Quantam Mechanics Flashcards
A new model
The Rutherford model did explain what kept the -e’s from crashing into the the nucleus
ground state
the normal configuration for an atom. all e-s are at their lowest possible energy state
Exited state
when energy is added to an atom through heat or electricity some electrons jump up to higher energy levels
absorption
when electrons go into higher levels but don’t stay there
emission
when the electrons go back to the ground state and it releases energy. and it does this in the form of light. we call this a photon
What kind of wave is light
electromagnetic wave
spectrum of light
radio, microwave, infrared, visible, ultraviolet, x-ray, gamma ray
radio is the largest wavelength, gamma is the smallest,
radio has the least hertz gamma and the most
how fast do electromagnetic waves travel
2x10 to the power of 8 m/s
wavelength
the distance from crest to crest or trough to trough (measured in nm)
frequency
the number wave lengths that pass per second (hertz- hz)
what is the formula for speed
speed= wavelength x frequency
c = λf or v
c= speed of light (m/s) λ= wavelenght n/m f or v= frequency
formula for the speed of a wave
Werner heisenberg= Particles behave like waves
showed that we could not know the speed and location of e’s at the same time (uncertainty principle)
Erwin shrödinger= Particles behave like waves
came up with the equation to show where the electrons could be along paths called wave functions
what does light behave like
light can also behave like a particle as it does in the photoelectric effect but it can also behave like a wave
photoelectric effect
when the light of certain frequencies shines on a metal, electrons are emitted
what did Albert Einstein win his award for
the photo-electric effect
Quantum Numbers
a set of 4 characters that describe the properties of each electron (every electron has its own 4-character code)
Orbital
an orbital is a 3-dimensional space around the nucleus that indicates the location of an e 90% of the time
Principal quantam number (1)
-symbolized by n=1,2,3 etc…
-indicates the main energy level
-occupied by the e (also called the shells)
-as n increases distance from the nucleus increases
azimuthal quantam number(2)
- symbolized by l=s,p,d,f or g hypothetically
-indicates the shape of the orbital
-different orbitals within the same energy levels called sublevels
-the max number of sublevels (orbital shapes) in an energy level equals the principal quantum number n
Magnetic quantum number (3)
-within sublevels, these are the orbitals
-indicates the orientation of the orbital around the nucleus
-each orientation can hold two e’s
-there are n squared orbitals per energy level
what does the s orbital look like
a circle
what does the p orbital look like
two ovals coming out from the center
what does the d sublevel look like
clover leaf with the ovals
what does the f sublevel look like
six ovals coming out of the center
Spin Quantum number (4)
-has only two possible values 1/2 or negative 1/2
-indicated the directions of the spins
a single orbital orientation has the ability to hold a max of two e’s which must have opposite spins
what is the electron configuration
arrangement of electrons in an atom
why are atoms lazy
they want to be in the lowest energy state possible
ground state electron configuration
this is the lowest energy arrangement of electrons for each element
three rules that govern electron placement
Aufbau principle
Hunds Rule
Pauli Exculsion Principle
Aufbau Principle
an electron occupies the lowest energy orbital that can receive it (lowest energy first)
Hunds Rule
orbitals of equal energy are each occupied by 1 electron of the same before any orbital is occupied by a 2nd electron
Pauli Exclusion principle
no two electrons in the same atom can have the same set of 4 quantum numbers (opposite spins) no two electrons can have the same numbers
electromagnetic radiation
Electromagnetic radiation in chemistry refers to energy that travels through space in the form of waves, which include visible light, ultraviolet, infrared, and other forms of radiation. c=λ⋅ν
Electromagnetic Spectrum
refers to the entire range of electromagnetic radiation which is categorized by wavelength or frequency that can interact with matter.
Interference pattern
refers to a pattern of light or other waves that occurs when two or more waves overlap and combine. this is a result of wave interference
Emission spectrum
refers to the range of wavelengths of light emitted by atoms or molecules. it is unique for every element because every element has a different electron configuration
Heisenberg uncertainty principle
In chemistry, it helps explain electron behavior and atomic orbitals. it talks about how it is impossible to know the position and momentum of a particle (like an electron) at the same time
orbitals
a region where the atom is 90% of the time. (s,p,d, and f) base on the mathematical equation that schrödinger did which describes the wave-like behavior of electrons
what did Schrödinger do for this
The Schrödinger equation explains the quantization of energy levels in atoms. It is fundamental to understanding the electron configurations in atoms and how electrons occupy specific orbitals.
