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Chem and physics > Chem and Phys Test 1 > Flashcards

Chem and Phys Test 1 Flashcards

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1
Q

Perioperative Heat Loss Timeframe

A

The patient core temperature drops the most in the first hour of induction.
Due to impairment of vasoconstriction and shivering responses.
Temperature stops dropping once it reaches 34.5 C

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2
Q

General anesthesia and temperature

A

Vasoconstriction is reduced and heat in the core moves to the periphery allowing core temperature to drop to anesthetic induced lowered threshold for vasoconstriction. Core to peripheral heat redistribution causes 0.5-1.55C drop in core temperature in the first hour of anesthesia

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3
Q

Thermoregulatory Vasoconstriction

A

Maintains temperature gradient between the core and periphery between 2-4C. Core (head, chest, and, pelvis) is insulated from environment by peripheral compartment

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4
Q

Most significant process in which patients experience heat loss during anesthesia

A

Radiation; accounts for 60% of heat loss

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5
Q

Which type of heat loss occurs when skin is prepped Chloaprep

A

Evaporation: warm heat from body causes liquid skin prep to turn to vapor.

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6
Q

Evaporation

A

Process in which liquid is changed to gas; requires energy to break hydrogen bondsBreathing causes heat loss through exhaled water vapor. Decrease gas flow rates, use humidification with patient who are intubated.

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7
Q

Complications of Hypothermia ( <35C)

A 
surgical site infection due to impaired vasoconstriction and decreased blood flow to area
dehiscence
bleeding due to impaired coagulation
ventricular ectopy
delayed drug metabolism
increased length of hospital stay
higher blood transfusion rates
impaired host defenses
thermal discomfort
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8
Q

Newton’s first law of motion

A

A body at rest or moving at a constant speed in a straight line will remain at rest or continue in a straight line at a constant speed unless it is acted upon by a force

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9
Q

Newton’s second law of motion

A

Force = mass x acceleration

The rate of change of momentum of an object is directly proportional to the momentum of the force applied.

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10
Q

Newton’s third law of motion

A

Every action has an equal and opposite reaction
When one object exerts a force on a second object, the second object exerts a force that is equal in magnitude and opposite in direction

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11
Q

Heat loss

A

Transfer of energy from a higher concentration of the a lower concentration

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12
Q

Radiation

A

Charged particles are accelerated and release electromagnetic wavelengths. Heat is then transferred from body to cooler environment. Vasodilation effect of anesthesia causes increased blood flow from body’s core to periphery. Cover body surfaces not being operated on lessens heat loss.

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13
Q

Convection

A

Heat has higher kinetic energy and rises due to less density. Cold air lower energy molecules due to greater density. As heat rises from body, colder molecules fall and are heated by the body’s warmth; creating air currents. Heat is lost from the body and air is warmed. Decrease the temperature in the room.

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14
Q

Conduction

A

Heat is transferred from warmer object physically touching cooler object. Ex: warm patient body on cool OR table. Place warm blankets on OR table.

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15
Q

Standard measure of force

A

Newton; kg*meter/second^2

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16
Q

average gravity on Earth

A

9.80665 m/s^2

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17
Q

1 newton

A

force of 100,000 dynes, Ex: SVR, PVR measurement

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18
Q

Vectors

A 
magnitude and direction 
displacement: distance with direction
velocity: speed with direction 
acceleration: how quickly speed changes
force
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19
Q

Scalars

A 
magnitude only;
volume
density
speed
mass
time
temperature
distance
work
pressure
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20
Q

Resultant

A

addition of 2 vectors; must take into account value and direction

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21
Q

Velocity

A

displacement/time, 0 if end at the same location

meter/sec

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22
Q

Work

A

Work = force x distance (or displacement)
Amount of energy necessary to move an object from one point to another
If work is done on you –> you gain heat
If you do work on something –> you lose heat
Unit: Joule = kg* m^2 / s^-2
(no change in volume/energy/distance = no work done)

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23
Q

penetrating injury damage depend on what 3 factors

A
  1. type of wounding instrument (knife, missile (bullet or fragment)
  2. velocity of the missile at time of impact
  3. characteristics of tissue which it passes (bone, fat, muscle, blood vessels, nervous tissue, organs)
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24
Q

Lower velocity wounds

A

inflict injury by lacerating and cutting tissue.

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25
Q

Moderate to high velocity wounds

A

result from deceleration of object as it passes through tissue, causing kinetic energy to transfer to surrounding tissue.

