We need to find an element that is able tohave a lot of un-paired electrons. The moredegenerate (same energy) orbitals asublevel/subshell has, the more unpairedelectrons the atom can contain. The periodictable below has highlighted all of theelements that are filling electrons intosublevels/subshells with degenerate orbitals(multiple orbitals of equal energy, such as thethree p orbitals in a p subshell).18PERIODIC TABLE OF THE ELEMENTSHНеNAVAVIACNO140 .00 0 20.184 ISLi BeBF NeNa Mg22.9912AI Si PSCIAr1019K Ca Sc Ti v Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr53 54Rb Sr Y Zr Nb Mo Te Ru Rh Pd Ag Cd In Sn Sb Te1 XeCs Ba La Hf Ta w Re Os Ir Pt Au Hg TI Pb Bi Po At RnFr Ra 'Ac Rf Db Sg Bh Hs Mt Ds Rg*Lanthanide Series Ce Pr Nd Pm Sm Eu Gd Tb| Dy Ho Er Tm Yb Lu14424 (145)92tActinide Series Th Pa U15197 15725 158.93 162.50 1649395 96 97 9 100 101 102 103Pu Am Cm Bk| Cf Es Fm Md No Lr140.12 140150.4174979394X232.04 2104 2.05(237)(244Explain which regions of the periodic tablewould be best for holding multiple unpairedelectrons. Make sure to discuss whatsubshell is being filled with electrons in eachof those regions of the periodic table

Lone pair or unpaired electron are those electrons which are present in outermost shell of atom. Let…

We need to find an element that is able to have a lot of un-paired electrons. The more degenerate (same energy) orbitals a sublevel/subshell has, the more unpaired electrons the atom can contain. The periodic table below has highlighted all of the elements that are filling electrons into sublevels/subshells with degenerate orbitals (multiple orbitals of equal energy, such as the three p orbitals in a p subshell). PERIODIC TABLE OF THE ELEMENTS H 14 16 VIA Не 17 NA VIA 4.00 Li Ве B CNOF Ne Na Mg 2Al Si P S CIA. 22 2430 19 20 K Ca Sc Ti v Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 30.0 37 38 Rb Sr Y Zr Nb Mo Te Ru Rh Pd Ag Cd In Sn Sb Te I Xe- 56 Cs Ba "La Hf Ta w Re Os Ir Pt Au Hg TI Pb Bi Po At Rn IN 87 Fr Ra 'Ac Rf Db Sg Bh Hs Mt Ds Rg (22 202as *Lanthanide Series Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu 4012 4 2 4 7 9 "Actinide Series Th Pa Ux Pu Am Cm Bk Cf Es Fm Md No Lr 100 101 102 10 Explain which regions of the periodic table would be best for holding multiple unpaired electrons. Make sure to discuss what SU subshell is being filled with electrons in each of those regions of the periodic table

We need to find an element that is able to have a lot of un-paired electrons. The more degenerate (same energy) orbitals a sublevel/subshell has, the more unpaired electrons the atom can contain. The periodic table below has highlighted all of the elements that are filling electrons into sublevels/subshells with degenerate orbitals (multiple orbitals of equal energy, such as the three p orbitals in a p subshell). PERIODIC TABLE OF THE ELEMENTS H 14 16 VIA Не 17 NA VIA 4.00 Li Ве B CNOF Ne Na Mg 2Al Si P S CIA. 22 2430 19 20 K Ca Sc Ti v Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 30.0 37 38 Rb Sr Y Zr Nb Mo Te Ru Rh Pd Ag Cd In Sn Sb Te I Xe- 56 Cs Ba "La Hf Ta w Re Os Ir Pt Au Hg TI Pb Bi Po At Rn IN 87 Fr Ra 'Ac Rf Db Sg Bh Hs Mt Ds Rg (22 202as *Lanthanide Series Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu 4012 4 2 4 7 9 "Actinide Series Th Pa Ux Pu Am Cm Bk Cf Es Fm Md No Lr 100 101 102 10 Explain which regions of the periodic table would be best for holding multiple unpaired electrons. Make sure to discuss what SU subshell is being filled with electrons in each of those regions of the periodic table

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 126CP

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Similar questions

No currently known elements contain electrons in g ( l=4) orbitals in the ground state. If an element is discovered that has electrons in the g orbital, what is the lowest value for n in which these g orbitals could exist? What are the possible values of m l ? How many electrons could a set of g orbitals hold?
The first ionization energy of helium is 2370kJmol1 , the highest for any element. (a) Define ionization energy and discuss why for helium it should be so high. (b) Which element would you expect to have the highest second ionization energy? Why? (c) Suppose that you wished to ionize some helium by shining electromagnetic radiation on it. What is the maximum wavelength you could use?
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.
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.
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