Identify each statement as true or false: (a) Ionization energiesare always negative quantities. (b) Oxygen has a larger firstionization energy than fluorine. (c) The second ionizationenergy of an atom is always greater than its first ionizationenergy. (d) The third ionization energy is the energy neededto ionize three electrons from a neutral atom.

Identify each statement as true or false: (a) Ionization energiesare always negative quantities. (b) Oxygen has a larger firstionization energy than fluorine. (c) The second ionizationenergy of an atom is always greater than its first ionizationenergy. (d) The third ionization energy is the energy neededto ionize three electrons from a neutral atom.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter8: The Periodic Table: Structure And Trends

Section: Chapter Questions

Problem 8.11QE

See similar textbooks

Similar questions

6.82 A particular element has the following values for its first four ionization energies: 900, 1760, 14, 850, and 21,000 kJ/mol. Without consulting a list of ionization energy values, determine what group in the periodic table this element belongs in.
7.89 Which of the following properties show a clear periodicvariation: (a) first ionization energy, (b) molar mass ofthe elements, (c) number of isotopes of an element,(d) atomic radius?
(a) What is the general relationship between the size of anatom and its first ionization energy? (b) Which element inthe periodic table has the largest ionization energy? Whichhas the smallest?
Given the following information, identify the groupfrom the periodic table that contains elements that behave likemain-group element “E.”(i) The electron affinity of E is greater than zero.(ii) The ionization energy (IE) trend for element E is: firstionization energy < second ionization energy <<< thirdionization energy.(iii) Samples of E are lustrous and are good electricalconductors.
What is the relationship between the ionization energy of ananion with a 1- charge such as F- and the electron affinity ofthe neutral atom, F?
What is the relationship between the ionization energy of an anion with a -1 charge, such as F−, and the electron affinity of the neutral atom, F? Express your answer in terms of EF, which represents the electron affinity of the neutral atom, F.
7.20 Without referring to a periodic table, write the electronconfiguration of elements with the following atomicnumbers: (a) 9, (b) 20, (c) 26, (d) 33.
7.85 Arrange the following isoelectronic species in order ofincreasing ionization energy: O2−, F−, Na+, Mg2+.
7.119 The first four ionization energies of an element areapproximately 738, 1450, 7.7 × 103 , and 1.1 × 104kJ/mol.To which periodic group does this element belong?Explain your answer.
Based on the ionization energies of the alkali metals (see Section3.7), which alkali metal would you expect to undergo the most exothermic reaction with chlorine gas? Write a balanced chemical equation for the reaction.
Explain the relationship of the first ionization energy of an element and its atomic number.
4. What does presenter say about the relationship between the number of valence electrons of the main-group element and the group number of that element (except helium)?