Chemistry Chapter 3
Atoms and Atomic
Theory…
1
Law of Conservation of Mass
Mass is neither
created nor destroyed
during chemical or
physical reactions.
Antoine Lavoisier
Total mass of reactants
=
Total mass of products
2
Dalton’s Atomic Theory
(1808)
1. All matter is composed of extremely
small particles called atoms
2. Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
John Dalton
elements differ in size, mass, and
other properties
3. Atoms cannot be subdivided, created, nor
destroyed
4. Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
5. In chemical reactions, atoms are combined,
separated, or rearranged
3
Modern Atomic Theory
Several changes have been made to Dalton’s theory.
Dalton said:
Atoms of a given element are identical in
size, mass, and other properties; atoms of
different elements differ in size, mass, and
other properties
Modern theory states:
Atoms of an element have a characteristic
average mass which is unique to that
element.
4
Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or destroyed
Modern theory states:
Atoms cannot be subdivided, created, or destroyed
in ordinary chemical reactions. However, these
changes CAN occur in nuclear reactions!
5
Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.
Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.
6
Some Modern
Cathode Ray Tubes
7
Thomson’s Atomic Model
Thomson believed that the electrons were like plums
embedded in a positively charged “pudding,” thus it was
called the “plum pudding” model.
8
Mass of the Electron
1909 – Robert Millikan
determines the mass of
the electron.
The oil drop apparatus
Mass of the
electron is
9.109 x 10-31 kg
9
Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them, therefore All
elements must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass
10
Rutherford’s Gold Foil
Experiment
 Alpha particles are helium nuclei that are
emitted from some radioactive substances
 Particles were fired at a thin sheet of gold foil
 Particle hits on the detecting screen (film) are
recorded
11
Rutherford’s Findings
 Most of the particles passed right through
 A few particles were slightly deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”
Conclusions:
 The nucleus is small
 The nucleus is dense (very dense)
 The nucleus is positively charged
12
Atomic Particles (summary info)…
Particle
Electron
Proton
Neutron
Charge
Mass (kg)
-1
9.109 x 10-31
+1
1.673 x 10-27
Location
Electron
cloud
Nucleus
0
1.675 x 10-27
Nucleus
13
The Atomic
Scale
 Most of the mass of the
atom is in the nucleus
(protons and neutrons)
 Electrons are found
outside of the nucleus (the
electron cloud)
 Most of the volume of
the atom is empty space
“q” is a particle called a “quark”
14
Atomic Number
Atomic number of an element is the number of
protons in the nucleus of each atom of that
element.
Element
Carbon
Phosphorus
Gold
# of
protons
6
15
Atomic #
79
79
6
15
15