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1 (Atomic structure and periodic)
1.1
- Alistotle
- -John Dalton
Michael Faraday
electrolysis
J.J. Thomson cathode ray tube
cathode ray 1
1
e/m x108 R. A. Millikan
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1 2
oil drop experiment x10-19 x10-31
canal ray proton
E.R. Rutherford
nucleus
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1 3
1932 J. Chadwickbombard Beryllium Be
neutron
e p n 1
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)
-1 +1 0
9.109382x10-28 1.672622x10-24 1.674927x10-24
0.0005485799 1.007276 1.008665
1.
atomic number, Z
mass number, A
X Z A
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1 4
=
= =
(Z) = 11 =A Z = 23 - 11 = 12 =
(isotope) (Z) (A)
(Hydrogen) H11 (Deuterium) H21
(Tritium) H31
(isotone)
3919K
4020Ca 20
(isobar) 146C 14
7N
1.3
John Dalton
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1 5
Sir Joseph John Thomson)
. . 1920
1.5
4
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1 6
1
r
K L, M, N, K, L, M, n = 1, n = 2, n = 3
1.6
1.4 (energy levels shell)
n n 1, 2, K, L, M, N, O, P, Q n=1
n2 n=1 (shell K) = 2(1)2 =2
n=2 = 2(2)2 = 8 n=3 = 2(3)2 = 18
n= = 2()2 = 32 n= = 2()2 = n= = 2()2 = 2 n=7 = 2(7)2 = 98
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1 7
(n) (sub-levels sub-shells) s p d f
sp d f (orbital)
s p 6 d f
s p d f p s n=1 n=2 n=3
1.7
3d 4s
s 3d
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1 8
8 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p
1.8
C z = 6 1s2 2s2 2p2 2
Pauli exclusion principle
Aufbau principle
O _ -
paired electron single electron
1.7 Hund's rule
degenerate orbitalp d
7N = 1s2 2s2 2p6
1s 2s 2p
-
1 9
filled configurationhalf- filled configuration
19
7N = 1s2 2s2 2p6
1s 2s 2p
Ne = 1s2 2s2 2p6 1s 2s 2p
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1 10
12
s 2s 2p 3s 3p 4s 3d 4p H
He
Li
Be
B
C
N
O
F
Ne
Na
Mg
Al
Si
P
S
Cl
Ar
K
Ca
Sc
Ti
V
Cr
Mn 25
Fe 26
Co 27
Ni 28
Cu 29
Zn 30
Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36
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1 11
1. 1.2.1
18 Antoine Lavoisier23 1870 65
1925 23 118
s- Li Na K Rb Cs Fr
periodic table
Johann
Dobereiner) 1817 3 (triads)
1.10 , Li 7 , Ca 40 , Cl 35 , Na 23 , Sr 88 , Br 80
, K 39 , Ba 137 , l 129 1.10
Na Sr Br 2
=
-
1 12
Cu (63.6), Ag (108), Au (197) Zn (65.4), Cd (112.4), Hg (200.6) Ni (58.7), Pd (106.4), Pt (195.1)
Ag, Cd Pd
. .1864 John Alexander Reina Newlands 8
1 ,
1.11
H 1 F 8 Cl 15 Co/Ni 22 Br 29 Pd 36 I 42 Pt/Ir 50
Li 2 Na 9 K 16 Cu 23 Rb 30 Ag 37 Cs 44 Tl 53
Gl 3 Mg 10 Ca 17 Zn 25 Sr 31 Cd 34 Ba/V 45 Pb 54
Bo 4 Al 11 Cr 18 Y 24 Ce/La 33 U 40 Ta 46 Th 56
C 5 Si 12 Ti 19 In 26 Zr 32 Sn 39 W 47 Hg 52
N 6 P 13 Mn 20 As 27 Di/Mo 34 Sb 41 Nb 48 Bi 55
O 7 S 14 Fe 21 Se 28 Ro/Ru 35 Te 43 Au 49 Os 51
1.11
. .1869-1870 Julius Lother Meyer
Dmitri Ivanovich Mendeleev
