Question

Atomic Theory ◘ Quantum Model
Questions below; second unanswered

Answer 1

11) The Bohr model of the atom assumes that which of the following quantities for the electron in a hydrogen atom is/are quantized?
i. \(\large{\text{Speed}}\)
ii. \(\large{\text{Direction of Spin Axis}}\)
iii. \(\large{\text{Energy}}\)
iv. \(\large{\text{Radius of its orbit}}\)

The options are:\[\text{a. iii only}\]\[\text{b. i and iii}\]\[\text{c. iii and iv}\]\[\text{d. i, iii, and iv}\]\[\text{e. i, ii, and iii}\]

Answer 2

(Generalized question) How do you calculate the ground-state electron configuration of an element?

Answer 3

Its been such a long time since i did this stuff
I know that the energy is quantized (iii)

Answer 4

okay

Answer 5

and radius of the orbit is set that s (iv)

Answer 6

to be honest im not sure. If i had to make a guess it would be option (c. ) Not sure about the speed.

Answer 7

hmm

Answer 8

yeah, answer key says C

Answer 9

sorry

Answer 10

you got it right :P

Answer 11

- 0h ok. I'm going back 60 years!!!!!!

Answer 12

Eh?

Answer 13

@sammixboo @sweetburger @zepdrix

Answer 14

Thanks for the tags ! @moldybubblegum12 ☺

Answer 15

how did you make that :) face

Answer 16

@zzr0ck3r

Answer 17

\[\large{alt+\text{ (number pad) }1}\]

Answer 18

You could try looking for a video on youtube... i need some videos that cover this

Answer 19

Yep. Remember to use the number pad ☺
Alright I'll go look for some videos then!

Answer 20

oooohhhh @kittiwitti1 i thought you typed "alright go look for some videos then!"

Answer 21

xD

Answer 22

explain how to do the symbols... i cant do them ;-;

Answer 23

they're alt codes, just press ALT key and then one of the numbers at the same time (really, one after the other, don't let go of the ALT key until you hit the number)

Answer 24

The ground state configuration is actually just the Lyman Series.

It is the set of quantized energies when you go from n = 2,3,4,5 etc. to n = 1 (your ground state is n=1 for hydrogen)

There is a cute formula to work this out

\[\frac{ 1 }{ \lambda } = R_H (\frac{ 1 }{ n_f^2 } - \frac{ 1 }{ n_i^2 }) \]
R_H is Rydberg's constant roughly 1.097 x 10^7 /m
nf and ni are your final n and initial n.

So ground state configuration you have nf being 1 which reduces your equation to
\[\frac{ 1 }{ \lambda } = R_h(1-\frac{ 1 }{ n_i^2 })\]
The set of solutions gives rise to the Lyman series. If your final state is not n =1, you get other series like Balmer Series (nf=2), Paschen series (nf=3), Brackett Series (nf=4) and Pfund series (bf=5)

Lyman series, we can also write energy associated with the electron transition:
\[E= h \nu = \frac{ hc }{ \lambda } = hcR_H(1-\frac{ 1 }{ n_i^2 })\]

Answer 25

Quantum # Practice:
A: For \(n=4\), what are the possible values of \(l\)?
B: For \(l=3\), what are the possible values of \(m_{l}\) (also written as \(m\))?

My answer to the second is:\[\LARGE{m=-3,-2,-1,0,1,2,3}\]

Answer 26

I have no idea what that said ... I'm only in basic Chemistry lol @mww

Answer 27

^you'll have to learn it sooner or later

Answer 28

Well, yes, but looking at that just confuses me at the moment. ^-^;

Answer 29

To be honest, maybe because it's a summer class (or not, I did this in high school too), my professor just gave us a little chart of sorts to use... but I wanted to know if there was a more explicit way to do it

Answer 30

Well to start off with basically you should understand that electrons can exist in different configurations or states. The further away from the nucleus the greater the energy that electron has. So when an electron jumps between states (which are quantized) a discrete amount of energy is absorbed or releaed

Answer 31

Alright, I understand that

Answer 32

I think there was some sort of diagram with the Periodic Table that showed increasing reactivity or something with electron shells that would help students in my class with the configurations.

Answer 33

oh are you talking about subshells s, p, d, f

Answer 34

Yup.

Well, that aside, I seem to be having the most issues with the next set of problems

Answer 35

...when either \(n\), \(l\), \(m\) or \(s\) is given, how do I get the rest?
I believe that \(m\) is the range of \(\pm l\)... according to my class papers

Answer 36

\(\color{blue}{\text{Originally Posted by}}\) kittiwitti1
Quantum # Practice:
A: For \(n=4\), what are the possible values of \(l\)?
B: For \(l=3\), what are the possible values of \(m_{l}\) (also written as \(m\))?

My answer to the second is:\[\LARGE{m=-3,-2,-1,0,1,2,3}\]
\(\color{blue}{\text{End of Quote}}\)

These qeuestion, specifically

Answer 37

Ergh. *Questions

Answer 38

yes. that's correct. s (spin) is +/- 1/2

Answer 39

Wait, what?

Answer 40

I said that off my notes it says \(m=\pm l\) range

Answer 41

oh I was talking about the last quantum number which is spin, always +/- 1/2 but yes m is -l,...0,...+l

Answer 42

so then... did I get part B in that question right lol

Answer 43

and thanks for confirming! ☺