P17. The energy level diagram for a newly discovered element is shown below. Atoms of this element produce a strong spectral line at a wavelength of 713nm. Which transition on the energy level diagram is responsible for producing this strong spectral line? A) 3¹S-2³S B) 3¹S-2³P C) 2³P 2³S D) 2³P 1¹S E) 2³S-1¹S Energy (eV) -3¹S (2.76eV) -2³P (1.74eV) *2³S (1.44eV) 1¹s (0.00eV)

Below are the line spectra of Neon (Z = 10) and Lithium (Z = 3). Which of the following statements best explains why more spectral lines are observed for Neon as compared to Lithium? Neon (Ne) Lithium (Li) Select one: O a. Metals are held by stronger metallic bonds which makes emission more difficult. O b. O c. O d. Neon has more energy levels and electrons which allows more electronic transitions. Neon tends to fluoresce in nature thus more spectral lines are observed. Lithium requires more energy to excite because it prefers to form cations to achieve octet configuration. 19

f,g,h please

1) Write the full and noble gas configuration for Se. Full Electron Configuration: Response  Noble Gas Configuration: 2) The element represented by the following electron configuration is ____________. [Rn] 7s2 5f11 A)Rb B) Es C) Au D)Cf 3)Write the full and noble gas configuration for Cs. Full Electron Configuration: Noble Gas Configuration:  please answer the three question correct please