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Chem/Physics- Hannah > Chem final > Flashcards

Chem final Flashcards

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1
Q

Farenheit to Celcius

A

C= (F-32) x 5/9

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2
Q

Celcius to Farenheit

A

F= (C x 9/5) + 32

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3
Q

Force equation

A

force= mass x acceleration

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4
Q

Avogadro’s number

A

1 mole= 6.022 x 10^23

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5
Q

What is an atom?

A

it is the smallest unit of an element that still maintains the characteristics of the element (electron, proton, neutrons)

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6
Q

What is a molecule?

A

2 or more atoms that are chemically joined together; smallest unit that retains the physical and chemical properties of the substance (H2O, N2, O2)

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7
Q

What is an element?

A

a substance that cannot be separated into a smaller substance by chemical means; pure! examples include oxygen, nitrogen, and carbon

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8
Q

What is a compound?

A

contains atoms of different compounds chemically bound together in a fixed ratio; a molecule that contains at least two different elements

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9
Q

What is a physical change?

A

a simple change of state of matter (solid to liquid to gas)

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10
Q

What is a chemical change?

A

a change in the composition of matter, atoms, or molecules of 2 or more substances rearrange to form 2 or more new substances having different properties

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11
Q

Understand the relationship between gravity, mass, and weight.

A

Mass: a given quantity of matter in an object
Weight: the force acting on matter determines the weight
in space, we would have the same mass but we would be weightless because there is no gravity acting on matter in space

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12
Q

What is the difference between adhesive and cohesive forces?

A

adhesive: like to unlike molecules; water will climb up the sides of glass
Cohesive: like to like molecules; molecules exhibit a force of mutual attraction; water will attract towards itself and away from the glass in a beaker

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13
Q

What is the octect rule?

A

there will always try to be 8 molecules that exist in the outer shell

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14
Q

Describe covalent and ionic bonding.

A

covalent bonding is the sharing of electrons; it is the strongest bond type
ionic is the donation or acceptance of electrons to another molecule or compound

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15
Q

How much volume does 1 mole of gas occupy at STP?

A

22.4 L

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16
Q

The chemical properties of water that make it a good solvent for polar compounds

A

less dense in it’s solid state (when frozen), dipole, universal solvent, high BP/MP, latent heat and heat of vaporization, water dissociates into H+ and OH- which contributes to acid base balance
Electrons spend more time orbiting 0 than H. Dipoles exist when atoms of different electronegativities are bonded together. The solute in water with a charge will be attracted to the dipole of the water molecule. If something is not charged, it will not be attracted to the water and will not easily be “surrounded” by the water. Since oxygen has a higher electronegativity than hydrogen, the side of the molecule with the oxygen atom has a partial negative charge. A molecule with such a charge difference is called a dipole

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17
Q

Know how the subatomic particles contribute to mass

A

protons and neutrons (approx 1 amu) are really the only subatomic particles that contribute to mass since electrons have an insignificant mass

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18
Q

What is an isotope?

A

an isotope is an element that has the same number of protons but a different number of neutrons

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19
Q

What is nuclear radiation?

A

Ionizing radiation happens when an unstable atom (a radioactive isotope of an element) emits particles or waves of particles to become more stable. This process is called radioactive decay.

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20
Q

How does pK relate to onset time of an anesthetic?

A

the more unionized a drug is, the quicker the onset

is is the primary determinant of onset time

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21
Q

How does the unionized form of an anesthetic contribute to creating a conduction block?

A

it is the unprotonated, uncharged, base (B)- diffuses more easily through the nerve sheath, is required for diffusion into neuron; reflected clinically as onset of anesthesia

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22
Q

How does the ionized form of an anesthetic contribute to creating a conduction block?

A

binds to receptor site on the inside of cell membrane, responsible for suppression of the action potential; reflected clinically by the profoundness of the block

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23
Q

What are the determinants of blood pH?

A

strong ion difference, weak acids, pCO2, and dissociation of water

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24
Q

Hydrogen bonding

A

a special dipole-dipole where H binds to N, O, or F of another molecule

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25
Q

LDF bonding or Van der Waals

A

momentary attractions, not even official bonding; the longer the chain, the more likely LDFs will form

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26
Q

Dipole-dipole

A

when charged end of one molecule is attracted to the negative end of another molecule

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27
Q

What is an acid?

A

an acid (pitcher) is an electron donor

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28
Q

What is a base?

A

a base (catcher) is an electron acceptor

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29
Q

What is the difference between weak acids and strong acids?

A

with weak acids the equation can be reversed (goes in both directions)
With strong acids the equation can only go one way; it completely dissociates

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30
Q

Examples of weak acids include:

A

Hprotein, carbonic acid, phosphoric acid

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31
Q

Comment on the ionization and other properties of a protonated acid.

