1. Chapter 5
Electrons in Atoms

2. Section 5.1 Light and Quantized Energy
At this point in history, we are in the early 1900’s. Electrons were the 1st subatomic particle to be discovered.
Chemists have a Rutherford Model of the atom. There is a small, dense, positively charged center of the atom called a nucleus. Electrons move around outside the nucleus.

3. The Atom and Unanswered Questions
In Rutherford's model, the atom’s mass is concentrated in the nucleus and electrons move around it.
The model doesn’t explain how the electrons were arranged around the nucleus.
The model doesn’t explain why negatively charged electrons aren’t pulled into the positively charged nucleus.

4. In the early 1900s, scientists observed certain elements emitted visible light when heated in a flame.
Analysis of the emitted light revealed that an element’s chemical behavior is related to the arrangement of the electrons in its atoms.

5. The Wave Nature of Light
Visible light is a type of electromagnetic radiation, a form of energy that exhibits wave-like behavior as it travels through space.
All waves can be described by several characteristics.

6. The wavelength (λ) is the shortest distance between equivalent points on a wave.
The frequency (ν) is the number of waves that pass a given point per second.
The amplitude is the wave’s height from the origin to a crest.

7. What relationship do you see between λ, v, and c?

8. What relationship do you see between
The speed of light (3.00  108 m/s) is the product of it’s wavelength and frequency.
c = λν
What relationship do you see between
λ and ν?

9. Sunlight, or visible light, contains a continuous range of wavelengths and frequencies.
A prism separates sunlight into a continuous spectrum of colors – pg. 138.
The separation of white light by a prism
The electromagnetic spectrum includes all forms of electromagnetic radiation – pg. 139.

10. The Electromagnetic Spectrum

12. Visible Light …
Note the trends: Blue light has shorter λ, higher v, and
more energy. Red light has longer λ, lower v, and less
energy.
Brain Pop - The EM Spectrum

13. The wave model of light cannot explain all of light’s characteristics.
An example is the photoelectric effect , when electrons are emitted from a metal’s surface when light of a certain frequency shines on it (how solar calculators work).
Photoelectric Effect Simulation

14. Albert Einstein proposed in 1905 that light has a dual nature.
Einstein suggested a beam of light has wavelike and particlelike properties.
A photon is a particle of electromagnetic radiation with no mass that carries a quantum of energy.
Ephoton = h
Ephoton represents energy, h is Planck's constant (6.626 x J-s), &  represents frequency.

15. Atomic Emission Spectra
Light in a neon sign is produced when electricity is passed through a tube filled with neon gas and excites the neon atoms.
The excited atoms emit light to release energy.

16. Emission Spectrum for Hydrogen

17. The atomic emission spectrum of an element is the set of frequencies of the electromagnetic waves emitted by the atoms of the element.
Each element’s atomic emission spectrum is unique – they have their own fingerprints!
Absorption and Emission Spectra's

18. Section 5.2 Quantum Theory and the Atom
Bohr's Model of the Atom…
Bohr suggested that an electron moves around the nucleus only in certain allowed circular orbits - Planetary Atomic Model.
The lowest allowable energy state of an atom is called its ground state.
When an atom gains energy, it is in an excited state.

19. Planetary Atomic Model
Bohr Model

20. Bohr assigned a quantum number for each principal energy level.
He tried to predict the spectral lines for elements following Hydrogen, but was not successful.
The behavior of electrons is still not fully understood, but it is known they do not move around the nucleus in circular orbits.

21. Big Discoveries…
Louis de Broglie hypothesized that particles, including electrons, could also have wavelike behaviors.
Werner Heisenberg showed it is impossible to take any measurement of an object without disturbing it.

22. The Heisenberg uncertainty principle states that it is fundamentally impossible to know precisely both the velocity and position of a particle at the same time.
The only quantity that can be known is the probability for an electron to occupy a certain region around the nucleus.

23. Our Current Atomic Theory…
Erwin Schrödinger treated electrons as waves in a model called the quantum mechanical model of the atom. Most people call this the Electron Cloud Model.
This model applied to all elements!!!

24. Quantum Mechanical Model…
In the Quantum Mechanical Model, electrons are arranged in energy levels.
Energy levels are broken down into sublevels. The sublevels are named s, p, d, and f.
Sublevels are broken down into orbitals.
Each orbital may hold only one single pair of electrons.

25. The number of sublevels equals the energy level number.
Energy level 1 – 1 sublevel
Energy level 2 – 2 sublevels
Energy level 3 – 3 sublevels
and so on… until the
7th energy level
Sublevels contain a specific number of orbitals.
s – 1 orbital (2 e-)
p – 3 orbitals (6 e-)
d – 5 orbitals (10 e-)
f – 7 orbitals (14 e-)

26. Orbital Shapes…

27. So, …
n = 1 sublevel: 1s
n = 2 sublevels: 2s & 2p
n = 3 sublevels: 3s, 3p, & 3d
n = 4 sublevels: 4s, 4p, 4d, & 4f
The total number of electrons each level
can hold is determined by the formula
2n2.