This happens as more electrons are getting filled in the d-orbital. However, Sc does not show +2 oxidation state. Its electronic configuration is 4s2 3d1. It loses all the three electrons to form Sc3+. +3 oxidation state of Sc is very stable as by losing all three electrons, it attains stable noble gas configuration, [Ar].
a) Write the ground-state electron configuration and count the number of unpaired electrons in cesium. b) The photoelectric binding energy of cesium is 183.7 kJ/mol. Light having a wavelength of 2.4 x iO in falls upon a cesium surface in an evacuated tube. Calculate the minimum deBroglie wavelength of the emitted photoelectrons. 3.
Implications of the unpaired spins in Li-O 2 battery chemistry and electrochemistry: A minireview. DOE PAGES. Lau, Kah Chun; Lu, Jun; Luo, Xiangyi; ... 2014-07-17. Recent experime
So when the orbitals are empty 6s has a lower energy than 4f and 5d. But when these orbitals get filled with electrons, the 6s jumps in energy to be higher than the 4f and 5d energies. This happens at all s and d block intersections.
The electron configuration, [Ar] 4s1, is the ground state electron configuration of potassium. The electron configuration, [Ne] 3s2 3p4, is the ground state electron configuration of
iv) The ground-state electron configuration contains three unpaired 6 p electrons. Answer: (Book Ch2, Q94) i) Ne ii) S iii) Ag: [Kr]5s 1 4d 10 is the actual ground state electron configuration for Ag. * 11 valence electron Group 11. iv) Bi: [Xe]6s 2 4f 14 5d 10 6p 3; the three unpaired electrons are in the 6 p orbitals. 13.
The explanation for the presence of three unpaired electrons in the nitrogen atom can be given by Hund's rule. According to this rule, electron pairing in any orbital (s, p, d or f) cannot take place until each orbital of the same sublevel contains 1 electron. The electronic configuration of N is 1 s 2 2 s 2 2 p 3.
For example, the electron configuration of cerium (Ce, #58) is: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 2. and that of praseodymium (Pr, #59) is: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 3. The only difference between these two configurations is in the number of 4f electrons. Both the fifth and ...