4.2 The Quantum Atomic Model De Broglie Heisenberg Quantum
Numbers Orbitals Sublevels Slide 2 Louis De Broglie (1924) -
proposed e -s travel like a wave and not in a simple circular path.
De Broglie Bohr Slide 3 Heisenberg Uncertainty Principle Heisenberg
Uncertainty Principle states that it is impossible to know
precisely both the velocity and position of an electron at the same
time without changing it slightly. - Think of a spinning fan blade.
At any moment you do not know exactly where is it but you do know
the region in which it could be found. Slide 4 What happens to the
size of the rows & the # of seats as you get further from the
stage? Slide 5 Quantum Atomic Model Energy Level - 3-D shell around
the nucleus containing e -s of similar energy. There are 7 energy
levels Each energy level has a sublevel. The sublevels are s, p, d,
and f Each sublevel holds a specific orbital Slide 6 Review
Questions 1.What did de Broglie propose that was different than
Bohr? 2.What is Heisenberg uncertain of? 3.How many energy levels
are there? 4.What happens to the size of energy level and the # of
electrons it can hold as you travel farther from the nucleus?
5.What are the 4 sublevels? Slide 7 Orbitals Orbital a 3-D path in
which e -s travel. Each orbital holds 2 e -s (or 1 pair) 4
different orbitals - s, p, d, & f Slide 8 Sublevels - s, p, d
& f s - has 1 s orbital = 2 e - (1 pair) p - has 3 p orbitals =
6 e - (3 pair) d - has 5 d orbitals = 10 e - (5 pair) f - has 7 f
orbitals = 14 e - (7 pair) Slide 9 s Shapes of s & p orbitals p
Slide 10 Shapes of d orbital Slide 11 Quantum Atomic Model Energy
Level = The Rows: 1-7 Sublevel = The Section: s, p, d, f Orbital =
The Seat 1-2, 1-6, 1-10 1-14 76543217654321 s p d 1 2 3 4 5 6 1 2
12345678910 Slide 12 Review Questions 6. How many electrons does
each orbital hold? 7. What are the 4 different orbitals? 8. What
type of orbitals make up the s sublevel? the p? the d? the f? 9.
How many electrons are in the p sublevel? 10. How is the structure
of energy levels, sublevels and orbitals of an atom like an
auditorium? Slide 13 Sublevel Blocks of the Periodic Table Slide 14
How many blocks wide is the s sublevel? How many e -s can the s
level hold? How many orbitals? Slide 15 Sublevel Blocks of the
Periodic Table How wide is the p sublevel? Guess how many e -s the
p sublevel holds? How many orbitals? Slide 16 Sublevel Blocks of
the Periodic Table How wide is the d sublevel? Guess how many e -s
the d sublevel holds? How many orbitals? Slide 17 Sublevel Blocks
of the Periodic Table How wide is the f sublevel? How many e -s can
an f sublevel hold? How many orbitals? Slide 18 Sublevel Blocks of
the Periodic Table 12345671234567 If the Periodic Table was a
seating chart in an auditorium, what element would be sitting in
Row 2, Section P, Seat 2? Slide 19 Sublevel Blocks of the Periodic
Table 12345671234567 Row 2, Section P, Seat 2 is Silicon Slide 20
Think back to our the auditorium analogy Pretend the stage is the
nucleus and the elements are in their specific seats, sections
& rows. Slide 21 The Quantum Atomic Model Slide 22 The 4 Atomic
Models Slide 23 Compare the 4 Atomic Models Thomson, Rutherford,
Bohr & Quantum 11) Which ones have protons? 12) Which ones have
neutrons? 13) Which ones have a nucleus? 14) Where is the + charge
in each? 15) What is wrong with the Thomson model? 16) What is
wrong with the Rutherford model? 17) What is wrong with the Bohr
Model?