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26
Q

Most significant determinant of wound potential

A

velocity; bullet wounds have greater potential to inflict serious injury compared with a knife of handheld projectile

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27
Q

speed

A

distance traveled/time elapsed; m/s, mph

rate at which something moves of changes position

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28
Q

Blunt trauma injuries

A

Fractures, lacerations, external wounds, tearing by shearing forces, coup-contrecoup injuries

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29
Q

Pressure units

A

force/area; Pascal (Pa) = N/m^2

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30
Q

Gauge pressure

A

Pressure of a system above or below atmospheric pressure
Gauge pressure = total pressure -atmospheric pressure
0 reference point

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31
Q

1KPa

A

1000 Pa (Pascals)

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32
Q

1atm

A

101.3KPa

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33
Q

Second law of thermodynamics

A

Heat naturally flows from hot to cold; the only way for cold to flow to hot is via the addition of energy
Ex: Ball naturally flows from high position to low position at the top of a hill, but the ball cannot naturally go back up the hill
Change in entropy is > 0

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34
Q

Entropy

A

Natural processes move toward disorder; universal trend toward equilibrium; unidirectional
Low energy = energy concentrated
High energy = more spread out energy

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35
Q

Force

A

Push or pull required to produce an acceleration

Newtons or N

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36
Q

Kinetic Energy

A

Ability to do work; energy of motion

KE = 1/2 mv^2 (mass * speed)

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37
Q

Power

A

Rate at which energy is spent; rate of doing work
Power = work/time
Unit: Watts (W) = Joule/second

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38
Q

Syringe size and pressure

A

Syringe is an example of pressure generated by force over area
Pressure = force/area
Increase area over which same force is generated, decease pressure
Decrease area over which same force is generated, increase pressure

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39
Q

Barometer

A

tube closed at one end and open on the other; pressure of the atmosphere and the weight of mercury column = opposing forces. More air pressure = more force = increased height of mercury
P(atm) = density x gravity x height (pgh)
* Measure actual or absolute pressure
Total pressure = gauge pressure + atmospheric pressure

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40
Q

Manometer

A

U-shaped tube filled with a fluid of a known density; measures pressure difference
delta P = P (system) - P (atmosphere)
* measure gauge pressure

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41
Q

Bourdon Gauge

A

Used on gas cylinders; type of aneroid gauge bc they don’t use liquid.
Measure pressure difference btw pressure exerted by gas on cylinder and atmospheric pressure. Gas above atmospheric pressure enters coiled tube –> slight uncoil and pointer moves to show gauge pressure
*Measure gauge pressure

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42
Q

1 pascal

A

N/m2

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43
Q

Potential energy

A

stored energy
PE = mass * gravity * height
Ex: battery, plane in the air, chemical energy stored in food

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44
Q

Internal energy

A

kinetic energy + potential energy

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45
Q

First Law of Thermodynamics

A

Law of conservation of energy; energy cannot be created or destroyed

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46
Q

Third Law of Thermodynamics

A

Absolute; is considered void of energy, theoretically impossible to reach

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47
Q

Mass

A

Amount of matter in an object; resistance of an object to acceleration
Unit: Kg

48
Q

Enthalpy

A

Total amount of energy in a system

49
Q

Metric system Units

A

Length: meters
Mass: Kilograms
Temperature: Kelvin
Mole (mol): measures amount of material

50
Q

Acceleration

A

Rate at which velocity changes
Speeding up, slowing down, changing direction
Average acceleration = delta velocity/delta time
Units: m/s^2

51
Q

Weight

A

gravitational force exerted on an object by a much larger object
Unit: N
Weight (N) = mass (kg) x gravitational force (6.8m/s2)

52
Q

giga

A

10^9

53
Q

mega

A

10^6

54
Q

kilo

A

10^3

55
Q

deci

A

10^-1

56
Q

centi

A

10^-2

57
Q

milli

A

10^-3

58
Q

micro

A

10^-6

59
Q

nano

A

10^-9

60
Q

Accuracy

A

The agreement between experimental data and the true/expected value (within a margin of error)
Assessed via % error calculation
% error: [(measured value-true value)/(true value)] x 100

61
Q

Precision

A

Agreement between replicate measurements (over and over again yields the same result)
Standard deviation assesses precision
Smaller the ratio of the standard deviation to average value, the better the precision
Greater number of significant figures implies greater precision

62
Q

Most accurate core temp location in adults

A

Temporal artery; high ease of access and accuracy

63
Q

Density

A

represented by d or p (rho)
Density = mass / volume
Density will also have 2 units
Density of water = 1.0g/mL

64
Q

Specific gravity

A

Ratio between an object’s density and the density of water
SG = density of object / density of water
SG is dimensionless

