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NUR 724 Chem&Phys > Exam #1 > Flashcards

Exam #1 Flashcards

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1
Q

Force

A

the amount of energy to move an object
Force = mass x acceleration

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2
Q

Pressure

A

force over area, increasing the area in which force is applied results in a lower pressure
P=f/a

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3
Q

Work

A

transfer of energy by a force acting on an object as it is displaced
W=Fs (force*displacement)

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4
Q

Energy

A

the capacity to do work or the exertion of force (potential +kinetic energy)

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5
Q

Power

A

amount of energy transferred or converted per unit time
P= force/velocity

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6
Q

Force SI units

A

newton

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7
Q

Pressure SI units

A

pascal (Pa)

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8
Q

Work SI units

A

joule

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9
Q

Energy SI units

A

joule

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10
Q

Power SI units

A

watt

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11
Q

Conduction

A

energy transfer between 2 objects in direct contact
Ex- touching a cold surface

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12
Q

Convection

A

air passing by aka wind chill
Body heat is lost to surrounding cold air. The surrounding air becomes warmer and rises; cool air falls and replaces the warm air (it’s a current/cycle).

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13
Q

Radiation

A

electromagnetic transfer of energy away from a warm body– biggest contributor

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14
Q

Evaporation

A

liquids on skin evaporate, utilizing energy to turn liquid to vapor

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15
Q

how to mitigate radiation in the OR

A

head is always perfused and major contributor to radiation heat loss, so it should be covered

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16
Q

how to mitigate convection in the OR

A

covering the patient with warm blankets forced air warming device
Close air vents to prevent a draft

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17
Q

how to mitigate conduction in the OR

A

preheat the OR table
Cover the table with blankets if possible

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18
Q

how to mitigate evaporation in the OR

A

HME, air humidifier on airway circuit
Be careful when scrubbing the surgical site with CHG, prep necessary sites only

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19
Q

Newton’s first law

A

objects have a tendency to maintain velocity unless acted on by unbalanced force
Law of inertia

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20
Q

Newton’s first law r/t anesthesia

A

blood loss-blood will have the tendency to maintain velocity, unless acted upon, such as clots or external pressure
Trauma- a gunshot will stay in motion unless acted upon, such as a skull.

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21
Q

Newton’s second law

A

F=m*a
Force= mass • acceleration

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22
Q

Newton’s second law r/t anesthesia

A

pressure bag for fluids
force=mass of fluid*velocity of fluid

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23
Q

Kelvin to celsius conversion

A

Celsius + 273.15= Kelvin

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24
Q

Newton’s third law

A

for every action, there is an equal and opposite reaction
Law of reciprocal action

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25
Q

Newton’s third law r/t anesthesia

A

heart failure cardiomegaly
low EF-> increased blood volume in LV to push out, but the blood also pushes on the cardiac muscle, stretching it out
CPR- the action of the RN pushing DOWN on the chest, reciprocal action- chest recoil

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26
Q

First law of thermodynamics

A

energy can’t be created or destroyed, only transferred (heat)
Law of conservation of energy

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27
Q

Second law of thermodynamics

A

no spontaneous transfer of heat from cold to hot
Energy moves towards greater entropy/randomness

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28
Q

temperature =

A

avg. KE
Average heat loss/gain of a system (think of ice melting in a cup of water)

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29
Q

KE equation

A

(m|v|^2)/2

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30
Q

PE equation

A

mgh (massgravity forceheight)

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31
Q

zeroth law of thermodynamics

A

systems in thermal equilibrium do not exchange energy in the form of heat

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32
Q

gravity force constant

A

9.81 m/s/s = 1 Newton

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33
Q

what is a pascal

A

1N/1m2

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34
Q

entropy

A

The equilibration of energy. Energy moves from high to low concentration to achieve equilibrium. The difference in the gradient influences the flow of energy.

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35
Q

fahrenheit to celsius

A

(f-32)/1.8

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36
Q

scalar values

A

magnitude only
distance
speed

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37
Q

vector values

A

magnitude and direction
displacement
velocity

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38
Q

how do surgical wounds contribute to heat loss?

A

convection
The open wound releases heat to warm up the surrounding cool air.

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39
Q

Biggest drop of heat loss in the perioperative phase

A

during the first 30-60mins of anesthesia
The adult body loses 1C.

