minooka -electron configurations part 1
TRANSCRIPT
Orbitals and Electron Configurations
Orbitals and Electron Configurations
Where are the electrons?Where are the electrons?
The Rutherford AtomThe Rutherford Atom
Problems with the Rutherford Atom
Problems with the Rutherford Atom
Electrons should be attracted to the nucleus and repel each other
Couldn’t answer the question Why do the electrons stay in the electron
cloud? Why don’t the electrons collapse into the
massively positive nucleus?
Electrons should be attracted to the nucleus and repel each other
Couldn’t answer the question Why do the electrons stay in the electron
cloud? Why don’t the electrons collapse into the
massively positive nucleus?
The Bohr AtomThe Bohr Atom
Problems with the Bohr AtomProblems with the Bohr Atom
Fundamentally incorrect - only worked for the element Hydrogen
Couldn’t explain where the electrons were in atoms that had more than one electron
We don’t really know where an electron is at any one time, and we can’t predict it either
Fundamentally incorrect - only worked for the element Hydrogen
Couldn’t explain where the electrons were in atoms that had more than one electron
We don’t really know where an electron is at any one time, and we can’t predict it either
Things Bohr got rightThings Bohr got right
Energy Levels Ground State
Energy Levels Ground State
What we saw in the flame test labWhat we saw in the flame test lab
How we saw the light in the flame test lab
How we saw the light in the flame test lab
How we explain the light in terms of energy levels of the electrons in the atom
How we explain the light in terms of energy levels of the electrons in the atom
The difference between continuous and quantized energy
levels
The difference between continuous and quantized energy
levels
Albert Einstein’s contributionAlbert Einstein’s contribution
Developed quantum mechanics Showed that Isaac Newton’s theories for
motion do not give correct results when objects are traveling close to the speed of light
New equations in which the laws for motion are adjusted for the speed of light
Developed quantum mechanics Showed that Isaac Newton’s theories for
motion do not give correct results when objects are traveling close to the speed of light
New equations in which the laws for motion are adjusted for the speed of light
Max Planck’s contributionMax Planck’s contribution
German Physicist in the early 1900’s Said that Light is made up of discrete
bundles of energy called “quanta” (pleural of quantum)
Now known as “photon”
German Physicist in the early 1900’s Said that Light is made up of discrete
bundles of energy called “quanta” (pleural of quantum)
Now known as “photon”
Light has a Dual NatureLight has a Dual Nature
Behaves as both a particle (has properties of matter)
And a wave Has wave properties such as
Wavelength Frequency Speed (velocity)
Behaves as both a particle (has properties of matter)
And a wave Has wave properties such as
Wavelength Frequency Speed (velocity)
Photons of red and blue lightPhotons of red and blue light
Light as both a wave and a packet of energy
Light as both a wave and a packet of energy
Schrodinger and De BroglieSchrodinger and De Broglie
Mid-1920’s Louis Victor De Broglie from France Erwin Schrodinger from Austria Both young Physicists Suggested that if light can act like a wave
and a particle, then perhaps the same was true of the electron
Mid-1920’s Louis Victor De Broglie from France Erwin Schrodinger from Austria Both young Physicists Suggested that if light can act like a wave
and a particle, then perhaps the same was true of the electron
Wave-Mechanical ModelWave-Mechanical Model
Also called the quantum-mechanical model Electrons behave as both waves and
particles (like light) De Broglie and Schrodinger applied a
mathematical analysis to their idea and found that it worked for all atoms, not just hydrogen
Also called the quantum-mechanical model Electrons behave as both waves and
particles (like light) De Broglie and Schrodinger applied a
mathematical analysis to their idea and found that it worked for all atoms, not just hydrogen
Wave Mechanical ModelWave Mechanical Model
1. Electrons do not follow definite paths2. Electrons are in a diffuse cloud of negative
charge around the nucleus (like the Rutherford atom)
3. There are areas around the nucleus that correspond with certain energy levels (like the Bohr Model)
4. The areas around the nucleus where the electron probably is (energy levels) are called orbitals
1. Electrons do not follow definite paths2. Electrons are in a diffuse cloud of negative
charge around the nucleus (like the Rutherford atom)
3. There are areas around the nucleus that correspond with certain energy levels (like the Bohr Model)
4. The areas around the nucleus where the electron probably is (energy levels) are called orbitals
Firefly experimentFirefly experiment
Electron ProbabilityElectron Probability
The Hydrogen 1s OrbitalThe Hydrogen 1s Orbital
OrbitalsOrbitals
Do not have distinct boundaries (like earth’s atmosphere)
Boundary is mapped at 90% electron probability (by convention)
Electrons can be found outside of this boundary We can never map exactly where an electron is at
any given moment All elements have all of the orbitals
Do not have distinct boundaries (like earth’s atmosphere)
Boundary is mapped at 90% electron probability (by convention)
Electrons can be found outside of this boundary We can never map exactly where an electron is at
any given moment All elements have all of the orbitals
The first four principle energy levels
The first four principle energy levels
Sub-LevelsSub-Levels
As the Energy Level number increases, the further away from the nucleus the electron is, and the higher the energy level
The further away from the nucleus the energy level is, the more space there is to divide up
Each Energy level is divided further into sub-levels
As the Energy Level number increases, the further away from the nucleus the electron is, and the higher the energy level
The further away from the nucleus the energy level is, the more space there is to divide up
Each Energy level is divided further into sub-levels
How principle energy levels are divided into sub-levels (s,p,d,f)How principle energy levels are divided into sub-levels (s,p,d,f)
Second Principle Energy Level with sublevels corresponding to orbitalsSecond Principle Energy Level with sublevels corresponding to orbitals
1s and 2s orbitals (showing the relative size)
1s and 2s orbitals (showing the relative size)
The 2p orbitals (three of them)The 2p orbitals (three of them)
Diagram of Principle Energy Levels 1 and 2
Diagram of Principle Energy Levels 1 and 2
Relative size of the 1s, 2s, 3s orbitals
Relative size of the 1s, 2s, 3s orbitals
The 3d orbitalsThe 3d orbitals
Electron FillingElectron Filling
Aufbau Principle - electrons prefer the space closest to the nucleus
Therefore all of the electrons are arranged around the nucleus from lowest energy level to highest energy level
The most attractive orbital to any electron is the 1s orbital, then 2s, 2p, 3s, 3p, 4s, 3d, and so on
This corresponds to Bohr’s idea of the ground state
Aufbau Principle - electrons prefer the space closest to the nucleus
Therefore all of the electrons are arranged around the nucleus from lowest energy level to highest energy level
The most attractive orbital to any electron is the 1s orbital, then 2s, 2p, 3s, 3p, 4s, 3d, and so on
This corresponds to Bohr’s idea of the ground state
Electron fillingElectron filling
Pauli Exclusion Principle - orbitals can hold a maximum of two electrons
Electrons repel each other and don’t want to share the same space (same negative charge)
Electrons will share the same space if they are spinning in opposite directions (like a magnet)
Pauli Exclusion Principle - orbitals can hold a maximum of two electrons
Electrons repel each other and don’t want to share the same space (same negative charge)
Electrons will share the same space if they are spinning in opposite directions (like a magnet)