a)
For n=1, l can be 0
For l=0, ml can be only 0
The sets are:
(1,0,0,+1/2)
(1,0,0,-1/2)
b)
For n=2, l can be 0, 1
For l=0, ml can be only 0
For l=1, ml can be -1, 0, 1
The sets are:
(2,0,0,+1/2)
(2,0,0,-1/2)
(2,1,-1,+1/2)
(2,1,-1,-1/2)
(2,1,0,+1/2)
(2,1,0,-1/2)
(2,1,1,+1/2)
(2,1,1,-1/2)
c)
n=4 and l=2
For l=2, ml can be -2, -1, 0, 1, 2
The sets are:
(4,2,-2,+1/2)
(4,2,-2,-1/2)
(4,2,-1,+1/2)
(4,2,-1,-1/2)
(4,2,0,+1/2)
(4,2,0,-1/2)
(4,2,1,+1/2)
(4,2,1,-1/2)
(4,2,2,+1/2)
(4,2,2,-1/2)
ASAP PLRASE! 2. Using the (n, l, m ,me) notation, give the set of 4 quantum...
ASAP PLEASE! Chemistry 111 ADDITIONAL HOMEWORK PROBLEMS FOR CHAPTER 6 1. State the number of orbitals that can have the following designa- tions: a. 3p b. 4p c. n = 5 d. 60 e. 58 f. 75 2. Using the in, l, m , m) notation, give the set of 4 quantum numbers associated with each allowed electronic energy state in: a. the n = 1 shell b. the n = 2 shell the 4d subshell
ASAP PLEASE! Chemistry 111 ADDITIONAL HOMEWORK PROBLEMS FOR CHAPTER 6 1. State the number of orbitals that can have the following designa- tions: а. Зр с. n %3D 5 b. 4p d. 6d f. 7s e. 5f notation, give the set of 4 quantum 2. Using the (n, 1, m numbers associated with each allowed electronic energy state in: ms) the n 1 shell а. the n 2 shell b. the 4d subshell с.
8. For the principle quantum level n= 4, determine the allowable values of and give the designation of each subshell. allowable values of l= 0,1,2.3 designations of the subshells: S.P. O.FI 9. Label the following sets of quantum numbers as "allowed" or "not allowed." For each incorrect set, state why it is not allowed. a)n=3, 13, m, 0 not allowed ben cannot equal 3 only 0,112 b)n=4,2=3, m =2 c)n=4, 1=1, m,=1 d)n=5, 1=4, m=2 e)n=3,1=1, m,=2
Choose the answer that lists an allowed set of quantum numbers (n. I, and ml) for an electron in the specified subshell. Select one: on=5,1 = 3, and m/ = 3 is allowed for an electron in a 5f subshell. on = 4,1 = 3, and m = -3 is allowed for an electron in a 4d subshell. on=7,1 = 3, and m = 3 is allowed for an electron in a 7d subshell on=6,1 = 3, and m -...
Which of the following set of quantum numbers (ordered n,l,ml,ms) are possible for an electron in an atom? Quantum Number Rules Learning Goal: To learn the restrictions on each quantum number. Quantum numbers can be thought of as labels for an electron. Every electron in an atom has a unique set of four quantum numbers. The principal quantum number n corresponds to the shell in which the electron is located. Thus n can therefore be any integer. For example, an...
a) The quantum number n describes the of an atomic orbital and the quantum number l describes its b) When n = 3, the possible values of l are: c) What type of orbital corresponds to l = 3? d) What type of atomic orbital has 2 nodal planes? e) The maximum number of orbitals that may be associated with the quantum number set n = 4, l = 3, and ml = -2 is f) How many subshells...
a) Give the orbital notation for electrons in an orbital with the following quantum numbers: n = 3, l = 2, ml = -1 b) Select the possible orientation labels for electrons in an orbital with the following quantum numbers: n = 3, l = 2, ml = -1 Select one or more: a. dxz b. dxy c. s d. dyz e. py f. dx(2)-y(2) g. px h. pz i. dz(2) c) List all the possible combinations of quantum numbers...
Orbitals and Quantum Numbers Each atomic orbital is specified by a unique set of n, l and ml quantum numbers: 1a. What quantum number/s do the two spherical orbitals have in common? What quantum number/s would be different? Are these orbitals s, p or d? 1b. Write down a possible set (n, l, ml) of quantum numbers for each spherical orbital. 1c. Consider the dumb-bell shaped orbitals. What quantum number/s do these three orbitals have in common? What quantum number/s...
Complete the table by pairing each set of quantum numbers with the orbital it describes. If the set of quantum numbers is not possible, label it as not allowed. Use each orbital description as many times as necessary. Orbital Quantum numbers n= 1,= 1, me = 0 Answer Bank L LLLLLLLLLLL 5d n = 4,8 = 2, me = 2 n = 2, t = 1, me = -1 not allowed tuttttttLLLLLLLLLLLLLLL not allowed 33 0 n = 3, t...
For each of the following combinations of quantum numbers, make changes that produce an allowed combination. Count 3 for cach change of n, 2 for each change of land 1 for cach change of me. Which quantum number needs to be changed to produce the lowest possible count that you can obtain? 2. n = 3,1 = 0, m = -3 1 m b. n = 5,1 5, m 4 On c. n = 3,1 = 3, m = -3...