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40
Q

what part of the brain is responsible for regulating temperature

A

hypothalamus

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41
Q

populations where shivering is detrimental

A

TTM
Shock
hypoxemic
Increases metabolic demand and o2 consumption

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42
Q

temp value indicating hypothermia

A

95F
35C

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43
Q

4 factors that affect rates of flow on IV fluids

A

pressure gradient
viscosity of fluid
length of tube
radius of tube

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44
Q

medications that cause vasodilation during anesthesia

A

Basically everything!!
volatile anesthetics
lidocaine
propofol
versed
fentanyl
hydralazine
dex (depends on dose)

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45
Q

how does neuraxial anesthesia cause decreased body temperature

A

brain doesn’t receive cold signal, thinks its warm
efferent nerves that control vasoconstriction and shivering are blocked

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46
Q

how does rapid NS infusion lead to hyperchloremic acidosis

A

^^chloride levels
bicarb doesn’t want to leave the cell d/t all the chloride
chloride can’t break down H+ to be excreted
acids build up

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47
Q

difference between accuracy and precision

A

accuracy- how close readings are to target
precision- how close readings are to each other

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48
Q

how can accuracy be improved

A

recalibration
maintain consistent experimental conditions
control external factors that can introduce variability

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49
Q

how can precision be improved

A

education on proper use of the device to use the device consistently

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50
Q

density

A

mass/volume

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51
Q

specific gravity

A

density of object/density of water

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52
Q

density of water in g/cm^3

A

1.06

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53
Q

density of water in lbs/ft^3

A

62.4

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54
Q

baricity

A

the ratio of the density of LA and CSF

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55
Q

How to determine the pH of a buffer

A

Henderson equation
pH = pKa + log10 ([A–]/[HA])

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56
Q

define anion gap

A

difference between measured serum cations and anions under normal conditions

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57
Q

anion gap formula

A

(Na+K)-(Cl+HCO3)

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58
Q

How to apply physics principles to traumatic brain injuries

A

coup and contrecoup lesions
brain will continue to move until acted up (the skill) damaging the opposite side of the brain from where the injury occurred.

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59
Q

How is the Periodic Table organized

A

It is organized by groups- vertical columns, and periods - horizontal rows. And it also has subgroups by elemental properties.

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60
Q

Covalent bonds

A

The physical sharing of electrons. can hold up to triple bonds. This tends to be bonding between atoms that share similar electronegativity.

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61
Q

Ion - Ion bond

A

The strongest electrostatic bond, occurs along the outer shell. Have the highest boiling and melting points.

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62
Q

Electrostatic bonds

A

The attraction of electrons between atoms due to electron distribution or electronegativity. This includes ion-ion, ion-dipole, and dipole-dipole interactions

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63
Q

Ion

A

Atoms that have gained or lost electrons from their natural composition. These atoms either have a positive or negative charge

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64
Q

Anion

A

Atom that has gained one or more electrons, is negatively charged.

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65
Q

Cation

A

An atom that has lost one or more electrons, is positively charged.

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66
Q

Isotopes

A

Same number of protons but different number of neutrons. This leads to a different mass number.

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67
Q

Ion dipole bond

A

A weak bond due to partial charges being involved. However, the molecule itself does not have a formal charge.

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68
Q

Isomers

A

Molecules that have the same chemical formula but different structures. Although the number and type of atoms and bonds are the same, the arrangement is different.

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69
Q

Hydrocarbon

A

Molecules composed entirely of carbon and hydrogen atoms. They often are formed and straight chained with or without branches.

70
Q

Saturated hydrocarbon

A

Single bonded carbon chain with all available carbon bonds attached to hydrogen

71
Q

Unsaturated hydrocarbon

A

One or more double or triple bonds between carbon atoms

72
Q

-yne

A

Triple bonded carbon

73
Q

-ene

A

Hydrocarbon with double bonded carbon

74
Q

Cyclic hydrocarbon

A

Carbon chains in a ring structure. They May contain multiple carbon atoms with double or triple bonds.

75
Q

-ane

A

Hydrocarbon containing only single bonded atoms

76
Q

-yl

A

Saturated or unsaturated hydrocarbons that are missing hydrogens. Very reactive, usually bound to functional groups.

77
Q

-ryl

A

Cyclic hydrocarbons that are missing a hydrogen on any carbon. Tend to bind with functional groups, are reactive

78
Q

-Amine functional group

A

Ammonia derivative, loves to pair electrons on nitrogen
RNH2

79
Q

Alcohol functional group

A

ROH
Hydroxyl is highly polar, it easily forms hydrogen bonds with other polar molecules. The OH polarity allows alcohol to dissolve and many other polar molecules like water.

