All of the following are allowed energy levels except _. a) 3f b) 1s c) 3d d) 5p e) 6s

please see the attached image

What energy in kilojoules per mole are associated with this frequency (4.37 x 10^14 Hz)?  A. 2.91 x 1019  kJ/mol B. 200 kJ/mol C. 353 x 1017 kJ/mol D. 174 kJ/mol

Consider the transition of the electron in the hydrogen atom from n = 4 to n = 9. a) Is ΔE for this process positive or negative? b) Will the light be absorbed or emitted?    c) Does this transition correspond to an endothermic or exothermic reaction?

In the energy diagram below: -8.72 x 10-20 -1.36 x 10-19 -2.42 x 10-19 Energy -5.45 x 10-19 J -2.18 x 10-18 ) Has the electron absorbed or emitted a photon and what is the energy change for the electron? Oa. The electron emitted a photon and the change in energy of the electron was - 1.64 x 1018 J. Ob. The electron absorbed a photon and the change in energy of the electron was 1.64 x 10-18 J. c. The electron absorbed a photon and the change in energy of the electron was -1.64 x 10-18 J. Od. The electron emitted a photon and the change in energy of the electron was 1.64 x 1018 J.

For a Hydrogen Atom these energies can be calculated by the following equation: 1 Latulan he - - ATelacirun- R n Ru-2.179 x 10-18J (Hydrogen atom) The Helium Ion, Het, has energy levels similar to those of the hydrogen atom. The helium ion, like the hydrogen atom, has only one electron. This eliminates electron-electron interactions, and allows us to calculate the energies of the electron in each of the energy levels (n = 1, 2, 3 .) of the helium ion: 8.7149 x 10-18J Eçloetron - RH - 8.7149 x 1018J n (Helium Iou) The energy released as a photon (Ephoton), when the electron in the helium ion (He*) transitions from higher energy levels to lower energy levels in the ion, can be calculated by the equation: 1 + Ephoton - hc -- AEelectron - RHet ----- n? (Helitun Ion) 1 8.7149 x 1018J. n ni) (Helium Ion) Calculate the electron energies (Eelectron) of the first 4 energy levels in the helium ion (He*): n = [ Select ] x 10-18 J n2 = [ Select] v x 10-18 J n3 = [ Select] v x 1018 J n4 = [ Select)…

During photosynthesis in a certain plant, eight photons of 670-nm wavelength can cause the following reaction: 6CO2 + 6H2O → C6H12O6 + 6O2During respiration, when the plant metabolizes sugar, the reverse reaction releases 4.9 eV of energy per CO2 molecule. Determine the ratio of the energy released (respiration) to the energy absorbed (photosynthesis), a measure of photosynthetic efficiency.

"Photosynthesis is a process in which light energy is captured and stored by an organism, and the stored energy is used to drive cellular processes," (Blankenship, p. 1). Photosynthesis doesn't just happen in green plants; it can occur in bacteria, as well. It occurs when light- harvesting molecules absorb energy in the form of light and transfer it to a reaction center, where light energy is converted to chemical energy. Most of us know about chlorophyll as the light-harvesting molecule, but there are many forms of chlorophyll found in different organisms. However, they all have similar properties when interacting with light. PHOTOSYNTHETIC PIGMENTS 1.6 C 0.7 1.4 0.6 1.2- Soret 0.5 A 0.4 0.8 H COOCH, phytyl bacteriochlorophyll a 0.3 0.6 0.2 0.4 0.1 0.2 01 700 750 800 850 900 300 400 500 600 700 800 2 (nm) 2 (nm) Figure 4.7 Absorption (left) and fluorescence (right) spectra of bacteriochlorophyll a in diethyl ether. 5. Look at this figure from Blankenship's book, Molecular Mechanisms…

An electron in a hydrogen atom travels from energy level n = 2 to energy level n = 3.   Would the electron be absorbing or emitting this energy in this transition? What is the change in energy (ΔE) for this transition?   Show all work, including units and signs, and give your answer for ΔE to three significant figures.

need it fast!!   In a hydrogen atom, an electron loses energy from n = 5 to n = 2, a process that leads to some kind of “interaction” with electromagnetic radiation.  What is the wavelength of this light in nanometers? Do NOT include a sign with this answer. Rydberg's constant is equal to -2.179 x 10-18 J. Planck's constant is equal to 6.626 x 10-34 Joule-seconds. The speed of light is 3.00 x 108  meters per second. Express exponents as number followed by E followed by the power (e.g., 7.34E-12).