Chapters 2, 3, and 5 Flashcards
Define Atom
- means indivisible
- the basic building block of matter
What was Bohr’s theory?
an atom consisted of 3 fundamental particles: protons, neutrons, and electrons
define nucleus
- made up of protons and neutrons
- also called nucleons
- electrons surround the nucleus in defined energy levels (shells)
define a proton
- positively charged ion
define a neutron
- neutral charged or no electrical charge
define an electron
- negatively charged ion
- surrounds/orbits the atom
- low mass
- moves at a rapid pace = lots of kinetic energy
define ionization
- losing or gaining an electron
define anion
- negative ion
- when an atom gains an electron
- have a higher negative charge
define a cation
- positive ion
- when an atom loses an electron
- has a higher positive charge
define atomic charge
- Within each atom, each proton has one unit of positive charge, each electron has one unit of negative charge, and neutrons have no charge.
- aka fundamental particles
define binding energy
- a strong nuclear force that holds the nucleus together.
- Holds the protons and neutrons together in the nucleus.
- Also a measure of the amount of energy necessary to split an atom.
what are the 2 different types of binding energy?
- Nuclear binding energy
- Electron binding energy
- both are key determinate of x-ray production
define Nuclear binding energy
- if a particle strikes the nucleus with energy equal to the nucleus’s binding energy, it could break apart
define electron binding energy
- how electrons are held in their orbits.
- This energy depends on how close the electron is to the nucleus and how many protons are in the atom.
- energy decreases with each subsequent shell
What is the inner shell called?
- K shell
- has the strongest electron binding energy (since its closer to the nucleus)
What are the names of the other shells?
- K, L, M, N, O, P, etc
how many electrons does the K shell hold?
2 electrons
What formula is used to determine how much electrons a shell can carry ?
- 2n^2
- “n” represents the number of shells
- Ex.) Shell K is 1, Shell L is 2, and so forth
define mass defect
represents the energy necessary to hold the nucleus together
What are the 2 atomic reactions in the x-ray tube that produces x-rays?
- characteristic and bremsstrahlung
define characteristic
- the removal of orbital electrons from atoms.
- depends on electron-binding energy
define Bremsstrahlung
- involves attraction to the nucleus of the atom
- depends on Nuclear binding energy
define electron shells
- a sphere around a nucleus
- defined energy levels, each at a different distance from the nucleus
how many shells can fit in the outer shells?
- 8 electrons
define atomic number
- the number of protons it contains in the nucleus
define atomic mass number
- number of protons and neutrons an atom has in the nucleus
define elements
- the simplest form of substances that compose matter
- each is made up of one unique type of atom
- Ex.) O, N, He, Fe
define molecule
- two or more atoms bonded
define chemical compounds
- combinations of elements bonded together
- H2O, CO2
define chemical symbol
- abbreviation of the element
- H is for hydrogen
when looking at an element (in the periodic table), what is the superscript that is above the chemical symbol?
- atomic mass number
when looking at an element (in the periodic table), what is the superscript that is below the chemical symbol?
- atomic number
define isotope
- elements whose atoms have the same number of protons but a different number of neutrons
define isotone
- an element with the same number of neutrons, but different number of protons
define isobar
- elements that have a a different number of protons, but the same total number of of protons and neutrons (atomic mass number)
define isomer
- elements with the same number of protons and neutrons but with different amounts of energy within their nuclei
what would be an example of isotopes?
1/1 H and 2/1 H
what would be an example of isotones?
131/23 I and 132/54 Xe
what would be an example of isobar?
7/3 Li and 7/4 Be
what would be an example of an isomer?
99m Tc
define the periodic table
- a table that consists of multiple elements
- consists of periods and columns
- all are different types of metals
what is a period on a periodic table?
- top to bottom
- same number of electron shells
- increases as you move from top to bottom
- become larger and more complex
what is a group on a periodic table?
- left to right
- same number of electrons in the outer shell
- amount increases as you move from left to right
define compound
- a molecule that contains at least two different elements
define ionic bonding
- attraction of opposite charges
- one of the atoms gives up an electron and the other takes the extra electron
- the difference in their electrical charge attracts and bonds the two together
define covalent bonding
- two atoms sharing electrons
- outermost electron from one atom begins to orbit the nucleus of another adjacent atom
What does the size of an atom determine?
- the more large and complex an atom is, they have a higher chance for interactions
- the smaller and simple an atom is, they have a lesser chance of interaction
define an alpha particle
- made up of 2 protons and 2 neutrons
- have a positive charge
- How many protons does 131/53 I have?
a. 131
b. 53
c. 78
d. 184
b. 53
- How many nucleons are in (39/19 K)?
a. 39
b. 19
c. 20
d. 58
a. 39
- 132/54 Xe and 131/53 I are:
a. isomers.
b. isotopes.
c. isobars.
d. Isotones.
d. Isotones.
- 130/53 I and 131/53 I are:
a. isotopes.
b. isobars.
c. isotones.
d. Isomers.
a. isotopes.
- What is the maximum number of electrons that will occupy the outermost shell of an atom?
a. 2
b. 8
c. 18
d. 32
b. 8
- The maximum number of electrons that can occupy the P shell is:
a. 8.
b. 32.
c. 72.
d. 98.
c. 72.
- Atoms that bind together because of their opposite charges form:
a. covalent bonds.
b. convalescent bonds.
c. ionic bonds.
d. nonionic bonds.
c. ionic bonds.
- The horizontal periods of the periodic table contain elements with:
a. the same number of electron shells.
b. the same number of electrons.
c. the same chemical properties.
d. the same number of protons.
a. the same number of electron shells.
