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Radiology > The Structure of Matter > Flashcards

The Structure of Matter Flashcards

0
Q

The first group of people who recorded reference to the investigation of the structure of matter. They also thought that matter was composed of four substances : earth,water, air and fire

A

Greek - called greek atoms

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1
Q

It is the building block of the radiogrpaher’s understanding of the interaction between ionizing radiation and matter

A

Atom

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2
Q

What are the four basic essences when the combination of the four substances happen according to greek atom?

A

Wet
Dry
Hot
Cold

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3
Q

Where was the word atom originated?

A

Greek

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4
Q

atom in scientific explanation

A

Indivisible

A(not) + temon (cut) = cannot be cut (smallest)

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5
Q

How many substances or elements have been identified today? How many are naturally occuring and artificially producedL

A

112
92 - naturally occuring
20 - artificially produced

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6
Q

It is the smallest particle of matter that has the properties of an element

A

Atom

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7
Q

Particles that are much smaller that the atom

A

Subatomic particles

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8
Q

He showed that the elements should be classified according to integral value of the atomic mass

A

John Dalton, 1808

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9
Q

What is John Dalton’s physical combination of one type of atom with another called?

A

Eye-and-hook affair

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10
Q

According to him an element was composed of identical atoms that reacted the same way chemically. E.g. All oxygen atoms were alike

A

John Dalton

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11
Q

Eye-and-hook affair is explained by

A

John Dalton

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12
Q

Who invented the first periodic table of elements?

A

Dmitri Mendeleev

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13
Q

He showed that if the elements were arrenged in order of increasing atomic mass, a periodic reptition of similar chemical properties occured

A

Dmitri Mendeleev

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14
Q

During the time of Dmitri Mendeleev, how many elements had beed identified?

A

65

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16
Q

The subscript in each of the element in the periodic table is the _______ ________

A

Atomic number

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16
Q

True/False - all elements in the same group react chemically in a different fashion and have similar phisycal properties.

A

False

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17
Q

The superscript in each element in the periodic table is the _________ ____

A

Elemental mass

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18
Q

What do we call the group I in the periodic table of elements?

A

Alkali metals

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19
Q

The group VII in the periodic table of elements are called _______

A

Halogens

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20
Q

They are soft metals that combine readily with oxygen and react violently with water

A

Alkali metals - Group I

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21
Q

They are the group in the periodic table of elements which are easily vaporized and combine with metals to form water-soluble salts

A

Group VII - halogens

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22
Q

The group VIII elements in the periodic table is called

A

Noble gases

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23
Q

The group in the periodic table that are highly resistant to reaction with other metals

A

Noble gases - Group VIII

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24
Q

He described the atom as looking someting like a plum pudding

A

J.J Thomson

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25
Q

He concluded that electrons were integral part of all atoms

A

J.J. Thomson

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26
Q

The plum in the plum pudding theory by J.J Thomson represents the

A

Negative electric charges - electrons

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27
Q

The pudding in the plum pudding theory of J.J. Thomson is the

A

Shapeless mass of uniform positive electrification

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29
Q

True/false - the number of electrons was thought to be equal to the quantity of postitive electrification because the atom was known to be electrically neutral

A

True

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30
Q

He introduced the nuclear model of atom and disproved the Thomson’s model of atom

A

Ernest Rutherford, 1911

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31
Q

This model of atom described the atom as containing small, dense, positively charged center surrounded by a negative cloud of electrons

A

Nuclear model of atom

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31
Q

He states that “the number of electrons was thought to equal the quantity of postitive electrification because the atom was known to be electrically neutral”

A

J.J. Thomson

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32
Q

Who called the center of the atom the nucleus?

A

Ernest Rutherford

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34
Q

He improved Rutherford’s description of the atom and His model was a miniature solar system

A

Niels Bohr, 1913

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35
Q

The model of atom in which it describes that the electrons revolved about the nucleus in prescribed orbits of energy levels

A

Miniature solar system model

35
Q

The equipment used to mapped and identify the structure of the atomic nucleus

A

High-energy particle accelerators or atom smashers

36
Q

The atomic model after Bohr’s model, “atoms contains a small,dense, positively charged nucleus surruonded by negatively charged electrons that revolve in fixed, well-defined orbits about the nucleus”

A

Quantum Chromodynamics (QCD)

37
Q

The nucleus is also called

A

Nucleons

38
Q

The nucleons are composes of

A

Proton and neutron

39
Q

Protons and neutrons are held together by

A

Gluons

40
Q

What are the fundamental particles or the three primary constituents of an atom?

