Question

NEED HELP!!
Which of the following quantum number combinations is not allowed in an atom?

n = 2, l = 0, m subscript l = 0

n = 3, l = 2, m subscript l = -1

n = 6, l = 5, m subscript l = -4

n = 1, l = 0, m subscript l = 1

@ganeshie8

Answer 1

are you familiar with the quantum number rules?

http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch6/quantum.html#rules
Rules Governing the Allowed Combinations of Quantum Numbers

The three quantum numbers (n, l, and m) that describe an orbital are integers: 0, 1, 2, 3, and so on.
The principal quantum number (n) cannot be zero. The allowed values of n are therefore 1, 2, 3, 4, and so on.
The angular quantum number (l) can be any integer between 0 and n - 1. If n = 3, for example, l can be either 0=s, 1=p, or 2=d.
The magnetic quantum number (m) can be any integer between -l and +l. If l = 2, m can be either -2, -1, 0, +1, or +2.

Answer 2

Im so lost in Chemistry its crazy haha

but would it be A?

Answer 3

@Cuanchi

Answer 4

Yea you are lost!! I dont think that A is the correct answer.

Answer 5

D?!

Answer 6

That has better chances!! I would go for that, did you got it or just guessed

Answer 7

well i ruled out B and C so it had to be A or D

Answer 8

good approach!