Chapter%204:%20Glow%20in%20the%20Dark - PowerPoint PPT Presentation

About This Presentation
Title:

Chapter%204:%20Glow%20in%20the%20Dark

Description:

Chapter 4: Glow in the Dark – PowerPoint PPT presentation

Number of Views:101
Avg rating:3.0/5.0
Slides: 22
Provided by: Luke102
Learn more at: http://www.ctreg14.org
Category:

less

Transcript and Presenter's Notes

Title: Chapter%204:%20Glow%20in%20the%20Dark


1
Chapter 4 Glow in the Dark
2
Introductory Activity
  • List as many things as you can think of that
    glow
  • What do you have to do to make these glowing
    things glow?

3
Glow 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

4
Glow in the dark
Light
Electron structure
Periodic Table
Atomic structure
Periodicity
Atomic theory
5
Section 4.1Development of Atomic Theory
6
Daltons 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

7
Cathode 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
8
Cathode 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
9
Thomsons 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

10
Theories 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

11
Thomsons 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!
12
Gold 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

13
What happened in the experiment?
a
Gold foil
14
What 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

15
What 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

16
A 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

17
More 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.

18
The 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.

19
Pictures of the Bohr Models
20
Use 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

21
Modern 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)
Write a Comment
User Comments (0)
About PowerShow.com