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RAD TECH > RAD PRO > Flashcards

RAD PRO Flashcards

1
Q

Building block of the radiographer’s
understanding of the interaction
between ionizing radiation and
matter.

A

ATOM

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2
Q

“atomos”

A

indivisible

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3
Q

It is the smallest unit of a chemical
element possessing the properties
of that element

A

ATOM

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4
Q

It rarely exists alone, and they are
often combined with other atoms
to form a molecule.

A

ATOM

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5
Q

the first group of people
who first thought of atomism.

A

GREEK ATOM

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6
Q

Scientists at that time thought that all
matter was composed of four
substances: earth, water, air, and
fire

A

GREEK ATOM

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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

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8
Q

modified by
four basic essences:

A

wet, dry, hot,
and cold

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9
Q

composed of four
substances:

A

earth, water, air, and
fire.

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10
Q

DALTON ATOM NAME

A

John Dalton

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11
Q

DALTON ATOM DATE

A

1808

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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

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13
Q

According to Dalton, an element was
composed of identical atoms that
reacted the same way chemically.

A

DALTON ATOM

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14
Q

The physical combination of one
type of atom with another was
visualized as being an eye and -
hook affair

A

DALTON ATOM

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15
Q

50 years after Dalton’s work

A

PERIODIC TABLE

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16
Q

Showed that elements were arranged in
order of increasing atomic mass, a periodic
repetition of similar chemical properties
occurred

A

Dmitri Mendeleev

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17
Q

Mendeleev’s periodic table contained ____
discovered elements

A

63

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18
Q

Each block represents an element.

A

PERIODIC TABLE

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19
Q

The superscript is the atomic number

A

PERIODIC TABLE

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20
Q

The subscript is the elemental mass.

A

PERIODIC TABLE

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21
Q

All elements in the same group/column
react chemically in a similar fashion and
have similar physical properties

A

PERIODIC TABLE

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22
Q

Late 1890

A

THOMPSON ATOM

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23
Q

THOMPSON ATOM FULL NAME

A

Joseph John Thompson

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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

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25
Q

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.

A

THOMPSON ATOM

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26
Q

RUTHERFORD EXPERIMENT FULL NAME

A

Ernest Rutherford

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27
Q

The number of electrons was thought to
equal the quantity of positive
electrification because the atom was
known to be electrically neutral.

A

THOMPSON ATOM

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28
Q

1911 RUTHERFORD EXPERIMENT

A

1911

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29
Q

Through a series of ingenious experiments,
he disproved Thomson’s model of the atom

A

RUTHERFORD EXPERIMENT

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30
Q

He introduced the nuclear model, which
described the atom as containing a small,
dense, positively charged center
surrounded by a negative cloud of
electrons

A

RUTHERFORD EXPERIMENT

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31
Q

He called the center of the atom the
nucleus

A

RUTHERFORD EXPERIMENT

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32
Q

BOHR ATOM FULL NAME

A

Niels Bohr

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33
Q

Niels Bohr

A

1913

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34
Q

Improved Rutherford’s description of the
atom.

A

BOHR ATOM

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35
Q

Bohr’s model was a miniature solar system
in which the electrons revolved about the nucleus in prescribed orbits or energy
levels.

A

BOHR ATOM

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36
Q

Contains small, dense, positively charged
nucleus surrounded by negatively charged
electrons that revolve in fixed, well-defined
orbits about the nucleus

A

BOHR ATOM

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37
Q

QUANTUM MODEL SCIENTIST

A

Erwin Schrödinger

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38
Q

QUANTUM MODEL

A

1926

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39
Q

Instead of thinking of electrons as tiny
particles moving in fixed orbits,
Schrödinger’s model treats electrons as
wave-like entities

A

Erwin Schrödinger

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40
Q

quantum model shifts the
idea of electrons from fixed paths to fuzzy
regions probability, giving us a more
accurate way to understand atomic
structure.

