Intro to Medical Radiography - Exam 1

Radio waves, light, and x-rays are all examples of _________ energy.

 

thermal

 

electromagnetic

 

electrical

 

nuclear

electromagnetic

What is the removal of an electron from an atom called?

 

Pair production

 

Ionization

 

Electricity

 

Irradiation

Ionization

The biggest source of man-made ionizing radiation exposure to the public is ______________.

 

nuclear power plants

 

atomic fallout

 

smoke detectors

 

diagnostic x-rays

diagnostic X-rays

Ionizing radiation is capable of removing ____________ from atoms as it passes through the matter.

 

neutrons

 

ions

 

electrons

 

protons

electrons

Today, radiology is considered to be a(n) ___________ occupation.

 

high-risk

 

safe

 

dangerous

 

unsafe

safe

What does ALARA mean?

 

All Level Alert Radiation Accident

 

As Low As Reasonably Achievable

 

As Low As Regulations Allow

 

Always Leave A Restricted Area

As Low As Reasonably Achievable

Filtration is used to ____________________.

 

absorb low-energy x-rays

 

remove high-energy x-rays

 

fabricate gonadal shields

 

restrict the useful beam to the body part imaged

absorb low-energy x-rays

___________ is a special quantity of radiologic science.

 

Mass

 

Velocity

 

Radioactivity

 

Momentum

Radioactivity

A moving object has ____________ energy

 

nuclear

 

potential

 

kinetic

 

electromagnetic

kinetic

In a neutral atom, the atomic number does NOT indicate the number of:

protons.

electrons.

neutrons.

neutrons.

The L shell can hold _______ electrons.

8

4

2

1

8

The simplest form of the substances that form matter is the:

compound.

atomic mass number.

atomic number.

element.

element.

The number of protons and neutrons in the atom’s nucleus is the:

atomic mass number.

element.

atomic number.

compound.

atomic mass number

The electron shell closest to the nucleus is lettered

“M”.

“K”.

“H”.

“E”.

“K”

Two or more atoms that bond together form a(n)

atomic mass number.

atomic number.

compound.

element.

compound

Except for the K shell, the maximum number of electrons that can be in the outermost shell of an atom is

32.

8.

4.

16.

8

The number of protons in an atom’s nucleus is reflected in its

atomic number.

element.

atomic mass number.

compound.

atomic number

If an atom has 15 electrons, which will be the outermost shell?

“M”

“L”

“N”

“O”

M

The N shell can hold _______ electrons.

64

8

4

32

32

The force that holds the protons and neutrons together in the nucleus is the

proton/neutron energy.

electron binding energy.

atomic energy.

nuclear binding energy.

nuclear binding energy.

If an atom has the same number of electrons and protons it will

have a negative charge.

be electrically neutral.

none of these.

have a positive charge.

be electrically neutral

A negative ion is

an atom with more electrons than protons.

an electron.

an atom with more neutrons that electrons.

an atom with more protons than electrons.

an atom with more electrons than protons

When an atom becomes negatively or positively charged it is usually due to a change in the number of

protons.

all of these.

neutrons.

electrons.

electrons

The electron binding energy is stronger when:

there are more protons and the electron is farther from the nucleus.

there are more protons and the electron is closer to the nucleus.

there are fewer protons and the electron is farther from the nucleus.

there are fewer protons and the electron is closer to the nucleus.

there are more protons and the electron is closer to the nucleus.

The electrons stay in orbit around the nucleus because of:

their attraction to the neutrons.

their attraction to the protons.

their attraction to the other electrons.

all of these.

their attraction to the protons.

A positive ion is:

an atom with more protons than electrons.

an atom with more neutrons that electrons.

an atom with more electrons than protons.

a proton.

an atom with more protons than electrons.

If an atom has more electrons than protons, it will:

have neither a positive nor negative charge.

be electrically neutral.

have a positive charge.

have a negative charge.

have a negative charge.

The electron binding energy does NOT depend on:

how close it is to the nucleus.

how many protons there are in the nucleus.

how many neutrons there are in the nucleus.

how many neutrons there are in the nucleus.

If a particle strikes a nucleus with the same amount of energy as the atom’s nuclear binding energy:

the atom will become a positive ion.

it can fuse the atom.

the atom will become a negative ion.

it can split the atom.

it can split the atom.

