6ab 10mins asap Part AConstruct the orbital diagram to show the electron configuration of phosphorus, P.Be sure to arrange the subshells in order of energy, with the lowest-energy subshell at the left and the highest-energy subshell at the right.Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all.• View Available Hint(s)ResetHelp1s2s2p3s3p3d4s4p4d4f1LG2G2G2G2G2G2G2G2G2G1G1G1G1G1 Part BConstruct the orbital diagram to show the electron configuration of iron, Fe.Be sure to arrange the subshells in order of energy, with the lowest-energy subshell at the left and the highest-energy subshell at the right.Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all.• View Available Hint(s)Reset Help1s2s2p3s3p3d4p4d4fG2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G1G1G1G1G1G1G1

According to the Aufbau principle, the electrons are filled according to the increasing energy of…

Construct the orbital diagram to show the electron configuration of phosphorus, P. Be sure to arrange the subshells in order of energy, with the lowest-energy subshell at the left and the highest-energy subshell at the right. Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all. ► View Available Hint(s) Reset Help 1| 1L 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f G2 G2 G2| G2| G2 G2 G2 G2 G2 G1 G1 G1 G1 G1

Construct the orbital diagram to show the electron configuration of phosphorus, P. Be sure to arrange the subshells in order of energy, with the lowest-energy subshell at the left and the highest-energy subshell at the right. Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all. ► View Available Hint(s) Reset Help 1| 1L 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f G2 G2 G2| G2| G2 G2 G2 G2 G2 G1 G1 G1 G1 G1

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 12ALQ

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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.
Many times the claim is made that subshells half-filled with electrons are particularly stable. Can you suggest a possible physical basis for this claim?
Without looking at data in the text, sketch a qualitative graph of the third ionization energy versus atomic number for the elements Na through Ar, and explain your graph.
Which atom would be expected to have a half-filled 4s subshell?
Suppose that the spin quantum number could have the values 12,0 and 12 . Assuming that the rules governing the values of the other quantum numbers and the order of filling sublevels were unchanged, (a) what would be the electron capacity of an s sublevel? a p sublevel? a d sublevel? (b) how many electrons could fit in the n=3 level? (c) what would be the electron configuration of the element with atomic number 8? 17?
Which atom would be expected to have a half-filled 6p subshell?
Answer the following questions: (a) Without using quantum numbers, describe the differences between the shells, subshells, and orbitals of an atom. (b) How do the quantum numbers of the shells, subshells, and orbitals of an atom differ?
Write the valence-electron configuration of each of the following elements, basing your answer on the element’s location on the periodic table. uranium, Z=92 c. mercury, Z=80 manganese, Z=25 d. francium, Z=87
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Use the aufbau procedure to obtain the electron configuration and orbital diagram for atoms of the following elements. (a) Be (b) B (c) Ne (d) Rb
• list the number of orbitals of each type (1s, 3p, etc) in an atom.