元素周期表 - 维基百科，自由的百科全书

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電子層

0族電子數

週期↓

I A

VIII A （0）

1

1 H 氫 1.008

II A

III A

IV A

V A

VI A

VII A

2 He 氦 4.003

K

2

2

3 Li 鋰 6.941

4 Be 鈹 9.012

5 B 硼 10.81

6 C 碳 12.01

7 N 氮 14.01

8 O 氧 16.00

9 F 氟 19.00

10 Ne 氖 20.18

L K

8 2

3

11 Na 鈉 22.99

12 Mg 鎂 24.30

III B

IV B

V B

VI B

VII B

VIII B （VIII）

I B

II B

13 Al 鋁 26.98

14 Si 矽 28.09

15 P 磷 30.97

16 S 硫 32.04

17 Cl 氯 35.45

18 Ar 氬 39.95

M L K

8 8 2

4

19 K 鉀 39.10

20 Ca 鈣 40.08

21 Sc 鈧 44.96

22 Ti 鈦 47.87

23 V 釩 50.94

24 Cr 鉻 52.00

25 Mn 錳 54.94

26 Fe 鐵 55.84

27 Co 鈷 58.93

28 Ni 鎳 58.69

29 Cu 銅 63.55

30 Zn 鋅 65.38

31 Ga 鎵 69.72

32 Ge 鍺 72.63

33 As 砷 74.92

34 Se 硒 78.97

35 Br 溴 79.90

36 Kr 氪 83.80

N M L K

8 18 8 2

5

37 Rb 銣 85.47

38 Sr 鍶 87.62

39 Y 釔 88.91

40 Zr 鋯 91.22

41 Nb 鈮 92.91

42 Mo 鉬 95.95

43 Tc 鎝 [97]

44 Ru 釕 101.1

45 Rh 銠 102.9

46 Pd 鈀 106.4

47 Ag 銀 107.9

48 Cd 鎘 112.4

49 In 銦 114.8

50 Sn 錫 118.7

51 Sb 銻 121.8

52 Te 碲 127.6

53 I 碘 126.9

54 Xe 氙 131.3

O N M L K

8 18 18 8 2

6

55 Cs 銫 132.9

56 Ba 鋇 137.3

57 La 鑭 138.9

58 Ce 鈰 140.1

59 Pr 鐠 140.9

60 Nd 釹 144.2

61 Pm 鉕 [145]

62 Sm 釤 150.4

63 Eu 銪 152.0

64 Gd 釓 157.2

65 Tb 鋱 158.9

66 Dy 鏑 162.5

67 Ho 鈥 164.9

68 Er 鉺 167.3

69 Tm 銩 168.9

70 Yb 鐿 173.0

71 Lu 鎦 175.0

72 Hf 鉿 178.5

73 Ta 鉭 180.9

74 W 鎢 183.8

75 Re 錸 186.2

76 Os 鋨 190.2

77 Ir 銥 192.2

78 Pt 鉑 195.1

79 Au 金 197.0

80 Hg 汞 200.6

81 Tl 鉈 204.4

82 Pb 鉛 207.2

83 Bi 鉍 209.0

84 Po 釙 [209]

85 At 砈 [210]

86 Rn 氡 [222]

P O N M L K

8 18 32 18 8 2

7

87 Fr 鍅 [223]

88 Ra 鐳 [226]

89 Ac 錒 [227]

90 Th 釷 232.0

91 Pa 鏷 231.0

92 U 鈾 238.0

93 Np 錼 [237]

94 Pu 鈽 [244]

95 Am 鋂 [243]

96 Cm 鋦 [247]

97 Bk 鉳 [247]

98 Cf 鉲 [251]

99 Es 鑀 [252]

100 Fm 鐨 [257]

101 Md 鍆 [258]

102 No 鍩 [259]

103 Lr 鐒 [266]

104 Rf 鑪 [267]

105 Db 𨧀 [268]

106 Sg 𨭎 [267]

107 Bh 𨨏 [270]

108 Hs 𨭆 [271]

109 Mt 䥑 [278]

110 Ds 鐽 [281]

111 Rg 錀 [282]

112 Cn 鎶 [285]

113 Nh 鉨 [286]

114 Fl 鈇 [289]

115 Mc 鏌 [290]

116 Lv 鉝 [293]

117 Ts 鿬 [294]

118 Og 鿫 [294]

Q P O N M L K

8 18 32 32 18 8 2

圖解：

在標準狀況下，序號綠色者為氣體；序號藍色者為液體；序號黑色者為固體；序號灰色者為未知相態。​

• 化學元素豐度
