1. Bohr & Schrödinger

2. The Bohr Model
Recall Bohr’s model of the atom: 2 Ar 8 8 18

3. Bohr’s model of the atom was famous because it could explain the bright line spectrum

4. 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

8. E1
Ground state

9. E1
Ground state
1st excited state

10. E1 E1 packet of light photon Ground state 1st excited state

11. E2
Ground state

12. 2nd excited state

13. E2-E1 E2 E2 1st excited state Ground state 2nd excited state

15. 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

16. quantum

17. 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

18. Dalton
Thomson
Rutherford
Bohr
Schrödinger

19. 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

20. 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

21. 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

22. White Light Spectrum
Emission Spectrum of H

23. 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

26. 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

27. 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

28. 2s

29. 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

30. s orbital
p orbital
d orbital
f orbital

31. 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

36. 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

37. # 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