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MTAP 1 > Chemistry week 1 > Flashcards

Chemistry week 1 Flashcards

1
Q

first laboratory attached to a hospital

A

Munich, Germany: Hugo Wilhelm von Ziemssen (1895)

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2
Q

William Pepper Laboratory of Clinical Medicine at University of
Pennsylvania (Philadelphia).

A

US

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3
Q

looked back on experiments of Antoine-Laurent
de Lavoisier in pneumatic chemistry

A

Henry bence Jones

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4
Q

“few and scanty, indeed, are the
rays of light which chemistry has flung on the vital mysteries.”

A

Robert James Graves (1796–1853)

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5
Q

– first used the term “clinical
chemical laboratory” (“klinisch-chemischen Laboratorium”)

A

Johann Joseph Scherer (1814– 1869)

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6
Q

– complained that clinicians
do not use their chemistry laboratory services except when needed for
“luxurious embellishment for a clinical lecture,”

A

Max Josef von Pettenkofer (1818–1901)

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7
Q

defined as the measurement system used in many
countries such as the United States using pounds, yard, miles, pint, etc

A

English system

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8
Q

derived from the Greek word “metron” meaning
“measure”. This system of measurement is used in scientific work
which includes gram, meter, and liter.

A

Metric system

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9
Q

Reporting of laboratory results is often expressed in terms of

A

Substance concentration or mass of the substance

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10
Q
  • It is the modern form of the metric system and is the world’s most
    widely used system of measurement; used in both everyday commerce
    and science.
  • Preferred in scientific literature and clinical laboratories
  • Consists of seven independent base units, each unit represented by a
    symbol
A

System international

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11
Q

Seven base of SI Units
Length -
Mass -
Time -
Quantity of substance -
Electric current -
Thermodynamic temperature -
Luminous intensity -

A

Length - Meter
Mass - Kilogram
Time - Second
Quantity of substance - Mole
Electric substance - Ampere
Thermodynamic temperature - kelvin
Luminous intensity - candela

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12
Q

Substance being dissolved

A

Solute

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13
Q

Substance in which the solute is dissolved

A

Solvent

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14
Q

Weight or volume of the solute present in a specified amount of the solvent or solution

A

Concentration of solution

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15
Q

Weight in volume percent solution (W/V)

A

Grams of solute (g) / volume of solution X 100

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16
Q

Volume in volume percent solutions (V/V)

A

Volume of solute (g) / Volume of solution X100

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17
Q

Weight in weight percent solution (W/W)

A

Grams of solute (g)/ Grams of solution X 100

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18
Q

Molarity

A

Number of moles of solute/ volume of solution in liters
OR
Mass of solute in grams/ MW of solute X volume of solution (L)

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19
Q

Molality

A

Moles of solute/ Mass of solvent in kilograms
OR
Mass of solute in grams/ MW of solute X mass of solvent (kg)

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20
Q

The combining capacity or power of an atom of an element compared to hydrogen whose combining capacity is taken as one

A

Valence

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21
Q

number of units that can replace 1 mole of HYDROGEN ions

A

Acid

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22
Q

number of units that can replace 1 mole of HYDROXYL ions

A

Base

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23
Q

Normality

A

molarity X valence
or
grams of solute/ volume solvent in liters X EW

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24
Q

Dilution

A

C1V1 = C2V2

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25
Q

Cab be heated up to 400-500c
Resistant to heat, corrosion, and thermal shock
Used when heating or sterilization is required

A

Borosilicate glass

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26
Q

Six times stronger than Borosilicate. Can be heated up to 800C

A

Corex

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27
Q

Acid and alkali resistant
Can be heated to 900C

A

Vycor

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28
Q

Most common resistant Borosilicate glassware in the laboratory

A

Beakers, Flasks, Pipettes

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29
Q

Made by removing all elements from borosilicate glass
Has good optical qualities, temperature capabilities, and is radiation-resistant
Not used for the type of glassware in the laboratory

A

High silica glass

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30
Q

Partially used for strong ALKALINE solution
Referred to as soft glass because it’s thermal resistance is much less than borosilicate glass
Used for digestion with strong ALKALI is made
For strong BASIC solution

A

High Alkali-Resistant glass

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31
Q

Amber container for solutions that can be deteriorated with light

A

Low actinic glass (actinic meaning relating to or denoting light able to cause photochemical reactions)

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32
Q

Used for the manufacture of weighing bottles
Develops less static surface changes
Poor resistance to high temp
Composed of mixture of the oxides of silicon, calcium, and sodium

A

Standard flint glass / Soda-lime glass

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33
Q

Used in light fitters, lamp bulbs, and lightning lenses
“Stained glass”

A

Colored and Opal glasses

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34
Q

Have thin metallic oxide permanently fine-bonded to the surface of the glass
Electronic application as heat shield to protect against infrared light

A

Coated glass

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35
Q

Mostly soda-lime, lead, and borosilicate of high optical purity
Used in making prisms, lenses, and optical mirrors

A

Optical glasses

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36
Q

Have higher thermal resistance, chemical stability, and corrosion resistance like borosilicate glasses
Useful in hot plates, tabletops, and heat exchanges

A

Glass ceramics

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37
Q

Made of soda-lime and lead
Useful in preventing transmission of huge energy radiation as gamma ray and x-rays

A

Radiation-absorbing glasses

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38
Q

Beginning to replace glassware in the laboratory setting
unique high resistance to corrosion and breakage as well as its varying flexibility, had made it most appealing
Inexpensive
Disposable to avoid carry-over contamination

A

Plastic wares

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39
Q

Unique group of resins with relatively inert properties
Unaffected by acids, alkalis, salt solutions, and aqueous solutions
Can be autoclaved

A

Polyolefins

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40
Q

Most common light source that has iodine or bromine vapor

A

Tungsten Iodine lamp

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41
Q

contains small amounts of halogen such as
iodine to prevent the decomposition of the vaporized tungsten from the very hot filament. Have fuse silica envelop which could provide high intensity of UV Light

A

Quartz Halide lamp

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42
Q

provides energy source with high output
in the UV range (down to 165 nm). Most commonly used for UV work.

A

Deuterium discharge lamp

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43
Q

used above 800 nm

A

Infrared Energy source

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44
Q

Wavelength of visible light

A

340-700 nm

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45
Q

Below 340 nm wavelength

A

Ultraviolet

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46
Q

Above 700nm wavelength

A

Infrared region

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47
Q

An electrically heated rod of rare earth element oxides

A

Merst glower

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48
Q

Uses silicon carbide

A

Globar

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49
Q

Exits narrow bands of energy at well-defined places in the spectrum (UV and Visible)

A

Mercury vapor lamp

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50
Q

Emits sharp line spectrum

A

Low pressure mercury lamp

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51
Q

Emits continuous spectrium

A

Medium and High-pressure Mercury lamp

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52
Q

Consists of a gas-tight chamber containing anode, a cylindrical cathode, and insert gas such as helium or argon. LIGHT SOURCE OF Atomic Absorption Spectophotometry

A

Hollow Cathode lamp

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53
Q

Minimizes unwanted or stray light and prevents the entrance of scattered light into the monochromator system

A

Entrance Slit

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54
Q

Isolate specific wavelength of light

A

Monochromator

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55
Q

Wide band pass filters (SB of 50nm).