A

protonated, unionized, liphophillic, crosses membrane, active, hydrophobic

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32
Q

Comment on the ionization and other properties of a protonated base.

A

protonated, ionized, hydrophillic, will not cross membranes, inactive, liphophobic

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33
Q

The onset of an anesthetic is determined by

A

the pK, the more unionized a drug is, the faster the onset time

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34
Q

How are the ionized and unionized form of a local anesthetic involved in the process of producing a conduction block?

A

unionized- onset time

ionized- reflected by the profoundness of the block

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35
Q

What is the CO2 hydration reaction?

A

CO2+ H2o H2CO3 HCO3- + H+

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36
Q

The determinants of blood pH are:

A

strong ion difference, weak acids, pCO2, and dissociation of water

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37
Q

Weak acid buffers include:

A

hemoglobin, proteins, and phosphate

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38
Q

Strong acids include

A

lactate, keto acids, and sulfate

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39
Q

Force equation

A

force= mass x acceleration
kg x m/s^2
measured in Newtons or Dynes

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40
Q

Work equation

A

work= force x distance
kg x m^2/s^2
Result is Joules

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41
Q

Potential energy equation

A

Potential energy= height x gravity x mass
m x 9.8 m/s2 x kg
Result is Joules

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42
Q

Power equation

A

Power= work/time

Joules/sec. (WATTS!)

43
Q

Absolute 0’s for Kelvin, celcius, and farenheit

A

Kelvin: 0
Celcius: -273
Far: -459

44
Q

Reynold’s number equation

A

velocity x density x diameter/viscosity

45
Q

When gas is turbulent, this is determinant of flow

A

density
it influences the probability that interactions between fluid molecules will occur
obeys Graham’s law

46
Q

When gas is laminar, this is the determinant of flow

A

viscosity

obeys Pouisellie’s law

47
Q

What is Pouiselle’s Law?

A

Flow = pi x r^4 x delta p/ 8 x viscosity x length

48
Q

Solubility of solid in a solution

A

the greater the temperature of the solvent, the greater the amount of solid solute dissolved (usually)

49
Q

Solubility of gases in a solution

A

the greater the temperature of the solvent, the less gas will be dissolved in the solvent

50
Q

Henry’s law:

A

C= P (in)/ Kh (out)

51
Q

Graham’s Law:

A

diffusion coefficient= solubility of gas/ square root of GMW

52
Q

Fick’s Law:

A

diffusion rate= area x diffusion coefficient x P1-P2/thickness

53
Q

Law of Laplace:

A

cylinder: T= PR
sphere: 2T= PR

54
Q

Heat is equal to

A

Heat = I^2/area

55
Q

Electromagnetic wave properties:

A

possess both wavelength and frequency

Each wave is energy so if the wavelength is shorter then it means there is more energy

56
Q

Wave Particle duality theory

A

EMR travels as photons of energy and can be thought of as a particle and a wave depending on how it is observed and measured

57
Q

EMR propagates as:

A

a wave & a particle

58
Q

The energy of EMR is

A

inversely proportional to its wavelength
short wavelength/high frequency= high energy
long wavelength/low frequency= low energy

59
Q

When EMR is quantized this means that

A

it is emitted in discrete quantities of energy

EMR energy is characterized by the energy of the photon (energy is greater for photons of higher frequency)

60
Q

The wavelength is

A

the distance between peak to peak or trough to trough

61
Q

The relationship between wavelength and frequency

A

Wavelength and frequency are inverse of each other

62
Q

EM waves represent propagation of

A

energy from a source
it follows the inverse square law 1/d^2
it will dissipate as distance increases

63
Q

The absorbed dose is

A

the amount of energy deposited for unit of mass

64
Q

the equivalent dose is

A

the absorbed dose multiplied by a converting factor based on the biologic effects of the type of energy

65
Q

The roentegen equivalent man (rem)

A

is the amount of ionizing radiation required to produce the same biological effect as one rad of high penetration X-rays
milliroentgen= mrem

66
Q

The variable number of neutrons in the nucleus of an atom (isotopes)

A

leads to the process of nuclear decay that produces radiation
it will have a tendency to spontaneously rearrange itself into a new combination of particles which are more stable- decay process

67
Q

During the decay process

A

bundles of excess energy (radiation) are emitted from the nucleus in several ways: beta, alpha, and gamma radiation
all of these are ionizing

68
Q

Beta particle radiation occurs when

A

the neutrons are excessive, a neutron can convert itself to a proton and an electron. the electron is ejected at very high speed

69
Q

Alpha particle radiation occurs when

A

2 protons and 2 neutrons are ejected as 1 particle

70
Q

Gamma radiation occurs when

A

the nucleus is in an excited state it can emit a “packet of energy” known as a photon. the number of protons and neutrons are NOT altered but instead the nucleus moves from a higher to a lower energy state
* most damaging

71
Q

What protection is needed for alpha, beta, and gamma particles?

