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RTCA244 Image production 2 > matter and fundamentals > Flashcards

matter and fundamentals Flashcards

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1
Q

Matter

A

anything that occupies space and has mass/inertia

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2
Q

Atom

A

all matter is composed of fundamental building blocks

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3
Q

What is a primary characteristic of matter?

A

Mass

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4
Q

The quantity of matter remains unchanged regardless of its state. But it can be transformed from

A

one size, shape, and form to another

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5
Q

What is energy?

A

ability to do work

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6
Q

The unit of energy in radiology is:

A

electron volt {eV}

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7
Q

Potential energy (PE)

A

the ability to do work by virtue of position

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8
Q

Formula for potential energy

A

PE=mgh
M=mass
H= distance above earth
G= acceleration due gravity (9.8 m/s2)

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9
Q

Kinetic energy (KE)

A

the energy of motion

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10
Q

Formula Kinetic energy (KE)

A

KE= 1/2 mv^2

m=mass
v=velocity

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11
Q

The work that can be done when an electron moves through an electric potential difference (volatage)

A

electrical energy

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12
Q
  • Energy of motion at the molecular level

- it is the kinetic energy of molecules

A

Thermal energy (heat)

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13
Q

energy that is contained within the nucleus of an atom

A

nuclear energy

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14
Q

controlled nuclear energy

A

nuclear reactor

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15
Q

uncontrolled energy of the nuclear energy

A

atomic bomb

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16
Q

energy that is transmitted through space as a combination of electric and magnetic field

A

electromagnetic energy

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17
Q

what is the most important energy in the field of radiology?

A

Electromagnetic energy

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18
Q

Another name for electromagnetic energy:

A

radiant energy or radiation

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19
Q

type of radiation that is capable of removing an orbital electron from the atom with which it interacts

A

ionizing radiation

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20
Q

Interaction between radiation and matter

A

ionization

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21
Q

what are interchangeable?

