6 H20) + 6 CO2)- C6H1206(s) + 6 O2), AH-+2803 kl/mol. In order to form 78.155 g of C6H1206 (molar mass 180.156 g/mol), at least mol of photon with wavelength 423.7 nm is needed. (c 2.998 * 10° m/s; h= 6.626 x 1034 s; NA 6.022 x 1023 mol) Note: Input numerical value without unit. Pay attention to significant figures.

Calculate the wavelength of light, in nm, emitted from a mol of photons as they transition from the n=6 to n=3 in the hydrogen atom. Report four significant figures.

问题4 The Li2+ion is originally in the n = 7 excited state. The atom then emits a photon, transitioning to a different energy state. If the energy of the emitted photon is measured to be 11.1057 eV, what is the quantum number n of the final state that the Li2+ atom ends up in after emitting the photon?

17. Which of the elements highlighted in Figure P7.3 forms monatomic ions by (a) losing an s electron? (b) losing two s electrons? (c) losing two s electrons and a d electron? (d) adding an electron to a p orbital? (e) adding electrons to two p orbitals? FIGURE P7.3

Calculate the most probable radius, rmp, at which an electron will be found when it occupies a 1s orbital of a hydrogenic atom of atomic number Z, and tabulate the values for the oneelectron species from H to Ne9+ .

How many unpaired electrons are there in the following ground-state atoms and ions? For each one, show work on how you arrived at your answer. (a) N (b) P 3- (c) Na+

00 P: Pr Figure 2 Figure 2 shows the boundary surface of 2p orbitals of a hydrogenic atom in three dimensions. (i) What are the number 2 and the letter p in the name '2p orbital stand for? 2 (v) Describe how the px, Py and pz orbitals are differentiated and named as such. (vi) Some people say that the non-spherical shapes of the orbitals in Figure 2 can only be obtained by using quantum mechanics. Do you agree? Elaborate. N

True or false? For the hydrogen atom, (a) the allowed energy levels are E = -(13.60 eV)/n2 and E >= 0; (b) any photon with energy Ephoton >= 13.60 eV can ionize a hydrogen atom in the n = 1state; (c) Any photon with Ephoton >= 0.75(13.60 eV) can cause a hydrogen atom to go from the n =1 state to the n = 2 state.

What is the wavelength (in nm) of a photon required to excite an electron from n = 2 to n = 6 in a He* ion? Submit an answer to three signficant figures.

Calculate the energy (J) required to excited the electron in Be3+ from principal energy level n = 3 to level n = 7. Also calculate the wavelength(nm) of light that must be absorbed by a hydrogen atom in its ground state to reach this excited state.