Based on experimental observations of light and particles

Based on experimental observations of light and particles

• Based on experimental observations of light and particles

• Developed through rigorous mathematical computations

• Bridges physics and chemistry

• Generally described as quantum mechanics aka quantum chemistry

Energy that exhibits wave-like behavior that travels through space at 186,000 mi/s; 3 x 108 m/s

• Energy that exhibits wave-like behavior that travels through space at 186,000 mi/s; 3 x 108 m/s

• Described by the Electromagnetic Spectrum.

Waves have 4 primary characteristics:

• Waves have 4 primary characteristics:

• 1. Wavelength: distance between two peaks in a wave.

• 2. Frequency: number of waves per second that pass a given point in space.

• 3. Amplitude: the height of the wave.

• 4. Speed: speed of light is 2.9979  108 m/s.

Focus on 2 of the primary characteristics:

• Focus on 2 of the primary characteristics:

• 1. Wavelength: distance between two peaks in a wave.

• 2. Frequency: number of waves per second that pass a given point in space.

• 3. Amplitude: the height of the wave.

• 4. Speed: speed of light is 2.9979  108 m/s.

 = c / 

•  = c / 

•  = frequency (s1)

•  = wavelength (m)

• c = speed of light (m s1)

E = change in energy, in J

• E = change in energy, in J

• h = Planck’s constant, 6.626  1034 J s

•  = frequency, in s1

•  = wavelength, in m

• c = speed of light

Energy has mass

• Energy has mass

• E = mc2

• E = energy

• m = mass

• c = speed of light

 = wavelength, in m

•  = wavelength, in m

• h = Planck’s constant, 6.626  1034 J .s = kg m2 s1

• m = mass, in kg

•  = frequency, in s1

Continuous spectrum: Contains all the wavelengths of light.

• Continuous spectrum: Contains all the wavelengths of light.

• Absorbtion vs.Emission

• http://chemistry.beloit.edu/BlueLight/pages/elements.html

• Line (discrete) spectrum: Contains only some of the wavelengths of light.

As protons are added one by one to the nucleus to build up the elements, electrons are similarly added to these hydrogen-like orbitals.

• As protons are added one by one to the nucleus to build up the elements, electrons are similarly added to these hydrogen-like orbitals.

In a given atom, no two electrons can have the same set of four quantum numbers ( n, l, ml , ms ).

• In a given atom, no two electrons can have the same set of four quantum numbers ( n, l, ml , ms ).

• Therefore, an orbital can hold only two electrons, and they must have opposite spins.

The lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli principle in a particular set of degenerate orbitals.

• The lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli principle in a particular set of degenerate orbitals.

Based on experimental observations of light and particles

• Based on experimental observations of light and particles

• Developed through rigorous mathematical computations

• Bridges physics and chemistry

• Generally described as quantum mechanics aka quantum chemistry

The more accurately we know a particle’s position, the less accurately we can know its momentum or vice versa.

• The more accurately we know a particle’s position, the less accurately we can know its momentum or vice versa.

1. Principal QN ( integer n = 1, 2, 3, . . .) : relates to size and energy of the orbital.

• 1. Principal QN ( integer n = 1, 2, 3, . . .) : relates to size and energy of the orbital.

• 2. Angular Momentum QN ( integer l or )= 0 to n  1) : relates to shape of the orbital.

• 3. Magnetic QN (integer m l or m  = + l to l) : relates to orientation of the orbital in space relative to other orbitals.

• 4. Electron Spin QN : (ms = +1/2, 1/2) : relates to the spin state of the electron.

Representative Elements (A Groups): s (l=0) and p (l=1) (N, C, Al, Ne, F, O)

• Representative Elements (A Groups): s (l=0) and p (l=1) (N, C, Al, Ne, F, O)

• Transition Elements: d (l=2) orbitals (Fe, Co, Ni, etc.)

• Lanthanide and Actinide Series (inner transition elements): f (l=3) orbitals (Eu, Am, Es)

Representative Elements (A Groups): fill s and p orbitals (Na, Al, Ne, O)

• Representative Elements (A Groups): fill s and p orbitals (Na, Al, Ne, O)

• Transition Elements: fill d orbitals (Fe, Co, Ni)

• Lanthanide and Actinide Series (inner transition elements): fill 4f and 5f orbitals (Eu, Am, Es)

1. Can obtain Group A valence electron configurations

• 1. Can obtain Group A valence electron configurations

• 2. Can determine individual electron configurations.

• This information can be used to:

• a. Predict the physical properties and general chemical behavior of the elements.

• b. Identify metals and nonmetals.

• c. Predict ions & formulas of compounds