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rad 325 physics test 2
test 2 review
88
Physics
Graduate
11/29/2009

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Term
Velocity =
Definition
v= d/t
Term
 Four systems of units for base quantities
Definition
SI, MKS, CGS, and BRITISH
Term
Average velocity =
Definition
v avg= Vf + Vo / 2
Term
Acceleration =
Definition
a= Vf - Vo /t
Term
If velocity is constant, acceleration is
Definition
zero
Term
acceleration is the rate of change of velocity with
Definition
time.
Term
the unit for velocity is
Definition
m/s
Term
a body will remain at rest or will continue to move with constant velocity in a strait line unless acted upon by an external force (what law of newtons law of motion?)
Definition
1st law (inertia)
Term
the force that acts upon an object is equal to the mass x acceleration produced
Definition
2nd law of motion (force)
Term
for every action, there is an equal and opposite reaction.
Definition
3rd law of motion (action/reaction)
Term
force F= ?
Definition
mass x acceleration
m x a
Term
Units for Force
Definition
Newtons
Term
Weight is a force on a body caused by
Definition
pull of gravity upon it.
Term
weight is the product of
Definition
mass and the acceleration of gravity on earth
Term
Weight w = ?
Definition
m x g
mass of object x acceleration due to gravity
Term
momentum is the product o
Definition
mass and velocity
Term
the total momentum before any interaction is equal to
Definition
the total momentum after the interaction
Term
momentum 'p' =
Definition
mass x velocity
Term
units for p momentum
Definition
kg.m/s
Term
work is the product of ...
the unit is...
Definition
force and distance
(J) joule
Term
Work W =
Definition
f x d
Term
power is the rate of
Definition
doing work
Term
the SI unit of power is
the british unit of power is
Definition
joule/second J/s or watt (W)
horsepower hp
Term
power p= ?
Definition
work/time w/t
Term
Energy is the ability to do
Definition
work
Term
the unit of energy is
Definition
J joule
Term
the energy of an object in motion
Definition
kinetic energy
Term
energy stored in position of configuration
Definition
potential energy
Term
KE =
Definition
(1/2)mv^2
Term
PE =
Definition
mgh
mass, accel. from gravity, distance above earths surface
Term
units of exposure in air
trad. and SI
Definition
Trad. roentgen
SI coloums/kg
Term
absorbed dose
trad. and SI
Definition
trad. RAD
SI Gray
Term
occupational/public dose (equiv. dose)
trad. and SI
Definition
REM= trad.
SI= Sievert
Term
Radioactivity units
trad. and SI
Definition
trad. curie
si = bq
Term
pressure is measure by a
Definition
barometer
Term
pressure is quoted in units of (2) ?
Definition
mmHg or cmHg
Term
NTP
Definition
normal temperature and pressure
0 degrees celcius and 76 cmHg
Term
3 things can vary in dealing with gas laws
Definition
volume pressure and temp
Term
chemicals that cannot be broken down into simpler chemical forms
Definition
elements
Term
the results of two or more elements linked together chemically
Definition
compound
Term
the smallest part of an element that can exist and still retain the chemical properties of that element
Definition
atom
Term
the smallest part of a compound that still retains the chemical properties of that compound. number of atoms linked together
Definition
molecule
Term
Rutherford described the nuclear model
Definition
small dense positive center surrounded by negative electrons
Term
bohr later improved the nuclear model. idea of
Definition
electrons at different energy levels
Term
at center of the atom is the nucleus. contains
Definition
protons and nuetrons
Term
the proton has ___ charge
neutron has ___ Charge
Definition
proton +
neutron is neutral no charge
Term
electrons have ___ charge
Definition
negative e-
Term
what holds the electrons in their energy levels
Definition
the electric force of attractions between the electrons and the positive nucleus
Term
atomic number is the
Definition
number of protons (also the number of electrons)
Term
what determines the chemical properties?
Definition
# of protons
# of nuetrons does not
Term
what would varying the number of neutrons do
Definition
change the mass of the element
Term
atomic number represented by
Definition
z (subscript)
Term
atomic mass represented by
Definition
a (superscript)
Term
the different electron shells represent different levels of
Definition
potential energy
Term
the further a shell is from the nucleus,
Definition
the greater its PE
Term
energy levels are represented by
Definition
K, l , m , n , o ....
Term
2n^2 gives you ...
Definition
electron limit ( n is the shell number )
Term
the strength of attachment of an electron to the nucleus is called
Definition
the binding energy
Term
the closer the electron is to the nucleus, the
Definition
more tightly it is bound
Term
the further away an electron is to the nucleus...
Definition
higher the PE lower the binding energy
Term
all matter is made up of
Definition
elements and compounds
Term
______ is the smallest part of an element
Definition
atom
Term
_________ is the smallest part of a compound
Definition
Term
the energy needed to release an electron is the same as
Definition
the binding energy
Term
when atoms have the same atomic number but different mass number
Definition
isotope
Term
results when changed number of neutrons
Definition
isotope
Term
unstable nuclei of radioactive isotopes will try to return to a stable state by
Definition
emitting beta particles and gamma rays
Term
when atoms of different elements have the same mass number, but still a different atomic number
Definition
isobar
Term
when was radioactivity first discovored?
Definition
by HENRI BECQUEREL in 1896
Term
a phenomenon in which radiation is given off by the nuclei of the element
Definition
radioactivity
Term
nuclides eventually break up and emit particles and/or radiation energy from their nuclei = this is radioactivity and the unstable isotopes are called
Definition
radionuclides
Term
_____________ have been usd as radiation therapy sources, but are also used in nuclear medicine
Definition
radionuclides
Term
radioactivity is a ____ process
Definition
nuclear; it does not involve the orbital electrons; thus is not influenced by chemical changes nor by variations in env.
Term
protons have like charges and would normally
Definition
repel each other and break up the nucleus
Term
some nuclide's, especially ones with high atomic numbers are ....no matter how many neutrons are present.
Definition
unstable
Term
uranium, with an atomic number of 92, has no...
Definition
stable isotope
Term

after disintegration, a new nuclide is formed which may or may not be stable... known as

Definition
daughter products
Term
examples of the many unstable isotopes that occur naturally are...
Definition
uranium and radium
Term
radioisotopes can be man-made in nuclear reactors and particle accelerators such as
Definition
Sr-90 and Co-60
Term
the common way in which isotopes can be produced is by altering the number of
Definition
neutrons in the nucleus
Term
isotopes can otherwise be produced by bombarding atoms with high speed...
Definition
protons, deuterons, and alpha particles
Term
what are the four modes of radioactive decay?
Definition

alpha particle 

beta particle

electron capture

gamma emission and internal conversion

Term
the emission of an alpha particle is associated with the breakdown of ____________ such as uranium and radium
Definition
heavy elements
Term
the process of radioactive decay which is accompanied by the ejection of a 
Definition
positive or negative electron from thenucleus
Term
___________ and __________ do not exist in the nucleus, but are created at the instant of the decay process
Definition
positrons and negatrons
Term
phenomenon in which one of the orbital electrons is captured by the nucleus and so transforms a proton into a neutron
Definition
electron capture
Term
besides gamma emission, a nucleus can also lose energy by _______
Definition
internal conversion ... process in which the excess energy is passed on to one of the orbiting electrons, which is then ejected.
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