A

Erwin Schrödinger

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41
Q

The atom can be viewed as a miniature
solar system whose sun is the nucleus and
whose planets are the electrons

A

ATOM

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42
Q

The arrangement of electrons around the
nucleus determines the way atoms interact.

A

ATOM

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43
Q

An atomic particle is extremely small, its
mass is expressed in atomic mass units
(amu) for convenience.

A

ATOMIC MASS UNIT

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44
Q

one atomic mass unit is equal to one
twelfth the mass of a carbon-12 atom.

A

ATOMIC MASS UNIT

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45
Q

*JJ. Thompson
*Shell
*Negative charge
*9.11 x 10
-31 kg
*AMU: 0.000549

A

ELECTRONS

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46
Q

*Eugene Goldstein
*Nucleus
*Positive charge
*1.673 x 10
-27 kg

A

PROTONS

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47
Q

*James Chadwick
*Nucleus
*Neutral charge
*1.675 x 10
-27 kg
*AMU: 1.00867

A

NEUTRONS

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48
Q

Maximum number of electrons that can
exist in each shell increases with the
distance of the shell from the nucleus.

A

ELECTRON ARRANGEMENT

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49
Q

The total number of electrons in the orbital
shells is exactly equal to the number of
protons in the nucleus

A

IONIZED ATOM

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50
Q

An atom has an extra electron or has had
an electron removed.

A

IONIZED ATOM

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51
Q

It is not electrically neutral but carries a
charge equal in magnitude to the
difference between the numbers of
electrons and protons

A

IONIZED ATOM

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52
Q

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.

A

IONIZATION

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53
Q

process of removing the electron to an
atom.

A

IONIZATION

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54
Q

The closer an electron is to the nucleus, the
more tightly it is bound.

A

ELECTRON BINDING ENERGY

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55
Q

Strength of attachment of an electron to
the nucleus

A

ELECTRON BINDING ENERGY

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56
Q

a certain amount of
energy to remove an electron from the
atom.

A

Ionization Energy

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57
Q

Atoms are identified by their atomic
symbols

A

ATOMIC

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58
Q

is the atomic symbo

A

X

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59
Q

is the mass number (number of protons
plus neutrons)

A

A

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60
Q

is the atomic number (number of
protons)

A

Z

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61
Q

The number of neutrons (N) in an
atom can be determined by the
equation

A

N = A - Z

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62
Q

Energy emitted and transferred through
space.

A

RADIATION

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63
Q

Transfer of energy

A

RADIATION

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64
Q

“electromagnetic energy”

A

RADIATION

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65
Q

*“electromagnetic radiation’”

A

RADIATION

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66
Q

type of radiation
that can remove an orbital electron from
the atom with which it interacts.

A

Ionizing Radiation

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67
Q

series of energy
waves composed of oscillating electric and
magnetic fields traveling at the speed of
light

A

Non-Ionizing Radiation

68
Q

usually occurs farther away from the
charged particle’s trajectory than
ionization.

A

EXCITATION

69
Q

excited atom wil de-excite and emit a low
energy ultraviolet photon.

A

EXCITATION

70
Q

each excitation event reduces the charged
particle’s velocity

A

EXCITATION

71
Q

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

A

NATURAL ENVIRONMENTAL RADIATION

72
Q

particulate and electromagnetic
radiation emitted by the sun and
stars.

A

Cosmic

73
Q

sun is the largest source of cosmic
radiation

A

Cosmic

74
Q

Results from deposits of uranium,
thorium, and radionuclides in the
earth

A

Terrestrial

75
Q

the largest source of natural
environmental radiation.

A

RADON

76
Q

Radioactive gas that is produced by
the natural radioactive decay of
uranium which is present in trace
quantities in Earth

A

RADON

77
Q

Found in nuclear power plants

A

URANIUM

78
Q

Mineral coming from the earth

A

URANIUM

79
Q

NATURAL RADIATION

A
  • Concrete
  • Bricks
  • Gypsum wall board or “drywall”
80
Q

Any radiation sources produced by
humans

A

MAN MADE RADIATION

81
Q

MAN MADE RADIATION

A

They may be produced for use of
their radiation, or for other
purposes using the processes taking
place in them

82
Q

contains Americium 241

A

Smoke detectors

83
Q

Timex indiglo – contains Tritium.

