Suppose an atom with its nucleus at the origin has an electron in a 2p, orbital. Complete each row of the table below by deciding how P the probability of finding the electron at point A, compares to P, the probability of finding the electron at point B. point A point a compare Pa to P. 100 pm in front of the nucleus, along the y axis. 100 pm to the left of the nudeus, along the x axis o ,P, 100 pm below the nucleus along the -z axis, 100 pm behind the nucleus, along the +y axis, 100 pm above the nucleus, along the +z axis. 100 pm to the right of the nucleus, along the +x axis.

Suppose an atom with its nucleus at the origin has an electron in a 2p, orbital. Complete each row of the table below by deciding how P the probability of finding the electron at point A, compares to P, the probability of finding the electron at point B. point A point a compare Pa to P. 100 pm in front of the nucleus, along the y axis. 100 pm to the left of the nudeus, along the x axis o ,P, 100 pm below the nucleus along the -z axis, 100 pm behind the nucleus, along the +y axis, 100 pm above the nucleus, along the +z axis. 100 pm to the right of the nucleus, along the +x axis.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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References Use the References to access important values if needed for this question. The Pauli Exclusion Principle tells us that no two electrons in an atom can have the same four quantum numbers. For an electron in the 2p orbital shown above, enter a possible value for each quantum number. n = mį = Give ONE example. m, = Give ONE example. Though a given electron only has one value for mi, there are possible m, values for electrons in 2p orbitals.
O ELECTRONIC STRUCTURE Interpreting the angular probability distribution of an orbital This sketch is about 800 pm wide. The coordinate (x, y, and z) axes are also shown. You can rotate the sketch for a better view of the orbital by dragging the slider with your mouse. i II IIIII Suppose an atom with its nucleus at the origin has an electron in a 2p, orbital. Complete each row of the table below by deciding how P, the probability of finding the electron at point A, compares to PR, the probability of finding the electron at point B. point A point B compare PA to P P 100 pm in front of the nucleus, along the -y axis. 100 pm to the left of the nucleus, along the -x axis. O P. = P. O P, > P 100 pm behind the nucleus, along the +y axis. 100 pm below the nucleus along the -z axis. O P, = P O P,> P O P, P, Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessibility MacBook Pro
Use the References to access important values if needed for this question. In the Bohr model of the hydrogen atom, the electron occupies distinct energy states. One transition between energy states of the hydrogen atom is represented by the picture. n=x TTH n=4- n=3 n-2 n=1 - In this transition an electron moves from the n = Energy is - The electron moves - 6 in this process. I the nucleus. tv♫♫ ON al ZA Cas W References level to the n = N MacBook Pro level. 11 IT T T 11
D. Give the quantum numbers for the last electron of each element given in Part II following the table below. Element 1 subshell N - 7 1s22s22p3 70 Ga,17⁰ Ar 1840 Sb,1122 112 AU79197 n main energy level 2 s=0 p=1 d=2 f=3 1 m₁ orbital -1 to 0 to +1 -1, 0, +1 +1 m₂ magnetic spin (+1/2, -1/2) +1/2
Consider an electron in a hydrogen atom that undergoes a transition from n = 3 to n = 7.a. Is the atom undergoing absorption or emission?b. What is the change in energy of the atom?c. What is the wavelength (in nm) of the photon absorbed or emitted?d. What is the frequency of the photon absorbed or emitted?
5. Down a group in the periodic table: Do you think the ionization energy of Lithium (Li) is larger or smaller than that of Sodium (Na)?A. Larger B. Smaller C. Same D. Don’t KnowWhat did you base your answer on?6. Across a row in the periodic table: Do you think the ionization energy of Lithium (Li) is larger or smaller than that of Neon (Ne)?A. Larger B. Smaller C. Same D. Don’t KnowWhat did you base your answer on?
1, eight electrons with n = = 2, A neutral atom has two electrons with n = and seven electrons with n = 3. Assuming this element is in its ground state, supply the following information: a. atomic number Atomic number = b. total number of s electrons s electron(s) c. total number of p electrons p electron(s) d. total number of d electrons d electron(s) e. Is the element a metal, metalloid, or nonmetal? metal O metalloid nonmetal
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