LECTURE:
ATOMIC MASS/MASS NUMBER
ISOTOPES
RADIOACTIVE ISOTOPES
MASS SPECTROMETER
HYDROGEN SPECTRUM
ATOMIC MASS, MASS NUMBER
The
atomic mass number is the
AVERAGE of all the isotopes of an
element (will be a decimal number)
The mass number is the number of
protons and neutrons in a single
atom (will be a whole number)
CALCULATING ATOMIC MASS
NUMBER
 Chlorine
has 2 naturally occurring
isotopes: 35Cl and 37Cl. They are
abundant at 75% and 25%, respectively.
Calculate the atomic mass of Cl.
CALCULATING % ABUNDANCE FROM
ATOMIC MASS OF KNOWN ISOTOPES
 Iridium is composed of almost entirely
191Ir and 193Ir. Its molar mass is 192.2 g
mol-1. What are the naturally occurring
percentages of the two isotopes?
RADIOACTIVE ISOTOPES
 Radioactive
isotopes of all elements can
be produced by exposing the natural
element to a flux of slow-moving neutrons
in a nuclear reactor; the nucleus captures
neutrons
USES OF “RADIOISOTOPES”
 CARBON-14
DATING
C-14 is found in all living things due to the
exchange occurring in the carbon cycle
 When an organism dies, the C-14 proportion
stops and begins to decay
 Half-Life = 5,700 years

USES OF “RADIOISOTOPES”
TRACERS
Radioisotopes can be used biologically
 Ex. Iodine radioisotopes can be ingested
(drank) to measure the activity of the thyroid
gland (which absorbs iodine)
 The increase in radioactivity of the gland is
then measured

USES OF “RADIOISOTOPES”
 INTENSE
RADIATION
Some radioisotopes produce intense
radioactivity (gamma rays)
 EX. Co-60; which is used in radiation
treatment or industrially to monitor the
thickness of a steel plate from a rolling mill

MASS SPECTROMETER
A
mass spectrometer is an instrument
which separates particles according to
their masses.
 VAPORIZED
 IONIZED
 ACCELERATED
 DEFLECTED
 DETECTED
ELECTROMAGNETIC SPECTRUM
 The
study of the emission of light by atoms and
ions is the most effective technique for
deducing the electronic structure of atoms.
 The best evidence that electrons in an atoms
surround the nucleus in certain allowed energy
levels, or orbitals, comes from a study of the
emission spectra of elements.
ELECTROMAGNETIC SPECTRUM
 Remember
the flame test????
 Excited electrons will absorb energy and
jump to higher energy levels.
 To return to ground state, they will emit
light energy of a characteristic color.
 Ex.
Lithium – RED
 Sodium - YELLOW

ELECTROMAGNETIC SPECTRUM
 Energy
levels are
not evenly
spaced, so as the
wavelength gets
shorter (and
frequency gets
higher) the lines
in the spectrum
will converge
BALMER SERIES - HYDROGEN
APPLICATION PROBLEMS
Which
of the following are usually
found in the nucleus of an atom?
A.
B.
C.
D.
Electrons and neutrons only.
Neutrons only.
Protons, neutrons, and electrons.
Protons and neutrons only.
APPLICATION PROBLEMS
The number
of 135Ba is
A.
B.
C.
D.
56
82
138
194
of neutrons in an atom
APPLICATION PROBLEMS
How
many electrons would have
about the same mass as a proton or a
neutron?
A.
B.
C.
D.
200
500
2000
5000
APPLICATION PROBLEMS
Which
one of the following is not a
common use of a radioactive
isotope?
A.
B.
C.
D.
As a fuel in fuel cells
Irradiating tumors in patients with
cancer
Measuring the rate of uptake of a
drug that has been swallowed
Finding the age of rocks
APPLICATION PROBLEMS
 Radioisotopes
of normally stable
elements are
Chemically extracted from the natural
element
B. Mined from scarce underground deposits
C. Formed from the stable element in nuclear
reactors
D. Produced through chemical reactions of
the stable element
A.
APPLICATION PROBLEMS
 Identify
A.
B.
C.
D.
E.
the following subatomic particles
The particle that has a much lower mass
than the others ______________________
The particle that has no electrical charge
______
The particle that is not found in the nucleus
____________
The number of these in the nucleus is equal
to the atomic number ___________
The particle that is gained or lost when ions
form __________________