(a)
Interpretation:
From the given titanium species, one with diamagnetic property has to be identified.
Concept Introduction:
Diamagnetic: When atoms or ions with all electrons are paired their magnetic field effectively cancels each other. Substances with paired electrons are called diamagnetic. They are weakly repelled by magnetic fields.
(b)
Interpretation:
The titanium species that attracted more to magnetic field has to be explained.
Concept Introduction:
Paramagnetic: Atoms or ions with unpaired electrons are attracted to magnetic field. Substances with unpaired electrons are called paramagnetic.
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Chapter 5 Solutions
OWLv2 for Moore/Stanitski's Chemistry: The Molecular Science, 5th Edition, [Instant Access], 1 term (6 months)
- Consider 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_forward6. Gallium arsenide (GaAs) is used in the red lasers of bar-code readers. (a) Write the full, ground state electron configuration of both gallium and arsenic. (b) Identify how many valence electrons each atom has. (c) Using electron configurations, show what the most likely ions to form would be for both Ga and As. (d) Predict whether (i) the most likely ion for gallium be smaller or larger than its neutral atom and (ii) the arsenic ion be smaller or larger than its neutral atom. Explain your predictions.arrow_forwardDetermine the number of valence electrons and give the electronic confi guration of the valence electrons of each element: (a) nitrogen; (b) potassium.arrow_forward
- 5. Draw orbital diagrams for the ground states of: (a) Terbium, Tb, a lanthanide element. (b) The manganese(II) ion, Mn2+. (c) The sulphide ion, S2–. (d) Silver, Ag.arrow_forwardGive the values of the four quantum numbers of an electron in the following orbitals: (a) 3s, (b) 4p, (c) 3d.arrow_forward(a) How does the Bohr model differ from the quantum mechanical model of the atom? Describe at least 2 differences.(b) Define each of the 4 quantum numbers (n, l, ml, ms) and what they physically represent about the orbital and/or electron.(d) How many quantum numbers are needed to completely define a specific orbital? Provide the quantum numbers for the 2s orbital.(d) How many quantum numbers are needed to completely define a specific electron? Provide the quantum numbers for the second electron to fill into a 2s orbital.arrow_forward
- Answer the following. (a) Write out the electronic configuration of the ground state for fluorine (Z = 9). O 1s²2s²2p¹ O 1s²2s²2p² O 1s²2s²2p³ O1s²2s²2p4 O 1s²2s²2p5 O 1s²2s²2p6 (b) Write out the values for the set of quantum numbers n, l, m, and må for each of the electrons in fluorine. (In cases where there are more than one value, enter the positive value first. Enter positive values without a '+' sign in front of them. Include all possible values.) 1s states n = 2s states n = 2p states n= l = P یے || = m = 0m₂ = m m m m m ms m S S m ms ms S ms = ms ms || || || = || = || ||arrow_forwardThe ground configuration of a Ti2+ ion is [Ar]3d2 (a) What is the term of lowest energy and which level of that term lies lowest? (b) How many states belong to that lowest level?arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning