Structure of the atom – Flashcards
Unlock all answers in this set
Unlock answersWhat is the energy difference btwn n=3 , n=4 and n=1,n=2 Include why? |
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) |
define the quantum number ' n', what does a larger n indicate? |
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) |
| define the quantum 'l' |
decides the : shape and number of subshells within a given principal energy level (shell) |
| How does'n' affect 'l' ? |
n limits l ! For any given value of n, 'l 'can only have values in the range of : 0 to (n-1)
|
If n=1, what does that mean in refernce to: # subshells value of 'l'?
|
n=1 1 subshell (so the 1st principal energy level has only 1 subshell) l= 0 (only) (s) |
If n=2, what does that mean in refernce to: # subshells value of 'l'? |
2 subshells (the 2nd prinipal energy level) 'l '= 0 and 1 (s) and (p) |
If n=3, what does that mean in refernce to: # subshells value of 'l'and name the oribtal you are in |
3 shells (3 principal energy level) l=0, 1, 2 (s, p, d ) |
If n=4, what does that mean in refernce to: # subshells value of 'l'? |
4 subshells l: 0 (s), 1 (p), 2 (d) ,3 (f) *remember (n-1)= l
|
The maximum number of the electrons within the any given subshell?
in reference to n& l?
|
2n2
4l +2 |
| What does the quantum mumber ml mean? |
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) |
| What are the values for ml? |
integers btwn : -l to + l
including 0 ex: if l=1 (-1,0,1) |
| Give the l,ml values for the s oribtal |
l=0 ml=0
* remember the s shell has 1 oribital |
| Give the l,ml values for the p oribtal |
l=1 ml= -1 ,0,1 the p shell oribtal has '3'oribtals |
give # oribitals in the following subshells: s,p,d,f |
s: 1 orbitals p: 3 d: 5 f:7
(as you go to next level you add 2) |
| What does the quantum number ms stand for: |
magnetic spin of the ELECTRON has values of : +1/2 to - 1/2 |
| Give the formula how to calculate the energy value of a quantum |
E= hf
where h= 6.626 x 10-34 (Planks) f= frequency of a photon (could also be v)
|
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. |
f= c λ
c= 3 x 108 m/s (speed of light )
λ= wavelength (nm) need to mult by 109 |
Give Avagrados constant Planks
|
avagrados: 6.023 x 1023 (there is a holiday celebrated at 6:02,time is always positive)
planks: 6.626 x 10 -34 (down the plank) |
Define Hund's rule Pauli's exclusion principal |
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. |
| Which elements on periodic table have half filled orbitals in order to decrease their stablilites? |
Cr Cu Ag Au |
Fix this config for Cr so that is more stable: [Ar] 3d4 4s2 |
| [Ar] 3d5 4s1 |
Fix this config for Cu so that is more stable: [Ar] 3d9 4s2 |
[Ar] 3d10 4s1
its adding to that big d instead of having more e- furhther from nucleus, makes it more reactive |
Fix this config for Ag so that is more stable: [Kr] 4d9 5s2 |
| Kr] 4d10 5s1 |
fix this config so that is more stable: [Xe] 4f14 5d9 6s2 |
| [Xe] 4f14 5d10 6s1 |
Define 'l' Define'ml' Give the example of the p oribital |
l: # of subshells and shape for a value of 'n' ml: 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) |
atomic weight def give unit |
weight of an element as an average of the isotopes of a particular element
unit:grams per mole |
| isotope def |
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) |
| Do isotopes have different # of protons or electrons or both? |
| no isotopes only differ in the # of neutrons |
| atomic emission spectrum def |
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). |
| atomic absorption spectrum def |
spectrum of light created when an atom's electron's are excited to higher energy levels
*remember this requires energy to be absorbed |
| paramagnetic material |
| has unpaired electrons |
| diamagnetic material |
| no unpaired electrons |
| heisenberg uncertanity principal def |
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) |
| is an electron always static (referring an energy levels)? |
| no, even when an electron is in its ground state the electron is not completly static. |