A

alpha: distance
Beta: distance & some shielding
Gamma: distance, lead shields, concrete walls

72
Q

What is ionizing radiation?

A

IOnizing radiation is radiation with enough energy to remove tightly bound electrons from the atom’s orbits
causes the atom to become charged or ionized
can cause damage because it causes damage to DNA, RNA, proteins, and lipid

73
Q

Lasers cannot produce

A

genetic mutations because they utilize non-ionizing heat (poses no threat to cellular DNA)

74
Q

Lasers can cause

A

damage to the eyes because the light can be refracted to the back of the eye

75
Q

Recommended yearly limits of radiation are

A

5,000 mrem to the torse

maximum dose to the fetus of a pregnant worker may not exceed 500 mrem over 9 month gestation

76
Q

The greatest risk of rem exposure is

A

C-arm

77
Q

How far should you stand to minimize the exposure of the C-arm or Xray machine?

A

6 feet

78
Q

The intensity of any radiation is

A

intensity= 1/d^2

79
Q

X-ray safety lies within 3 factors:

A

distance from the source, barriers (shielding) and exposure time

80
Q

The photons of ionizing radiation have sufficient energy for

A

the separation of water molecules into positive and negative ions

81
Q

The energy of laser photons is

A

insufficient for the production of ions

cannot produce genetic mutations b/c it is non-ionizing

82
Q

Laser is

A

light amplification by stimulated emission of radiation

it is the light emitted when electrons jump from more distant orbital’s to orbital’s closer to the nucleus

83
Q

Laser light is distinguished by

A

monochromatic (one wavelength, one color), coherent (waves are synchronous), collimated (focused into a narrow beam)

84
Q

The three characteristics of lasers allow it to

A

generate intense light beams, deliver intense energy to a small target site, and send such beams efficiently and accurately through lenses

85
Q

Primary mechanism of tissue interaction include:

A

photochemical (UV and blue end of visible)

thermal (all wavelengths)

86
Q

There are two types of lasers:

A

continuous wave- power consistent

Pulsed: pause period allows for laser to emit high energy each pulse

87
Q

Photochemical:

A

UV and visible wavelengths: photon absorption excites molecules which may react to form unwanted chemical products

88
Q

Clinical lasers are used for

A

coagulation, cutting, and vaporization

89
Q

Laser safety patient risk include

A

airway fire, bleeding, pneumo, and cuff failure from laser penetration

90
Q

Personnel risk from laser injury include

A

laser injury, inhalation of surgical smoke

91
Q

The maximum permissible exposure or MPE

A

determines level of eye/skin protection needed

92
Q

Eye protection is of utmost importance with lasers because

A

the lens of the eye multiplies power density at the retina

retina is the location of photoreceptors

93
Q

Eyewear must be labeled with

A

the rated wavelength and optical density (OD)

94
Q

Wearers must ensure that eyewear

A

has sufficient OD at the laser’s wavelength

95
Q

Optical density is

A

indicates inverse of amount of light transmitted by a material at that wavelength
means there is high absorbance
the higher the OD the less transmission and then we have to pick the proper wavelength

96
Q

A laser’s minimum required OD is listed on laser’s warning sign

A

ensure eyewear OD is larger

97
Q

Most healthcare laser systems are

A

class 4: hazardous to view beam, skin hazard and fire hazard

98
Q

Reflections and lasers

A

specular (mirror like) reflections are more hazardous than diffuse reflections; keep shiny surfaces away from the field

99
Q

How does biological damage occur?

A

o Electrons are released from atoms–>hit and bump into water molecules–>release free radicals–> unstable and damage DNA, RNA, proteins, and lipids–>Over a lifetime it can cause issues such as leukemia

100
Q

Pressure relief valve:

A

if the pressure in the tube exceeds the valve pressure, then the valve is pushed up revealing vents through which pressure can be dissipated
ambu bag

101
Q

Pressure reducing valve:

A

oxygen tank

102
Q

Relationship between pressure, flow, and resistance

A

Flow= pressure/resistance

flowmeter: as flow increases, resistance decreases so pressure stays the same

103
Q

Relationship between pressure, force, and surface area

A

Pressure= force/area

same force distributed over a smaller area leads to increased pressure

Chem/Physics- Hannah (9 decks)

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