A

Glass filters

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56
Q

Used to eliminate light below a given wavelength

A

Sharp Cut-Off types

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57
Q

Use dielectric material of controlled thickness between 2 thinly silvered pieces of glass

A

Narrow band pass

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58
Q

Lease expensive, pass a relatively wide band of radiant energy and have a low transmittance of the selected wavelength.
Not precise but inexpensive, simple, and useful

A

Colored glass filter

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59
Q

Colored glass filter band pass

A

35-50nm or more

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60
Q

Utilizes the wave character of light to enhance the intensity of the desired wavelength by constructive interference and eliminates other by destructive inference and reflections

A

Interference filter

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61
Q

Interference filter band pass

A

10-20nm

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62
Q

Wedge-shaped pieces of glass, quartz, NaCl, or some other material that allows transmission of lights
Disperse the white light into continuous spectrum of colors
can be rotated, allowing the only desired wavelength to pass through an exit slit

A

Prisms

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63
Q

Most commonly used monochromators
Produce linear spectrum or orders directed towards the exit slit and may need accessory filters for stray light
Prepared by depositing a thin layer of aluminum copper alloy

A

Diffraction gratings

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64
Q

Controls the width of light beam

A

Exit slit

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65
Q

Used to hold the solution in the instrument whose concentration is to be measured.

A

Cuvette/ Sample cell / Analytical cell

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66
Q

Cuvettes for solutions that do not etch glass

A

Borosilicate glass cuvette

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67
Q

Cuvettes that does not absorb UV radiation below 320nm

A

Quartz or plastic cuvette

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68
Q

Cuvettes that are good for 340 nm and above

A

Alumina Silica glass

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69
Q

Electron tube amplifying a current that can convert transmitted energy into an equivalent amount of electrical or photoelectric energy

A

Detectors (Photodetectors)

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70
Q

Most commonly used detector
Uses a series of electrodes to internally amplify the photo signal before leaving the tube

A

Photomultiplier tube

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71
Q

Simplest method of displaying output of the detection system

A

Meter

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72
Q

Used to check the wavelength accuracy

A

Didymium and holmium oxide filter

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73
Q

Verifies the absorbance accuracy on linearity

A

Neutral Density filters and Dichromate solution

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74
Q

Uses TWO photodetectors, for the sample beam and reference beam

A

Double beam in Space

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75
Q

Uses ONE photodetector and alternately passes the monochromatic light through the sample cuvette and then reference using a chopper

A

Double beam in time

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76
Q

The Principles are
* Measures concentration of element by detecting absorption of
electromagnetic radiation by atoms, rather than by molecules.
* The element is not excited but they are dissociated from their chemical
bonds and placed in the unionized, unexcited ground state.
* It is ideal for alkali metals that are not easily excited (e.g. calcium,
magnesium).
* Uses propane acetylene for flame emission

A

Atomic absorption spectrophotometry

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77
Q

Selects the desired wavelength from a spectrum of wavelength which could either be a prism or diffraction gratings

A

Monochromator

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78
Q

Uses photomultiplier tubes to measure the intensity of the light signal

A

Detector

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79
Q
  • Instrument modification: electric furnace to break chemical bonds
    (electrothermal atomization)
  • Tiny graphite cylinder
  • Electric current -> cylinder walls -> evaporates the solvent -> ashes the
    sample -> heats the unit to incandescence to atomize the sample
  • Deuterium Lamp – secondary source (background correction)
  • Zeeman Effect – presence of an intense static magnetic field will cause
    the wavelength of the emitted radiation to split into several
    components
A

Flameless AAS

80
Q

Used in tandem with mass spectrometry

A

Inductively coupled plasma

81
Q

Measurement of emitted light when an electron in an atom becomes excited by heat energy produced by the flame

A

Filter photometry, Flame emission spectrophotometry or Flame emission photometry

82
Q

The unknown sample is made to react with a known solution in the presence of an indicator

A

Volumetric (Titrimetry)

83
Q

Schales and Schales

A

Chloride determination

84
Q

EDTA titration

A

Calcium determination

85
Q

It is the solution of the pure form of the sample and its derivatives and the determination of its dry weight

A

Gravimetric

86
Q

Determines the amount of light emitted by a molecule after excitation by electromagnetic radiation

A

Fluorometry

87
Q

The chemical reaction yields an electronically excited
compound that emits light as it returns it to its ground state, or that transfers its energy to another compound, which then produces
emission

A

Chemiluminiscence

88
Q

Measurement of the light BLOCKED by a suspension of a particulate

A

Turbidimetry

89
Q

It is the measurement of light SCATTERED by a small particles at an angle to the beam incident on the cuvette

A

Nephelometry

90
Q

Measures the disintegration per minute of time of a radioisotope

A

Scintillation counter

91
Q

It is based on measuring changes in the colligative properties of solutions that occur owing to variations in particle concentration

Measure the osmolality of an aqueous solution

A

Osmometry

92
Q

Separation of a mixture based on specific differences of the physical-chemical characteristics of the different components on a supporting medium called absorbent or sorbent

A

Chromatography

93
Q

Measures the electrical potential due to the activity of free ions

A

Potentiometry

94
Q

Sensitive and SELECTIVE for the ION it measures

A

Ion selective electrode

95
Q

Measurement of amount of electricity at a fixed potential

Follows faraday’s law

A

Coulometry

96
Q

Measurement of the amount of CURRENT that flows when a constant VOLTAGE is applied to the measuring electrode

A

Amperometry

97
Q

measurement of DIFFERENCES in CURRENT at a CONSTANT VOLTAGE
Follows the Ilkovic Equation

A

Polarography

98
Q

Measurement of the CURRENT FLOW between two NON-POLARIZABLE electrodes between which a known ELECTRICAL POTENTIAL is established

A

Conductometry

99
Q

Measurement of the current after which a potential is applied to an electrochemical cell

A

Voltammetry

100
Q

Migration or movement of charged particles in an electric field

A

Electrophoresis

101
Q

Measures the concentration of solute particles in a solution

A

Osmometer

102
Q

Glucose decreases by ___ % in 1 hour due to glycolysis of RBC in the sample

A

5-7%

103
Q

Rate of decrease of glucose in Room temp

A

7mg/dL per hour

104
Q

Rate of decrease of glucose in ref temp

A

1-2 mg/dL per hour

105
Q

Choice of sample for glucose test

A

Sodium Fluoride

106
Q

Maintains acidic pH of 4-5 to inhibit bacterial activity in 24H urine sample

A

5 mL glacial acetic acid

107
Q

Requested during insulin shock and hyperglycemic ketonic coma

A

RBS

108
Q

glucose load for non-pregnant px

A

75g

109
Q

Glucose load for pregnant px

A

100g

110
Q

Glucose load for a child px

A

1.75g /kg of body weight

111
Q

Ferric Chloride + Acetoacetic Acid = Red Solution

A

Gerhardt’s Test

112
Q

Acetoacetic Acid + Nitroprusside = Purple Color

A

Nitroprusside

113
Q

Cupric Ions into Cuprous Ions

A

Copper reduction method

114
Q

o Uses Phosphomolybdic Acid (PMA)
o Result to molybdenum blue

A

Folin Wu method

115
Q

o Uses Arseno-molybdic Acid (AMA)
o Accurate but labor intensive and difficult to automate
o Cu2+ ->Cu+
o Cu+ reduces AMA to molybdenum blue

A

Nelson-Somogyi Method

116
Q

Cu + Neocupreine = Yellow to Yellow Orange

A

Neocupreine Method

117
Q

Copper reduction forms a Brick Red Solution

A

Benedict’s Method/Fehling’s Reagent

118
Q

Ferric Ions into Ferrous Ions
* Inverse colorimetry which focuses on the disappearance of color
o Fe3+ → Fe2+
▪ Fe (CN)3 → Fe (CN)2
o Yellow → colorless measured at 400 nm

A

Ferric Reduction (Hagedorn Jensen)

119
Q

o Most sensitive method
o Uses acetic acid heated at 100OC
o O-toluidine is carcinogenic and poisonous
o Absorbance read at 630 nm
o Glucose + O-Toluidine → Glycosylamine (Green) or Shiff’s Base
o Interferences: Maltose and Galactose

A

Dubowski Method (O-Toluidine Method)

