Concept explainers
Carotenes are molecules with alternating
(a) What is the energy of the
(b) What is the energy of the
(c) What is the
(d) If, by the Bohr frequency condition,
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Chapter 10 Solutions
Physical Chemistry
- although we associate Pz 2. Now we will move on to diatomic molecules. In atoms all p-orbitals are equivalent with m/= 0, and px py with m/= ±1. In diatomic molecules these orbitals are in fact separated, with pz associated with o orbitals along the internuclear axis and px py associated with л orbitals (m/= ±1). In determining electron configurations we do indeed separate them: N₂ (KK¹ 0₂²). and O2 (KKogu ng *2). 4 a. Two excited states of N₂ are associated with Tu transitions. Tg and og → ou* i. Draw the MO energy level scheme (p-orbitals only) for the N₂ ground state and for these two excited states. ii. Obtain the term symbols for the two excited states and order them according to Hund's rules. iii. Write the wave functions for each of the terms obtained in ii) above. iv. Pick one wave function from each excited state and show it obeys the Pauli Principle.arrow_forwardAt large interatomic separations, an alkali halide moleculeMX has a lower energy as two neutral atoms, M + X; atshort separations, the ionic form (M+)(X-) has a lowerenergy. At a certain distance, Rc, the energies of the twoforms become equal, and it is near this distance that theelectron will jump from the metal to the halogen atom during a collision. Because the forces between neutral atomsare weak at large distances, a reasonably good approximation can be made by ignoring any variation in potentialV(R) for the neutral atoms between Rc and R - `. For theions in this distance range, V(R) is dominated by theirCoulomb attraction.(a) Express Rc for the first ionization energy of the metalM and the electron affinity of the halogen X.(b) Calculate Rc for LiF, KBr, and NaCl using data fromAppendix F.arrow_forward10. Consider two hydrogen atoms. The electron in the first one is in n=1 state, whereas in the second the electron is in the n=3 state. (a) which atom is in the ground state configuration? Why? (b) Which orbital has a larger radius? (c) Which electron is moving faster and why? (d) Which electron has a lower potential energy? (e) Which atom has higher ionization energy? Hint: assume that the radius of the n=3 orbital is =5 rBarrow_forward
- What is the energy difference between the F2 molecule and the separated atoms? Express your answer in kilojoules per mole to three significant figures. 5 ΑΣΦ Energy difference = ? kJ/molarrow_forwardPhotoelectron spectroscopy studies of silicon atoms excited by X-rays with wavelength 9.890 × 10-1º m show four peaks in which the electrons have speeds 2.097 × 107 m s-!, 2.093 x 107 m s-!, 2.014 × 107 m s', and 1.971 x 107 m s-1. (Recall that 1 J = 1 kg m² s-2.) (a) Calculate the ionization energy of the electrons in each peak. (b) Assign each peak to an orbital of the silicon atom.arrow_forwardV7.arrow_forward
- 8C.4 (a) the moment of inertia of a CH4 molecule is 5.27 x 10^-47 kg m^2. What is the minimum energy needed to start it rotating? 8C.5 (a) use the data in 8C.4 (a) to calculate the energy needed excite a CH4 molecule from a state with l=1 to a state with l=2arrow_forward2. Electrons in molecules can be found in orbitals that extend over more than one atom. Consider one electron that is confined in a molecular orbital that extends over 8 adjacent carbon atoms. The electron can move freely between the 8 atoms. a) Using the one-dimensional particle-in-the-box model, calculate the energy required to promote an electron from the n = 2 to the n = 5 level. The length of the box is determined by the C-C bond distance, which is 139 pm.Note: The following information may or may not be useful. ?? = ?2ℎ28???2 Planck's constant = 6.626 x 10-34 J·s; Mass of Electron = 9.109 x 10-28 g; Rydberg constant = 1.097 x 107 m-1; Speed of Light = 2.998 x 108 m·s-1 b) What frequency of light would cause this excitation?c) Now imagine a straight chain of 2000 carbon atoms. Assume that the orbital extends over the entire chain and repeat the calculation for the required energy to promote an electron from the n = 2 to n = 5 level. d) Would you expect…arrow_forwardConsider these ground-state ionization energies of one-electron species:H=1.31X10³kJ/mol ,He⁺=5.24X10³kJ/mol Li²⁺=1.41X10⁴kJ/mol (a) Write a general expression for the ionization energy of anyone-electron species. (b) Use your expression to calculate theionization energy of B⁴⁺. (c) What is the minimum wavelengthrequired to remove the electron from the n=3 level of He⁺?(d) What is the minimum wavelength required to remove the electron from the n=2 level of Be³⁺?arrow_forward
- 14)ASAP PLZarrow_forwardPhotoelectron spectroscopy applies the principle of the pho-toelectric effect to study orbital energies of atoms and mol-ecules. High-energy radiation (usually UV or x-ray) is absorbedby a sample and an electron is ejected. The orbital energy can becalculated from the known energy of the radiation and the mea-sured energy of the electron lost. The following energy differ-ences were determined for several electron transitions:ΔE 2→1=4.098X10⁻¹⁷J, ΔE 3→1=4.854X10⁻¹⁷J, ΔE 5→1=5.242X10⁻¹⁷J, ΔE 4→2=1.024X10⁻¹⁷J Calculate the energy change and the wavelength of a photon emitted in the following transitions:(a) Level 3→2 (b) Level4→1 (c) Level5→4arrow_forward2) The ionization energy of potassium is 4.34 eV; the electron affinity of iodine is 3.06 eV. At what separation distance will the KI molecule gain enough Coulomb energy to overcome the energy needed to form the K+ and I ions?arrow_forward
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning