What is the lowest principal quantum number an electron can have?

[justwantin]

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I was reviewing Chemistry the Easy, an older study guide for self study chem, and I came across question #2 for the chapter review. It reads:

2. What is the lowest principal quantum number an electron can have?

A. 0
B. 1
C. 2
D. 3

I chose answer B, or 1, just because I can look at the periodic table and look at hydrogen (1s^1). However, the answer the book claims is C, or 2.

Is this just an error, or am I missing something?

 

[Akarat]

I was reviewing Chemistry the Easy, an older study guide for self study chem, and I came across question #2 for the chapter review. It reads:

2. What is the lowest principal quantum number an electron can have?

A. 0
B. 1
C. 2
D. 3

I chose answer B, or 1, just because I can look at the periodic table and look at hydrogen (1s^1). However, the answer the book claims is C, or 2.

Is this just an error, or am I missing something?

I think it's an error, because if n = 0, then the lowest l (the Azimuthal quantum number) would be -1, and that can't be right.

Last time I checked,
l = 1, s orbital
l = 2, p orbital
l = 3, d orbital
Etc...

 

[Doctorb2b]

I also believe it's an error, principal quantum numbers can only take on positive integer numbers

 

[kpatel1123]

l=0 is the s subshell not l=1. l=n-1. Therefore, s is l=0, p l=1, d l=3 etc. Easy way to remember this is the equation for the max number of electrons per subshell, 4l+2. Thus, for the s subshell l=0 and then the max number of electrons in s subshell is 2, bc it only has 1 orbital.

 

[milski]

l is not the principal quantum number, it's azimuthal quantum number.

The lowest principal quantum number is n=1, it's a type in the textbook.

 

[dudewheresmymd]

Yeah n=1 is the lowest as milski said...if you look at electron configurations it's always 1s2...2s2...2p6 That first "1"preceding the s2, is n=1, and the "l" would be 0 in that case (l always goes from 0 too n-1, where s=0, p=1, d=2, f=3...)