A

Watches

84
Q

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

A

RADIUM GIRLS

85
Q

When they asked about radiums
safety, they were assured by their
managers that they had nothing to
worry about

A

RADIUM GIRLS

86
Q

Most significant contributors in
man-made exposure by ionizing
radiation to the public.

A

MEDICAL PROCEDURES

87
Q

Professionals are exposed to
radiation due to their occupations
and to the sources they are working
with.

A

MEDICAL PROCEDURES

88
Q

Phenomenon of spontaneous
emission of such particles from the
nucleus.

A

RADIOACTIVITY

89
Q

Discovered by Antoine Henri
Becquerel in 1896.

A

RADIOACTIVITY

90
Q

it has excess nuclear energy,
making it unstable

A

RADIOACTIVE ISOTOPES

91
Q

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.

A

ALPHA DECAY

92
Q

An electron created in the nucleus is
ejected from the nucleus with
considerable kinetic energy and
escapes from the atom

A

BETA DECAY

93
Q

Equivalent to a helium nucleus

A

Alpha Particles

94
Q

They are light particles with an atomic mass number of 0 and carry one unit of negative or positive charge

A

Beta Particles

95
Q

No mass and no charge

A

Photons

96
Q

it is composed of electromagnetic
rays.

A

GAMMA

97
Q

are different types of nuclear
arrangements characterized by
mass and atomic number

A

Nuclides

98
Q

STABLE nuclei

A

Nuclides

99
Q

are also nuclides but they have too
few or too many neutrons and/or
protons

A

Radionuclides

100
Q

UNSTABLE nuclei

A

Radionuclides

101
Q

The process by which an unstable atomic
nucleus spontaneously emits particles and
energy and transforms itself to another
atom to attain stability.

A

ATOMIC STABILITY

102
Q

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

A

Alpha Decay

103
Q

Properties of an Alpha Particle

A
  • Discrete energy
  • Short range
  • Specific ionization
104
Q

A radionuclide converts a neutron
into a proton.

A

Beta Minus Decay

105
Q

The excess energy is released as a
NEGATRON and ANTINEUTRINO.

A

Beta Minus Decay

106
Q

The result of beta emission
therefore is to increase the atomic
number by one while the atomic
mass number remains the same.

A

Beta Minus Decay

107
Q

Radionuclide converts a proton into
a neutron.

A

Beta Plus Decay

108
Q

Radionuclide converts a proton into
a neutron by capturing its own
electron resulting in the release of
CHARACTERISTIC X-RAY or AUGER
ELECTRON.

A

Electron Capture

109
Q

Radionuclide in its excited state
deexcites by emission of one or
more HIGH FREQUENCY PHOTON.

A

Gamma Decay

110
Q

Radioisotopes disintegrate into
stable isotopes of different
elements at a decreasing rate so
that the quantity of radioactive
material never quite reaches zero.

A

RADIOACTIVE HALF LIFE (T1/2)

111
Q

Time required to reduce initial
activity to one-half

A

HALF-LIFE

112
Q

time required so that the
activity of the radionuclide is reduced to
50%

A

PHYSICAL

113
Q

time required for the body
to eliminate half of an administered
dosage of any substance

A

BIOLOGICAL

114
Q

time required for a
radioactive elimination in the body to be
dismissed by 50%.

A

EFFECTIVE

115
Q

“electromagnetic energy”

A

Photons

116
Q

This energy exists over a wide
range called an energy continuum

A

Photons

117
Q

uninterrupted (continuous) ordered sequence. * Examples: free-flowing rivers and sidewalks

A

CONTINUUM

118
Q

Late in the 19th century

A

James Clerk Maxwell

119
Q

Showed that visible light has both
electric and magnetic properties.