65
Q

Specific Gravity and temperature

A

Can decrease specific gravity by increasing temp of the substance.
Increasing temp expands the volume (increases the volume) –> decreased density
CSF example:
Med injected that has higher specific gravity than CSF will sink
Med injected that has lower specific gravity than CSF will float
Sample with specific gravity greater than 1 is denser than water and will sink
Sample with specific gravity less than 1 is less dense than water and will float

66
Q

Ion

A

molecule/atom that have net electric charge; either gained or lost electrons
* positive or negative charge

67
Q

Cation

A

atom that has lost an electron

positive charge

68
Q

Anion

A

atom that has gained an electron

negative charge

69
Q

Organic ions vs inorganic ion

A 
Organic ions: contain carbon
Ex: Phosphate intracellularly (ATP)
Can be lowered by diuretics
Inorganic: do not contain carbon
Ex: Phosphate extracellularly
70
Q

Significant figures

A

Digits in a measured value that have physical meaning and can be reproductively determined
Nonzero digits are always significant
Captive zeros are always significant
Leading zeros are never significant
Trailing zeros are only significant when the number contains a decimal point
When adding/subtracting: keep smaller number of decimal places and round
When multiplying/dividing: keep smaller number of significant figures and round

71
Q

Matter

A

anything that has mass and takes up space

72
Q

Atoms

A

building blocks of matter, have 3 particles
Protons: positively charged with a mass of 1 amu
Neutrons: electrically neutral and have a mass of 1 amu
Electrons: negatively charged, smaller mass than protons and neutrons

73
Q

Elements

A

contain only a single type of atom; always electrically neutral, so each atom must have an equal number of protons and electrons

74
Q

Compounds

A

contain 2 or more kinds of atoms
Molecules: group of atoms chemically bonded together into unit by covalent bonds, electrically neutral
Ions: positively or negatively charged ions; have no identifiable discrete units

75
Q

Pure substances

A

cannot be physically separated into simpler components. mostly metals, nonmetals, and metalloids
Ex: steel, iron, gold, copper

76
Q

Mixtures

A

comprised of 2+ substances and can be separated into smaller components through physical process
Homogeneous: uniform in chemical and physical properties. Ex: blood, wine, coffee, air
Heterogeneous: not uniform between component. Ex: emesis, salad

77
Q

Atomic number

A

Number of protons in the nucleus

Determines identity of atom

78
Q

Mass number

A

sum of atomic number and neutron number

79
Q

Neutron number

A

Mass number - atomic number

80
Q

Isotopes

A

have the same atomic number but different mass number; same number of protons, different number of neutrons

81
Q

Order of elements

A

Elements are listed in order of increasing atomic number, each successive element has one additional proton

82
Q

Vertical columns (groups/families)

A

Elements in each group have similar chemical and physical properties

83
Q

Rows (Periods)

A

Periods represent adding electrons to quantum energy levels in the atom

84
Q

Classifying elements on periodic table

A

Representative elements have a group number with an A
Transition elements have a B designation in their group #
Inner transition elements are located at the bottom of table

85
Q

Chemical nomenclature

A

Determine of metal or nonmetal
Molecular compounds are comprised of nonmetals
Ionic compounds are almost always comprised of a metal and a nonmetal

86
Q

Naming molecular compounds

A

Name each element
Indicate how many of each element is present with prefix multiplier (mono, di, tri, tetra, penta, hexa, hepta, octa)
Add suffix “-ide”
Dihydrogen monoxide (H2O)

87
Q

Naming ions and compounds

A

Ion is an atom or group of atoms with a charge

Ionic compounds have ions and are held together by ionic bonds

88
Q

Monatomic cations of metals

A

Representative metals form cations where ionic charge equals the group number; group number equals # of electrons in outer shell; gives away electrons to fill shell
Name the element and add ion or cation
Na1+ = sodium ion

89
Q

Monatomic anions of nonmetals

A

Representative nonmetals: ionic charge is based on number of electrons the nonmetal needs to gain in order to fill shell
Name the element and add suffix “ide”
Cl 1- = Chloride ion

90
Q

Transition metals: Cations

A

If transition metal forms only one cation, name like representative cation
If transition metal forms more than one cation, name metal and indicate charge on the cation with Roman numerals in parenthesis
Fe 2+: Iron (II) ion

91
Q

Polyatomic ions

A

Formed from 2+ nonmetals that are bonded together in a way that results in net electrical charge
Ion with larger number of oxygen atoms is given “ate”,
Ion with smaller number of atoms oxygen is given “ite”
SO4 2-: sulfate
SO3 2-: sulfite

