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- Consider the representations of the p and d atomic orbitals in Figs. 2-15 and 2- 17. What do the + and signs indicate?State which of the following orbitals cannot exist according to the quantum theory: 3p, 4s, 2f, and 1p. Briefly explain your answers.What does wave-particle duality mean? What are its implications in our modem view of atomic structure?
- What are quantum numbers? What information do we get from the quantum numbers n, l, and ml? We define a spin quantum number (ms), but do we know that an electron literally spins?Spinets are solids with the general formula M2+ (M3+)2O4 (where M2+ and M3+ are metal cations of the same or different metals). The best-known example is common magnetite, Fe3O4 [which you can formulate as (Fe2+)(Fe3+)2O4]. A crystal of a spinet (a) Given its name, it is evident that magnetite is ferromagnetic. How many unpaired electrons are in iron(II) and in iron(III) ions? (b) Two other spinets are CoAl2O4 and SnCo2O4. What metal ions are involved in each? What are their electron configurations? Are the metal ions paramagnetic, and if so, how many unpaired electrons are involved?Chapter 3 introduced the concept of a double bond between carbon atoms, represented by C=C , with a length near 1.34 Å. The motion of an electron in such a bond can be treated crudely as motion in a one-dimensional box. Calculate the energy of an electron in each of its three lowest allowed states if it is confined to move in a one-dimensional box of length 1.34 Å. Calculate the wavelength of light necessary to excite the electron from its ground state to the first excited state.
- Suppose that the spin quantum number did not exist, and therefore only one electron could occupy each orbital of a many-electron atom. Give the atomic numbers of the first three noble-gas atoms in this case.6.103 Atomic absorption spectroscopy is based on the atomic spectra of the elements being studied. It can be used to determine the impurities in a metal sample. If an element is present, light at the appropriate wavelength is absorbed. You are working with a metal stamping company and the rolled steel you use to form panels for automobile doors is failing at an alarming rate. There is some chance that the problem is unacceptably high levels of manganese in the steel. Given that the atomic spectrum of manganese has three lines near 403 nm, how could you use a spectrometer to determine the amount of manganese in the steel?5. Which of the following is the electron configuration of O2- ? a. 1s2 2 s 2 p b. 1s2 2s2 2pt c. 1s 2s 2 pl d. 1s 2s 2 p5 6. What is the electronic configuration for the 26Fe+2: 26FE+3: 29Cu+1: 29Cu+2: 7. Write the electronic configuration of 24Cr: 24Cr3+: 24Cr6+: a. Does 24CR6 paramagnetic or diamagnetic cation? b. Give the four quantum numbers of the last electron in 24Cr 24Cr3+ 24Cr6. c. Among of the above substances which is the most stable? Justify.
- 1. Which of the following is the configuration of carbon? а. 1522522p2 d. 1s22s12p4 b. 1s22s22p4 е. none of the above с. 1s22s12p3 2. Which statement is the best description of chlorine, Cl2? a. polar molecule d. ionic compound b. polar bonds, non polar molecule e. none of the above с. non polar molecule 3. The ion PCI4" has a structure that would be described as? a. octahedral d. T-shaped b. Square planar e. see-savw c. trigonal pyramidal 4. Which of the following substances would not be polar? a. Hydrogen chloride b. sulfur dioxide c. Ammonia d. Carbon disulfide 5. What does a double bond consist of? a. none of the other choices is correct. b. Two sigma bonds c. Two pi bonds d. One sigma and a pi bond e. Two sp3 bonds6. What is the electronic configuration for the 26Fe+2: 26Fe+3: 29Cu 1: 29Cu+z: 7. Write the electronic configuration of 24Cr: 24Cr3: 24Cr6+: a. Does 24Cr6+ paramagnetic or diamagnetic cation? b. Give the four quantum numbers of the last electron in 24Cr 24Cr3+ 24Cró+. c. Among of the above substances which is the most stable? Justify.Below is a representation of the electronic configuration for a neutral species. What atom does this correspond to? 1s² 2s² 2p 3s² 3p5 O a. Cl O b. P O c. Al O d. K O e. Sc