, ,
periodic Law 1.3
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1 13
1.3 . 1869 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 Pd = 106.6 Os = 199 H = 1 Cu = 63.4 Ag = 108 Hg = 200 Be = 9.4 Mg = 24 Zn = 65.2 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 J = 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
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Dmitri Ivanovich Mendeleev, 1834-1907 1859
1869
63 8 1861 27
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1 14
1864-1869
1869 1
2
3
1.4 44, 68 72 Eka-boron, Eka-aluminium Eka-silicon Eka
Eka-boron Sc), Ga)
Ge) Eka-silicon
1.4 ekasilicon
Eka-silicon
1871)
1886) (amu) 73 72.3
(g/cm3) 5.5 5.47 J/(g-1 C-1) 0.31 0.32
C 960 MO2 GeO2 MCl2 GeCl2
(g/cm3) 4.7 4.70 C 100 86
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1 15
. .1913 . . Henry G. J. MoseleyAu Hg Tl I
Co (Ni)
1.2.2
vertical column groups horizontal rowperiods
main groups transitionmetal groups
H He
Li Ne Na Ar
A B) K Kr B Rb Xe Cs Rn Fr Mt
La CeLu lanthanide
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1 16
series AcTh Lractinide series A B
A IA-VIIA1A- A
B IB-VIIBB- B
IA alkaline metal Li Na K Rb Cs
Fr IIA alkaline earth metal Be
Mg Ca Sr Ba Ra VIA charcogen O S Se Te Po VIIA halogen F Cl Br I At VIIIA inert gas noble gas
He Ne Ar Kr Xe Rn
metalloid B Si Ge As Sb Te VIIIA
synthetic elements
U Mt
-ium 0 = (nil) 5 = (penta) 1 = (un) 6 = (hexa) 2 = bi) 7 = (hepta) 3 = (tri) 8 = (octa) 4 = (quata) 9 = (enna)
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1 17
Uniloctium Unoium
1.12
1.2.3
100
(periodic properties)
1.13 (1.13 (
1.13
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1 18
1.13
(ionization energy)
IE
1 1 1
2, 3 2 3 IE1, IE2 IE3 (eV) (kJ/mol) 1eV = 96.5 kJ/mol
1, 2 3 Be
Be(g) Be+(g) + e- IE1 = 906 kJ/mol
Be+(g) Be2+(g) + e- IE2 = 1763 kJ/mol
Be2+(g) Be3+(g) + e- IE3 = 14855 kJ/mol 1 (Na)
(1s2 2s2 2p6 3s1) 2 10
Na+
Na2+ Na3+
-
1 19
1.5 (Be)
(N)(He) (Ne) (Ar) 114
15 3 (kJ/mol)
114 IE1
-
1 20
IE3>IE2>IE1
(full filled) (half filled) ns2 np6 np3
Be (1s2 2s2) N (1s2 2p2 2s2) 1.14
ns2 np6
11Na = 1s2 2s2 2p6 3s1
10Ne = 1s2 2s2 2p6
p
(electron affinity) EA
(eV) (kJ/mol)
Cl (g) + e- Cl- (g) + 348 Jkmol-1
( 7)
8
1.15
1.15
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1 21
VIA 1.6 s2p5 8 1
s2p6 1 (F)
(Ne) (CI) F)
F(g) + e- F-(g) EA = -328 kJ/mol
F(1s2 2s2 2p5) + e- F-(1s2 2s2 2p6) Electron Affinities and Electron Configurations for the First 10 Elements in the Periodic Table
Element Electron Affinity (kJ/mol) Electron Configuration H 72.8 1s1 He
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1 22
1954
F 4.0 3.5, 3.0 3.0
1.16 1.17
1.16
117
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1 23
(metal, non-metal and semi-metal) 109
IA, 2A ( ), 3A, 4A 5A ( ),
(B)(Si) (Ge) (As) (Sb) (Te) (Po)
(Ap)
( )
1.18
118
119