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!HSC - Chemistry > womomo > Flashcards

womomo Flashcards

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1
Q

Colour of Litmus in an acidic solution

A

Red

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2
Q

Colour of Litmus in a basic solution

A

Blue

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3
Q

Colour of Universal Indicator [Increasing pH]

A

Red — Purple

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4
Q

pH Colour Range of Phenolphthalein

A

Colourless - Pink; Colour Change [8.3 - 10]

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5
Q

pH Colour Range of Methyl Orange

A

Red - Yellow; colour change [3.1 - 4.4]

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6
Q

pH Colour Range of Bromothymol Blue

A

Yellow - (Green) - Blue; colour change [6.0 - 7.6]

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7
Q

Describe the detoxification process of the cycad

A

The seeds of the cycad are toxic and carcinogenic, thus:

Anaerobic Fermentation and Leaching:
Fermentation involves soaking and burning the plant to fully ripen.
Leaching involves placing the cycad seeds in dilly bags and dissolve the water-soluble toxins under running water. Still water is not used as the toxins are not fully soluble

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8
Q

Describe a natural buffer system

A

Seawater has a buffer system involving carbonic acid and hydrogen carbonate.

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9
Q

Describe the Indigenous treatment of acids and bases

A

Clay and ochre were dried and crushed before adding water to form a paste, applied to the skin or ingested.

Clay is a detoxifying agent that neutralises excess acid in the stomach, relieving stomach pains

Aluminium [HCl + Al 3+]

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10
Q

Chemical Makeup of Complex Ions

A

Transitional Metal + Ligand Molecule/Ion

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11
Q

Common Examples of Ligands

A

Water, Ammonia, Chloride, Hydroxide

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12
Q

Purpose of the Ligand in a Complex Ion

A

Ligands act as an electron donor

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13
Q

Formal Term for the bond between the transitional metal and the ligand

A

Coordinate covalent bond

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14
Q

Recall the general solubility rules

A

SNAAP + Group 1 metals:
Sodium
Nitrate
Ammonium
Acetate
Potassium

Exception: Lithium Phosphate

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15
Q

Describe the use of neutralisation reactions in industry

A

Sodium Carbonate is used to neutralise acid spills and acidic wastage to minimise environmental damage; weak bases are used as exothermic.

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16
Q

Limitations of pH indicators

A

Limitations:
- The substance must be in solution or gaseous; can only measure moisture
- Destroys sample
- Slightly acidic
- Qualitative not quantitative
- Solution must be colourless/ transparent or translucent or will distort results
- Affected by temperature

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17
Q

Flame Colour of Barium Ion

A

Pale Green

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18
Q

Flame Colour of Calcium Ion

A

Orange-Red

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19
Q

Flame Colour of Magnesium Ion

A

No Colour

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20
Q

Precipitation Test for Barium Ion

A

Addition of sulfate ion produces a white precipitate

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21
Q

Precipitation Test for Calcium Ion

A

Addition of sulfate ion produces a white precipitate

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22
Q

Flame Colour of Lead Ion

A

Trick Question; Poisonous as a vapour

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23
Q

Precipitation Test for Silver Ion

A

Addition of chloride ion produces a white precipitate
Addition of bromide ion produces a cream precipitate
Addition of an iodide ion produces a yellow precipitate

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24
Q

Precipitation Test for Copper Ion

A

Addition of a strong base produces a blue precipitate

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25
Q

Flame Colour of Copper Ion

A

Blue-Green

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26
Q

Precipitation Test for Iron (II) Ion

A

Addition of a strong base produces a green precipitate

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27
Q

Precipitation Test for Iron (III) Ion

A

Addition of a strong base produces a brown precipitate

28
Q

Sequence for testing cations

A

Chloride ions, sulfate ions, hydroxide/base

29
Q

Precipitation Test for Chloride Ion

A

Addition of silver ion produces a white precipitate; decomposes in sunlight

30
Q

Precipitation Test for Bromide Ion

A

Addition of silver ion produce a cream precipitate

31
Q

Precipitation Test for Iodide Ion

A

Addition of silver ion produces a yellow precipitate

32
Q

Precipitation Test for Hydroxide Ion

A

Addition of copper ion produces a blue precipitate
Addition of iron (II) ion produces a green precipitate
Addition of iron (III) ion produces a brown precipitate

Litmus - Blue

33
Q

Test for Acetate Ion

A

Litmus - Red

34
Q

Test for Carbonate Ion

A

Nitric acid; bubbling [limewater test]

35
Q

Precipitation Test for Sulfate Ion

A

In acidic solution, white precipitation with barium

36
Q

Precipitation Test for Phosphate Ion

A

In basic solution, white precipitation with barium

37
Q

Sequence for testing anions

A

Nitric acid, barium, ammonium + barium, silver

38
Q

Recall the properties of a standard

A
  • High purity
  • Accurately known chemical composition
  • Free of moisture (does not absorb water, which would reduce purity)
  • Chemically stable
  • High molar weight (variations in mass have reduced effect on moles)
39
Q

In preparation for titration, recall rinsing

A

Volumetric Flask - Distilled water (water is added eventually to the graduation mark)
Burette - Distilled water + Titrant
Pipette - Solution
Conical Flask - Distilled water