A

matter and energy

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22
Q

matter and energy was first described by

A

albert einstein in the theory of relativity

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23
Q

mass-energy equivalence equation

A

E=mc2

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24
Q

3 basic measurable quantities

A

length, mass, time

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25
unit of Length
based on meter. which used to be the distance between two engraved lines on a platinum-iridium bar.
26
1mm = ____m
.001
27
1cm= ___m
.01m
28
1km=____m
1000m
29
Unit of mass
kilogram 1 kg = the mass of 1000 cm3 of water at 4o C.
30
unit of time
second | It is based on the vibration of Cesium atoms.
31
- a measure of how fast an object is moving | - the rate of change of its position with time
Velocity (speed)
32
Formula for velocity
v=d/t D=distance t= time
33
FPF
furlongs per fortnight
34
FPS
feet per second
35
MPH
miles per hour
36
the rate of change of velocity
acceleration it is a measure of how quickly or slowly the velocity is changing
37
formula for acceleration
A= Vf-Vi/t ``` vf= final velocity Vi= initial velocity t= time ```
38
Newton's Laws of motion: First law
A body will remain at rest or will continue to move with constant velocity in a straight line unless acted on by an external force.
39
Newton's Laws of motion: Second law
The force (F) that acts on an object is equal to the mass (m) of the object times the acceleration (a) produced. F = ma
40
Newton’s Laws of Motion: third law
For every action, there is an equal an opposite reaction.
41
The force on a body due to the pull of gravity.
Weight | WT.= mg
42
The value of acceleration due to gravity on the moon | is only about _______ that on the Earth.
1/6
43
Defined as the force applied to an object times the distance over which it is applied.
work
44
formula for work
W = Fd
45
The rate of doing work
power
46
formula for power
P= work/t=fd/t
47
The KE of the random motion of molecules.
Heat
48
Unit of heat
Calorie; defined as the heat necessary to raise the temperature of 1g of water 1oC.
49
Numeric prefixes
``` Mega: one million (106) Kilo: one thousand (103) Centi: one one-hundreth (10-2) Milli: one one-thousandth (10-3) Micro: one one-millionth (10-6) ```
50
matter is usually found in nature in __________ form, as a mixture of ________ composition.
impure, indefinite
51
the smallest particle of an element that has the characteristic properties of the element
atom
52
The Smallest Subdivision of a substance having the Characteristic properties of that substance.
molecule
53
Any material that has a definite, constant composition.
substance
54
Simple substance
Elements --- cannot be decomposed to simpler substances by ordinary means. [Na, Fe, Pb, O2, H2, W(tungstun)]
55
Complex substance
-formed by chemical union of two or more elements in definite Proportions (NaCl, H2O, HCl, H2SO4 C22H12O11). -These can be decomposed by chemical (or other) means.
56
Greek word for Atom
Atomos which means uncut
57
Most widely held theory of atomic structure is the ____________. First proposed in ______ by _______.
Bohr Atom; 1913; niels bohr
58
Protons
-positively charged -Small mass (1.6 x 10-24g) (~ 1850 x mass of e-) -
59
All protons are _____, but each element has its own _______ _______ of protons.
identical; characteristic number
60
Neutrons
- no charge | - same mass as proton; (1.6 x 10-24g)
61
The positively charged nucleus contains most of the _____ of the atom.
MASS
62
Electron
- negatively charged - extremely small mass - orbit the nucleus in specific energy levels/orbits/shells
63
Shell start with the letter:
K
64
formula for maximum number of electrons in a shell
2N^2
65
Neutral atom
one in which the total number of orbital electrons equals the total number of protons in the nucleus.
66
Atomic Number
- The # of protons in the nucleus. - The “atomic number” of each element distinguishes it from all other elements - symbolized by " Z"
67
Mass number
majority of the mass is in its nucleus (protons and neutrons) symbolized by "A"
68
Chemical Symbols
The shorthand notation used to denote a specific element or isotope of an element. X-is the generic symbol for the elements
69
Isotope
Atoms of the same element having different mass numbers Difference is in the number of neutrons in the nucleus.
70
Isobars
Two or more atoms with the same atomic weight (mass #) but with different atomic numbers.
71
Isomers
Two or more atoms with the same molecular formula, but different physical and chemical properties
72
Isotones
Two or more atoms with the same # of neutrons but having different # of protons in the nucleus.
73
Same Z#; different A#; #neutrons different
isotope
74

| Different Z#, same A#; #neutrons different

| isobars

75
Same Z#; same A; #neutrons same
isomers
76
Different z#, Different A#, #neutons same
isotones
77
The energy required to remove an e- from a particular shell and beyond the range of the nucleus
binding energy
78
The closer a shell is to the nucleus the______ the binding energy
GREATER
79
The higher the z#, the _____ the binding energy.
GREATER
80
The property of elements that is determined by the number of e- in the Outer shell.
CHEMICAL BEHAVIOR
81
Octet Rule
An atom tends to be chemically stable when its outer shell contains exactly 8 e-. The only exception to this is Helium with 2 e- in the outer shell.
82
Ions
Atoms that either lose or gain electrons. Positive ion-lose electron Negative ion-gain
83
Valance
The number of e- lost, gained, or shared by an atom in chemical combination.
84
Bond
Two or more elements are joined together by one of | several different types of chemical bonds.
85
Ionic bond
Bond between 2 ions. It is a transfer of e- between the elements.
86
Covalent bond
Sharing of e- between 2 or more atoms
87
Ionization
The process of converting atoms to ions. Produced exclusively by the addition or removal of outer shell electrons
88
Types of ionization
1. Exposure of matter to X-rays of Gamma Rays 2. Exposure of matter to a stream of electrons. Ex. Cathode to anode 3. Exposure of certain elements to light. Ex fluoro 4. Thermionic emission ex. Cathode, space charge
89
Group Number of periodic table
represent the outer shell, how many electrons in the outer shell
90
Period number of the periodic table
period number represent how many electrons shells they have

RTCA244 Image production 2 (5 decks)

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