Black and White Periodic Table

Periods

Periodic Table of The Elements

1A 1

Groups

8A 18

1

1 H (G)

1.01

2A 2

3

4

2 Li (S) Be (S)

6.94

9.01

# of protons

Element (physical state

at STP)

Atomic Weight

3A 4A 5A 6A 13 14 15 16

5

B (S)

10.81

6

C (S)

12.01

7

N (G)

14.01

8

O (G)

16.00

7A 17

9

F (G)

19.00

2

He (G)

4.00

10

Ne (G)

20.18

3

11

Na (S)

12

Mg (S)

22.99 24.31

3B 3

4B 4

5B 5

6B 6

7B 7

8B

1B

2B 13

14

15

16

17

18

8

9

10

11

12

Al (S) Si (S) P (S)

26.98 28.09 30.97

S (S)

32.07

Cl (G) Ar (G)

35.45 39.95

4

19

K (S)

20

21

Ca (S) Sc (S)

22

Ti (S)

23

V (S)

24

25

26

27

28

29

30

31

32

33

34

35

36

Cr (S) Mn (S) Fe (S) Co (S) Ni (S) Cu (S) Zn (S) Ga (S) Ge(S) As (S) Se (S) Br (L) Kr (G)

39.10 40.08 44.96 47.87 50.94

52.00

54.94 55.85

58.93 58.69 63.55 65.39 69.72 72.64 74.92 78.96 79.90 83.80

5

37

Rb (S)

38

Sr (S)

85.47 87.62

6 55

56

Cs (S) Ba (S)

132.91 137.33

39

Y (S)

88.91

*

40

Zr (S)

91.22

41

Nb (S)

92.91

42

Mo (S)

95.94

43

Tc (L)

[98]

44

Ru (S)

101.07

45

Rh (S)

102.91

46

Pd (S)

106.42

47

48

49

50

51

52

Ag (S) Cd (S) In (S) Sn (S) Sb (S) Te (S)

107.87 112.41 114.82 118.71 121.76 127.60

53

I (S)

126.90

54

Xe (G)

131.29

72

Hf (S)

178.49

73

Ta (S)

180.95

74

W (S)

183.84

75

76

Re (S) Os (S)

186.21 190.23

77

Ir (S)

192.22

78

Pt (S)

195.08

79

80

81

82

83

84

Au (S) Hg (L) Tl (S) Pb (S) Bi (S) Po (S)

196.97 200.59 204.38 207.2 208.98 [209]

85

At (S)

[210]

86

Rn (G)

[222]

7 87

88

Fr (S) Ra (S)

~

104

105

106

107

108

109

110

111

112 113 114 115

116

117

118

Rf (X) Db (X) Sg (X) Bh (X) Hs (X) Mt (X) Ds (X) Rg (X) Cn (X) Nh (X) Fl (X) Mc (X) Lv (X) Ts (X) Og (X)

[223] [226]

[267]

[268]

[271]

[272]

[270]

[276]

[281]

[280] [285] [284] [284] [288] [289]

[293]

[294]

Lanthanide Series * Actinide Series ~

57

La (S)

138.91

89

Ac (S)

[227]

58

Ce (S)

140.12

90

Th (S)

232.04

59

Pr (S)

140.91

91

Pa (S)

231.04

60

Nd (S)

144.24

92

U (S)

238.03

61

Pm (S)

[145]

93

Np (S)

[237]

62

Sm (S)

150.36

94

Pu (S)

[244]

63

64

Eu (S) Gd (S)

151.97 157.25

95

96

Am (S) Cm (S)

[243]

[247]

65

Tb (S)

158.93

97

Bk (S)

[247]

66

Dy (S)

162.50

98

Cf (S)

[251]

67

Ho (S)

164.93

99

Es (S)

[252]

68

Er (S)

167.26

100

Fm (S)

[257]

69

Tm (S)

168.93

101

Md (S)

[258]

70

Yb (S)

173.04

102

No (S)

[259]

71

Lu (s)

174.97

103

Lr (S)

[262]

Provided by

The Academic Center for Excellence

1

Periodic Table of Elements Updated Summer 2019

Periodic Table Key

Group labels 1, 2, 3, etc. are recommended by the Interna onal Union of Pure and Applied Chemistry (IUPAC); the labels 1A, 2A, 3B, etc. are more common American usage.

