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Rad Science 1 > Ch 2: Atom Structure and Measurements > Flashcards

Ch 2: Atom Structure and Measurements Flashcards

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1
Q

quantifies radioactivity

A

Curie

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2
Q

List some properties of xray and gamma photons

A

ionize (high energy)
cannot be focused, refracted, or reflected
Can be restricted (collimate), filtered, absorbed and remitted
cannot see, hear, feel, or smell
causes certain materials to fluoresce
travels at the speed of light

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3
Q

radiation monitors are usually calibrated to what unit of measure

A

Roentgen (R) or milliroentgens (mR)

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4
Q

how to convert R to mR

A

divide by 1000 (move decimal three places to the left)
1 mR = 1/1000 R

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5
Q

What is the SI unit for Roentgen

A

C/kg
Coulombs per kg

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6
Q

What is RAD/Gy used to measure?

A

radiation absorbed dose
describes patient dose
amount absorbed into the body

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7
Q

How do you convert Gy to RAD

A

multiply by 100 (move decimal two places to the right)
1 Gy = 100 RAD

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8
Q

What does Rem (Sievert) measure?

A

quantity of radiation received from all sources
used for occupational exposure
used to address the possibility of damage (dose to biological effect)

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9
Q

How to convert from rem to SV?

A

divide by 100 (move decimal two places to left)
1 rem = 0.01 Sv
100 rem = 1 Sv

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10
Q

Convert mSv to Sv

A

divide by 1000 (move decimal three places to left)
1 mSv = 1/1000 Sv

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11
Q

What unit of measure would you use for each scenario?
1) Leakage radiation from tube
2) Cumulative lifetime dose of rad tech
3) Patient wants to know amount of radiation received for a certain xray

A

1) Reontgen (R)
2) Rem (Sv)
3) Rad (Gy)

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12
Q

What is the SI unit for Curie?

A

Becquerel (Bq)

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13
Q

How do unstable atoms try to achieve stability?

A

decay and releasing excess energy in the form of electromagnetic gamma radiation and particles

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14
Q

Where and what is Curie (Ci) used for most?

A

measure radioactivity in nuclear power plants and radiation therapy
commonly used in nuclear medicine (commonly use MilliCurie/mCi)

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15
Q

Atoms are ____ dimensional

A

3

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16
Q

Can atoms be divided?

A

No, they are indivisible

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17
Q

What is the Bohr atom?

A

his theory the atom has 3 fundamental components: electrons, neutrons, protons

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18
Q

T/F An atom is very solid, with limited space for electrons to orbit.

A

False
Atoms are composed of mostly space, electron orbits are large compared to the nucleus

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19
Q

A majority of an atoms mass is the ____

A

nucleus

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20
Q

Electrons orbit the nucleus at almost the speed of ____ in fixed, precise orbits

A

light

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21
Q

T/F An electron’s mass is 1/2000 of the mass of a proton or nuetron.

A

true

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22
Q

A change in the electric charge of an atom usually is due to what?

A

gain or loss of an electron
ionization

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23
Q

The nucleus is held together by a strong force called what?

A

binding energy

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24
Q

Describe some jobs of binding energy.

A

holds together the protons and neutrons
overcomes the tendency for like charges to repel
holds the electrons in their orbits

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25
Q

What are the letter values of the electron shells?

A

Starts at K at the innermost shell and works down the alphabet

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26
Q

T/F An electron shell always fills to capacity.

A

false

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27
Q

What happens to excess electrons when a shell is filled?

A

Starts a new shell

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28
Q

Binding energy is the minimum required energy to ____ an atom

A

split

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29
Q

What is the binding energy of a tungsten atom’s K shell?

A

69.5

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30
Q

quantifies radiation intensity in air

A

Roentgen

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31
Q

quantifies occupational exposure or dose equivalent

A

REM/Sievert

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32
Q

considers the type of radiation and biological affect (whats the damage)

A

REM

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33
Q

measures Xray intensity in air

A

roengten

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34
Q

quantifies energy deposited into tissue by all types ionizing radiation

A

REM/Sievert

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35
Q

total quantity of radiation

A

RAD

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36
Q

affected by intensity of radiation, SID, time

A

RAD/gray

37
Q

classification elemental relationships based on # of protons, neutrons, electrons

A

Isos

38
Q

atoms of elements have the same # of protons (atomic number) but different # of neutrons

A

Isotope

39
Q

atoms of elements have same #of neutrons but different # of protons

A

Isotone

40
Q

atoms of elements have same # of protons and neutrons (atomic #) but different # of electrons

A

Isobar

41
Q

same atomic # and atomic mass # but vary in energy in nucleus

A

Isomer

42
Q

Which Isos is used most in rad?