92
Q

Electrolytes

A

Substance that dissolves in water to give a solution that conducts electricity
The few ionic compounds that readily dissolve in water are electrolytes because they separate into ions that freely and independently move around in the solution; free movement –> electricity conduction
Molecular compounds are nonelectrolytes, unless they have acid or base properties
Tap water conducts electricity because it contains a fair concentration of electrolytes
Pure water is a non electrolyte and does not conduct electricity

93
Q

Reduction

A

Gain of electron

94
Q

Oxidation

A

Loss of electron

95
Q

Hydrolysis

A 
Use of water to split molecular bonds
H-R-R-OH + H-OH -> 1 large molecule is broken up into 2 smaller molecules
H-R-OH and H-R-OH
Ex: Polymer to monomer
Starch + H2O = Glucose + Glucose
Polypeptide + H2O = Amino acid
96
Q

Amino Acids

A

DNA –> (transcription) mRNA -> (translation) - tRNA + amino acids -> protein formation
Proteins = chain of amino acids
Amino group + Carboxyl group + Alpha carbon + R group

97
Q

Lipids

A

Partly hydrophobic; partly hydrophilic
Function: energy storage, signaling, membrane structure
Hydrophilic head; hydrophobic chain

98
Q

Proteins

A

Building block = amino acid
Amino acids connected by peptide bonds
Primary structure: sequence of amino acids in peptide chain

Secondary structure: how amino acid chain twists on itself. Hydrogen bonds btw H and N form bond btw carbonyl.
Ex: alpha helix coil stabilized by hydrogen bonds. Common in wool
Ex: beta pleated sheet -> nearby linear strands of polypeptide chains line up in linear fashion. Common in silk

Tertiary Structure: how polypeptide chain folds to form globular structure. Hydrogen bonding and London forces.

99
Q

Carbohydrates

A 
1 Oxygen:2 Carbon ration
Building block is glucose
Glucose = monosaccharide
Glucose chain = polysaccharide
Energy store
100
Q

Phase 1 metabolism

A

Uses enzymes (oxidases) to unmask polar groups (-OH and -O’s) on the drug
Drug + O2 + NADPH –> Drug-O + H20 + NADP+
NADPH acts as reducing agent
Mainly uses cytochrome p450 to produce result
* Requires oxygen
CYP3A4: metabolizes > 50% of drugs
CYP2D6: famous for polymorphisms

101
Q

Phase 2 metabolism- Conjugation reaction

A

Uses enzymes (transferases) to transfer small endogenous polar molecules onto a drug to make it more water soluble.
UGT: UDP-glucuronsyltransferase -> glucuronidation
GST:Glutathione conjugation
NAT: Acetylation
SULT: Sulfation
Oxygen NOT required

102
Q

Krebs cycle

A

Glycolysis of glucose (6 carbon) -> 2 pyruvic acids (2 3-carbon) -> 2 net ATP + 2 NADH ->
Acetyl CoA in prep for Krebs cycle

Acetyl CoA merges w/ Oxoloacetic acid -> citric acid
Citric acid -> oxidized to Oxoloacetic acid -> 6x CO2 + 10 NADH + 4 ATP + 2 FADH2
10 NADH -> oxidized in electron transport chain -> 30 ATP
2 FADH2 -> oxidized in electron transport chain -> 4 ATP
4 + 4 + 30 = 38 total ATP

Glycolysis occurs in cytoplasm
Krebs cycle occurs in mitochondria
Catabolic reaction: breakdown of glucose to make ATP
Acetyl CoA: general catabolic intermediary that enters Krebs cycle to create ATP via glucose, protein, fat metabolism

103
Q

Polar molecules

A

Hydrophilic; partial or full charge

104
Q

DNA

A

Sugar backbone is composed of deoxyribose

Bases: thymine, adenine, guanine, cytosine

105
Q

RNA

A

Sugar backbone is composed of ribose

Bases: uracil, adinine, guanine, cytosine

106
Q

3 ways to denature protein

A

Heat, heavy metal ions (Ag+, Hg2+)

107
Q

Monosaccharides

A

Glucose, fructose, galactose

108
Q

Disaccharides

A

Sucrose, Lactose, Maltose

109
Q

Polysaccharides

A

Starch, Glycogen, Cellulose

110
Q

3 ways to denature protein

A

Heat
Heavy metal ions (Ag+, Hg2+)
Changes in pH

111
Q

Monosaccharides

A

1 sugar

Glucose, fructose, galactose

112
Q

Disaccharides

A

2 sugars

Sucrose, Lactose, Maltose

113
Q

Polysaccharides

A

Complex sugar

Starch, Glycogen, Cellulose

114
Q

Saturated alkane formula

A

C(n)H(2n+2)

115
Q

Phosphate esters

A

DNA & RNA backbone

Chem and physics (8 decks)

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