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APEX > Unit 12 - Chemistry & Physics > Flashcards

Unit 12 - Chemistry & Physics Flashcards

1
Q

complete transfer of valence electrons

A

ionic bond

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2
Q

equal sharing of valence electrons

A

covalent bond

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3
Q

unequal sharing of valence electrons

A

polar covalent bond

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4
Q

3 components of an atom

A
  1. protons
  2. neutrons
  3. electrons
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5
Q

what 2 components of an atom make up the nucleus?

A

protons and neutrons

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6
Q

what determines an atom’s atomic number

A

number of protons

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7
Q

the predictable orbit electrons travel in is called a

A

shell

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8
Q

electrons in the outermost shell are called

A

valence electrons

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9
Q

what makes the atom non-reactive (inert)

A

full shell

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10
Q

what is a molecule?

A

2 or more atoms bonded together

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11
Q

what gives an atom a neutral charge

A

electrons = # protons

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12
Q

what gives an atom a positive charge

A

protons > # electrons

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13
Q

what gives an atom a negative charge

A

electrons > # protons

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14
Q

what is an ion?

A

an atom that carries a positive or negative charge

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15
Q

what is a cation

A

an atom with a positive charge (it has lost electrons)

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16
Q

what is an anion

A

an atom with a negative charge (it has gained electrons)

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17
Q

which tends to ionize, metals or non-metals?

A

metals

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18
Q

bond that involves the complete transfer of valence electron(s) from one atom to another

A

ionic bond

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19
Q

bonding common among acids and bases

A

ionic bond

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20
Q

key example of a polar covalent bond

A

water - region near oxygen atom is relatively negative and region near hydrogen atom is relatively positive

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21
Q

what explains why a hydrophilic solute dissolves in water

A

since water is a polar molecule, it’s also attracted to other polar molecules and ions

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22
Q

what describes a very weak intermolecular force that holds molecules of the same type together

A

Van der Waals Forces

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23
Q

molecular bonds in decreasing order of strength

A

covalent > ionic > polar covalent > Van der Waals

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24
Q

Dalton’s law of partial pressures

A

total pressure is equal to the sum of the partial pressures exerted by each gas in the mixture

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25
Q

how to convert partial pressure to volumes percent for a liquid

A

volumes % = (volume of solute/volume of solution) / 100

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26
Q

how to convert partial pressure to volumes percent for a gas

A

volumes % = (partial pressure / total pressure) * 100

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27
Q

convert volumes percent to a partial pressure

A

partial presure = (volumes %/100) * total pressure

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28
Q

Henry’s law

A

at a constnt temperature, the amount of gas that dissolves in a solution is directly proportional to partial pressure of that gas over the solution

Or - the higher the gas pressure, the more it will dissolve into a liquid (assuming constant temp)

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29
Q

which law explains why emergence is prolonged in hypothermic patients

why?

A

Henry’s law

the solubility of the gas is increased and less of it leaves the body per unit of time

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30
Q

according to Henry’s law, how does partial pressure affect solubility?

A

decreased pressure = decreased solubility

increased pressure = increased solubility

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31
Q

how does temperature affect solubility

A

decreased temp = increased solubility

increased temp = decreased solubility

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32
Q

solubility of CO2 vs O2

A

CO2 is ~20 times more soluble than O2

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33
Q

oxygen delivery calculation

A

DO2 = CO * [(1.34 * Hgb * SpO2) + (PaO2 * 0.003)} * 10

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34
Q

how to calculate the amount of CO2 dissolved in the blood

A

PaCO2 x 0.067 mL/dL/mmHg

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35
Q

how is most CO2 transported in the blood

A

in the form of bicarbonate or bound to hgb

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36
Q

how does “overpressurizing” during induction work

A

if you significantly increase the concentration of volatile anesthetic at the alveolocapillary interface, can hasten its transfer into the bloodstream and ultimately the brain

