1.) Which of the following combinations represent real orbitals and which are im

ID: 544822 • Letter: 1

Question

1.) Which of the following combinations represent real orbitals and which are impossible?

1s [ Select ] ["Real", "Impossible"]

2d [ Select ] ["Real", "Impossible"]

3p [ Select ] ["Real", "Impossible"]

5s [ Select ] ["Real", "Impossible"]

2.)

For the natural elements, the highest occupied shape is the f orbital. The g orbital would be the next shape following f.

In what level (n) would the lowest energy g orbitals exist?

How many orientations of the g orbitals would there be?

What is the maximum number of electrons that can exist in the g sublevel?

I got 4,9,and 18 but one of thte values is wrong and i sont know which one and why it owuld be wrong. Thankyou,

Kahtia Johnso

1)
1s is real
2d is impossible because n=2 can’t have d orbital (only 2s and sp are allowed)
3p is real
5s is real

2)
for g, l = 4
so, n must be 5
Answer: n=5
l=4 for g orbitals
number of orientation = number of orbitals = 2*l+1
= 2*4+1
= 9
Answer: 9

maximum number of electrons = number of orbitals * 2
= 9*2
= 18
Answer: 18

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