Question

1. Which of the following set of quantum numbers (ordered n, ℓ, mℓ, ms) are possible for an electron in an atom? Check all that apply.

a. 3, 2, 2, -1/2

b. -1, 0, 0, -1/2

c. 3, 2, 1, -1

d. 4, 3, 4, -1/2

e. 2, 2, 2, 1/2

f. 4, 3, -2, 1/2

g. 5, 2, 1, -1/2

h. 3, 1, -2, -1/2

2. How many possible combinations are there for the values of l and ml when n = 2? Express your answer as an integer. 3. Identify which sets of quantum numbers are valid for an electron. Each set is ordered (n,ℓ,mℓ,ms). Check all that apply.

a. 4,3,1,-1/2

b. 3,2,-1,-1/2

c. 1,0,0,1/2

d. 2,3,1,1/2

e. 3,1,-1,1/2

f. 0,2,1,-1/2

g. 2,2,-1, 1/2

h. 2,1,1,1/2

i. 2,-2,-2,-1/2

j. 1,3,0,1/2

k. 4,3,4,-1/2

L. 3,2,1,1

Answer 1

a) Possible and these values indicates electron in 3d subshell.

b) thiis set is not possible because n has negative value.

c) It is not possible becuase spin quantum number has value greater than 1/2

d) It is not possible because ml value is greater than l value.

e) It is not possible becuase l value is equal to n value. l should have values from 0 to n-1

f) It is possible and this set indicates electron in 4f subshell

g) It is possible and this set indicates electron in 5d subshell

h) It is not possible because ml should have values from -l to +l

There are three possible sets they are

a) , f) and g)

2) When n =2, l has 0 and 1 values

then possible combinations for l and ml are

0 and 0

1 and +1

1 and 0

1 and -1

total; combinations are 4

3) Valid sets are

a. 4,3,1,-1/2

b. 3,2,-1,-1/2

c. 1,0,0,1/2

e. 3,1,-1,1/2

h. 2,1,1,1/2