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37
Q

gas law that describes the transfer rate of gas through a tissue medium

A

Fick’s law of diffusion

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38
Q

according to Fick’s law, rate of transfer is directly proportional to:

A
  • partial pressure difference (driving force)
  • diffusion coefficient (solubility)
  • membrane surface area
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39
Q

according to Fick’s law, rate of transfer is inversely proportional to:

A
  • membrane thickness

- molecular weight

40
Q

law that explains diffusion hypoxia

A

Fick’s law

41
Q

law that explains a patient with severe COPD has a reduced alveolar surface area and therefore slower rate of inhalation induction

A

Fick’s law

42
Q

law that explains the calculation of cardiac output

A

Fick’s law

43
Q

law that explains drug transfer across the placenta

A

Fick’s law

44
Q

Graham’s law

A

molecular weight of a gas determines how fast it can diffuse through a membrane

45
Q

according to Graham’s law, the rate of diffusion of a gas is inversely proportional to:

A

the square root of the gas’s molecular weight

46
Q

law that explains the second gas effect

A

Graham’s law

47
Q

Boyle’s law calculation

A

P1 * V1 = P2 * V2

48
Q

Charles’s law calculation

A

V1/T1 = V2/T2

49
Q

Gay Lussac’s law calculation

A

P1/T1 = P2/T2

50
Q

Boyle’s law

A

at a constant temperature, the volume of a given mass of gas varies inversely with absolute pressure

51
Q

Charles’ Law

A

at a constant pressure the volume of a given mass varies directly with the absolute temperature

52
Q

Gay Lussac’s law

A

at a constant volume the absolute pressure of a given mass of gas varies directly with the absolute temperature

53
Q

these are examples of which law:

  • pneumatic bellows
  • diaphragmatic contraction increases Vt
  • squeezing a bag valve mask
  • using bourdon pressure gauge to calculate how much O2 is left in a cylinder
A

Boyle’s law

54
Q

LMA cuff rupturing when placed in an autoclave is an example of which law

A

Charles

55
Q

oxygen tank exploding in a heated environment is an example of which law

A

Gay-Lussac’s

56
Q

what is the ideal gas law

A

unifies Boyle’s, Charles’s, and Gay-Lussac’s laws into a single equation

PV = nrT

  • P = pressure
  • V = volume
  • n = # moles
  • r = constant 0.0821 liter-atm/K/mole
  • T = temperature
57
Q

during laminar flow, quadrupling the radius will cause flow to increase by a factor of:

A

256

58
Q

Ohm’s law

A

the current passing through a conductor is directly proportonal to the voltage and inversely proportional to the resistance

59
Q

Ohm’s law adapted to fluid flow

A

flow = pressure gradient/resistance

60
Q

symbol for cardiac output

A

Q

61
Q

symbol for SVR

A

R

62
Q

Poiseuille’s law

A

adaptation of Ohm’s law that incorporates vessel diameter, viscocity, and tube length

Q = (π * R^4 * △P) / 8 * η * L

  • Q = blood flow
  • R = radius
  • △P = arteriovenous pressure gradient (Pa-Pv)
  • η = viscosity
  • L = length of tube
63
Q

what factor exhibits the greatest impact on flow

A

radius

64
Q

how does temperature affect viscocity

A

inversely proportional

  • decreased temp = increased viscosity and resistance
  • increased temp = decreased viscosity and resistance
65
Q

application of Poiseuille’s law to deliver RBCs faster

A
  • increase radius with large bore IV
  • increase pressure gradient with pressure bag or raise IV pole
  • decrease viscosity by diluting the blood with NS or running through fluid warmer
  • use shortest tubing possible
66
Q

what law explains that polycythemia reduces microvascular flow

A

Poiseuielle’s

67
Q

what is Reynolds’ number

A

allows us to predict the type of flow that will occur in a given situation

Reynolds’ number = (density * diameter * velocity) / viscosity

68
Q

according to Poiseuille’s law, what is laminar flow dependent on?

