Write the electron configuration for atoms of chlorine Cl in their ground state and use it to predict which of the following PES spectra would be generated by these atoms. II 347 29.1 2.38 22.7 2.05 37.1 3.93 042 239 16.05 1.00 100 10 100 10 lonization Energy (MJ/mol) lonization Energy (MJ/mol) II IV 273 20.2 2.44 309 24.1 2.82 26.8 1.25 31.5 1.52 100 10 100 10 lonization Energy (MJ/mol) lonization Energy (MJ/mol) Number of Electrons Number of Electrons Number of Electrons Number of Electrons

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n-4 to the n- 1 principal energy level. (Rydberg constant: R-3.29x10¹5 s-¹) O 8.22 × 10¹4-1 O 1.03 x 108 sl O 1.35 x 10-51 1 O 3.08 x 10¹5 s-l1 O 2.06 x 1014 -1

Which of the following could represent the electron configuration of an excited state phosphorus atom? [Ne]3s23p25s1 [Ne]3s23p3 [Ne]3s13p3 [Ne]3s23p35s1 [Ne]3s23p4

Consider the element vanadium (Z=23)a) There is a line in the vanadium spectrum at 318.5nm.i. What is the frequency of the line?ii. What is the energy difference between the two levels responsible for this line in kJ per mole?iv. The ionization energy of vanadium from the ground state is 650.2 kJ/mol. Assume that the transition in (3) is from the ground state to an excited state. If that is the case, calculate the ionization energy from the excited state.

Why is it significant that colour emitted from the hydrogen emission spectrum is not white

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

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(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

What is the frequency of light emitted when a hydrogen electron drops from the n=2 energy level (E2= -5.5 x 10-19 J) to the n=1energy level (E1 = -22 x 10-19 J)?a. 16.5 x 10-12 Hzb. 3.0 x 1010 Hzc. 1.2 x 10-21 Hzd. 2.5 x 1015 Hze. 1.1 x 10-28 Hz