• 元素的电子组态列表
• 元素收藏
• 元素列表
• 化学序
• 标准模型
• 核素圖
• 化學元素發現年表
• 擴展元素週期表

1. ^ ^{1.0 1.1} 自然界中有多少元素天然存在是复杂的问题，至今仍未完全解决。地球中大量存在的最重元素是92号元素铀，但铀可通过自发裂变释放中子，铀原子捕获中子后就会通过β衰变变成更重的93号元素镎和94号元素钚。^[10]这两种元素的丰度甚至比前92号元素最稀有的几种元素（如钷、钫、砹）的丰度还高（见地球的地壳元素丰度列表）。理论上，钚原子还能捕获更多中子，产生更重的元素，但它们的丰度少到无法探测。^[10]在太阳系形成之初，短寿命元素仍未衰变殆尽，因此天然存在的元素要多于94种。96号元素锔是前94号元素以外最长寿的元素，可能已通过宇宙射线到达地球，但至今尚未发现它。^[10]普瑞兹毕尔斯基星含有直到99号元素锿的所有元素，^[11]100号元素镄也可能曾存在于加蓬奥克洛的天然核反应堆中，但现已衰变殆尽。^[3]更重的元素有可能在超新星或中子星碰撞的r-过程中产生，但未被确认。目前不确定r-过程能产生多少元素。计算结果认为它能产生质量数280-290的核素，但它们会迅速β衰变成会自发裂变的核素，因此r-过程产生的超重元素有99.9%都会在一个月内衰变。^[12]如果这些超重元素够长寿，它们也能通过宇宙射线到达地球，但至今仍未找到它们。^[10]
2. ^ 以下几种元素是先在实验室中合成后，才在自然界中发现的：锝（43号）、钷（61号）、砹（85号）、镎（93号）、钚（94号）。
3. ^ 少数版本的周期表中会将中子作为0号元素列出。
4. ^ 元素分区的方式与此叙述实际上略有出入。例如，氦是位于第18族（0族）中的元素，但划分时它被分在s区；此外，d亚层在第11族（I B族）就已经被填满了，第12族（II B族）中新电子填入的是s亚层，但它仍然被分入d区。
5. ^ 图中不包括稀有气体、砹、钫、镅和镅之后的所有元素，因其数据不详。
6. ^ 视标度种类的不同，电负性最大和最小的元素可能与此所列的存在差别。在某些标度中，氖元素的电负性最大，钫元素的电负性最小。
7. ^ 尽管目前一般认为铹原子基态电子排布中，最外层应是 p 电子，且铹元素应具有活泼金属的特点，即在溶液中能形成正一价离子，但试图证明这些特点的实验还尚未获得过成功。^[57]早先的观点认为，铹原子最外层可能是 d 电子^[57]，这对于金属态的铹而言可能仍然成立；但气态的铹原子拥有的则很可能是 p 电子。^[58]
8. ^ 戴明的18列周期表的一种原型是亚当斯1911年版的16列周期表. [2018-08-01]. （原始内容存档于2016-04-18）.。亚当斯的版本中，主表不含稀土元素及“放射性元素”（即锕系元素）。出于节省空间的目的，它们被单独用加字符号和大括号补注出来（稀土元素加在钡和“钇下元素”之间，锕系元素加在“碲下元素”和“碘下元素”之间）。参见 Elliot Q. A. (1911). "A modification of the periodic table". Journal of the American Chemical Society. 33(5): 684-688 (687).
9. ^ 用于容纳重于铋的元素（如钍、镤、铀）的第二个超长行早在1892年就已经被引入。但早先的研究者一般认为这些元素是第三行过渡金属铪、钽、钨的同族元素。直到锕系元素与镧系元素间的电子结构相似性被揭示出来以前，锕系元素作为一组“内过渡元素”而单独存在的观点都不受学界主流认可。参见van Spronsen, J. W. (1969). The periodic system of chemical elements. Amsterdam: Elsevier. p. 315–316, ISBN 0-444-40776-6。
10. ^ 关于这些周期表的具体形状，参见The Internet database of periodic tables. [2016-02-28]. （原始内容存档于2016-03-24）.。
11. ^ “第3族的元素究竟应该如何确定”纯粹是因为镧系元素的插入才成为一个话题，因为钪-钇-镧-锕之间的性质渐变和第2族钙-锶-钡-镭的表现其实是一致的。^[148]
12. ^ 将镧系元素从周期表主表中分离出来的做法是由捷克化学家博胡斯拉夫·布劳纳于1902年首创的。他将这些元素放在了第4族锆元素的下方。这种编排模式是基于“小行星假说”而创设的，该假说类比太阳系中小行星通常占据独立轨道的运行方式，提出了这种镧系元素单独排布的模式。此前，大多数人都是直接将镧系元素（不成功地）填充进老式8列周期表的I~VIII族中。这种1902年正式发布的编排模式实际上早在1895年即出现在书面记录中，而“化学小行星”的概念更是早在1881年就出现在了他写给门捷列夫的信中。其他一些作者通常会把镧系元素放进第3族、第3~4族或第2~4族中。1922年，尼尔斯·玻尔进一步把镧系元素置于s区与d区之间。1949年，格倫·西奧多·西博格（重新）引进了时下通行的周期表编排方式，即将镧系与锕系元素置于脚注位置上。