RAD PRO Flashcards
(165 cards)
1
Q
Building block of the radiographer’s
understanding of the interaction
between ionizing radiation and
matter.
A
ATOM
2
Q
“atomos”
A
indivisible
3
Q
It is the smallest unit of a chemical
element possessing the properties
of that element
A
ATOM
4
Q
It rarely exists alone, and they are
often combined with other atoms
to form a molecule.
A
ATOM
5
Q
the first group of people
who first thought of atomism.
A
GREEK ATOM
6
Q
Scientists at that time thought that all
matter was composed of four
substances: earth, water, air, and
fire
A
GREEK ATOM
7
Q
According to them, all matter could
be described as combinations of
these four basic substances in
various proportions, modified by
four basic essences: wet, dry, hot,
and cold
A
GREEK ATOM
8
Q
modified by
four basic essences:
A
wet, dry, hot,
and cold
9
Q
composed of four
substances:
A
earth, water, air, and
fire.
10
Q
DALTON ATOM NAME
A
John Dalton
11
Q
DALTON ATOM DATE
A
1808
12
Q
An English school teacher published
a book summarizing his
experiments, which showed that the
elements could be classified
according to integral values of
atomic mass.
A
DALTON ATOM
13
Q
According to Dalton, an element was
composed of identical atoms that
reacted the same way chemically.
A
DALTON ATOM
14
Q
The physical combination of one
type of atom with another was
visualized as being an eye and -
hook affair
A
DALTON ATOM
15
Q
50 years after Dalton’s work
A
PERIODIC TABLE
16
Q
Showed that elements were arranged in
order of increasing atomic mass, a periodic
repetition of similar chemical properties
occurred
A
Dmitri Mendeleev
17
Q
Mendeleev’s periodic table contained ____
discovered elements
A
63
18
Q
Each block represents an element.
A
PERIODIC TABLE
19
Q
The superscript is the atomic number
A
PERIODIC TABLE
20
Q
The subscript is the elemental mass.
A
PERIODIC TABLE
21
Q
All elements in the same group/column
react chemically in a similar fashion and
have similar physical properties
A
PERIODIC TABLE
22
Q
Late 1890
A
THOMPSON ATOM
23
Q
THOMPSON ATOM FULL NAME
A
Joseph John Thompson
24
Q
While investigating the physical properties
of cathode rays (electrons), he concluded
that electrons were an integral part of all
atoms.
A
THOMPSON ATOM
25
He described the atom as looking
something like a plum pudding, in which
the plums represent negative electric
charges (electrons) and the pudding was a
shapeless mass of uniform positive
electrification.
THOMPSON ATOM
26
RUTHERFORD EXPERIMENT FULL NAME
Ernest Rutherford
27
The number of electrons was thought to
equal the quantity of positive
electrification because the atom was
known to be electrically neutral.
THOMPSON ATOM
28
1911 RUTHERFORD EXPERIMENT
1911
29
Through a series of ingenious experiments,
he disproved Thomson's model of the atom
RUTHERFORD EXPERIMENT
30
He introduced the nuclear model, which
described the atom as containing a small,
dense, positively charged center
surrounded by a negative cloud of
electrons
RUTHERFORD EXPERIMENT
31
He called the center of the atom the
nucleus
RUTHERFORD EXPERIMENT
32
BOHR ATOM FULL NAME
Niels Bohr
33
Niels Bohr
1913
34
Improved Rutherford's description of the
atom.
BOHR ATOM
35
Bohr's model was a miniature solar system
in which the electrons revolved about the nucleus in prescribed orbits or energy
levels.
BOHR ATOM
36
Contains small, dense, positively charged
nucleus surrounded by negatively charged
electrons that revolve in fixed, well-defined
orbits about the nucleus
BOHR ATOM
37
QUANTUM MODEL SCIENTIST
Erwin Schrödinger
38
QUANTUM MODEL
1926
39
Instead of thinking of electrons as tiny
particles moving in fixed orbits,
Schrödinger's model treats electrons as
wave-like entities
Erwin Schrödinger
40
quantum model shifts the
idea of electrons from fixed paths to fuzzy
regions probability, giving us a more
accurate way to understand atomic
structure.
Erwin Schrödinger
41
The atom can be viewed as a miniature
solar system whose sun is the nucleus and
whose planets are the electrons
ATOM
42
The arrangement of electrons around the
nucleus determines the way atoms interact.
ATOM
43
An atomic particle is extremely small, its
mass is expressed in atomic mass units
(amu) for convenience.
ATOMIC MASS UNIT
44
one atomic mass unit is equal to one
twelfth the mass of a carbon-12 atom.
ATOMIC MASS UNIT
45
*JJ. Thompson
*Shell
*Negative charge
*9.11 x 10
-31 kg
*AMU: 0.000549
ELECTRONS
46
*Eugene Goldstein
*Nucleus
*Positive charge
*1.673 x 10
-27 kg
PROTONS
47
*James Chadwick
*Nucleus
*Neutral charge
*1.675 x 10
-27 kg
*AMU: 1.00867
NEUTRONS
48
Maximum number of electrons that can
exist in each shell increases with the
distance of the shell from the nucleus.