Atomic masses in brackets are the most stable isotope of radioac ve elements. The physical states of the elements at STP (standard temperature, 0? C, and standard pressure, 1 atm) are either S

(solid), L (liquid), or G (gas). X designates synthe cally prepared elements. Elements in group 1A (except H) are alkali metals, in 2A are alkaline earth metals, in 3B--2B are transi on metals, in 8A

are noble (rare) gases, and in 7A (except At) are halogens. Elements with bold borders are metalloids, underlined

Ac nium

Ac

Aluminum Al

Americium Am

An mony Sb

Argon

Ar

Arsenic

As

Asta ne

At

Barium

Ba

Berkelium Bk

Beryllium Be

Bismuth

Bi

Bohrium

Bh

Boron

B

Bromine

Br

Cadmium Cd

Calcium

Ca

Californium Cf

Carbon

C

Cerium

Ce

Cesium

Cs

Chlorine

Cl

Chromium Cr

Cobalt

Co

Copernicium Cn

Copper

Cu

Curium

Cm

Darmstad um Ds

Dubnium

Db

Dysporosium Dy

Einsteinium

Es

Erbium

Er

Europium

Eu

Fermium

Fm

Flerovium

Fl

Fluorine

F

Francium

Fr

Gadolinium

Gd

Gallium

Ga

Germanium

Ge

Gold

Au

Hafnium

Hf

Hassium

Hs

Helium

He

Holmium

Ho

Hydrogen

H

Indium

In

Iodine

I

Iridium

Ir

Provided by The Academic Center for Excellence

Iron

Fe

Krypton

Kr

Lanthanum

La

Lawrencium

Lr

Lead

Pb

Lithium

Li

Livermorium Lv

Lute um

Lu

Magnesium

Mg

Manganese

Mn

Meitnerium

Mt

Mendelevium Md

Mercury

Hg

Molybdenum Mo

Moscovium

Mc

Neodymium Nd

Neon

Ne

Neptunium

Np

Nickel

Ni

Nihonium

Nh

Niobium

Nb

Nitrogen

N

Nobelium

No

Oganesson

Og

2

Osmium

Os

Oxygen

O

Palladium

Pd

Phosphorus

P

Pla num

Pt

Plutonium

Pu

Polonium

Po

Potassium

K

Praseodymium Pr

Promethium Pm

Protac nium Pa

Radium

Ra

Radon

Rn

Rhenium

Re

Rhodium

Rh

Roentgenium Rg

Rubidium

Rb

Ruthenium

Ru

Rutherfordium Rf

Samarium

Sm

Scandium

Sc

Seaborgium

Sg

Selenium

Se

Silicon

Si

Silver

Ag

Sodium

Na

Stron um

Sr

Sulfur

S

Tantalum

Ta

Techne um

Tc

Tellurium

Te

Tennessine

Ts

Terbium

Tb

Thallium

Tl

Thorium

Th

Thulium

Tm

Tin

Sn

Titanium

Ti

Tungsten

W

Uranium

U

Vanadium

V

Xenon

Xe

Y erbium

Yb

Y rium

Y

Zinc

Zn

Zirconium

Zr

Periodic Table of Elements Updated Summer 2019

Electronega vity

Periodic Table Trends

Metallic Character

Atomic Radius

Increasing

Increasing

Increasing

Increasing

Electronega vity is measured on a unitless scale that ranges from 0.7 to 4.0 that represents the likelihood of an atom a rac ng an electron. Noble gases are assigned a value of 0 as they do not a ract electrons.

Increasing

Metallic character describes how much an element exhibits the physical and chemical proper es of metals.

Increasing

The atomic radius is a physical measurement of the distance from the center of an atom to the outer shell of electrons.

Ionic Radius

Ioniza on Energy

La ce Energy

Increasing

Decreasing

Increasing

Increasing

Ionic radius follows the same trend as the atomic radius. However, in most cases, nonmetals form anions and metals form ca ons, and the difference in charge affects the radius. Therefore, nonmetals and metals must be considered independent of each other.

Increasing

Ioniza on energy is the amount of energy (kJ/mol) required to remove an electron from the valence shell of the atom. The value also increases when removing subsequent electrons within the atom. Excep ons: Groups 3A and 6A have lower ioniza on energies as compared to groups 2A and 5A.

La ce energy (kJ/mol) describes the energy that is released when ions combine to form a compound. Both an increase in an atom's charge, and a decrease in atomic radius will lead to an increase in la ce energy.

Provided by

The Academic Center for Excellence

3

Periodic Table of Elements Updated Summer 2019

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