Bohr & Schrödinger
The Bohr Model Recall Bohr’s model of the atom: 2 Ar 8 8 18
Bohr’s model of the atom was famous because it could explain the bright line spectrum
continuous discontinuous discrete bands The spectrum of white light is _________________, it shows all the colours of the rainbow The spectrum of energized gas is _________________, it shows _________________. discontinuous discrete bands
E1 Ground state
E1 Ground state 1st excited state
E1 E1 packet of light photon Ground state 1st excited state
E2 Ground state
2nd excited state
E2-E1 E2 E2 1st excited state Ground state 2nd excited state
When particles are exposed to energy ground state (lowest energy state) atoms absorb specific energy and become “excited” an electron moves to a higher shell excited atoms then release the energy at specific frequencies to get back to ground state the electron moves back to its original shell, emitting a photon (packet of light) the difference between two particular energy levels is called the quantum the lines in the spectrum are produced when electrons de-excite
quantum
Bohr’s model was proven significantly wrong in 2 ways: electrons don’t revolve around the nucleus in circles the model can only predict energies H
Dalton Thomson Rutherford Bohr Schrödinger
Recap What does “ground state” refer to? A. A hydrogen atom B. Lowest energy state of an atom C. Highest energy state of an atom D. When the atom is on the ground B. Lowest energy state of an atom
Recap How does an electron become “excited?” A. The atom it resides in reacts with another atom B. It absorbs energy and jumps shells C. It absorbs specific amounts of energy and jumps shells D. When it sees a particle of opposite charge C. It absorbs specific amounts of energy and jumps shells
Recap What is a photon? A. A packet of light B. An excited proton C. An excited electron A Chinese wonton stuffed with Vietnamese noodles A. A packet of light
White Light Spectrum Emission Spectrum of H
Recap What is an orbital? A. The path an electron takes around the nucleus B. Lobes C. The shape of the nucleus D. Mathematical description (probability) of where to find an electron in an atom D. Mathematical description (probability) of where to find an electron in an atom
8.2 - Quantum Mechanics: Schrödinger’s atomic model Schrödinger’s model describes the probability of where to find an electron in an atom orbital: the region of space around a nucleus where an electron can be found orbitals are described by quantum numbers
1st or principal quantum number (n) Symbols What does it mean? 1st or principal quantum number (n) 2nd quantum number (l) 3rd quantum number (m) 4th quantum number (ms) 1, 2, 3 … Size and energy level
2s
1st or principal quantum number (n) Symbols What does it mean? 1st or principal quantum number (n) 2nd quantum number (l) 3rd quantum number (m) 4th quantum number (ms) 1, 2, 3 … Size and energy level s, p, d, f Orbital shape
s orbital p orbital d orbital f orbital
1st or principal quantum number (n) Symbols What does it mean? 1st or principal quantum number (n) 2nd quantum number (l) 3rd quantum number (m) 4th quantum number (ms) 1, 2, 3 … Size and energy level s, p, d, f Orbital shape x, y, z Orbital orientation
1st or principal quantum number (n) Symbols What does it mean? 1st or principal quantum number (n) 2nd quantum number (l) 3rd quantum number (m) 4th quantum number (ms) 1, 2, 3 … Size and energy level s, p, d, f Orbital shape x, y, z Orbital orientation ½ or -½ Electron spin
# of Orbitals in a Subshell Maximum # of Electrons in Subshell Each energy level has a specific set of orbitals and each one represents where a maximum of 2 electrons can be found. Orbital Type Begins at n= # of Orbitals in a Subshell Maximum # of Electrons in Subshell s 1 1 2 p 2 3 6 d 3 5 10 f 4 7 14