Title: Chapter%204:%20Glow%20in%20the%20Dark
1Chapter 4 Glow in the Dark
2Introductory Activity
- List as many things as you can think of that
glow - What do you have to do to make these glowing
things glow?
3Glow in the dark
- This chapter will introduce the chemistry needed
to understand how glowing things work - Section 4.1 History of Atomic Theory
- Section 4.2 Atomic Structure
- Section 4.3 Electron Structure
- Section 4.4 Periodic table
- Section 4.5 Periodicity
- Section 4.6 Light
- Section 4.7 Light and matter
4Glow in the dark
Light
Electron structure
Periodic Table
Atomic structure
Periodicity
Atomic theory
5Section 4.1Development of Atomic Theory
6Daltons Atomic Theory
- John Daltons theory based on experiments in
early 1800s - All matter is made of tiny particles atoms
- Atoms cannot be created, divided, destroyed or
changed into other types of atoms - Atoms of the same element have identical
properties - Atoms of different elements have different
properties - Atoms of different elements combine in
whole-number ratios to form compounds - Chemical changes join, separate or rearrange
atoms in compounds
7Cathode Ray Tubes
A cathode ray is a ray of light traveling in a
vacuum (no other particles inside)
The ray travels from one metal plate to another
as the plates are connected to electricity
Cathode ray
Metal plate (anode) to which stream travels
Metal plate (cathode) releases stream
8Cathode Ray Tubes Charge
In the late 1800s, JJ Thomson put charged plates
outside the tube
Negatively charged plate
-
Ray is deflected away from negative plate and
towards positive plate
Positively charged plate
It made no difference what type of metal he used
in the tubeall material produced this stream
that curved towards the positive charge
9Thomsons conclusions
- The evidence from Thomsons work showed that
there was something negatively charged in atoms - Since all types of metal produced the same
result, the negative charge is in all types of
atoms - Since atoms were overall neutral, if there was a
negative charge there had to also be a positive
charge - In 1897, Thomson announced that the rays were
electrons and they had a negative charge
10Theories change
- Thomsons evidence showed Daltons idea of solid,
uniform atoms was incorrect. - Eugene Goldstein conducted experiments to label
the positive part protons and determined it has
the same charge as the electron (with opposite
sign) but is 1837 times heavier! - Thomson developed the plum pudding model.
- Since most of us arent familiar with plum
pudding, you can think of it as a chocolate
cookie dough theory
11Thomsons Theory
The chips are the negative electrons. The
dough is the positive portion The chips are
stationary and dont move within the
dough Remember, officially this theory is
called plum pudding but its the same idea!
12Gold Foil Experiment
- Hans Geiger performed experiments in the early
1900s where he bombarded very thin gold foil
with radioactive particles (alpha particles ?) - They expected these relatively heavy particles to
go through the atoms with a small deflection
13What happened in the experiment?
a
Gold foil
14What did he see?
- Most of the alpha particles passed straight
through with no deflection - These particles did not run into anything
- Some did deflect slightly
- These particles ran into something much smaller
than themselves - A few were reflected back the direction they came
from - These particles ran into something very dense
15What did that mean?
- Atoms are mostly empty space
- Electrons (the smaller particles) were the cause
of the small deflections - There must be a small area of the atom with most
of its mass (the protons) that caused the
reflections. - He called this small, dense area the nucleus
16A third particle
- The protons and electrons could explain the
charges of the various parts of the atom - They could not explain the total mass of the
atoms - Neutrons were proposed in 1920s but not
confirmed until 1932 by James Chadwick - Neutrons had mass similar to protons and no
charge. They were located in the nucleus
17More changes to the theory
- Niels Bohr performed experiments with hydrogen
atoms light - He determined that electrons are in levels
according to how much energy they have and that
only certain energy amounts were allowed.
18The Bohr Model
- It consists of the nucleus with protons
neutrons and electrons in concentric orbits
(circles) outside the nucleus - The circle closest to the nucleus contains the
lowest energy electrons - The first level can hold 2 electron, then the
next two levels can each hold 8 and then levels
farther out can hold 18.
19Pictures of the Bohr Models
20Use of the Bohr Model now
- We no longer believe electrons are in concentric
circles, but this is still a convenient way to
show energy levels on 2-dimensional paper
21Modern Atomic Theory
- In the 1920s, Bohrs research lead the way for
the study of quantum mechanics (the study of tiny
particles) - Modern atomic theory uses calculus equations to
show how the subatomic particles act as both
particles and waves - These equations show the most probable location
of electrons in the atom (known as atomic
orbitals)