A

James Clerk Maxwell

120
Q

Photons are energy disturbances
that move through space at the
speed of light (c).

A

Velocity

121
Q

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.

A

Velocity

122
Q

Photons have no mass and
therefore no identifiable form, they
do have electric and magnetic fields
that are continuously changing in a
sinusoidal fashion.

A

Velocity and Amplitude

123
Q

Describe interactions among
different energies, forces, or masses
that can otherwise be described
only mathematically

A

Field

124
Q

One-half the range from crest to
valley over which the sine wave
varies

A

Amplitude

125
Q

Shows three examples of a
sinusoidal variation

A

Amplitude

126
Q

Distance between consecutive wave
crests or other similar points on the
wave.

A

Wavelength

127
Q

Represented by the Greek letter
lambda (λ).

A

Wavelength

128
Q

Number of wavelengths that pass a
point of observation per second.

A

Frequency

129
Q

The rate of rise and fall

A

Frequency

130
Q

Represented by f has units of Hertz
(1 Hz = 1 cycle per second)

A

Frequency

131
Q

Velocity, Frequency, and
Wavelength

A

Wave Parameters

132
Q

Needed to describe electromagnetic
energy

A

Wave Parameters

133
Q

The relationship among these
parameters is important.

A

Wave Parameters

134
Q

A change in one affects the value of
the others. Velocity is constant

A

Wave Parameters

135
Q

Remember:

A

The shorter the wavelength, the
higher the frequency.

136
Q

A continuum of electromagnetic
energy

A

Electromagnetic Spectrum

137
Q

viewing condition of
radiographic & fluoroscopic images are
critical to diagnosis

A

*Visible light Region

138
Q

fundamental to producing a
high-quality radiograph.

A

X-ray Region

139
Q

with the introduction of MRI, become more
important in medical imaging.

A

*Radiofrequency Region

140
Q

The wave of moving molecules

A

Ultrasound

141
Q

It requires matter

A

Ultrasound

142
Q

It cannot exist in vacuum

A

Ultrasound

143
Q

Diagnostic ultrasound is not part of
the electromagnetic spectrum!

A

Ultrasound

144
Q

It occupies the smallest segment of
electromagnetic spectrum

A

Visible Light

145
Q

It is described in terms of
wavelength

A

Visible Light

146
Q

Range: 400 nm (violet) to 700 nm
(red)

A

Visible Light

147
Q

The deviation of course occurs
when photos of visible light
traveling in straight lines pass from
one transparent medium to another

A

Refraction

148
Q

Longer wavelength than visible light

A

Infrared

149
Q

Shorter wavelength than
microwaves

A

Infrared

150
Q

It heats any substance on which it
shines (radiant heat)

A

Infrared

151
Q

● Radiowaves
● Range: 0.3 kHz-300 GHz
● Low energy & long wavelength

A

Radiofrequency

152
Q

Very-short wavelength RF, lower
than infrared.

A

Microwave

153
Q

It is emitted from the electron cloud

A

X-Rays

154
Q

It is produced in diagnostic imaging
systems

A

X-Rays

155
Q

It comes from inside the nucleus of
radioactive atom

A

Gamma Ray

156
Q

It is emitted spontaneously from
radioactive material

A

Gamma Ray

157
Q

Wave-Particle Duality

A

Wave-Particle Duality

158
Q

X-ray photons behave more like
particles

A

Wave-Particle Duality

159
Q

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

A

Wave-Particle Duality

160
Q

not at all
(transmission)

A

TRANSPARENCY:

161
Q

partially
(attenuation)

A

TRANSLUCENCY

162
Q

completely (absorption) *
e.g. black glass

A

OPACITY

163
Q

the structures that
absorb x-rays

A

RADIOPAQUE

164
Q

the structures that
transmit x-rays

A

RADIOLUCENT

165
Q

It states that the intensity of
radiation at a location is inversely
proportional to the square of
distance from the source of
radiation.

A

Inverse Square Law

RAD TECH (1 decks)

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