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DAY 1 > Analytical Chemistry > Flashcards

Analytical Chemistry Flashcards

1
Q

most general or top-most; physical/chemical principle

A

technique

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2
Q

application of technique on specific matrix

A

method

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3
Q

set of written instruction on application of method for sample

A

procedure

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4
Q

most specific; set of written guidelines

A

protocols

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5
Q

purity ≥ 95%

A

American Chemical Society (ACS)

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6
Q

high purity; dilutions of ACS

A

Reagent or Analytical Reagent (AR)

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7
Q

meets standard of US Pharmacopeia

A

USP

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8
Q

meets standard of National Formulary

A

NF

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9
Q

relatively high quality but unknown levels of impurity; used in general labwork when AR is not required

A

Laboratory

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10
Q

low grade (purity ≤ 90%); supplied in bulk; for quality testing only

A

Technical or Commercial

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11
Q

type of gravimetry where thermal or chemical energy is used to remove volatile species

A

volatilization gravimetry

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12
Q

steps in gravimetry

A

weigh sample -> sample dissolution -> analyte precipitation -> digestion -> filtration and washing -> drying/ignition -> weigh residue

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13
Q

Which oxides are acidic/basic?

A
  • Metal oxides: basic
  • Nonmetal oxides: acidic
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14
Q

acid produces H+ in aqueous solution

A

Arrhenius acid

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15
Q

base produces OH- in aqueous solution

A

Arrhenius base

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16
Q

acid is proton donor

A

Bronsted-Lowry acid

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17
Q

base is proton acceptor

A

Bronsted-Lowry base

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18
Q

acid is e- pair acceptor

A

Lewis acid

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19
Q

base is e- pair donor

A

Lewis base

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20
Q

List the strong bases

A

OH- with Li, Na, K, Mg, Ca, Ba

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21
Q

List common diprotic acid (and base)

A

sulfuric and sulfurous acid, carbonic acid, hydrogen sulfide (H2S), oxalic acid (H2C2O4), malonic acid (H2C3H2O4)

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22
Q

Common tripotic acid (and base)

A

phosphoric acid (H3PO4)

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23
Q

in complexation, metals act as

A

Lewis acid

24
Q

in complexation, ligands act as

A

Lewis base

25
Q

primary valence

A

oxidation state/number; charge of metal

26
Q

secondary valence; coordination number

A

number of binding ligands

27
Q

serves as sequestering agent to inactivate metal ions by binding or chelation

A

EDTA

28
Q

analyte, titrant, and indicator in Liebig method

A

alkali cyanide, silver nitrate, potassium iodide

29
Q

Ksp at 25° C

A

1.82x10^-10

30
Q

factors and their effect on solubility, s (M)

A

common ion effect (decreases), weak acid formation (increases), complex ion formation (increases)

31
Q

Volhard indicator and titrant

A

ferric alum (blood-red complex), thiocyanate

32
Q

Mohr indicator and titrant

A

potassium oxalate (red ppt), silver nitrate

33
Q

Fajans indicator and titrant

A

DCF (pink) or eosin/tetrabromofluorescein (for Br-, I-. SCN-), silver nitrate

34
Q

Iodimetry vs Iodometry

A

iodimetry - direct titration of analyte (RA) with iodine (OA); iodometry - indirect determination of analyte (RA) thru excess iodide (RA), consequently titrated with thiosulfate with starch indicator

35
Q

spontaneous reaction to produce electricity; cell potential is positive

A

voltaic/galvanic cell

36
Q

non-spontaneous reaction; cell potential is negative

A

electrolytic cell

37
Q

where oxidation occurs

A

anode in anolyte

38
Q

where reduction occurs

A

cathode in catholyte

39
Q

5 basic components of spectroscopy

A

source -> wavelength selector -> sample in cell or cuvette -> detector -> signal processor

40
Q

line vs continuum source

A

line - emits radiation over selected wavelength; continuum - over a broad range of wavelength

41
Q

filter vs monochromator

A

filter - no continuous variation of wavelength; monochromator - has continuous variation

42
Q

spectroscopy most extensively employed in quantitative analysis

A

UV-Vis

43
Q

spectroscopy for structure elucidation of inorganic and organic compounds

A

IR

44
Q

decrease in no. of photons passing through the sample; measurement of this decrease

A

attenuation; absorbance

45
Q

the plot of absorbance vs photon’s energy

A

absorbance spectrum

46
Q

limitations of Beer’s law (ideal)

A

monochromatic light, only transmitted light reaches the detector, one absorbing species, and dilute solution

47
Q

5 steps in mass spectroscopy

A

vaporization -> ionization -> acceleration -> deflection -> detection

48
Q

plot of intensity of each ion vs m/z ratio

A

mass spectrum

49
Q

tallest peak in spectrum

A

base peak; also known as M (molecular weight) peak in simple molecules

50
Q

other peaks in a spectrum are due to

A

fragmentation

51
Q

2 old ways of IR sample preparation

A

Nujol mull and pressed pellets - spectra of solids; thin-film cells - solution phase

52
Q

plot of transmitted light vs wavenumber

A

IR spectrum plot

53
Q

functional group region

A

has 1 or 2 bands of functional group; at 4000 to 1500 cm^-1

54
Q

fingerprint region

A

complex set of bands unique for every compound; at <1500 cm^-1

55
Q

plot of intensity vs chemical shift

A

NMR spectrum plot

DAY 1 (8 decks)

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