Use the rules for determining electron configurations to write the electron configuration for P. Express your answer in complete form in order of increasing orbital energy. For example, 1s? 2s? should be entered as 1s^22s^2. • View Available Hint(s) 1s^22s^22p^63s^23p^23p^3 Previous Answers Submit X Incorrect; Try Again; 13 attempts remaining

Use the rules for determining electron configurations to write the electron configuration for P. Express your answer in complete form in order of increasing orbital energy. For example, 1s? 2s? should be entered as 1s^22s^2. • View Available Hint(s) 1s^22s^22p^63s^23p^23p^3 Previous Answers Submit X Incorrect; Try Again; 13 attempts remaining

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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Similar questions

In defining the sizes of orbitals, why must we use an arbitrary value, such as 90% of the probability of finding an electron in that region?
Is the following statement true or false? The hydrogen atom has a 3s orbital. Explain.
The table below is partially completed for subshells A and B, where subshell B is the next subshell higher in energy compared to subshell A. For example, if subshell A is the 4s subshell, then subshell B would be the 3d subshell. Use this criteria and the information provided to complete the table.
The energy emitted when an electron moves from a higher energy state to a lower energy state in any atom can be observed as electromagnetic radiation. (a) Which involves the emission of less energy in the H atom, an electron moving from n = 4 to n = 2 or an electron moving from n = 3 to n = 2? (b) Which involves the emission of more energy in the H atom, an electron moving from n = 4 to n = 1 or an electron moving from n = 5 to n = 2? Explain fully.
(a) Give the complete electron configuration (1s22s22p) of aluminum in the ground state. (b) The wavelength of the radiation emitted when the outermost electron of aluminum falls from the 4s state to the ground state is about 395 nm. Calculate the energy separation (in joules) between these two states in the Al atom. (c) When the outermost electron in aluminum falls from the 3d state to the ground state, the radiation emitted has a wavelength of about 310 nm. Draw an energylevel diagram of the states and transitions discussed here and in (b). Calculate the separation (in joules) between the 3d and 4s states in aluminum. Indicate clearly which has higher energy.
In the second row of the periodic table, Be, N, and Ne all have positive (unfavorable) electron affinities, whereas the other second-row elements have negative (favorable) electron affinities. Rationalize why Be, N, and Ne have unfavorable electron affinities.
6.29 A mercury atom emits light at many wavelengths, two of which are at 435.8 and 546.1 nm. Both of these transitions are to the same final state. (a) What is the energy difference between the two states for each transition? (b) lf a transition between the two higher energy states could be observed, what would be the frequency of the light?