- Which of the following is considered a nucleon?
a. proton
b. electron
c. alpha particle
d. beta particle
a. proton
- What is the maximum number of electrons permitted in the M shell?
a. 8
b. 18
c. 32
d. 50
b. 18
define electromagnetic radiation
- no mass
- carries energy in waves as electric and magnetic disturbances in space
- travels in the speed of light (3 x 10^8)
define the electromagnetic spectrum
- ordering or grouping the different electromagnetic radiations
- all waves have the same velocity ( 3 x 10^8)
- vary on energy, wavelength, and frequency
What is are the levels of the electromagnetic spectrum from lowest energy to greatest?
- Radiowaves
- Microwaves
- Infrared light
- visible light
- ultraviolet light
- x-rays
- gamma rays
define the nature of electromagnetic radiation
- electric and magnetic disturbances traveling through space
- They all have the same velocity (3 x 10^8)
- vary only in their energy, wavelength, and frequency
What is the wavelength (m) and frequency (HZ) for radiowaves?
Wavelength (m): >1 x 10^-1
Frequency (Hz): >3 x 10^9
What is the wavelength (m) and frequency (HZ) for microwaves?
Wavelength (m): 1 x 10^-1 - 1 x 10^-3
Frequency (Hz): 3 x 10^9 - 3 x 10^11
What is the wavelength (m) and frequency (HZ) for Infrared Light (IR)?
Wavelength (m): 1 x 10^-3 - 7 x 10^-7
Frequency (Hz): 3 x 10^11 - 4 x 10^14
What is the wavelength (m) and frequency (HZ) for Visible light?
Wavelength (m): 7 x 10^-7 - 4 x 10^-7
Frequency (Hz): 4 x 10^14 - 8 x 10^14
What is the wavelength (m) and frequency (HZ) for Ultraviolet?
Wavelength (m): 4 x 10^-7 - 1 x 10^-8
Frequency (Hz): 8 x 10^14 - 3 x 10^17
What is the wavelength (m) and frequency (HZ) for X-rays?
Wavelength (m): 1 x 10^-8 - 1 x 10^-13
Frequency (Hz): 3 x 10^17 - 3 x 10^19
What is the wavelength (m) and frequency (HZ) for Gamma rays?
Wavelength (m): <10^-11
Frequency (Hz): >3 x 10^17
define electromagnetic radiation
- form of energy that originates from the atom
- emitted when changes in atoms occur
- can exist apart from matter and can travel through a vacuum
- it’s pure energy
- does not require a medium to travel
what is the formula when calculating electromagnetic radiation?
- E=hf
- E is energy
- h is Planck’s constant
- f is frequency
what’s the difference between an electromagnetic radiation vs. a mechanical radiation?
- electromagnetic does not need a medium to travel
- mechanical requires a medium in order to travel to other locations
define amplitude
- maximum height of a wave
define wavelength
- measure of the distance from the peak of one wave to the other
define frequency
- number of waves that pass a given point per second
what is the relationship between wavelength and frequency?
- inverse
- the longer the wavelength, the shorter the frequency
what is the unit to measure frequency?
- Hertz
- One hertz is defined as one cycle per second
What is the formula to calculate wavelength and frequency?
- c = fλ
- C is the constant of speed of light (3 x 10^8)
- f is frequency
- λ is wavelength
how can electromagnetic radiation be characterized when it interacts with matter?
- if its a high energy photon (x-rays and gamma rays), it’s characterized as a particle
- if its a low energy photon (radiowaves and microwaves) it’s characterized as a wave
define inverse square law in radiation
- the intensity of radiation diminishes by the square of the distance from the source
- used to calculate the change in the intensity (quantity) of radiation reaching the image receptor with changes in distance.
define wave particle duality
- how electromagnetic radiation exhibits properties of both a particle and a wave, depending on its energy and environment.
What are the characteristics of x-rays and gamma rays?
- highest-energy members of the electromagnetic spectrum
- can burn the skin
- the ability to ionize matter
- dangerous in general and harmful to the patient if misused
- can damage molecules and deoxyribonucleic acid (DNA) and cause chemical changes in cells
What’s the difference between an x-ray and a gamma ray?
- source of energy
Where do gamma rays originate?
- nuclei of atoms
where do x-rays originate?
- interactions between electrons and atoms
define Radiowaves
- low end of the energy spectrum
- commonly used in MRI
- radiowaves do not ionize atoms.
define microwaves
- transmit cell phone signals and heat food.
- do not ionize atoms
define infrared light
- low-energy, electromagnetic radiation just above microwaves
- “beam” information between electronic devices
- Ex.) TV remote to a TV
- infrared light does not ionize atoms
define visible light
- represents the colors visible to the human eye
- visible light does not ionize atoms
- White light consists of all of the colors of the visible spectrum together
- The color black represents absorption of all of the color wavelengths
define ultraviolet
- causes darkening of the skin
- Ultraviolet light can be harmful
- causes skin cancer (by the activation of melanocytes)
- does not ionize the atoms
define x-rays
- used in medical imaging
- used in radiation therapy
- can ionize atoms
define gamma rays
- used in medicine imaging
- used in radiation therapy
- can ionize atoms
how are alpha/ beta particles similar to x-rays and gamma rays?
- they have the energy to ionize matter.
define particulate radiation
- physical particles originating from radioactive atoms with the ability to ionize matter
- alpha particles
- beta particles
define radioactivity
- process by which an atom with excess energy in its nucleus emits particles and energy to regain stability
define radioactive
- Elements that are composed of atoms with unstable nuclei
define radioactive decay
- process of a radioactive element giving off excess energy and particles to regain stability
define half-life
- the rate at which a radioactive substance decays
- length of time it takes for half the remaining atoms in a quantity of a particular radioactive element to decay
- used to measure radioactivity