A

Electron
Proton
Neutron

42
Q

The atomic model in which the sun is nucleus and the planets are the electrons

A

Miniature solar system model

43
Q

A very small particles that carry one unit of negative electric charge

A

Electron

44
Q

What is the mass of an electron?

A

9.1 x 10^-11 kg

45
Q

One atomic mass unit is equal to

A

One half the mass of a carbon 12 atom

46
Q

The electron mass is equal to how many amu?

A

0.000549 amu

47
Q

Atomic mass number of electron is

A

Zero

48
Q

The mass of a proton is

A

1.673 x 10^-27 kg

48
Q

The atomic mass number of proton and neutron is

A

One

49
Q

The mass of the neutron is

A

1.675 x 10^-27 kg

50
Q

It carries one unit of postive electric charge

A

Proton

51
Q

A fundamental particle that is very small but contains nearly all the mass of the atom

A

Neutron

52
Q

It carries no charge; it is electricall neutral

A

Neutron

53
Q

The atom is essentially ______ ______

A

Empty space

54
Q

electron orbits are grouped into different _____

A

Shells

55
Q

It determines the chemical behavior of an atom

A

Number of protons

56
Q

The chemical element is determined by the

A

Number of protons

57
Q

Atoms that have the same number of protons but differ in the number of electrons

A

Isotopes

58
Q

Electrons can exist only in certain shells, which represent different _______ ________ ________

A

Electron binding energies

59
Q

Electron binding energies are also called

A

Energy levels

60
Q

The elecron orbital shells are given the codes of

A

K,L,M,N and so forth , it represent the relative binding energies of electrons from closest to the nucleus to farthest from nucleus

61
Q

True/False - the closer and electron is to the nucleus, the lesser is its binding energy

A

False

62
Q

In their normal state, atoms are electrically _______; the electric charge on the atom is zero.

A

Neutral

63
Q

The most complex naturally occuring element

A

Uranimum

64
Q

True/false - the total number of electrons in the orbital shells is equal to the number of protons in the nucleus

A

True

65
Q

If an atom has an extra electron or has had an electron removed, it is said to be _________

A

Ionized

66
Q

True/False - am ionized atom is not electrically neutral but carries a charge equal in magnitude to the difference between the numbers of eletrons and protons

A

True

67
Q

True/False - atoms can be ionized by the addition or subtraction of protons/false

A

False - cannot -

Proton - because they are bound very strongly together
Neutron - because they are electrically neutral

68
Q

After the electron is removed from an atom due to ionization the remaining atom is called a

A

Positive ion - contains one more positive charge than negative charge

69
Q

How many eV is required to remove an electron from an atom in a tissue?

A

34 eV

70
Q

It is the removal of an orbital electron from an atom

A

Ionization

71
Q

True/False - in all except the ligthest atoms, the number of neutrons is always greater than the number of protons

A

True

Large atom = abundance of neutrons over protons

72
Q

True/False - the maximum number of electrons that can exist in each shell decreases with the distance of the shell from the nucleus

A

False - increases

73
Q

The formula for calculating the maximum electrons per shell

A

2n^2

N = shell number or principal quantum number

74
Q

The number of electrons in the outermost shell of an atom is equal to its ______ in the periodic table

A

Group -

it is also determines the valence of an atom

75
Q

The number of outermost electrons shell of an atom is equal to ______ in the periodic table

A

Period

76
Q

True/False - no outer shell can contain more than eight electrons

A

True

77
Q

The atoms associated with the phenomenon of that instead adding electrons to next outer shell, electrons are added to an inner shell

A

Transitional elements

78
Q

It indicates the relative energy by which the electron is attached to the nucleus

A

Electron shells

79
Q

True/false - centripetal force is based on the basic law of electricty that sates that “opposite charges attract one another and like charges repel”

A

True

80
Q

The force that keeps an electron in orbit is the

A

Centripetal force/center-seeking force

81
Q

The strength of attachment of an electron to nucleus i ps called the _______ _______ _______

A

Electron binding energy

82
Q

The force that balances with centripetal force and maintain the distance of the electrons from the nucleus while traveling in a circular or elliptical path

A

Centrifugal force or flying-put-from-the-center force

84
Q

True/false - the closer an electron is to the nucleus, the more tightlty it is bound. So therefore K-shell have higher binding energies than other shell

A

True

85
Q

True/False - the greater the total number of electrons in an atom, the more tightly each is bound

A

True

Radiology (2 decks)

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