40
Q

Recall equivalence point

A

The point in titration where the acid and base react in their stoichiometric ratios

41
Q

Recall end point

A

The point in titration where a permanent colour change begins to be observed

42
Q

Recall aldehyde

A

An aldehyde [-al] has a carbonyl group bonded to a terminal carbon and a hydrogen atom; CHO

43
Q

Recall ketone

A

A ketone [-one] has a carbonyl group bonded to carbons

44
Q

Recall carboxylic acid

A

A carboxylic acid [-oic] has a carboxyl group bonded to a terminal carbon; COOH

45
Q

Recall esters

A

Esters are formed in acid [concentrationed sulfuric acid] catalysed condensation reactions called esterification (reactants: alkanol + alkanoic acid; product: ester + water)

Alkyl alkanoate

Carbonyl group bonded to the alkanoate

Reversible reaction; reflux surrounded by a condenser.
Hydrogen or hydroxide ions as catalyst

46
Q

Recall amine

A

An amine [-amine] has a nitrogen atom bonded to carbon and hydrogen atoms

47
Q

Recall amide

A

An amide [-amide] has a carbonyl group bonded to a nitrogen atom, which is bonded to hydrogen or alkyl groups

48
Q

Order the homologous groups in increasing boiling points

A
  1. Hydrocarbons
  2. Halogenated hydrocarbons
  3. Amines
  4. Esters, ketones, aldehydes
  5. Alcohols
  6. Carboxylic acids
  7. Amides
49
Q

State Markovnikov’s Rule

A

The proton (H) is attached to the carbon atom with greater number of adjacent hydrogen atoms.

50
Q

Combustion of hydrocarbons

A

In general, the combustion of hydrocarbons produces water vapour and carbon dioxide

51
Q

Which addition reaction(s) of alkenes requires a catalyst

A

Hydrogenation of alkene [metal catalyst Pt or Pd/C]

Hydration of alkene [weak acid catalyst (stong acids, e.g. HCl will react)]; forms an alcohol

52
Q

Substitution reaction of alkanes

A

Under UV as a source of energy; not catalyst:
Alkane + Halogen –> Halogenated Alkane

Preference to displace tertiary and secondary hydrogens

53
Q

Recall the bromine water test

A

The bromine water test is a test to differentiate between saturated and unsaturated hydrocarbons

Under conditions without UV light, an alkane cannot undergo a substitution reaction with bromine water but an addition reaction can occur

Decolourises from orange to colourless

54
Q

Given a halogenated hydrocarbon, how can an alcohol be formed?

A

The halogenated hydrocarbon can undergo a substitution reaction in a solution of hydroxide ions or water as the hydroxide ions will displace the halogen

55
Q

Recall the chemical process of fermentation

A

Fermentation is an anaerobic reaction [without oxygen]

Carbohydrate [Glucose] –> Alcohol [Ethanol] + Carbon Dioxide

Conditions:
- Yeast
- Acidic environment

56
Q

Identify the acidity of amines. Elaborate why

A

Amines are bases. The nitrogen atom’s electron lone pair allows amines to accept protons [Bronsted-Lowry base] to form a positively charged conjugate acid

57
Q

Recall the dehydration [elimination] of alkanol

A

The dehydration of alkanol requires a dehydrating agent [hot conc sulfuric acid] and forms alkene and water

58
Q

Recall the oxidation of alcohol

A

Primary Alcohols oxidise to form alkanal, in turn, carboxylic acid
Secondary Alcohols oxidise to form ketones
Tertiary Alcohols do not oxidise

59
Q

Recall oxidising agents

A

ACIDIFIED purple Potassium Permanganate ion [MnO4-] is reduced to the colourless Manganese ion [MN2+]

ACIDIFED orange Sodium Dichromate ion [Cr2O7 2-] is reduced to the green Chromium(III) ions, [Cr3+]

60
Q

Recall common amphiprotic species

A
  • Water
  • Hydrogen carbonate ion
  • H2PO4
  • HPO4
61
Q

Purpose of reflux

A

Reflux:
- Uses heat to increase reaction rate
- Prevents the loss of volatile substances through condensation –> increases yield
- Releases pressure, preventing the round bottom flash from shattering

62
Q

Confirmation Tests

A

Carboxylic acid:
- Litmus
- Sodium carbonate

Alkene:
- Bromine water
- Acidified potassium permanganate

Alcohol:
- CaCl2 [remove water] + sodium

63
Q

Lucas’ Test

A

A test for alcohols,
HCl + ZnCl2 [catalyst]
Tertiary alcohols - Turbidity
Secondary alcohols - Gradual Turbidity
Primary alcohols - No reaction at room temperature

64
Q

Features of biodiesel

A

Biodiesel is produced from oils or fats. The fuel is produced by transesterification—a process that converts fats and oils into biodiesel and glycerin (a coproduct).

Biodiesel gel in colder climates

65
Q

Features of biogas [CH4]

A

Biogas refers to the gas released in the breakdown of organic waste [proteins and carbohydrates] produced by chemical processes of anaerobic bacteria. The production of biogas involves the use of a digester

Biogas has a low energy output

66
Q

Features of Bioethanol

A

Bioethanol is produced from the fermentation of carbohydrates

!HSC - Chemistry (14 decks)

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