ELECTRON ARRANGEMENT
49
The total number of electrons in the orbital
shells is exactly equal to the number of
protons in the nucleus
IONIZED ATOM
50
An atom has an extra electron or has had
an electron removed.
IONIZED ATOM
51
It is not electrically neutral but carries a
charge equal in magnitude to the
difference between the numbers of
electrons and protons
IONIZED ATOM
52
a certain amount of energy to remove
an electron from the atom X-ray transfers
its energy to an orbital electron and ejects
that electron from the atom.
IONIZATION
53
process of removing the electron to an
atom.
IONIZATION
54
The closer an electron is to the nucleus, the
more tightly it is bound.
ELECTRON BINDING ENERGY
55
Strength of attachment of an electron to
the nucleus
ELECTRON BINDING ENERGY
56
a certain amount of
energy to remove an electron from the
atom.
Ionization Energy
57
Atoms are identified by their atomic
symbols
ATOMIC
58
is the atomic symbo
X
59
is the mass number (number of protons
plus neutrons)
A
60
is the atomic number (number of
protons)
Z
61
The number of neutrons (N) in an
atom can be determined by the
equation
N = A - Z
62
Energy emitted and transferred through
space.
RADIATION
63
Transfer of energy
RADIATION
64
"electromagnetic energy”
RADIATION
65
*“electromagnetic radiation'”
RADIATION
66
type of radiation
that can remove an orbital electron from
the atom with which it interacts.
Ionizing Radiation
67
series of energy
waves composed of oscillating electric and
magnetic fields traveling at the speed of
light
Non-Ionizing Radiation
68
usually occurs farther away from the
charged particle's trajectory than
ionization.
EXCITATION
69
excited atom wil de-excite and emit a low
energy ultraviolet photon.
EXCITATION
70
each excitation event reduces the charged
particle's velocity
EXCITATION
71
Radiation can be found in soils, in
our air and water, and in us because
it occurs in our natural environment,
we encounter it every day through
the food we eat, the water we drink,
and the air we breathe
NATURAL ENVIRONMENTAL RADIATION
72
particulate and electromagnetic
radiation emitted by the sun and
stars.
Cosmic
73
sun is the largest source of cosmic
radiation
Cosmic
74
Results from deposits of uranium,
thorium, and radionuclides in the
earth
Terrestrial
75
the largest source of natural
environmental radiation.
RADON
76
Radioactive gas that is produced by
the natural radioactive decay of
uranium which is present in trace
quantities in Earth
RADON
77
Found in nuclear power plants
URANIUM
78
Mineral coming from the earth
URANIUM
79
NATURAL RADIATION
- Concrete
- Bricks
- Gypsum wall board or “drywall”
80
Any radiation sources produced by
humans
MAN MADE RADIATION
81
MAN MADE RADIATION
They may be produced for use of
their radiation, or for other
purposes using the processes taking
place in them
82
contains Americium 241
Smoke detectors
83
Timex indiglo – contains Tritium.
Watches
84
The watch dials on which they
worked were extremely small, they
were instructed to use their lips to
bring their paint brushes to a fine
point
RADIUM GIRLS
85
When they asked about radiums
safety, they were assured by their
managers that they had nothing to
worry about
RADIUM GIRLS
86
Most significant contributors in
man-made exposure by ionizing
radiation to the public.
MEDICAL PROCEDURES
87
Professionals are exposed to
radiation due to their occupations
and to the sources they are working
with.
MEDICAL PROCEDURES
88
Phenomenon of spontaneous
emission of such particles from the
nucleus.
RADIOACTIVITY
89
Discovered by Antoine Henri
Becquerel in 1896.
RADIOACTIVITY
90
it has excess nuclear energy,
making it unstable
RADIOACTIVE ISOTOPES
91
a nucleus must be extremely
unstable to emit an alpha particle
but when it does, it loses two units
of positive charge and four units of
mass.
ALPHA DECAY
92
An electron created in the nucleus is
ejected from the nucleus with
considerable kinetic energy and
escapes from the atom
BETA DECAY
93
Equivalent to a helium nucleus
Alpha Particles
94
They are light particles with an atomic mass number of 0 and carry one unit of negative or positive charge
Beta Particles
95
No mass and no charge
Photons
96
it is composed of electromagnetic
rays.
GAMMA
97
are different types of nuclear
arrangements characterized by
mass and atomic number
Nuclides
98
STABLE nuclei
Nuclides
99
are also nuclides but they have too
few or too many neutrons and/or
protons
Radionuclides
100
UNSTABLE nuclei
Radionuclides
101
The process by which an unstable atomic
nucleus spontaneously emits particles and
energy and transforms itself to another
atom to attain stability.
ATOMIC STABILITY
102
A nucleus must be extremely
unstable to emit an alpha particle,
but when it does, it loses two units
of positive charge and four units of
mass
Alpha Decay
103
Properties of an Alpha Particle
* Discrete energy
* Short range
* Specific ionization
104
A radionuclide converts a neutron
into a proton.
