1. The Quantum Model of the Atom
Chapter 4
Section 2

2. Bohr’s Problems
Why did hydrogen’s ________exist around the nucleus only in ____________orbits?
Why couldn’t the electron exist in a ___________number of orbits with slightly different energies?
Why didn’t the Bohr model work for ____ atoms?

3. Louis de Broglie French scientist in the 1920s
Observed that the behavior of ________ is similar to the behavior of _________
Suggested that _________be considered _________
Other experiments confirmed that electrons have ____________properties

4. Electrons are Like Light
Electrons can be __________.
Electrons can show __________patterns
These are properties of __________!

5. Electrons as Particles and Waves
Electrons were determined to also have a dual ___________nature, like _______.
So……..where are they in the __________?
_____________________ was a German physicist that tried to
detect electrons.

6. Heisenberg Uncertainty Principle
________have about the same energy as a _________of light
When trying to detect an ________, and the photon of light ______________ __________
___________________________: it is impossible to determine simultaneously both the position and the velocity of an electron

7. Schrödinger Wave Equation
________________was an Austrian physicist
Said that electrons travel in __________
Only waves of __________energies, and therefore __________, provide solutions to the wave equation:

8. Quantum Theory
The foundation for modern ___________ theory was laid by Heisenberg’s _______________ and Schrödinger’s ________________.
______________________: describes mathematically the wave properties of electrons and other very small particles moving very fast

9. Quantum Theory
Electrons do ______travel around the nucleus in ________orbits.
They exist in certain regions called _____________.
__________: a three-dimensional _____ around the nucleus that indicates the __________location of an __________.

10. The Quantum Model- The Electron Cloud
______________- Statistical area where electrons should exist around the nucleus.
This is not a nice and neat set of circular paths
______________location of electrons but we can _______________represent where most of the electrons should “be.”

11. Electron Cloud

12. Quantum Numbers
________________: numbers (4 of them) that specify the properties of _______ _______and the properties of ________ in those orbitals
The first 3 quantum numbers result from solutions to the ____________________.
The fourth quantum number describes a fundamental state of the _________(its spin) that occupies an orbital

13. Principle Quantum Number (n)
It indicates the ________________ occupied by the electron and is symbolized by _____.
As n ________, the electron’s ______and its average __________from the nucleus ____________.
______number of ___________in a main energy level is indicated by _____.

14. Angular Momentum Quantum Number (l)
It indicates the _________of the orbital; which indicates the ________of orbital.
Energy __________: orbitals of different ________within a particular main energy level.

15. Angular Momentum Quantum Number (l)
For a specific _______energy level, the number of orbital ________possible is equal to _____.
Actual values for l start at 0 and increase up to (n-1).
The different shapes are designated ___, ____, _____, and ____, each with a specific number of orbitals.

16. Orbitals Energy level n=1: only ___sublevel, “___”
All s orbitals (s sublevel) are __________.
One s orbital can hold ____electrons.
There is one s orbital in ____energy level
Designated as ___, ___, ___, ___, etc.
If you have one electron in the 1s orbital, it is designated as ____, if you have two electrons, then ____.

17. Other Sublevels
The p sublevel has ___orbitals, each capable of holding ___electrons for a total of ___electrons.
The d sublevel has ___orbitals, each capable of holding ___electrons for a total of ___electrons.
The f sublevel has ___orbitals, each capable of holding ___electrons for a total of ___electrons.

18. Magnetic Quantum Number (ml)
It indicates the ___________of an orbital around the nucleus
___orbitals are __________, so they only have _______possible orientation
___orbitals are “___________” shaped and have ___possible orientations according to the Schrödinger’s equation.

19. Quantum Mechanical Model
An _______is the region of space where there is a high probability of finding an electron in an atom.
In the quantum mechanical atom, orbitals are arranged according to their size and shape.
The higher the energy of an orbital, the larger its size.
s-orbitals have a spherical shape

20. Shapes of p-Orbitals
Recall that there are three different p sublevels.
p-orbitals have a dumbbell shape.
Each of the p-orbitals has the same shape, but each is oriented along a different axis in space.

21. Location of Electrons in an Orbital
The orbitals are the region of space in which the electrons are most likely to be found.
An analogy for an electron in a p-orbital is a fly trapped in two bottles held end-to-end.

22. Shapes of d Orbitals Recall that there are five different d sublevels.
Four of the d orbitals have a clover-leaf shape and one has a dumbbell and doughnut shape.
There are
seven f
orbitals:

23. Spin Quantum Number (ms)
Indicates the two fundamental _______ states of an electron in an orbital
Has only two possible values: ___and ___
A single orbital can hold a maximum of _____electrons, but they must have ____________spin states.

24. Progression of Models- Summary
Electron Cloud (or Quantum) Model
Chapter 5