2. A graph shown below shows first ionization energies for elements from H to Ne. First ionization energy/kJ mol 2500 2000 1500 1000 500 T T T T 1 2 3 5 6 7 8 9 10 Atomic number a) Using arguments of electronic structure, explain why ionization energy of Li is much lower than that of H. (2 points) then dips at O. b) Using the same arguments, explain why ionization energy increases from B to N, and (3 points)

2. A graph shown below shows first ionization energies for elements from H to Ne. First ionization energy/kJ mol 2500 2000 1500 1000 500 T T T T 1 2 3 5 6 7 8 9 10 Atomic number a) Using arguments of electronic structure, explain why ionization energy of Li is much lower than that of H. (2 points) then dips at O. b) Using the same arguments, explain why ionization energy increases from B to N, and (3 points)

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter5: Quantum Mechanics And Atomic Structure

Section: Chapter Questions

Problem 39P: Without consulting any tables, arrange the following substances in order and explain your choice of...

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Before the element scandium was discovered in 1879, it was known as “eka-boron.” Predict the properties of scandium from averages of the corresponding properties of its neighboring elements in the periodic table. Compare your predictions with the observed values in Appendix F.
At large interatomic separations, an alkali halide molecule MX has a lower energy as two neutral atoms, M+X ; at short separations, the ionic form (M+)(X) has a lower energy. At a certain distance, Rc , the energies of the two forms become equal, and it is near this distance that the electron will jump from the metal to the halogen atom during a collision. Because the forces between neutral atoms are weak at large distances, a reasonably good approximation can be made by ignoring any variation in potential V(R) for the neutral atoms between Rc and R= . For the ions in this distance range, Rc is dominated by their Coulomb attraction. (a) Express Rc for the first ionization energy of the metal M and the electron affinity of the halogen X. (b) Calculate Rc for LiF, KBr, and NaCl using data fromAppendix F.
rite the proper charges so that an alkali metal, a noble gas, and a halogen have the same electron configurations. What is the number of protons in each“? The number of electrons in each? Arrange them from smallest to largest radii and explain your ordering rationale.
To ionize Mg to Mg2+ costs two times as much energy as to form Mg+. The formation of O2- is endothermic rather than exothermic as for O-. Nevertheless, magnesium oxide is always formulated as Mg2+ O2- rather than Mg+O-a) Give theoretical reason for formulation of Mg2+O2-b) What simple experiment could be done to predict that magnesium oxide wasnot Mg+O- ?
WLV2 | Online teachin X OWLV2 | Online teachin X b My Questions | bartleb X O mySigTau M COMM.1113: FUND OF x w.com/ilrn/takeAssignment/takeCovalentActivity.do?locator=assignment-take [References] Arrange the following groups of atoms in order of increasing first ionization energy. (Enter multiple answers as a comma-separated list.) a. Na, K, Mg b. Br, Ne, Rb c. Fe, P, O Submit Answer Try Another Version 3 item attempts remaining
The ability of atoms to associate with each other depends ona) the electronic structure and its spatial orientation.b) the electron affinity.c) The other two answers are correct.
Energy of Interaction of Point Charges Coulomb's Law yields an expression for the energy of interaction for a pair of point charges. V = V is the energy (in J) required to bring the two charges from infinite distance separation to distance r (in nm). Q1 and Q₂ are the charges in terms of electrons. (i.e. the constant in the above expression is 2.31x10-19 J nm electrons-2) d For a group of "point" charges (e.g. ions) the total energy of interaction is the sum of the interaction energies for the individual pairs. Calculate the energy of interaction for the square arrangement of ions shown in the diagram below. (+2) 2.31 x 10-1⁹Q1 Q2 d T d = 0.900 nm. (+2) d
Order the elements S, CI, and F in terms of increasing ionization energy. (lowest to highest) OF, S, CI O CI, F, S OF, CI, S OS, CI, F O S, F, CI
4. Predict which element of the following couples will have higher ionization energy. Justify your answer. a) Na vs. K: b) P vs. S: c) Mg vs. Al:
1.) a.) True or false: Elements with high ionization energies tend to have lave electron affinities as well. Explain why in terms of nuclear chargeb.) The size of the transition metals decreases slightly in going from left to right across the period. Explain in terms of nuclear charge.c.) Carbon monoxide has a larger bond dissociation energy (1072 Kj/mol) than molecular nitrogen (N2, 945 Kj/mol). Suggest an explanationd.) Given that both the electronic configuration of Ca ([Ar] 4s2 and Zn ([Ar] 3d10 4s2 end with 4s2, explain the difference between the first ionization energy of Ca (IE1 = 590Kj/mol) and Zn (IE1 =906 kJ/mol) e.) In general, ionization energies increase across a period from left to right. Explain why the second ionization energy of Cr is higher, not lower, than that of Mn f.) Which of each of the following pairs of molecules has the larger bond angle? Explain your reasoning. i.) PH3 and NH3
QUESTION ONE a. Complete the electron configurations using s, p, d notation for the following atoms or ions: CI Zn2+ AI3+ Cr b. State which has the larger radius, Al or Al3+. Justify your answer: Expl the factors infuench e ns ret loton neroy and ao Deriod snd dosna group ter to hese oloments. c. (i) Explain what is meant by first ionisation energy. (ii) Write a balanced equation for the first ionisation of a chlorine atom
Use the periodic table to (i) predict electron configurations for the following species: Arsenic ion, As3– Magnesium ion, Mg2+ Vanadium(II) ion, V2+ (ii) Write the electron configurations of each species in the noble gas notation. (iii) Draw an orbital diagram to represent 1 c above. Draw the Lewis electron dot structures of the following chemical species. In each case you must say whether or not the central atom obeys the Octet Rule. CS2 and H2S CF4 and SiH4 NH2Cl CO32– and BF3 PCl5 ClF3, XeF2, Calculate the formal charge on the Sulphur atom in the Sulphate anion structure shown below(picture attatched) Give the electron-pair and molecular geometries for NF3 and XeF4.

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