Transcript Chemistry Timeline #1

Atomic Structure
Image courtesy of www.lab-initio.com
Chemistry Timeline #1
B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”

2000 years of Alchemy
1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals
1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements
1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook
Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements
Dalton’s Atomic Theory (1808)
John Dalton
 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties
 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged
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.
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
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.
Thomson’s Atomic Model
J.J. Thomson
Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.
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
Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. 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
Rutherford’s Gold Foil Experiment
 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded
Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?
The Answers
Target #1
Target #2
Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”
Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged
Atomic Particles
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
The Atomic
Scale
Helium-4
 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
Image: User Yzmo Wikimedia Commons
.
About Quarks…
Protons and neutrons are NOT fundamental particles.
Protons are made of two “up” quarks and
one “down” quark.
Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons
.
Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold
# of protons Atomic # (Z)
6
6
15
15
79
79
Mass Number
Mass number (A) is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide
p+
n0
e-
Mass #
Oxygen - 18
8
10
8
18
Arsenic - 75
Phosphorus - 31
33
42
33
75
15
16
15
31
Atomic Masses
Atomic mass is the average of all the naturally
isotopes of that element.
Isotope
Symbol
Composition of
the nucleus
% in nature
Carbon-12
12C
6 protons
6 neutrons
98.89%
Carbon-13
13C
6 protons
7 neutrons
1.11%
Carbon-14
14C
6 protons
8 neutrons
<0.01%
Carbon = 12.011
Isotopic Notation
Z
• Isotopic Notation: A X
• Write the isotopic notation for the following
elements: Boron, Titanium, and Carbon
Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope
Protons
Electrons
Neutrons
Hydrogen–1
(protium)
1
1
0
Hydrogen-2
(deuterium)
1
1
1
Hydrogen-3
(tritium)
1
1
2
Nucleus
Using Isotopic Ratios to calculate
the average mass of an element
• Silver (Ag; Z = 47) has 46 known isotopes, but
only two occur naturally, 107Ag and 109Ag.
Given the following data, calculate the atomic
mass of Ag:
Isotope
Mass
Percent Abundance
107Ag
106.90509
51.84
109Ag
108.90476
48.16
Try one…
• Gallium has two naturally occurring isotopes:
69Ga (isotopic mass 68.9256 amu, 60.11%
abundance) and 71Ga (isotopic mass 70.9247
amu, 38.89% abundance) Calculate the average
atomic mass
Another one…
• Magnesium has three naturally occurring
isotopes seen in the table below:
Isotope
Mass
Percent Abundance
24Mg
23.9850
78.99
25Mg
24.9858
10.00
26Mg
25.9826
A little more complicated…
• Copper has two naturally occurring isotopes,
63Cu (isotopic mass 62.9396 amu) and 65Cu
(isotopic mass 64.9278). If copper has an
atomic mass of 63.546 amu, what is the
percent abundance of each isotope?