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CSMLS > Section D > Flashcards

Section D Flashcards

1
Q

Dalton’s Atomic Theory

A

All matter is made up of atoms
Atoms of a specific element are identical to each other, but different from atoms of any other elements
Compounds are combinations of atoms of two or more different elements
In chemical reactions, atoms are combined, separated or rearranged
They are never created or destroyed

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2
Q

IONS

A

An atom containing an equal number of protons and electrons is electrically neutral
Gain of electron —— convert the atom to a negative ion – known as Anion
Loss of electron —— convert the atom to a positive ion – known as Cation

Positively charged ion – usually metals
Negatively charged ion – usually nonmetals

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3
Q

( ionization)

A

An atom gain or loose electrons to create a stable outer valence shell

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4
Q

Ionic Bond

A

An ionic bond is a chemical bond that involves a metal and a nonmetal ion
Atoms either losing or gaining negatively charged electrons, reacting to form ions
Positive ions (metals) are attracted to negative ions (nonmetals)
In naming simple ionic compounds, the metal (cation) is always first, the nonmetal (anion) second

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5
Q

Flint glass (soda lime):

A

Inexpensive, low resistance to heat and chemicals. Used to make disposable test tubes

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6
Q

Borosilicate glass:

A

Nonreactive with most chemicals, high thermal (heat) resistance glassware
Used for most lab glassware

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7
Q

Quartz/Silica glass:

A

Very expensive, contains only silica quartz with excellent optical qualities
Used for high precision work – spectrophotometry cuvettes, microscope lens

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8
Q

Volumetric pipette

A

Used for critical/accurate measurements
Calibrated to deliver “TD” a single volume
Has a bulged out portion (bulb) in the middle

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9
Q

Serological/Graduated pipette

A

Calibration marks to the tip
Etched ring around the top – last drop must be blown out
Mainly used for preparing serial dilutions
Transfer total capacity or partial volumes

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10
Q

Mohr pipette

A

Not calibrated to the tip

Do not drain beyond last calibration marking

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11
Q

Acids

A

Substance that release hydrogen ion (H+) as the only cations, when dissolved in water/aqueous solution
(loss of protons / proton donors)
When using acid and water, acid is slowly added to water

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12
Q

Bases

A

Substances that produce hydroxide ions (OH-) when dissolved in water

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13
Q

Salts

A

ionic compounds composed of cations and anions with an electrically neutral product
An acid and a base react to form a salt

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14
Q

Electrolytes

A

Solution that carries (conducts) electricity
Acids, bases, and salts form electrolytes because they produce ions when dissolved in H2O
Ions act as moving electrical charges and carry electricity

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15
Q

Electrodes

A

electrode is an electric conductor / cell that is referred to as either an anode or a cathode

Opposites attract
Anode is (usually) positive
Cathode is (usually) negative
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16
Q

Non Electrolytes (Sugars)

A

Do not produce ions
Dissolve as molecules
Do not conduct electricity

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17
Q

pH

A

pH is a measure of the acidity or alkalinity/basicity of a solution

A measurement of hydrogen ions in solution
(Mathematically) pH is the negative logarithm of the activity of hydrogen ions concentration

alkaline is basic

Low pH  many H+ —> acidic solution
High pH  few H+ —> basic solution

A pH decrease of 1 indicates that the solution is 10 times more acidic.

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18
Q

pH of Body Fluids

A

gastric juices 1.0 – 2.0 (strong acid)
blood 7.35 - 7.45 (weak base)
bile 7.8 - 8.6 (weak base)
urine 4.5 – 8.0 (weak acid

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19
Q

Buffer Solution

A

A solution that will maintain a constant pH when a small amount of acid or base is added to it
It is composed of a mixture of a weak acid or base and a salt of the acid or base

When acid is added, a buffer will absorb H + using the salt portion
When a base is added, a buffer will release H+ from the acid portion; this will neutralize the OH-

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20
Q

Analytic Reagent (AR)

A

ultra pure - used for clinical analysis

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21
Q

Pharmaceuticals:

A 
Tested for toxic substance
United States Pharmacopeia (USP)
National Formulary (NF)
Canadian Pharmaceutical (CP)
Used to manufacture drugs
Can be used in most clinical lab
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22
Q

American Chemical Society (ACS)

A
  • high standard of purity
    HPLC water – Solvents manufactured specifically for use with HPLC instruments. Meet all ACS specifications. Submicron filtered
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23
Q

Technical/Commercial grade

A

low purity Never used in chemical labs

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24
Q

Lab Grade

A

used in educational labs

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25
Q

Concentration

A

the amount of solute per unit of solution/solvent

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26
Q

Molarity (M)

A

Number of moles of solute per liter (1000 mL) of solution
A mole is the gram molecular weight of an element or a compound
Moles/liter (mol/L)

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27
Q

Normality (N)

A

one gram equivalent of a solute per liter of solution

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28
Q

Colloids:

A

Mixture in which one substance is divided into minute particles
Tiny particles suspended in a liquid
Colloids do not pass through membranes and will not settle
Examples of colloids –
Fog, smoke, homogenized milk

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29
Q

Osmolality

A

Concentration of all particles in a fluid solution

Usually expressed as osmol/kg or Osm/kg

30
Q

Distillation

A

distilled water - organic materials removed

31
Q

Ion exchange (anion/cation resin)

A

deionized water - not very pure or sterile

32
Q

Reverse osmosis

A

pressure force water through semi permeable membrane

33
Q

Ultra filtration

A

remove particles , pyrogens and micro-organisms

34
Q

Type 1

A

Water of highest purity

35
Q

Type 11

A

Less pure, for general lab procedure

Distilled

36
Q

Type 111

A

Least pure, used for general washing

Tap water

37
Q

Water in the body

A

60% water contain within the cells as intracellular fluids

40% extracellular fluids (interstitial fluid in tissues and blood plasma)

38
Q

Best Accuracy for pH meter

A

A minimum of three standards are required for a calibration curve
a pH meter cannot be calibrated without a standardized buffer

39
Q

Covalent bonds

A

occur when two or more nonmetal atoms come together and share valence electrons to become stable
Each atom donating half of the electrons to be shared (equal sharing)
Covalent bonds are strong, they do not break when in water
Compounds containing covalent bonds are nonelectrolytes

40
Q

Electronegativity

A

attraction of an atom for electrons in a covalent bond
The attraction or affinity of an atom for electrons in a chemical bond (covalent)
Elements with high electronegativity attract electrons more easily

Non metals are more electronegativity than metals
Metals lose electrons more easily
Most covalent bonds involve atoms of non- metallic element

41
Q

Nonpolar covalent bond

A

Two atoms with the same electronegativity will share the bonding electron pairs equally

42
Q

Polar covalent bonds

A

If two bonded atoms have different electronegativity, the bonding pairs of electrons will be shared unequally
They are different atoms, difference in electronegativity, different charge at both ends of the molecule

43
Q

Hydrogen Bonds

A

The Hydrogen bond is weaker than covalent or ionic bonds

44
Q

Chemical indicator

A

any substance that gives a visible sign, usually by a colour change, of the presence or absence of athresholdconcentration of a chemical, such as an acid or an alkali in a solution
Used in titration to identify the endpoint of an acid-base reaction
Used to gauge pH values

45
Q

A pH indicator

A

change color over a narrow range ofpH valuesin solution
pH indicators display different colors between certain pH limits
Example:
Blue litmus paper turns red in acidic conditions, and red litmus paper turns blue under basic conditions

46
Q

Accuracy

A

how close a measure of measurement is to the actual or true value

47
Q

Precision

A

how close or how repeatable the results are

48
Q

Gaussian Distribution

A

when many sets of data fit one particular curve when graphed

49
Q

+/- 1 SD

A

68.3%

50
Q

+/- 2 SD

A

95.5%

51
Q

+/- 3 SD

A

97.7%

52
Q

What the % in the guassian curve known as

A

confidence intervals or empirical rule

53
Q

Average

A

also known an measure of central tendency

mean - sum of all numbers divided by the number of items in the set

54
Q

Median

A

also a measure of central tendency
middle of a set of numbers after placing them from highest to lowest
if two then divide

55
Q

Mode

A

also a measure of central tendency
the number that occurs most frequently
bimodal when one number occurs twice

56
Q

Measure of variation

A

to describe how spread out or scattered a data set is consists of range and standard deviation

57
Q

Range

A

difference between highest and lowest number

58
Q

Standard deviation

A

measure of precision

59
Q

Coefficient of variation

A

CV
used to compare precision of results when changing instruments
the more precise instrument will have a lower CV

60
Q

Outliers on Levey Jennings

A

values lying outside the established range

61
Q

Trend

A

six or more consecutive plots in one direction either up or down
-weakening light source
can be saw toothed
sudden failure of light source

62
Q

Shift

A

when 6 or more values fall on/above or on/below the mean line

63
Q

Systemic error

A

trend or shift

64
Q

Random Error

A

deviation away from calculated mean

anything outside of 3SD is unacceptable

65
Q

1 2 S rule

A

one value above +2s or below -2s but less than 3SD
Warning Rule - Red Flag Rule
Dont need to immedieately reject it

66
Q

1 3S

A

If one point falls outside the 3SD range

must reject

67
Q

2 2 S

A

if two consecutive points on the same side of hte mean exceed 2 sd but not 3SD
must reject

68
Q

R4S

A

if the difference between two consectutive data points is 4SD with one above 2SD and one below -2SD
Rejected

69
Q

41S

A

if 4 consecutuive points exceed 1SD on the same side of the mean
rejected

70
Q

10x

A

if 10 consecutive points fall on the same side of the mean

CSMLS (8 decks)

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