1. THE PERIODIC TABLE

2. 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)

3. 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?

4. 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

5. Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 31 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

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

7. Types of Elements
Metals

8. 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)

9. Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 31 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

10. Types of Elements
Metals
Nonmetals

11. 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

12. Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 31 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

13. Types of Elements
Metals
Nonmetals
Metalloids

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

15. Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 31 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

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

17. Table Organization
Rows – periods (1-7)

18. 1 Lanthanide Series Actinide Series H 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9F 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

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

20. Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 31 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

21. Group Names
1A – Alkali Metals

22. Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 31 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

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

24. Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 31 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

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

26. Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 31 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

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

28. Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 31 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

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

30. Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 31 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

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

32. Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 31 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

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

34. Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 31 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

35. 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

36. Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 31 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

37. 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

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

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

40. Transition metals Brittle metals Good conductors
Often form colorful compounds

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

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

43. Oxygen
Occur in elemental form in nature

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

45. Nitrogen group
Solid at Room Temperature
Found in rock

46. Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 31 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

47. 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

48. Lanthanide Series Actinide Series 1A 8A 1 H 2A 3A 4A 5A 6A 7A 2 He 31 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

49. 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

50. Periodic Trends 50

51. 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

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

53. 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

54. 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. 55

56. Atomic Radius Trend, cont’d.

57. 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

58. 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

59. 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

60. 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

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

62. Ionic Size, cont’d.

63. 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

64. 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

65. 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

66. 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

67. Ionization Energy Trends, cont’d

68. 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

69. 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

70. Electronegativity Trends, cont’d.

71. 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

72. 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

73. 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

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

75. 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

76. 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

77. 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?

78. That's All Folks!