The fundamental component of the atom that has the smallest mass is the

none of these.

neutron.

proton.

electron.

electron

If an atom has more protons than electrons, it will

have neither a positive nor negative charge.

have a negative charge.

be electrically neutral.

have a positive charge.

have a positive charge

The most commonly known modern atomic theory was developed by

Thomson.

Bohr.

Rutherford.

Dalton.

Bohr

The atomic nucleus contains:

electrons and neutrons.

all of these.

protons and electrons.

protons and neutrons.

protons and neutrons

The earliest atomic theory based on an arrangement similar to the solar system is attributed to:

Dalton.

Rutherford.

Bohr.

Thomson.

Rutherford

The mass of an atom is primarily due to the mass of the:

nucleus.

electrons.

neutrons.

protons.

nucleus

The component of the nucleus that has mass but no electrical charge is the:

proton.

none of these.

electron.

neutron.

neutron

The component of the nucleus that has a positive charge and mass is the:

none of these.

proton.

electron.

neutron.

proton

The three fundamental particles of the atom are the:

electron, nucleus, and proton.

neutron, electron, and proton.

element, nucleus, and electron.

nucleus, proton, and neutron.

neutron, electron, and proton.

The “plum pudding model” is associated with:

Rutherford.

Thomson.

Bohr.

Dalton.

Thomson

Define the following terms and provide with examples to support your discussion.

• Isotopes

• Isobars

• Isomers

• Isotones

Isotones are elements with the same number of neutrons. 

Isotopes are elements with the same number of protons. 

Isomers are elements with the same mass, atomic number, and everything except for their metastate is the same.

Isobars are elements with the same Atomic Mass Number. 

2 and 3

The word atom is derived from the Greek word atomos, meaning:

nuclear.

indivisible.

invisible.

small.

indivisible

2 and 5

Of the following fundamental particles, which two have approximately the same mass?

neutron and electron

electron and proton

proton and photon

neutron and proton

neutron and proton

In the early 1800s English chemist John Dalton theorized that:

atoms are unique to each element in size and mass.

elements form compounds.

a chemical reaction results from atoms being rearranged.

all of these.

all of these

129

Discovery of the electron is attributed to:

Bohr.

Rutherford.

Thomson.

Dalton.

Thomson.

Of the following radiations, the most penetrating should be a:

2.5 MeV beta particle

5.0 MeV alpha particle

12.0 MeV electron beam

100 KeV gamma ray

100 KeV gamma ray

An ionic bond results in an electrically charged molecule or compound.

False

True

False

Elements can only occur naturally.

False

True

False

The electrons rotate around the nucleus at a single energy level.

False

True

False

All compounds are molecules and all molecules are compounds.

False

True

false

Electron shells are the hard coating around the electron.

False

True

False

The outermost shell of an atom can hold fewer than 8 electrons.

False

True

True

In the middle of the periodic table of elements there are elements that don’t fit exactly into one of the eight groups.

False

True

True

Each element has an unchanging number of protons.

False

True

True

Each electron shell has a specific limit to the amounts of electrons it can hold.

False

True

True

The atoms of the elements at the top of the periodic table of elements are the most complex.

False

True

False

Atoms with the same atomic number and atomic mass number but have different energy within their nuclei are

isotones.

isomers.

isotopes.

isobars.

isomers

The periodic table of elements classifies by period and group. The group is the:

period.

row.

type of element.

column.

column

Atoms in each period have the same number of

electron shells.

electrons in the outermost shell.

electrons.

atomic mass number.

electron shells.

A compound consists of

all of these.

at least two different materials.

at least two elements.

at least two molecules.

at least two elements

The periodic table of elements classifies by period and group. The period is the

row.

group.

column.

type of element.

row

²³₁₁Na is an _______________ of ²²₁₁Na.

isobars

isotopes

isotones

isomers

isotopes

When the bond between two atoms is due to one atom giving up an electron and the other atom gaining an electron, it is called a

ionic bond.

compounding bond.

molecular bond.

covalent bond.

ionic bond

⁷₃Li and ⁷₄Be are

isomers.

isotopes.

isobars.

isotones.

isobars

¹³¹₅₃I and ¹³²₅₄Xe are

isotones.

isobars.

isomers.

isotopes.

isotones

Atoms in each group have the same number of

electron shells.

atomic mass number.

electrons.

electrons in the outermost shell.

electrons in the outermost shell.