Term
What is the energy difference btwn
n=3 , n=4
and
n=1,n=2
Include why? 

Definition
n=3 and n=4 has a smaller energy difference
(they are farther away from nucleus)
compared to
n=1 and n=2
(closer to nucleus) 


Term
define the quantum number ' n',
what does a larger n indicate? 

Definition
principal quantum number that has a integer value
↑n= ↑energy↑ oribtal radius
*remmeber high energy means more unstable (more likely to engage in chemical rxns they have further from nucleus) 


Term

Definition
decides the :
shape and number of subshells within a given principal energy level (shell) 


Term

Definition
n limits l !
For any given value of n, 'l 'can only have values in the range of :
0 to (n1)



Term
If n=1, what does that mean in refernce to:
# subshells
value of 'l'?


Definition
n=1
1 subshell
(so the 1st principal energy level has only 1 subshell)
l= 0 (only)
(s) 


Term
If n=2, what does that mean in refernce to:
# subshells
value of 'l'?


Definition
2 subshells
(the 2nd prinipal energy level)
'l '= 0 and 1
(s) and (p) 


Term
If n=3, what does that mean in refernce to:
# subshells
value of 'l'and name the oribtal you are in


Definition
3 shells
(3 principal energy level)
l=0, 1, 2
(s, p, d ) 


Term
If n=4, what does that mean in refernce to:
# subshells
value of 'l'? 

Definition
4 subshells
l: 0 (s), 1 (p), 2 (d) ,3 (f) *remember (n1)= l



Term
The maximum number of the electrons within the any given subshell?
in reference to n& l?


Definition


Term
What does the quantum mumber m_{l} mean? 

Definition
tells the particular orbital within a subshell where an electron is highly likely to be found at a given time.
(this tells us that , s shell has 1, p shell has 3, etc) 


Term
What are the values for m_{l}? 

Definition
integers btwn :
l to + l
including 0
ex: if l=1
(1,0,1) 


Term
Give the l,m_{l } values for the s oribtal 

Definition
l=0
ml=0
* remember the s shell has 1 oribital 


Term
Give the l,m_{l } values for the p oribtal 

Definition
l=1
ml= 1 ,0,1
the p shell oribtal has '3'oribtals 


Term
give # oribitals in the following subshells:
s,p,d,f 

Definition
s: 1 orbitals
p: 3
d: 5
f:7
(as you go to next level you add 2) 


Term
What does the quantum number m_{s} stand for: 

Definition
magnetic spin of the ELECTRON
has values of : +1/2 to  1/2 


Term
Give the formula how to calculate the energy value of a quantum 

Definition
E= hf
where h= 6.626 x 10^{34} (Planks)
f= frequency of a photon
(could also be v)



Term
1.Give formula for the frequency of a photon
2. What is the unit for the wavelength
and give the conversion to makeit work in the equation. 

Definition
f= c
λ
c= 3 x 10^{8}^{ }m/s
(speed of light )
λ= wavelength (nm)
need to mult by 10^{9} 


Term
Give Avagrados constant
Planks


Definition
avagrados: 6.023 x 10^{23}
(there is a holiday celebrated at 6:02,time is always positive)
planks: 6.626 x 10 ^{34}
(down the plank) 


Term
Define Hund's rule
Pauli's exclusion principal 

Definition
Hunds: every orbital in a subshell is singly occupied with 1 electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.
↑↑ , ↑↑ ,(the blue came first)
Pauli: states that no two electrons can have the same four quantum numbers. The first three may be similar but the four quantum number must be different. 


Term
Which elements on periodic table have half filled orbitals in order to decrease their stablilites? 

Definition


Term
Fix this config for Cr so that is more stable:
[Ar] 3d^{4} 4s^{2} 

Definition


Term
Fix this config for Cu so that is more stable:
[Ar] 3d^{9} 4s^{2} 

Definition
[Ar] 3d^{10} 4s^{1}
its adding to that big d instead of having more e furhther from nucleus, makes it more reactive 


Term
Fix this config for Ag so that is more stable:
[Kr] 4d^{9} 5s^{2} 

Definition


Term
fix this config so that is more stable:
[Xe] 4f^{14} 5d^{9} 6s^{2} 

Definition
[Xe] 4f^{14} 5d^{10} 6s^{1} 


Term
Define 'l'
Define'm_{l}'
Give the example of the p oribital 

Definition
l: # of subshells and shape for a value of 'n'
m_{l}: tells what specific oribital where you can find an electron in a subshell.
ex
n=2
l= 0,1 (2 subshells)
ml=1 ,0,3 (3 oribitals) 


Term
atomic weight def
give unit 

Definition
weight of an element as an average of the isotopes of a particular element
unit:grams per mole 


Term

Definition
a different form of the same element (will have a charge b/c it has gained or lossed electrons)
but has a different # of neutrons
do not confused with cations and anions (these happen with rxns etc) 


Term
Do isotopes have different # of protons or electrons or both? 

Definition
no isotopes only differ in the # of neutrons 


Term
atomic emission spectrum def 

Definition
spectrum of light created when an atom's electron's fall to to their ground state from a higher energy level
*remember this causes energy to be released (emitted). 


Term
atomic absorption spectrum def 

Definition
spectrum of light created when an atom's electron's are excited to higher energy levels
*remember this requires energy to be absorbed 


Term

Definition


Term

Definition


Term
heisenberg uncertanity principal def 

Definition
it is impossible to calc the:
momentum & position of an electron at the SAME time
(remember you can calculate the momentum and velocity at the same time) 


Term
is an electron always static (referring an energy levels)? 

Definition
no, even when an electron is in its ground state the electron is not completly static. 

