13:244G O12. Why does Li have a larger first ionization energy than Na?OA Because Li has only 3 electrons and they are less shielded from the force of attraction from the nucleus unlike those on NaOB Because Li is more electronegative than NaOC All of them aboveOD. None of them aboveAdd a caption...> Status (Custom)

Ionization energy :- The amount of energy required to remove an electron from an isolated neutral…

Answered: 12. Why does Li have a larger first…

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter11: Atomic Theory :the Quantum Model Of The Atom

Section: Chapter Questions

Problem 109E

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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?
Consider the representations of the p and d atomic orbitals in Figs. 2-15 and 2- 17. What do the + and signs indicate?
Using data from Problems 13 and 15, calculate the average distance of the electron from the nucleus in the Na 3s orbital, the Li 2s orbital, and the H 1s orbital. Explain the trend in your results.
Do atoms in excited states emit radiation randomly, at any wavelength? Why? What does it mean to say that the hydrogen atom has only certain discrete energy levels available? How do we know this? Why was the quantization of energy levels surprising to scientists when it was first discovered?
The energy of the 1s atomic orbital of hydrogen is -13.6 eV. a) What is the energy of the 1s atomic orbital of hydrogen in joules? b) Does this number remind you of something, if so, what? c) In all the energy level diagrams, what is used as a reference? What state of the system does the E=0 level correspond to? d) What is the ionization energy of the hydrogen atom in eV? e) The satabilization energy of the bonding molecualr orbital compared to the atomic orbitals is of 3.2 eV. What is the difference in energy between the H2 molecule and two isolated hydreogen atoms? f) What is the ionization energy of the H2 molecule in eV? In joules? g) What is the wavelength of a photon should have to achieve ionization of the H2 molecule? What domain of the spectrum is it in?
The ionization energy of lithium is 520.2 kJ/mole, and the electron affinity of hydrogen is 72.8 kJ/mole.(a) Find the separation distance in LiH at which the Coulomb potential energy equals the energy cost of removing an electron from Li and adding it to H.(b) The measured electric dipole moment of the molecule LiH is 2.00 × 10^−29 C · m. What is the fractional ionic character of LiH?(c) Instead of removing an electron from Li and attaching it to H, we could regard the formation of LiH as occurring by removing an electron from H and attaching it to Li (electron affinity = 59.6 kJ/mole). Why don’t we consider this as the formation process?
What type of electron orbital (i.e., s, p, d, or f) is deignated by n = 3, l = 2, ml = 1? n = 6, l =3, ml = 2? n = 4, l = 3, ml = 3?
Q.1(a) What were the important advance (s) as a result of which, idea of an electron orbitmovement was swapped by, the notion of probability of finding electron in an orbital?What name was given to the transformed atomic model? Also explain its variouspostulates.(b) Which quantum numbers revel information about the shape, energy, orientation, andsize of the orbitals? How many orbitals are possible for n=4? Which of these may bedescribed as gerade?(c) The signs of the unsquared wave functions are usually shown in plots of the squaredfunctions. Why do you think this practice exists? Give values of angular nodes andplane of 3p, 4d, 2p, 4f, 4s.(d) Predict the trend in values of slater’s constant of the every first element of each groupof p-block elements.
For multi-electron atoms, we use the shell model and effective corepotential to estimate the energy of each atomic orbitals.a) For carbon anion (C-1), estimate the energy of 1s and 2s atomic orbitals.b) Draw the energy level diagram and assign electrons for carbon anion(C-1).c) In one or two sentences, briefly describe what is the physical meaningof atomic orbitals.d) Lydia sets up a photoelectron spectroscopy experiment of the gaseouscarbon anion (C-1) using an UV light (λ = 300 nm). How many peaks do you expect to see in the final spectrum?e) Estimate the lowest kinetic energy of the ejected electrons.
Why is the electronic configuration of the yttrium atom [Kr]4d15s2 and that of the silver atom [Kr]4d105s 1?
Photoelectron spectra were acquired from a sample ofgaseous N2 using He(I) light with energy 21.22 eV as theionization source. Photoelectrons were detected withkinetic energy values 5.63 eV and also with 4.53 eV. Calculate the ionization energy for each group of electrons.Identify the MOs that were most likely the sources ofthese two groups of electrons.
What is the most probable position of a 1s electron in Li2+?

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12. Why does Li have a larger first ionization enengy than Na? OA Because Li has only 3 electrons and they are less shielded from the force of attraction from the nucleus unike those on Na OR Because Li is more electronegative than Na OC All of them above OD. None of them above