120
Q

Gold standard for glucose determination

A

Hexokinase method

121
Q

Glucose + ATP > G6PO4 + ADP

A

Hexokinase method

122
Q

Uses the principle of ion selective electrode

A

Clark electrode

123
Q

H2O2 + Organic dye → Red to Violet Colored

A

Trinder’s method

124
Q

▪ Uses Horseradish Peroxidase
▪ H2O2 → H2O + O2

A

Peroxidase method

125
Q

Disadvantage of Glucose Oxidase Reaction

A

Interferences:
▪ Oxidizing Agents (Bleach or Detergent): False increase in
glucose level
▪ Reducing Agents (Uric Acid, Vitamin C): False decrease in
glucose level

126
Q

Hexokinase method measures glucose at what wavelength

A

340nm

127
Q

Building blocks of other lipids

A

Fatty Acid

128
Q

Fatty acid storage and transport of metabolic interediates

A

TAG

129
Q

membrane structure, membrane signal transduction, storage of arachidonic acid, component of pulmonary surfactant

A

Phospholipids

130
Q

Membrane structure

A

Spingolipids

131
Q

Metabolic fuel

A

Ketone bodies

132
Q

Precursor for bile acids, and steroid hormones

A

Cholesterol

133
Q

Fat soluble vitamins

A

Vitamins A, D, E, and K

134
Q

2 major functions of lipids

A

Building blocks for TAG and phospholipid and Sources of metabolic energy

135
Q

Non esterified form. Found in the circulation formed by the hydrolysis of the lysosomes

A

Free cholesterol

136
Q

Covalently linked with one fatty acid that is also found in the circulation and is considered a neutral lipid

A

Esterified Cholesterol

137
Q

Simplest glycolipids

A

Cerebrosides

138
Q

Protein associated with the plasma lipoproteins

Regulates the plasma lipid metabolism by activating and inhibiting enzymes that are involved in the process

A

Apolipoproteins

139
Q

Major component of HDL

A

Apo A

140
Q

Major activator of LCAT

A

Apo A-1

141
Q

Activates hepatic lipase

A

Apo A-II

142
Q

Cofactor of LCAT

A

Apo A-IV

143
Q

Major protein component of LDL

A

Apo B

144
Q

Binds to LDL receptor

A

Apo B-100

145
Q

Structural role in chylomicron

A

APO b-48

146
Q

Major protein component of VLDL

A

APO C

147
Q

Activates LCAT

A

APO C-I

148
Q

Potent activator of LPL

A

Apo C-II

149
Q

Regulates rate of clearance of TAG

A

APO C-III

150
Q

Previously known as APO A-III
Serves as lysolecithin carrier

A

Apo D

151
Q

Recognizes cell receptors to target chylomicrons and VLDL remnants to the hepatic receptor

A

APO E

152
Q

Largest of the lipoprotein particles

A

Chylomicron

153
Q

Lowest density (lipoprotein)

A

Chylomicron

154
Q

Major carrier of exogenous triglyceride

A

Chylomicron

155
Q

Creamy layer on top of fasting serum that has been cooled overnight indicates the presence of?

A

Chylomicron

156
Q

Carry triglycerides from the liver to the cell

A

VLDL

157
Q

Most atherogenic lipoprotein (bad cholesterol)

A

LDL

158
Q

Synthesized in the liver and are responsible for transporting cholesterol from the liver to the PERIPHERAL TISSUE

A

LDL

159
Q

Severe elevations of TAG and LDL will result into?

A

Pancreatitis

160
Q

Good cholesterol

A

HDL

161
Q

Gathers cholesterol from tissues for transport back into the liver (reverse transport)

A

HDL

162
Q

Responsible for the mechanism of reverse transport

A

ABCA-1 (ATP- Binding cassette Protein A1)

163
Q

VLDL remnant

A

Intermediate density lipoprotein

164
Q

IVL migrates in what region in electrophoresis?

