Thermal X-ray radiation (PDF) - SRON

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Table 3.3: Binding energies (in eV) of 1s electrons in the K-shell of free atoms and ions in the ground state Z el I II III IV V VI VII VIII IX X XI XII XIII 1 H 13.6 2 He 24.59 54.4 3 Li 58 76 122 4 Be 115 126 154 218 5 B 192 206 221 259 340 6 C 288 306 325 344 392 490 7 N 403 426 448 471 494 552 667 8 O 538 565 592 618 645 671 739 871 9 F 694 724 754 785 815 846 876 954 1103 10 Ne 870 903 937 971 1005 1039 1074 1108 1196 1362 11 Na 1075 1101 1139 1177 1215 1253 1291 1329 1367 1465 1649 12 Mg 1308 1333 1360 1402 1444 1486 1528 1570 1612 1654 1762 1963 13 Al 1564 1590 1618 1646 1692 1738 1784 1830 1876 1922 1968 2086 2304 14 Si 1844 1872 1901 1930 1959 2009 2059 2109 2160 2210 2260 2310 2438 15 P 2148 2178 2208 2238 2269 2300 2354 2408 2462 2517 2571 2625 2679 16 S 2476 2508 2540 2571 2603 2636 2668 2726 2785 2843 2902 2960 3018 17 Cl 2829 2862 2896 2929 2962 2996 3030 3064 3126 3189 3252 3315 3377 18 Ar 3206 3241 3276 3311 3346 3381 3417 3452 3488 3554 3621 3688 3755 19 K 3610 3644 3681 3718 3754 3791 3828 3866 3902 3940 4010 4081 4152 20 Ca 4041 4075 4110 4149 4187 4225 4264 4303 4342 4380 4420 4494 4569 21 Sc 4494 4530 4567 4604 4644 4684 4724 4764 4805 4846 4886 4928 5006 22 Ti 4970 5008 5047 5086 5125 5167 5209 5251 5292 5335 5378 5420 5464 23 V 5470 5511 5551 5592 5633 5674 5717 5761 5805 5848 5893 5938 5982 24 Cr 5995 6038 6080 6122 6165 6208 6250 6295 6341 6387 6432 6479 6526 25 Mn 6544 6589 6633 6677 6721 6766 6810 6854 6901 6949 6997 7045 7094 26 Fe 7117 7164 7210 7256 7301 7348 7394 7440 7486 7535 7585 7636 7686 27 Co 7715 7763 7811 7859 7906 7954 8002 8050 8098 8146 8198 8250 8303 28 Ni 8338 8387 8436 8486 8535 8585 8635 8685 8735 8785 8835 8889 8943 29 Cu 8986 9035 9086 9137 9188 9240 9294 9344 9396 9448 9500 9552 9609 30 Zn 9663 9708 9760 9813 9866 9919 9973 10028 10082 10136 10190 10244 10298 Z el XIV XV XVI XVII XVIII XIX XX XXI XXII XXIII XXIV XXV XXVI 14 Si 2673 15 P 2817 3070 16 S 3076 3224 3494 17 Cl 3439 3501 3658 3946 18 Ar 3821 3887 3953 4121 4426 19 K 4223 4293 4363 4433 4611 4934 20 Ca 4644 4719 4793 4867 4941 5129 5470 21 Sc 5085 5164 5243 5321 5399 5477 5675 6034 22 Ti 5546 5629 5712 5795 5877 5959 6041 6249 6626 23 V 6028 6114 6201 6288 6375 6461 6547 6633 6851 7246 24 Cr 6572 6621 6711 6802 6893 6984 7074 7164 7254 7482 7895 25 Mn 7143 7191 7242 7336 7431 7526 7621 7715 7809 7903 8141 8572 26 Fe 7737 7788 7838 7891 7989 8088 8187 8286 8384 8482 8580 8828 9278 27 Co 8355 8408 8461 8513 8569 8671 8774 8877 8980 9082 9184 9286 9544 28 Ni 8998 9053 9108 9163 9217 9275 9381 9488 9595 9702 9808 9914 10020 29 Cu 9665 9722 9779 9836 9893 9949 10009 10119 10230 10341 10452 10562 10672 30 Zn 10357 10415 10474 10533 10592 10651 10709 10772 10886 11001 11116 11231 11345 17