80
Q

Phenol functional group

A

ROH
A simple phenol is polar due to the OH group. More complex finals like propofol are not water soluble.

81
Q

Oxidation

A

Process of losing electrons to another element.

82
Q

Reduction

A

Process of gaining electrons from another element

83
Q

What is oxidation and reduction based off?

A

The electronegativity of the elements. The more electronegative element will gain electrons or be reduced. The less electronegative element will lose electrons or be oxidized.

84
Q

Ethers functional group

A

ROR’
The group is attached using oxygen. They are nurt and don’t react to oxidizing or reducing agents. They are highly flammable.
Halogen substitution on ethers altars anesthetic characteristics such as blood, solubility and potency.

85
Q

Carbonyl functional group

A

Several functional groups have this arrangement. They are polar due to the electronegativity from oxygen.

86
Q

The different groups in the Carbonyl functional group

A

Aldehydes RCHO
Ketones RCOR’
Carboxylic acid RCOOH
Esters RCOOR
Amides RCONH2, RCONHR, RCONR2

87
Q

Alkali metals

A

Group 1
React violently with water

88
Q

Alkaline Earth metals

A

Group 2
React with water
usually bonded with other elements

89
Q

Metals

A

Group 3-12
Are solids at room temperature (except mercury/Hg is liquid)
Malleable
Good conductors of electricity

90
Q

Halogens

A

Group 17/7
Brittle
Not malleable
Poor conductors
Are corrosive - very reactive

91
Q

Noble gases

A

Group 8/18
Non reactive due to a full shell of electrons.
Colorless gases

92
Q

Enthalpy

A

The total energy possessed by a system
KE+PE

93
Q

Bond energy

A

The amount of energy needed to form or break a bond.
Energy is RELEASED when a bond is formed.
Energy is CONSUMED when a bond is broken.
** Covalent/short bids possess higher bond energies than the other bonds .

94
Q

Structural isomer

A

one in which two or more organic compounds have the same molecular formulas but different structures.
Ex-Isoflurane and enflurane are both volatile anaesthetic agents

95
Q

Stereo isomers

A

molecules have the same molecular formula and sequence of bonded atoms, but differ in the three-dimensional orientations of their atoms in space.
Ex-ropivacaine and levobupivacaine

96
Q

Heat production

A

The body produces heat through metabolism and muscle movements (shivering)

97
Q

Intraoperative Hypothermia

A

It’s a pattern-
The initial rapid drop in core temperature (1C in the first 30-60 min)
Slow linear reduction
Temperature stabilizer and remains unchanged

98
Q

Bourdon gauges

A

Used in anesthesia to measure high pressures and are zeroed referenced to ATM.
This type of gauge uses a coiled tube that expands as pressure is applied.

99
Q

Standardized atmospheric pressure

A

1 atm= 760 mmHg = 760 torr = 100kPa

100
Q

Law of Laplace

A

Describes the relationship between pressure, radius, and wall tension in cylinders and spheres.

101
Q

Law of Laplace equation for cylinders

A

Tension = pressure x radius
T=p*r

102
Q

Law of Laplace equation for spheres

A

The wall tension goes up twice as fast due to two planes of curvature.
2T= P x r
T= p x (r/2)

103
Q

Standard conditions for temperature and pressure (STP)

A

273.15 K= 0C
1 atm= 101.325 kPa

104
Q

Normal body temperature

A

37 C = 98.6 F
This may vary +/- 0.5 t C

105
Q

Humidity

A

A general term used to describe the amount of water vapor in a gas.

106
Q

2 parts that make up organic molecules

A

carbon
hydrogen

107
Q

why are functional groups important

A

they are the part of the compound that can undergo chemical reactions and transformations

108
Q

3 types of steroids

A

testosterone
estrogen
progesterone

109
Q

anesthetic agents are considered what kind of ethers?

A

halogenated

110
Q

4 categories of biomolecules

A

nucleic acids
proteins
carbohydrates
lipids

111
Q

alkanes

A

carbon-carbon single bonds

112
Q

alkenes

A

one or more carbon-carbon double bonds

113
Q

alkynes

A

one or more carbon-carbon triple bonds

114
Q

cis isomerism

A

hydrogens on same side @double bond site
Creates a bend in molecule
Can’t pack closely together
Liquid at room temp

115
Q

trans isomerism

A

hydrogens on opposite sides @double bond site
No bend in molecule
can be closely packed together
Solid @rm temp

116
Q

How are carbohydrates classified?

