1. Drill Determine the following for Na: Name of Element
Number of protons
Atomic number
Number of electrons
Mass number
Number of neutrons
Isotopic symbol

2. Objective
SWBAT:
Explore Electrons in order to describe their energies and positions.

3. SAT/HSA Enrichment
A particular toxin prevents cellular production of usable energy. Cells that are affected by this toxin are unable to carry out many of their normal functions.
If cells were exposed to this toxin, which of these processes would probably be least affected?
Mitosis
Diffusion
Respiration
photosynthesis

4. Quick Quiz
The Atom
5 MIN

5. Inquiry Activity
Observing Light Emission From Wintergreen Mints
Purpose:
Students observe light associated with the movement of electrons.
15 Min

6. Electrons in Atoms
Where are they located?

7. Models of the Atom
The scale model shown is a physical model. However, not all models are physical. In fact, several theoretical models of the atom have been developed over the last few hundred years. You will learn about the currently accepted model of how electrons behave in atoms.

8. The Development of Atomic Models
Rutherford’s atomic model could not explain the chemical properties of elements.
Rutherford’s atomic model could not explain why objects change color when heated.

9. The Development of Atomic Models
The timeline shoes the development of atomic models from 1803 to 1911.

10. The Development of Atomic Models
The timeline shows the development of atomic models from 1913 to 1932.

11. The Bohr Model
Bohr proposed that an electron is found only in specific circular paths, or orbits, around the nucleus.

12. The Bohr Model
Each possible electron orbit in Bohr’s model has a fixed energy.
The fixed energies an electron can have are called energy levels.
A quantum of energy is the amount of energy required to move an electron from one energy level to another energy level.

13. The Bohr Model
Like the rungs of the strange ladder, the energy levels in an atom are not equally spaced.
The higher the energy level occupied by an electron, the less energy it takes to move from that energy level to the next higher energy level.

14. The Quantum Mechanical Model
The quantum mechanical model determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus.

15. The Quantum Mechanical Model
Austrian physicist Erwin Schrödinger (1887–1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom.
The modern description of the electrons in atoms, the quantum mechanical model, comes from the mathematical solutions to the Schrödinger equation.

16. The Quantum Mechanical Model
The propeller blade has the same probability of being anywhere in the blurry region, but you cannot tell its location at any instant. The electron cloud of an atom can be compared to a spinning airplane propeller.

17. The Quantum Mechanical Model
In the quantum mechanical model, the probability of finding an electron within a certain volume of space surrounding the nucleus can be represented as a fuzzy cloud. The cloud is more dense where the probability of finding the electron is high.

18. Atomic Orbitals
An atomic orbital is often thought of as a region of space in which there is a high probability of finding an electron.
Each energy sublevel corresponds to an orbital of a different shape, which describes where the electron is likely to be found.

19. Atomic Orbitals
Different atomic orbitals are denoted by letters. The s orbitals are spherical, and p orbitals are dumbbell-shaped.

20. Atomic Orbitals
Four of the five d orbitals have the same shape but different orientations in space.

21. Atomic Orbitals
The numbers and kinds of atomic orbitals depend on the energy sublevel.

22. Atomic Orbitals Orbital Stimulation
The number of electrons allowed in each of the first four energy levels are shown here.
Orbital Stimulation

23. Quick Quiz
1.Rutherford's planetary model of the atom could not explain
a. any properties of elements.
b. the chemical properties of elements.
c. the distribution of mass in an atom.
d. the distribution of positive and negative charges in an atom.

24. Quick Quiz
2.Bohr's model of the atom proposed that electrons are found
a. embedded in a sphere of positive charge.
b. in fixed positions surrounding the nucleus.
c. in circular orbits at fixed distances from the nucleus.
d. orbiting the nucleus in a single fixed circular path.

25. Quick Quiz
3.What is the lowest-numbered principal energy level in which p orbitals are found?
a. 1
b. 2
c. 3
d. 4

26. Electron Distribution Using Peas Lab
Purpose:
Students will be able to describe differences in the nucleus and the electron cloud in order to analyze the structure of the atom.

27. Summary Where are electrons found?
How would you use electrons to help you find elements on the periodic table?
Name the 4 sublevels?
Whose theory does the Electron distribution lab follow? Explain.
Based upon what you know about the electron distribution in the electron cloud how would you determine the location of an electron?

28. Homework
Electron Distribution Using Peas worksheet.