A

Pre-beta or Beta region

165
Q

Sinking pre-beta lipoprotein

A

Lipoprotein (a) / LP(a)

166
Q

Related with CHD

A

Lipoprotein (a) / LP(a)

167
Q

Abnormal lipoprotein which is found in patient with obstructive jaundice

A

LpX

168
Q

Floating beta lipoprotein

A

Beta VLDL

169
Q

Contains Apo E

A

HDLc

170
Q

Deficiency in B-D-Galactosidase

A

Krabbe’s disease

171
Q

Deficiency in a-D-Galactosidase

A

Fabry’s Disease

172
Q

Deficiency in B-D-hexaminidase A

A

Tay-Sach’s Disease

173
Q

Deficiency in sulfatide sulfatase

A

Metachromatic Leukodystrophy

174
Q

Deficiency in Sphingomyelinase

A

Niemann-Pick disease

175
Q

Deficiency in B-D-Glucosidase

A

Gaucher’s Disease

176
Q

TAG values

A

Normal: <150mg/dL
Borderline High: 150-199mg/dL
High: 200-499 mg/dL
Very high: >500mg/dL

177
Q

o One step direct method (simplest approach)
o Cholesterol + H2SO4 + Glacial Acetic Acid + Acetic Anhydride =
Oxidation Products / Cholestedienyl Monosulfonic Acid (Green)
o Measure at 4 10 nm
o Other serum constituents such as hemoglobin and bilirubin
absorb strongly in this region and may produce falsely elevated
values.

A

Liebermann-Burchardt

178
Q

End product is Cholestadienyl disulfonic acid (red end color)

A

Salwoski reaction

179
Q

o Saponification → Extraction → Colorimetry (L-B)
o Precipitation of cholesterol esters after extraction separate
esterified from free cholesterol, permitting measurement of
only the free fraction
o Extraction: Specimen + Zeolite = Cholesterol
▪ Cholesterol esters → Hydrolysis → Free Cholesterol

A

Abell-Kendall Method

180
Q

Reference method for cholesterol determination

A

GCMS

181
Q

CDC reference method
Hydrolysis >
Extraction >
Leibermann-Buchard reaction

A

Hydrolysis > Alcoholic KOH
Extraction > Hexane
Leibermann-Buchard reaction

182
Q

Interferences in cholesterol determination

A

Bilirubin
Ascorbic Acid
Hemoglobin
>5mg/dL Bilirubin
Hemolysis - falsely increased cholesterol

183
Q

Increased or decreased cholesterol?
o Hyperlipoproteinemia Type II, III, and IV
o Biliary Cirrhosis
o Alcoholism
o Nephrotic Syndrome
o Primary Hypothyroidism
o Diabetes Mellitus / DM – poorly controlled

A

Increased cholesterol

184
Q

Increased or decreased cholesterol?
o Severe Hepatocellular Disease
o Malabsorption Syndrome
o Hyperthyroidism
o Malnutrition
o Severe Burns

A

Decreased cholesterol

185
Q

VLDL equation

A

TAG /5

186
Q

Total cholesterol

A

HDL + LDL + VLDL

187
Q

LDL if TAG <400

A

TC- (HDL+TAG/5)

188
Q

LDL IF TAG IS >400

A

TC - (HDL+TAG X . 016)

189
Q

LDL IF TAG IS MMOL/L

A

TC-(HDL+TAG/2.175)

190
Q

VLDL if MMOL/L

A

Tag/2.825

191
Q

VLDL if mg/dL

A

TAG/6.5

192
Q

Cholesterol conversion factor

A

0.026

193
Q

Tag conversion factor

A

0.0113

194
Q

LDL Reference value

A
  • Optimal: <100 mg/dL
  • Near Optimal/Above Optimal: 100-129 mg/dL
  • Borderline High: 130-159 mg/dL
  • High: 160-189 mg/dL
  • Very High: > 190 mg/dL
195
Q

Total cholesterol reference value

A
  • Desirable: <200 mg/dL
  • Borderline High: 200-239 mg/dL
  • High: > 240 mg/dL
196
Q

HDL reference value

A
  • Low: <40 mg/dL
  • High: >60 mg/dL

MTAP 1 (22 decks)

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