A

gas viscosity

69
Q

according to Graham’s law, what is turbulent flow dependent on?

A

gas density

70
Q

what is laminar flow

A
  • all molecules travel in parallel pattern
  • due to cohesive forces, molecules in the center of the tube travel at fastest rate while molecules near walls travel at slowest rate
71
Q

what 2 things form the nucleus

A

protons and neurons in the center of the atom

72
Q

what is avogadro’s number

A

says that 1 mole of any gas is made up of 6.023 x 10^23 atoms

a mole of gas is equal to the molecular weight of that gas in grams

73
Q

define specific heat

A

the amount of heat required to increase the temperature of 1 gram of a substance by 1 degree C

74
Q

solubility coefficient for oxygen

A

0.003 mL/dL/mmHg

75
Q

solubility coefficient for CO2

A

0.067 mL/dL/mmHg

76
Q

How does knowing the oxygen solubility coefficient help us calculate oxygen delivery?

A

Multiplying the Pa02 by oxygen’s solubility coefficient
(0.003 mL/dL/mmHg) allows us to calculate how much oxygen is dissolved in the blood.

77
Q

List 4 clinical examples of
Fick’s law

A
  1. Diffusion hypoxia
  2. A patient with severe COPD has a slower rate of inhalation induction
  3. Calculation of cardiac output
  4. Drug transfer across the placenta
78
Q

formula for Boyle’s law

A

P1 * V1 = P2 * V2

79
Q

formula for charles law

A

(V1/T1 = (V2/T2)

80
Q

formula for gay-lussacs law

A

(P1/T1) = (P2/T2)

81
Q

how does use of Heliox decrease airway resistance

A

turbulent flow is primarily dependent on gas density

inhaling lower density gas decreases Reynold’s number and improves flow turbulence when airway resistance is high

82
Q

examples of laminar flow

A
  • airflow in terminal bronchioles
  • systemic blood flow
83
Q

Re in terminal bronchioles

A

low (< 2000)

laminar flow

84
Q

Re in terminal bronchioles

A

low (< 2000)

laminar flow

85
Q

examples of Re > 4000

A

turbulent flow
* flow through orifice (glottis or annular space when FGF is high)
* airflow through medium-sized bronchi

86
Q

Bernoulli’s principle

A

describes the relationship between the pressure and velocity of a moving fluid or gas

87
Q

how does velocity affect pressure according to Bernoullis principle

A
  • If the fluid’s velocity is high, then the pressure exerted on the walls of the tube will be low.
  • If the fluid’s velocity is low, then the pressure exerted on the walls of the tube will be high.
88
Q

Venturi effect

A

As airflow in a tube moves past the point
of constriction, the pressure at the constriction decreases (Bernoulli principle). If the pressure inside
the tube falls below atmospheric pressure, then air is entrained into the tube (Venturi effect)

89
Q

examples of venturi effect

A

Jet ventilator, Venturi mask, and nebulizer

90
Q

describes how a jet flow attaches itself to a nearby surface and continues to flow along that surface even when the surface curves away from the initial jet direction

A

Coanda effect

91
Q

ex of coanda effect

A

Wall-hugging jet of mitral regurgitation and water that follows the curve of a glass

92
Q

illustrates the relationship between the wall tension, internal pressure, and radius

A

law of Laplace

93
Q

law of laplace equation applied to cylinders

A

tension = pressure * radius

94
Q

law of laplace equation applied to sphere

A

tension = (pressure * radius) / 2

95
Q

according to the law of laplace, the tendency of an alveolus to collapse is directly proportional to:

A

surface tension
(more tension = more likely to collapse)

96
Q

according to the law of laplace, the tendency of an alveolus to collapse is inversely proportional to:

A

alveolar radius
(smaller radius = more like to collapse)

97
Q

–left off on pg 9–

A

APEX (54 decks)

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