For problems 11-16, determine what elements are denoted by the following electron configurations: 11) 1s²2s²2p63s23p5 12) 1s²2s²2p63s23p64s23d 104p6 13) 1s²2s22p63s23p54s23d 104p65s24d7 14) [Kr] 5s²4d105p² 15) [Xe] 6s²4f12 16) 6s24f145d5

Which of the following electron configurations represent an excited state? Choose one or more: O (Ne]3s²3p² O [Ar]3A045\4p? O [Kr]4A05s+5pt O (Ne]3s²3p64s1

It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy (in kJ) for a mole of hydrogen atoms, making the assumption that ionization is thetransition from n = 1 to n = 00(infinity)

The complete electron configuration of vanadium, element 23, is A 1s 2s 2p°3s*3p5 B 1s 2s 2p°3s²3p°3d34s2 © 1525²2p103s²3p7 D 1s 2s 2p°3s*3p3 E 1s 2s 2p103s43p1

(b) Photoelectron spectroscopy data for the 1s sublevel of Ne and the 1s sublevel of Xe are represented below. In terms of Coulomb's law and atomic structure, explain why the peak for Ne is positioned so far to the right of the peak for Xe. Ne 3500 3000 2500 2000 1500 1000 500 Binding Energy (MJ/mol) Хе 3500 3000 2500 2000 1500 1000 500 Binding Energy (MJ/mol) Relative Number Relative Number of Electrons of Electrons

Circle each of the following that represent an acceptable set of quantum numbers for an electron in an atom