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 Mnf.) Which of each of the following pairs of molecules has the larger bond angle? Explain your reasoning. i.) PH3 and NH3 1.) a.) True or false: Elements with high ionizationenergies tend to have lave electron affinities as well.Explain why in terms of nuclear chargeb.) The size of the transition metals decreasesslightly in going from left to right across the period.Explain in terms of nuclear charge.c.) Carbon monoxide has a larger bond dissociationenergy (1072 Kj/mol) than molecular nitrogen (N2,945 Kj/mol). Suggest an explanationd.) Given that both the electronic configuration of Ca((Ar) 4s? and Zn ((Ar) 3d10 4s? end with 4s?, explain thedifference between the first ionization energy of Ca(IE1 = 590K¡/mol) and Zn (IE1 =906 kJ/mol)e.) In general, ionization energies increase across aperiod from left to right. Explain why the secondionization energy of Cr is higher, not lower, than thatof Mnf.) Which of each of the following pairs of moleculeshas the larger bond angle? Explain your reasoning.i.) PH3 and NH3

A few questions based on periodic table trends that is to be accomplished.

Answered: 1.) a.) True or false: Elements with…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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1.) a.) True or false: Elements with high ionization energies tend to have lave electron affinities as well. Explain why in terms of nuclear charge
b.) 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 explanation
d.) 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

1.) a.) True or false: Elements with high ionization
energies tend to have lave electron affinities as well.
Explain why in terms of nuclear charge
b.) 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 explanation
d.) Given that both the electronic configuration of Ca
((Ar) 4s? and Zn ((Ar) 3d10 4s? end with 4s?, explain the
difference between the first ionization energy of Ca
(IE1 = 590K¡/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

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