8A Representative elements s-block & p-block 1B – 8B

Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 3 1 H 2A 3A 4A 5A 6A 7A 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 11 Na 12 Mg 3B 4B 5B 6B 7B 8B 1B 2B 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 19 K 20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo 43 Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 55 Cs 56 Ba 57 La 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 85 At 86 Rn 87 Fr 88 Ra 89 Ac 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 111 112 114 116 118 Lanthanide Series 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu Actinide Series 90 Th 91 Pa 92 U 93 Np 94 Pu 95 Am 96Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr

Group Names 1A – Alkali Metals

Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 3 1 H 2A 3A 4A 5A 6A 7A 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 11 Na 12 Mg 3B 4B 5B 6B 7B 8B 1B 2B 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 19 K 20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo 43 Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 55 Cs 56 Ba 57 La 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 85 At 86 Rn 87 Fr 88 Ra 89 Ac 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 111 112 114 116 118 Lanthanide Series 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu Actinide Series 90 Th 91 Pa 92 U 93 Np 94 Pu 95 Am 96Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr

Group Names 1A – Alkali Metals 2A – Alkaline Earth Metals

Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 3 1 H 2A 3A 4A 5A 6A 7A 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 11 Na 12 Mg 3B 4B 5B 6B 7B 8B 1B 2B 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 19 K 20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo 43 Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 55 Cs 56 Ba 57 La 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 85 At 86 Rn 87 Fr 88 Ra 89 Ac 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 111 112 114 116 118 Lanthanide Series 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu Actinide Series 90 Th 91 Pa 92 U 93 Np 94 Pu 95 Am 96Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr

Group Names 1A – Alkali Metals 2A – Alkaline Earth Metals 3A – Boron Family

Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 3 1 H 2A 3A 4A 5A 6A 7A 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 11 Na 12 Mg 3B 4B 5B 6B 7B 8B 1B 2B 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 19 K 20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo 43 Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 55 Cs 56 Ba 57 La 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 85 At 86 Rn 87 Fr 88 Ra 89 Ac 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 111 112 114 116 118 Lanthanide Series 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu Actinide Series 90 Th 91 Pa 92 U 93 Np 94 Pu 95 Am 96Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr

Group Names 1A – Alkali Metals 2A – Alkaline Earth Metals 3A – Boron Family 4A – Carbon Family

Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 3 1 H 2A 3A 4A 5A 6A 7A 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 11 Na 12 Mg 3B 4B 5B 6B 7B 8B 1B 2B 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 19 K 20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo 43 Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 55 Cs 56 Ba 57 La 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 85 At 86 Rn 87 Fr 88 Ra 89 Ac 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 111 112 114 116 118 Lanthanide Series 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu Actinide Series 90 Th 91 Pa 92 U 93 Np 94 Pu 95 Am 96Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr

Group Names 1A – Alkali Metals 2A – Alkaline Earth Metals 3A – Boron Family 4A – Carbon Family 5A – Nitrogen Family

Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 3 1 H 2A 3A 4A 5A 6A 7A 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 11 Na 12 Mg 3B 4B 5B 6B 7B 8B 1B 2B 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 19 K 20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo 43 Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 55 Cs 56 Ba 57 La 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 85 At 86 Rn 87 Fr 88 Ra 89 Ac 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 111 112 114 116 118 Lanthanide Series 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu Actinide Series 90 Th 91 Pa 92 U 93 Np 94 Pu 95 Am 96Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr

Group Names 1A – Alkali Metals 2A – Alkaline Earth Metals 3A – Boron Family 4A – Carbon Family 5A – Nitrogen Family 6A – Oxygen Family

Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 3 1 H 2A 3A 4A 5A 6A 7A 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 11 Na 12 Mg 3B 4B 5B 6B 7B 8B 1B 2B 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 19 K 20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo 43 Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 55 Cs 56 Ba 57 La 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 85 At 86 Rn 87 Fr 88 Ra 89 Ac 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 111 112 114 116 118 Lanthanide Series 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu Actinide Series 90 Th 91 Pa 92 U 93 Np 94 Pu 95 Am 96Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr

Group Names 1A – Alkali Metals 2A – Alkaline Earth Metals 3A – Boron Family 4A – Carbon Family 5A – Nitrogen Family 6A – Oxygen Family 7A – Halogens

Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 3 1 H 2A 3A 4A 5A 6A 7A 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 11 Na 12 Mg 3B 4B 5B 6B 7B 8B 1B 2B 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 19 K 20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo 43 Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 55 Cs 56 Ba 57 La 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 85 At 86 Rn 87 Fr 88 Ra 89 Ac 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 111 112 114 116 118 Lanthanide Series 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu Actinide Series 90 Th 91 Pa 92 U 93 Np 94 Pu 95 Am 96Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr

Group Names 1A – Alkali Metals 2A – Alkaline Earth Metals 3A – Boron Family 4A – Carbon Family 5A – Nitrogen Family 6A – Oxygen Family 7A – Halogens 8A or 0 – Noble Gases

Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 3 1 H 2A 3A 4A 5A 6A 7A 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 11 Na 12 Mg 3B 4B 5B 6B 7B 8B 1B 2B 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 19 K 20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo 43 Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 55 Cs 56 Ba 57 La 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 85 At 86 Rn 87 Fr 88 Ra 89 Ac 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 111 112 114 116 118 Lanthanide Series 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu Actinide Series 90 Th 91 Pa 92 U 93 Np 94 Pu 95 Am 96Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr

Group Names 1A – Alkali Metals 2A – Alkaline Earth Metals 3A – Boron Family 4A – Carbon Family 5A – Nitrogen Family 6A – Oxygen Family 7A – Halogens 8A or 0 – Noble Gases d-block – Transition Metals

Family Characteristics Alkali Metals Very reactive These metals do not occur freely in nature Soft metals Explode in water

Alkaline earth metals Do not occur naturally as an element Second most reactive Tend to be basic in solution Silver in color

Transition metals Brittle metals Good conductors Often form colorful compounds

Boron Family Do not occur normally as an element in nature All are scarce except for Aluminum

Carbon Family Metals and metalloids Vary in chemical and physical properties Occur in elemental form

Oxygen Occur in elemental form in nature

Halogen Group Found in earths crust Fluorine is the most abundant in this group

Nitrogen group Solid at Room Temperature Found in rock

Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 3 1 H 2A 3A 4A 5A 6A 7A 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 11 Na 12 Mg 3B 4B 5B 6B 7B 8B 1B 2B 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 19 K 20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo 43 Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 55 Cs 56 Ba 57 La 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 85 At 86 Rn 87 Fr 88 Ra 89 Ac 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 111 112 114 116 118 Lanthanide Series 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu Actinide Series 90 Th 91 Pa 92 U 93 Np 94 Pu 95 Am 96Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr

Group Names 1A – Alkali Metals 2A – Alkaline Earth Metals 3A – Boron Family 4A – Carbon Family 5A – Nitrogen Family 6A – Oxygen Family 7A – Halogens 8A or 0 – Noble Gases d-block – Transition Metals f-block – Inner Transition Metals Lanthanide series Actinide series

Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 3 1 H 2A 3A 4A 5A 6A 7A 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 11 Na 12 Mg 3B 4B 5B 6B 7B 8B 1B 2B 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 19 K 20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo 43 Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 55 Cs 56 Ba 57 La 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 85 At 86 Rn 87 Fr 88 Ra 89 Ac 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 111 112 114 116 118 Lanthanide Series 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu Actinide Series 90 Th 91 Pa 92 U 93 Np 94 Pu 95 Am 96Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr

Miscellaneous Facts Atomic #’s ≥ 83 are radioactive Seven diatomic elements H2 N2 O2 F2 Cl2 Br2 I2 What are the representative elements? The first 20 elements on the periodic table They form a 7 on the periodic table H2 N2 O2 F2 Cl2 Br2 I2

Periodic Trends 50

Periodic Trends Many properties of the elements change in a predictable way as you move through the periodic table These systematic variations are called periodic trends 51

Atomic Radius Distance from center of an atom’s nucleus to its outermost electrons 52

Atomic Radius Trend Down a group Increases as you go down a group Why? Adding another principal energy level where the outermost electrons reside Shielding increases which decreases the effective nuclear charge on the outer electrons Atoms are getting bigger 53

Atomic Radius Trend, cont’d. Across a period (row) Decreases across a row Why? Gain protons as move from left to right (gaining positive charge or increasing effective nuclear charge) Increases the pull on the electrons that are all about the same distance from the nucleus Same principal energy level Shielding is constant for all electrons A stronger attractive force shrinks the electrons’ orbitals and makes the atom smaller 54

55

Atomic Radius Trend, cont’d.

In Your Notes…. Write a definition of atomic radius in your own words What is the group trend? Explain why… What is the period trend? Explain why…. Share your definition, trends and explanations with a partner

Ions Atoms that are charged (not neutral) Created by atoms gaining or losing e- Loss of e- - positive ion called a cation Gain of e- - negative ion called an anion No change in # of p+ 58

Ionic Size (Radius) Distance from the center of the nucleus to the outermost electron Metals: neutral atom is larger than its cation Cations are formed when atoms lose their valence electron(s) In turn, they lose an entire principal energy level This reduces the repulsive force between the remaining electrons allowing them to be pulled closer to the nucleus Increases the effective nuclear charge (remaining electrons “feel” a stronger attraction to the nucleus; i.e., fewer e-, same number of p+). Li atom 0.152 nm Li+ ion 0.060 nm 1s22s1 1s2 59

Ionic Size, cont’d. Nonmetals: neutral atom is smaller than its anion Anions are formed when atoms gain electron(s) to complete their outermost energy level This increases the electric repulsive forces between the electrons spreading them further apart Decreases the effective nuclear charge (shielding stays the same) F-1 ion 0.133nm F atom 0.072 nm 1s22s22p6 1s22s22p5 60

Ionic Size, cont’d. Group Trend: generally increase going down Period Trend: generally decreases across the row 61

Ionic Size, cont’d.

Ionization Energy Energy required to remove a valence electron Approximates how strongly an atom holds onto its outermost electrons High ionization energy = tightly held electrons (hard to remove) Low ionization energy = outermost electrons easily removed giving the atom a positive charge 63

Ionization Energy Trends Group Trend: decreases down a group Valence electrons feel less of the positive charge from nucleus because: As the size of the atom increases, the shielding from the filled energy levels increases and the distance from the nucleus increases The valence electrons feel less of the positive charge from the nucleus (decreasing effective nuclear charge) 64

Ionization Energy Trends, cont’d Period Trend: increases across a period Nuclear charge increases and the shielding effect is constant (same distance from nucleus) Greater attraction from the nucleus A stronger attractive force shrinks the electrons’ orbitals and makes the atom smaller Noble gases have the highest ionization energies in any period 65

Ionization Energy, cont’d First Ionization Energy – energy required to remove the outermost electron Second Ionization Energy – energy required to remove the next electron Successive Ionization Energy – energy required to remove additional electrons (3rd, 4th, etc.) 66

Ionization Energy Trends, cont’d

Electronegativity Ability of an atom to attract electrons in a chemical bond Fluorine is the most electronegative element Noble gases have no electronegativity Cannot be directly measured 68

Electronegativity Trends Group Trend: increases going UP a group Less shielding, stronger effective nuclear charge Period Trend: Increases across a period Constant shielding, increasing effective nuclear charge 69

Electronegativity Trends, cont’d.

Periodic Trend Down A Group Across a Row Atomic radius Ionic Radius Ionization Energy Electron Affinity Electronegativity Reactivity (How vigoriously the atom will react) Metallic character Density As metallic characters decrease

Reactivity Metal Nonmetals Based on ionization energy The lower the ionization energy the higher the chemical reactivity Increased metallic character (larger sea of electrons) Which metal is most reactive? Nonmetals Uses electronegativity The higher the electronegativity the higher the chemical reactivity Which nonmetal is most reactive? 72

Practice Which of the following atoms has the highest electronegativity? Cs, K, or Li Si, Al, or S Which of following metals is more reactive? Ca, Sr, or Ba Which of the metals in question 2 has the lowest ionization energy? 73

Practice Which of the following metals has the highest ionization energy? Ni, Mn, or Zn 74

Octet Rule Atoms tend to lose, gain or share electrons in order to get a full set of eight valence electrons Exceptions: Duet rule: Hydrogen gains 1 get to look like He Lithium and beryllium lose 1 and 2, respectively, to look like He Filled s & p orbitals are extremely stable

Isoelectric Atoms &/or ions that have the same number of electrons Also same electron configuration Example: Na+, Ne, & F- All have 10 electrons All have the same electron configuration

Practice: Which of the following atoms &/or ions are isoelectric? K+, P3-, F-, Ca2+, Na+, Sr2+ How many electrons do these have? Which one has the smallest radius?

That's All Folks!