11c Answer the following questions regarding ionizationenergy.Part CReset HelpshieldingWhen comparing the first ionization energies of elements within the same period, itnoted that boroneffectivelyhas afirst ionization energy than beryllium. This is due to theof theelectrons from thesubshell to an area closer to the nucleus, which is not possible for2stheelectron present in theatom. As a result, this electron isgreatershielded, making itto remove.penetrationeasiersmallerberyllium2pboronharderineffectively

Ionisation Energy : The amount of energy required to remove most loosely bound electron from the…

When comparing the first ionization energies of elements within the same period, it is noted that boron has a electrons from the shielding effectively first ionization energy than beryllium. This is due to the of the subshell to an area closer to the nucleus, which is not possible for 25 the electron present in the atom. As a result, this electron is greater shielded, making it to remove. penetration

When comparing the first ionization energies of elements within the same period, it is noted that boron has a electrons from the shielding effectively first ionization energy than beryllium. This is due to the of the subshell to an area closer to the nucleus, which is not possible for 25 the electron present in the atom. As a result, this electron is greater shielded, making it to remove. penetration

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter11: Modern Atomic Theory

Section: Chapter Questions

Problem 11ALQ: r Questions 11—13, you will need to consider ionizations beyond the first ionization energy. For...

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(a) Predict the atomic number of the (as yet undiscovered) alkali-metal element in the eighth period. (b) Suppose the eighth-period alkali-metal atom turned out to have atomic number 137. What explanation would you give for such a high atomic number (recall that the atomic number of francium is only 87)?
r Questions 11—13, you will need to consider ionizations beyond the first ionization energy. For example, the second ionization energy is the energy to remove a second electron from an element. Compare the first ionization energy of helium to its second ionization energy, remembering that both electrons come from the 1s orbital. l> X Y First 170 200 second 350 400 Third 1800 3500 fouth 2500 5000 entify the elements X and Y. There may be more than one answer. so explain completely.
In each of the following sets of elements, which element would he expected to have the highest ionization energy? msp;a.Cs,K,Lic.l,Br,Clb.Ba,Sr,Cad.Mg,Si,S
The energy needed to remove one electron from a gaseous potassium atom is only about two-thirds as much as that needed to remove one electron from a gaseous calcium atom, yet nearly three times as much energy as that needed to remove one electron from K+ as from Ca+ . What explanation can you give for this contrast? What do you expect to be the relation between the ionization energy of Ca+ and that of neutral K?
Cesium is used extensively in photocells and in television cameras because it has the lowest ionization energy of all the stable elements. (a) What is the maximum kinetic energy of a photoelectron ejected from cesium by 520 nm light? Note that if the wavelength of the light used to irradiate the cesium surface becomes longer than 660 nm, no photoelectrons are emitted. (b) Use the rest mass of the electron to calculate the velocity of the photoelectron in (a).
The outermost electron in an alkali-metal atom is sometimes described as resembling an electron in the corresponding state of a one-electron atom. Compare the first ionization energy of lithium with the binding energy of a 2s electron in a one-electron atom that has nuclear charge Zeff , and determine the value of Zeff that is necessary for the two energies to agree. Repeat the calculation for the 3s electron of sodium and the 4s electron of potassium.
The first ionization energies of As and Se are 0.947 and 0.941 MJ/mol, respectively. Rationalize these values in terms of electron configurations.
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.
Discuss briefly the difference between an orbit (as described by Bohr for hydrogen) and an orbital (as described by the more modern, wave mechanical picture of the atom).
Describe the properties of an electron associated with each of the following four quantum numbers: n,l,ml, and ms.