Beta Minus Decay
105
The excess energy is released as a
NEGATRON and ANTINEUTRINO.
Beta Minus Decay
106
The result of beta emission
therefore is to increase the atomic
number by one while the atomic
mass number remains the same.
Beta Minus Decay
107
Radionuclide converts a proton into
a neutron.
Beta Plus Decay
108
Radionuclide converts a proton into
a neutron by capturing its own
electron resulting in the release of
CHARACTERISTIC X-RAY or AUGER
ELECTRON.
Electron Capture
109
Radionuclide in its excited state
deexcites by emission of one or
more HIGH FREQUENCY PHOTON.
Gamma Decay
110
Radioisotopes disintegrate into
stable isotopes of different
elements at a decreasing rate so
that the quantity of radioactive
material never quite reaches zero.
RADIOACTIVE HALF LIFE (T1/2)
111
Time required to reduce initial
activity to one-half
HALF-LIFE
112
time required so that the
activity of the radionuclide is reduced to
50%
PHYSICAL
113
time required for the body
to eliminate half of an administered
dosage of any substance
BIOLOGICAL
114
time required for a
radioactive elimination in the body to be
dismissed by 50%.
EFFECTIVE
115
“electromagnetic energy”
Photons
116
This energy exists over a wide
range called an energy continuum
Photons
117
uninterrupted (continuous) ordered sequence. * Examples: free-flowing rivers and sidewalks
CONTINUUM
118
Late in the 19th century
James Clerk Maxwell
119
Showed that visible light has both
electric and magnetic properties.
James Clerk Maxwell
120
Photons are energy disturbances
that move through space at the
speed of light (c).
Velocity
121
Some sources give the speed of
light as 186,000 miles per second,
but in the SI system of units, it is
3×10
8 m/s.
Velocity
122
Photons have no mass and
therefore no identifiable form, they
do have electric and magnetic fields
that are continuously changing in a
sinusoidal fashion.
Velocity and Amplitude
123
Describe interactions among
different energies, forces, or masses
that can otherwise be described
only mathematically
Field
124
One-half the range from crest to
valley over which the sine wave
varies
Amplitude
125
Shows three examples of a
sinusoidal variation
Amplitude
126
Distance between consecutive wave
crests or other similar points on the
wave.
Wavelength
127
Represented by the Greek letter
lambda (λ).
Wavelength
128
Number of wavelengths that pass a
point of observation per second.
Frequency
129
The rate of rise and fall
Frequency
130
Represented by f has units of Hertz
(1 Hz = 1 cycle per second)
Frequency
131
Velocity, Frequency, and
Wavelength
Wave Parameters
132
Needed to describe electromagnetic
energy
Wave Parameters
133
The relationship among these
parameters is important.
Wave Parameters
134
A change in one affects the value of
the others. Velocity is constant
Wave Parameters
135
Remember:
The shorter the wavelength, the
higher the frequency.
136
A continuum of electromagnetic
energy
Electromagnetic Spectrum
137
viewing condition of
radiographic & fluoroscopic images are
critical to diagnosis
*Visible light Region
138
fundamental to producing a
high-quality radiograph.
X-ray Region
139
with the introduction of MRI, become more
important in medical imaging.
*Radiofrequency Region
140
The wave of moving molecules
Ultrasound
141
It requires matter
Ultrasound
142
It cannot exist in vacuum
Ultrasound
143
Diagnostic ultrasound is not part of
the electromagnetic spectrum!
Ultrasound
144
It occupies the smallest segment of
electromagnetic spectrum
Visible Light
145
It is described in terms of
wavelength
Visible Light
146
Range: 400 nm (violet) to 700 nm
(red)
Visible Light
147
The deviation of course occurs
when photos of visible light
traveling in straight lines pass from
one transparent medium to another
Refraction
148
Longer wavelength than visible light
Infrared
149
Shorter wavelength than
microwaves
Infrared
150
It heats any substance on which it
shines (radiant heat)
Infrared
151
● Radiowaves
● Range: 0.3 kHz-300 GHz
● Low energy & long wavelength
Radiofrequency
152
Very-short wavelength RF, lower
than infrared.
Microwave
153
It is emitted from the electron cloud
X-Rays
154
It is produced in diagnostic imaging
systems
X-Rays
155
It comes from inside the nucleus of
radioactive atom
Gamma Ray
156
It is emitted spontaneously from
radioactive material
Gamma Ray
157
Wave-Particle Duality
Wave-Particle Duality
158
X-ray photons behave more like
particles
Wave-Particle Duality
159
The principle that states that both
wave & particle concepts must be
retained, because wave-like
properties are exhibited in some
experiments & particle-like
properties are exhibited in others
Wave-Particle Duality
160
not at all
(transmission)
TRANSPARENCY:
161
partially
(attenuation)
TRANSLUCENCY
162
completely (absorption) *
e.g. black glass
OPACITY
163
the structures that
absorb x-rays
RADIOPAQUE
164
the structures that
transmit x-rays
RADIOLUCENT
165
It states that the intensity of
radiation at a location is inversely
proportional to the square of
distance from the source of
radiation.
Inverse Square Law