A

monosaccharides
disaccharides
polysaccharides

117
Q

most carbohydrates and triglycerides are metabolized through what type of reaction

A

hydrolysis

118
Q

What is RNA

A

copy of DNA used to make proteins

119
Q

What is DNA

A

blue print for all cell activities

120
Q

What is a carbonyl group

A

carbon double bonded to oxygen

121
Q

Bonds in organic compounds

A

covalent

122
Q

bonds in inorganic compounds

A

ionic

123
Q

organic compounds soluble or insoluble in water?

A

insoluble

124
Q

do organic compound aqueous solutions conduct electricity

A

no

125
Q

do organic compounds burn

A

yes

126
Q

are organic compound reactions slow or fast

A

slow

127
Q

inorganic compounds soluble or insoluble in water?

A

soluble

128
Q

do inorganic compound aqueous solutions conduct electricity

A

yes they form ions

129
Q

do inorganic compounds burn

A

no

130
Q

are inorganic compound reactions slow or fast

A

fast

131
Q

arenes

A

hydrocarbon that forms one or more benzine-line rings

132
Q

carboxylic acids

A

combination of a carbonyl and a hydroxyl group
-COOH

133
Q

chiral

A

different from mirror image

134
Q

racemic drugs

A

mix of both enantiomers

135
Q

enantiomer

A

same molecule, different layout
may he superimposable (achiral carbon) or non superimposable (chiral carbon)

136
Q

anatomy of a triglyceride

A

glycerol backbone, 3 fatty acid chains

137
Q

glycolysis

A

the process of breaking down glucose (yields 2 ATP)

138
Q

gluconeogenesis

A

synthesis of new glucose from noncarb precurors

139
Q

glycogenesis

A

the creation of glycogen from glucose

140
Q

glycogenolysis

A

the breakdown of glycogen back to glucose

141
Q

how are lipids metabolized prior to krebs cycle

A

beta oxidation

142
Q

how are carbs metabolized prior to krebs cycle

A

glycolysis

143
Q

urea cycle

A

mechanism to remove ammonia from body

144
Q

ammonia

A

by produce of amino acid catabolism

145
Q

where does urea cycle occur

A

liver

146
Q

nucleotides are made up of what 3 parts?

A

phosphate group
nitrogenous base
pentose sugar

147
Q

what type of molecule is ATP

A

nucleic acid

148
Q

3 types of RNA

A

messenger RNA (mRNA)
ribosomal RNA (rRNA)
transfer RNA (tRNA)

149
Q

messenger RNA

A

comes from DNA holds info

150
Q

ribosomal RNA

A

where protein synthesis occurs

151
Q

transfer RNA

A

codon

152
Q

hydroxyl group

A

OH

153
Q

sulfhydryl group

A

SH

154
Q

amino group

A

NH2

155
Q

methyl group

A

CH3

156
Q

hydroxyl polar or nonpolar

A

polar

157
Q

sulfhydryl polar or nonpolar

A

less polar

158
Q

carbonyl group polar or nonpolar

A

polar

159
Q

carboxyl group pH

A

acidic

160
Q

amino group pH

A

basic

161
Q

methyl group polar or nonpolar

A

nonpolar

162
Q

phosphate group pH

A

acidic

163
Q

losing electrons

A

oxidation

164
Q

gaining electrons

A

reduction

165
Q

what reaction creates polysaccharides

A

dehydration synthesis

166
Q

what reaction breaks down starches to glucose

A

hydrolysis

167
Q

3 components of amino acids

A

amino group
carboxyl group
side chair R groupp

168
Q

Phase I metabolism

A

typically uses CYP450
uses enzymes called oxidases to unmask or introduce polar groups (OH or O) on the drug

169
Q

Electronegativity

A

This is how polar molecules are created. Highly electronegative elements have a larger ratio of proton core so the core has a more positive charge. The shells have a more negative charge since they are filled with electrons. The strong positive core tends to pull and hog all the electrons from other less electronegative elements, such as hydrogen.

170
Q

Hydrogen bond

A

This is the strongest type of bond. It is based on electronegativity. Since oxygen is more electronegative, it will pull and hog all of the electrons from hydrogen. This makes water polar.

171
Q

Why is water polar?

A

When you look at the water molecule, the oxygen end is a more negative area and the hydrogen end is a more positive area.
Water is not an ion. It still has an overall neutral charge. To be an ion, water would have to completely lose or gain electrons. The oxygen and hydrogen are sharing electrons but oxygen is hogging most of the electrons.

NUR 724 Chem&Phys (4 decks)

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