Consider the orbitals shown here in outline.800(x)(y)(Z)What is the maximum number of electrons contained in an orbital of type (x)? Of typeHow many orbitals of type (x) are found in a shell with n = 2? How many of type (y)? HeWrite a set of quantum numbers for an electron in an orbital of type (x) in a shell with ne (y) in a shell with n = 2. Of an orbital of type (z) in a shell with n =3.What is the smallest possible n value for an orbital of type (x)? Of type (y)? Of type (z)?What are the possible / and m, values for an orbital of type (x)? Of type (y)? Of type (z)?State the Heisenberg uncertainty principle. Describe briefly what the principle implies.

According to the concept of quantum chemistry, orbitals are the places in which probability of…

Nhat is the maximum number of electrons contained in an orbital of type (x)? Of type How many orbitals of type (x) are found in a shell with n = 2? How many of type (y)? F Nrite a set of quantum numbers for an electron in an orbital of type (x) in a shell with e (y) in a shell with n = 2. Of an orbital of type (z) in a shell with n = 3. What is the smallest possible n value for an orbital of type (x)? Of type (y)? Of type (z) What are the possible / and m, values for an orbital of type (x)? Of type (y)? Of type () State the Heisenbera uncertainty principle Describe briefly what the principle implies

Nhat is the maximum number of electrons contained in an orbital of type (x)? Of type How many orbitals of type (x) are found in a shell with n = 2? How many of type (y)? F Nrite a set of quantum numbers for an electron in an orbital of type (x) in a shell with e (y) in a shell with n = 2. Of an orbital of type (z) in a shell with n = 3. What is the smallest possible n value for an orbital of type (x)? Of type (y)? Of type (z) What are the possible / and m, values for an orbital of type (x)? Of type (y)? Of type () State the Heisenbera uncertainty principle Describe briefly what the principle implies

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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Suppose an atom with its nucleus at the origin has an electron in a 1s orbital. Complete each row of the table below by deciding how PA, the probability of finding the electron at point A, compares to PB, the probability of finding the electron at point B. This sketch is about 200 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. point A 10 pm to the left of the nucleus, along the -x axis. 10 pm in front of the nucleus, along the -y axis. Continue 10 pm to the right of the nucleus, along the +x axis. point B 10 pm behind the nucleus, along the +y axis. 10 pm below the nucleus along the -z axis. 10 pm above the nucleus, along the +z axis. compare PA to PB OP PA P OPA B O PA
Which of the following sets of quantum numbers describes an electron in the 5s subshell? A. n = 5, l = 1, ml = 1, ms = -1/2 B. n = 5, l = 0, ml = 0, ms = -1/2 C. n = 5, l = 2, ml = 2, ms = +1/2 D. n = 5, l = 4, ml = 4, ms = -1/2 E. n = 5, l = 3, ml = 0, ms = +1/2
1. Sketch the shape of the orbital with the quantum numbers n=3, {=0 and mẹ = 0 2. The sketch of the shape of the subshell with the quantum numbers n=4, €=2 3. The highest orbital possible in n= 4 %3D
[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 3p orbital shown above, enter a possible value for each quantum number. eq n = eg eq Give ONE example. req m, = Give ONE example. req Though a given electron only has one value for m, there are v possible m values for electrons in 3p orbitals. 2reg Submit Answer Retry Entire Group No more group attempts remain 2req
Match each of the following with its correct answer How many electrons are in the following quantum number orbital, n=2,1=1, ml =1, ms = +1/2 Choose... Choose... Give the designation for the following quantum number,n=3, /=0 3P 4. 35 2. How many electrons are in the following quantum number orbital, n=2,1= 1 Choose... How many electrons are in the following quantum number orbital, n-2, 1 = 1, ml =D1 Choose... Give the designation for the following quantum number, n=3, /= Choose.. v
Q8a. Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error and explain .I. n = 5, l = 3, ml =-3II. n = 4, l = 4, ml =0III. n = 4, l = 0, ml =-1IV. n = 3, l = 1, ml = -2V. n = 3, l = 2, ml =+3
Which of the following sets of quantum numbers can describe an electron with spin down in a 5f orbital? On = 5 l = 4 mg = -2 m, = - On = 5 l = 3 me = -3 m, = + On = 5 l = 3 mg = -2 m; = - O n = 5 l = 2 me = 0 1 m, = - 1/2
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 A' the probability of finding the electron at point A, compares to P the probability of finding the electron at point B. B' point A point B compare PA to PB O 'A Р. A В A В P = P 100 pm behind the nucleus, along the +y axis. 100 pm to the left of the nucleus, along the -x axis. A В Р. > Р. A В P Р A В
What is the maximum number of electrons that can be identified with each of the following sets of quantum numbers? If there are none, enter 0. a. n = 2, ms -1/2 electron(s) = 3 electron(s) c. n = 4, l = 0, me electron(s) b. n = 3, l = d. n = 6, l = = electron(s) 0, ms 1, me = -1 = +1/2
Indicate whether the following sets of quantum numbers are allowed. If it is, indicate the orbitalthat the electron occupies. If it isn’t, indicate why.a. n = 0, l = 0, ml = 0, ms = +½b. n = 6, l = 0, ml = 1, ms = +½c. n = 1, l = 0, ml = 0, ms = -1d. n = 5, l = 1, ml = -1, ms = +½e. n = 4, l = 4, ml = 0, ms = -½f. n = 2, l = 0, ml = 0, ms = +½g. n = 4, l = 2, ml = -1, ms = -½
Which of the following is NOT a valid set of quantum numbers? Select one: а. n = 2, 1 = 1, and ml= +1 O b. n = 3, 1 = 2, and ml= -2 С. n = 6, I = 5, and ml= 0 O d. n = 2,1 = 2, and ml= +1