3.4 Transitions between different levels 3.4.1 Relative ordering of terms with the same configuration First we discuss the rules of Hund 1 for terms that correspond with one electron configuration in LS coupling: 1. Of all terms with the same value of L the term with the highest multiplicity (i.e., maximum S, spin vectors ↑↑) has the lowest energy. For example triplet terms have a lower energy than the corresponding singlet terms. 2. Of all terms with the same multiplicity the one with the highest L value (i.e., orbital angular momenta ↑↑) has the lowest energy. 3. Of all levels of one term the lowest energy is due to the state with the minimum value of J if the corresponding outer electron shell is filled with less than half of the maximum number of electrons, and due to the maximum value of J if the outer shell is filled with more than half of the maximum number of electrons. Example 3.7. Calcium in a 3dnp state has terms 3 F, 3 D, 3 P, 1 F, 1 D and 1 P; of all these terms, the 3 F term has the lowest energy. Example 3.8. See Fig. 3.9. Figure 3.9: Illustration of Hund’s rules and Landé’s interval rule. Furthermore, there is the interval rule of Landé 2 , which is strictly speaking only valid in LS coupling: the energy interval between two subsequent levels (J and J+1) in a multiplet is proportional to the highest quantum level (J + 1). Example 3.9. In a 4 D term (J = 1, 3 2 3:5:7. , 5 and 7 2 2 2 ) the separations have the ratio 1 Named after Friedrich Hund (1896-1997) 2 named after Alfred Landé (1888-1976) 18
Page 1 and 2: High Energy Astrophysics Jelle Kaas
Page 3 and 4: 3.1 Introduction Thermal X-ray radi
Page 5 and 6: Figure 3.2: The observed X-ray spec
Page 7 and 8: Figure 3.6: X-ray spectrum of the S
Page 9 and 10: series of alkaline spectra). The no
Page 11 and 12: • The first atomic shell (n = 1)
Page 13 and 14: Z El 1s 2s 2p 3s 3p 3d 4s Ground te
Page 15 and 16: m l1 s 1 m l2 s 2 M L M S +1 + +1
Page 17: 3.3 Energy levels We have seen the
Page 21 and 22: Figure 3.10: Transitions between a
Page 23 and 24: 3.5 Abundances of the elements With
Page 25 and 26: 3.6 Basic processes In order to be
Page 27 and 28: leading to Here the constant S 0 is
Page 29: 3.6.3 Radiative transition probabil
Page 32 and 33: Figure 3.12: Fluorescence yield as
Page 34 and 35: The formula of Younger While the Lo
Page 36 and 37: 3.6.6 Excitation-Autoionisation In
Page 38 and 39: 3.6.7 Photoionisation Figure 3.20:
Page 40 and 41: 3.6.9 Radiative recombination Radia
Page 42 and 43: 3.6.10 Dielectronic recombination T
Page 44 and 45: 3.7 The ionisation balance In order
Page 46 and 47: of computing time. Therefore one us
Page 48 and 49: 3.8 Continuum emission processes Af
Page 50 and 51: decays back to the 1s orbit by a ra
Page 52 and 53: Inner-shell ionisation The third li
Page 54 and 55: 3.9.3 Line width For most X-ray spe
Page 56 and 57: Table 3.6: The strongest emission l
Page 58 and 59: Table 3.8: Some important iron line
Page 60 and 61: with τ(λ) = τ 0 ϕ(λ) (3.83) wh
Page 62 and 63: Table 3.9: The most important X-ray
Page 64 and 65: where the hydrogen column density N
Page 66 and 67: source itself. Fortunately, with hi
Page 68 and 69:
Figure 3.35: Stability for the ioni
Page 70:
Table 3.10: Wavelengths in Å of th
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