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~One Last Dance~ > Chemistry > Flashcards

Chemistry Flashcards

1
Q

Recall the Colour of Litmus in an acidic solution

A

Litmus is red in an acidic solution

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2
Q

Recall the Colour of Litmus in a basic solution

A

Litmus is blue in a basic solution

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3
Q

Recall the Colour of Universal Indicator [Increasing pH]

A

Red — Purple

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4
Q

Recall the pH Colour Range of Phenolphthalein

A

Colourless - Pink; Colour Change [8.3 - 10]

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5
Q

Recall the pH Colour Range of Methyl Orange

A

Red - Yellow; colour change [3.1 - 4.4]

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6
Q

Recall the 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 and in a closed system, an equilibrium would be formed

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8
Q

Identify 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

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10
Q

Recall the compound(s) used for 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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11
Q

Recall the 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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12
Q

Recall the properties of a primary standard

A

A primary standard has:

  • High purity
  • Stable in air and in solution; does not react with moisture
  • Soluble
  • High molar mass
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13
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

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14
Q

Recall the equivalence point in a titration

A

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

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15
Q

Recall the end point in a titration

A

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

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16
Q

Recall aldehyde

A

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

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17
Q

Recall ketone

A

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

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18
Q

Recall carboxylic acid

A

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

19
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

20
Q

Recall amine

A

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

21
Q

Recall amide

A

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

22
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
23
Q

State Markovnikov’s Rule

A

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

24
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 (strong acids, e.g. HCl will react)]; forms an alcohol

25
Q

Recall the 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

26
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

27
Q

Explain why alcohols become more non-polar as the size increases

A

Alcohols consist of a non-polar and a polar region, with the hydroxide causing the polar region. As the alcohol increases in size, the non-polar region dominates the polar hydroxide

Thus as the size of the alcohol increases, it becomes less soluble in water

28
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

29
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

30
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

31
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

32
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

33
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+]

34
Q

Recall common amphiprotic species

A

Amphiprotic species:

  • Water
  • Hydrogen carbonate ion
  • H2PO4
  • HPO4
35
Q

Recall the 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

36
Q

Recall the confirmation tests

A

Carboxylic acid:
- Litmus
- Sodium carbonate

Alkene:
- Bromine water
- Acidified potassium permanganate

Alcohol:
- CaCl2 [remove water] + sodium

37
Q

Recall saponification

A

Saponification is the process of producing soaps. The process involves the hydrolysis of triglycerides (fats) using a strong base such as NaOH instead of water

Glycerol as a by-product

38
Q

Describe the structures of soaps

A

Soap has a long hydrocarbon ‘tail’. As this component of the molecule is non-polar, it will repel polar substances like water, being hydrophobic.

The carboxylate (RCOO-) region of a soap molecule, the ‘head’, is anionic. This charged region is polar and readily dissolves in water, being hydrophilic.

39
Q

Describe how soaps function

A

Soaps form an emulsion between oils and water:

The non-polar hydrocarbon tails are embedded into the oil particles, facing away from the water (solvent) as they are hydrophobic.

When soap molecules surround an oil particle, a micelle is formed. The polar, charged hydrophilic carboxylate heads, dissolved in the water, suspend the particle in water, creating an emulsion.

40
Q

Explain why soaps cannot be used in acidic solutions

A

The protonation of the carboxylate head reduces its hydrophilicity and ability to act as an emulsifier

41
Q

Explain how useful soaps are in hard water (high concentrations of calcium and magnesium ions)

A

Soaps have little to no use case in hard water as the soap molecules precipitate with the metal ions

42
Q

Case Studies for Chemical Synthesis and Design

A

Haber Process:
Production of Ammonia from Nitrogen and Hydrogen gas
Exothermic – Temperature conflicts with Kinetic Factors
Iron Catalyst – Fe3O4

Location near natural gas / chlor-alkali factories
Possible thermal production; heat can be reused as energy
No by-products
Reactants are economically viable

Solvay Process:
Sodium Chloride + Calcium Carbonate –> Sodium Carbonate + Calcium Chloride
Calcium chloride slurry waste. Discharged into the ocean, minimal pH impact
Thermal pollution –> Calcium chloride is discharged at ~100 degrees
Location: Adelaide; Proximity to the ocean [disposal + salt] + limestone, coal

43
Q

Recall how calorimetry can be improved

A
  • Place a lid
  • Move the flame closer
  • Insulating materials on the side to shield

~One Last Dance~ (6 decks)

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