A

Isotopes

43
Q

In the periodic table, periods are…

A

rows

44
Q

Each period says what about those groups of elements?

A

same number of electron shells
atoms become more complex as period increases
period # = # of electron shells

45
Q

In the periodic table, groups are arranged in…

A

columns

46
Q

The group column says what about those atoms?

A

same number of electrons in their outer shell
Group # = # of electrons in outer shell

47
Q

Atomic number is the same as the number of what?

A

protons
and electrons (stable atom)

48
Q

atomic mass number is equal to what?

A

of protons and neutrons

49
Q

A stable atom would have equal number of what?

A

Protons = electrons

50
Q

Define an element

A

simplest for of a substance that composes matter
one type of atom in an element

51
Q

Define a molecule

A

two or more atoms bonded together

52
Q

Define a chemical compound

A

combo of elements (atoms) bonded together

53
Q

Formula to determine max # of electrons a shell would hold is…

A

2n^2

54
Q

Does an electron shell always fill to capacity?

A

Not in the case of the outer shell
Inner shells fill up

55
Q

What happens if there are electrons left over if a shell is filled?

A

A new shell is formed (the outer shell) and the binding energy of that shell is distributed to the electrons to hold them in place (higher energy holding the electrons than if the shell were full)

56
Q

What are the three fundamental components of an atom?

A

electrons
neutrons
protons

57
Q

What is the electrical charge of each component of an atom?

A

electron - negative
neutron - no charge
proton - positive

58
Q

Where are the components of an atom located in the atom?

A

electron - orbit outside the nucleus
neutron - within the nucleus
proton - within the nucleus

59
Q

Describe an electrically neutral atom

A

same number of protons and electrons

60
Q

How does an atom become negative or positively charged

A

negative charge - more electrons than protons
Positive charge - more protons than electrons

61
Q

Electron shells are lettered beginning with K as the inner most shell.
Which electron shells have the most energy, the inner shell or the outer shell? Why??

A

inner shell
fewer electrons in those rings, so each one gets more energy distributed to it

62
Q

The K shell will always hold a maximum of _______ electrons.

A

2

63
Q

Two or more atoms bonded together are called…

A

molecules

64
Q

Number of protons and neutrons that are in the nucleus of an atom is the ________ (number)

A

atomic mass number

65
Q

Simplest form of a substance. Made of one type of atom. Unchanging number of protons.

A

element

66
Q

The outermost shell will always hold a maximum of ______ electrons

A

8

67
Q

What is the formula used to determine how many electrons will fit in each shell?

A

2n^2

68
Q

Combinations of elements

A

compound

69
Q

The number of protons in the nucleus

A

atomic number

70
Q

Element whose atoms have same number of protons and neutrons but different amounts of ((energy)) within nuclei

A

isom(e)r

71
Q

Element whose atoms have the same amount of ((protons)) but a different amount of neutrons.

A

isoto(p)es

72
Q

Element whose atoms have different number of protons but the same ((atomic)) number

A

isob(a)rs

73
Q

Element whose atoms have the same number of ((neutrons)) but a different number of protons

A

isoto(n)es

74
Q

The columns on the periodic table are referred to as…

A

group

75
Q

What is the same about the atoms in each column in the periodic table?

A

same number of electrons in the outer shell (valence electrons)

76
Q

The column number says what about that atom?

A

How many valence electrons it has

77
Q

The rows on the periodic table are referred to as…

A

periods

78
Q

The period number says what about that atom?

A

the number of electron shells it has

79
Q

What is the same about the atoms in each row of the periodic table?

A

same number of electron shells

80
Q

Describe the two types of bonding that takes place to form molecules…

A

ionic - attraction of opposite charges, one will lose an electron while the other gains one
covalent - two or more atoms sharing electrons

81
Q

Simplest form of a substance. Made of one type of atom. Unchanging number of protons

A

element

82
Q

number of neutrons and protons that are in the nucleus of an atom

A

mass number

83
Q

Two or more atoms bonded together

A

molecule

84
Q

combinations of elements

A

compounds

85
Q

the number of protons in the nucleus

A

atomic number

86
Q

The mass number of an element is almost always ____ (larger/smaller) than the atomic number.

A

larger

87
Q

On the periodic table, what components are typically shown on an element square and where are they located?

A

Chemical Symbol - two letters in the middle
Atomic mass number - on top or the larger number
Atomic number - on bottom or the smaller number

88
Q

T/F All compounds are considered molecules, but not all molecules are compounds

A

True
Molecule - two or more atoms
Compound - two or more of combo of different atoms

Rad Science 1 (11 decks)

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