Quantum Mechical Model of Atom Flashcards
Who proposed the Uncertainty Principle and what does it explain?
Heisenberg
It is impossible to measure the position and momentum (speed) of an object SIMULTANEOUSLY( the more accurate one variable is the less accurate the other is). This principle invalidates Bohr’s model because he assigns fixed circular orbits and specific energy levels simultaneously.
Who proposed that all matter behaves like waves and has wavelength properties?
Louis de Broglie
*small wavelengths have a great influence on very small objects like electrons (larger objects=less affected by wavelengths)
What is an experiment that shows de Broglie’s hypothesis?
The double slit experiment shows how light creates an interference pattern like a wave when forced to travel through two slits before hitting a wall. Also, shows how atoms act differently when observed as when observed, the light forms the normal pattern when it passes through the two slits, instead of the wave pattern.
Who derived a new equation that allowed him to predict the location of an atom over time using statistical probabilities and Bohr’s energy levels?
Schrödinger
Explain Schrödinger’s Quantum Model diagram
Thousands of dots surround a nucleus and forms a circular and eventually, spherical shape, with the addition of a y axis. Every dot is a mass solution to Schrödinger’s wave equation with the cut off point of 95%.
What are the 4 numbers of the code system of quantum numbers?
- principle quantum # (n)- describes orbital size and energy level (higher n value=larger orbital and faster speed)
- orbital shape quantum # (l)- what shaped orbital to look in to find an electron (ranges from 0 to n-1)
- magnetic quantum # (ml)- tells you how many orbitals of the shape there is (ranges from -1 to +1)
- spin quantum # (ms)- the direction of the half spin in an orbital (2 electrons with different spins can occupy an orbital)
What are the 4 shapes of orbitals and their associated L value?
s (spherical) orbital- l=0
p (peanut) orbital- l=1
d (daises) orbital- l=2
f (freaking complicated) orbital- l=3
How many orbitals are associated with 5f?
n=5 l=3 ml= -3,-2,-1,0,1,2,3 = 7 orbitals
How do you calculate each possible orbiting using quantum numbers?
each orbital is represented using a box:
-an s orbital is 1 box
-a p orbital box is composed of 3 boxes
-a d orbital box is composed of 5 boxes
-a f orbital box is composed of 7 boxes
each box contains 1-2 half spins where the up arrow is + 1/2 and the down is -1/2 (represents # of electrons in orbital)
What is the Pauli Exclusion Principle?
no 2 electrons in an atom have the same set of quantum numbers ( in one orbit, there is a -1/2 spin and a +1/2 spin)
How do you draw a ground state orbital diagram? (list and explain the 4 steps)
- place the electrons into orbitals of increasing energy level (boxes)
- all orbitals with same amount of energy must be filled before moving higher (must contain 2 half spins per box)
- each orbital with same amount of energy receives 1 electron (+1/2 spin) before being paired with another electron (with a -1/2 spin)
Draw an orbital diagram for P and then write the 4 quantum number for its last electron
1s box with +1/2 spin and -1/2 spin 2s box “ “ 2p box is with full half spins 3s box with full half spins 3p box with only +1/2 spins in each box n=3 l=1 ml=-1,0,1 ms= +1/2
How do you write a ground state electron configuration?
write the first 2 quantum numbers of the orbital, then the number of electrons using a superscript number (ex P=1s^2 2s^2 2p^6 3s^2 3p^3)
How do you write the condensed format of the electron configuration?
place previous noble gas in [ ] brackets, then add extra electrons to get to element (ex P= [Ne] 3s^2 3p^3 )
*use noble gas as reference because they have a full n level of electron orbitals