西博格的这种编排方式最早出现于1944年，并由他本人与1945年重新发表在期刊《化学化工新闻》上。这种编排主张直到1949年才终于为一些作者所认同。同年，西博格称处理锕系元素最好的方法是和镧系一样，将其排在周期表底部。参见：Thyssen P. and Binnemans K. (2011). "Accommodation of the Rare Earths in the Periodic Table: A Historical Analysis". In K. A. Gschneider Jr. (ed). Handbook on the Physics and Chemistry of the Rare Earths. 41. Amsterdam: Elsevier, pp. 1–94; Seaborg G. T. (1994). Origin of the Actinide Concept'. In K. A. Gschneider Jr. (ed). Handbook on the Physics and Chemistry of the Rare Earths. 18. Amsterdam: Elsevier, pp. 1–27.
13. ^ 圖表的更多例子請見: 彼得·阿特金斯 (2006). Shriver & Atkins Inorganic Chemistry (4th ed.). Oxford: Oxford University Press • Myers et al. (2004). Holt Chemistry. Orlando: Holt, Rinehart & Winston • Chang R (2000)。Essential Chemistry (2nd ed.). Boston: McGraw-Hill
14. ^ 第三族的钪-钇-镥-铹表的例子详见 Rayner-Canham G. & Overton T. (2013). Descriptive Inorganic Chemistry (6th ed.). New York: W. H. Freeman and Company • Brown et al. (2009). Chemistry: The Central Science (11th ed.). Upper Saddle River, New Jersey: Pearson Education • Moore et al. (1978). Chemistry. Tokyo: McGraw-Hill Kogakusha
15. ^ 碱度随原子半径增加而逐渐增强是同一金属族的特征，但这并不是钇下方出现镥而非镧的根本原因。基于同样的理由，尽管第2族碱土金属中的镁（弱碱性）属于“可溶族”，而钙、锶、钡（碱性更强）属于“碳酸铵族”，但它们仍然都被排在第2族中。参见Moeller et al. (1989). Chemistry with Inorganic Qualitative Analysis (3rd ed.). SanDiego: Harcourt Brace Jovanovich, pp. 955–956, 958.
16. ^ 虽然金属铹基态价层排布中有一个p电子，但简单的建模研究表明，在凝聚态和一般的化学环境中，该元素具有6d价电子，因而性质类似镧系元素。^[166]其它重锕系元素也具有这个特点。^[163]
17. ^ 关于第3族上放置所有镧系和锕系元素的例子，参见Housecroft C. E. & Sharpe A. G. (2008). Inorganic Chemistry (3rd ed.). Harlow: Pearson Education • Halliday et al. (2005). Fundamentals of Physics (7th ed.). Hoboken, NewJersey: John Wiley & Sons • Nebergall et. al. (1980). General Chemistry (6th ed.). Lexington: D. C. Heath and Company
18. ^ Karol (2002, p. 63)认为，当原子序数变得如天文数字般大时，引力效应会变得显著，因而能够克服超重原子核明显的不稳定现象。因此，原子序数约为10²¹的中子星被认为代表目前宇宙中最重的已知元素。（中子星内部可有部分游离质子与电子，因而原子序数可能非常大。——译注）参见Karol P. J. (2002). "The Mendeleev-Seaborg periodic table: Through Z-1138 and beyond". Journal of Chemical Education.79 (1): 60-63.
19. ^ 周期表历史上最权威的专家之一^[186]埃里克·赛睿早年间即已意识到多种类型的周期表各有其价值，但近些年也支持存在一种“最优周期表”的观点。^[185]

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