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!HSC - Chemistry > womomo > Flashcards

womomo Flashcards

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
Flame Colour of Copper Ion
Blue-Green
26
Precipitation Test for Iron (II) Ion
Addition of a strong base produces a green precipitate
27
Precipitation Test for Iron (III) Ion
Addition of a strong base produces a brown precipitate
28
Sequence for testing cations
Chloride ions, sulfate ions, hydroxide/base
29
Precipitation Test for Chloride Ion
Addition of silver ion produces a white precipitate; decomposes in sunlight
30
Precipitation Test for Bromide Ion
Addition of silver ion produce a cream precipitate
31
Precipitation Test for Iodide Ion
Addition of silver ion produces a yellow precipitate
32
Precipitation Test for Hydroxide Ion
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
Test for Acetate Ion
Litmus - Red
34
Test for Carbonate Ion
Nitric acid; bubbling [limewater test]
35
Precipitation Test for Sulfate Ion
In acidic solution, white precipitation with barium
36
Precipitation Test for Phosphate Ion
In basic solution, white precipitation with barium
37
Sequence for testing anions
Nitric acid, barium, ammonium + barium, silver
38
Recall the properties of a standard
- 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
In preparation for titration, recall rinsing
Volumetric Flask - Distilled water (water is added eventually to the graduation mark) Burette - Distilled water + Titrant Pipette - Solution Conical Flask - Distilled water
40
Recall equivalence point
The point in titration where the acid and base react in their stoichiometric ratios
41
Recall end point
The point in titration where a permanent colour change begins to be observed
42
Recall aldehyde
An aldehyde [-al] has a carbonyl group bonded to a terminal carbon and a hydrogen atom; CHO
43
Recall ketone
A ketone [-one] has a carbonyl group bonded to carbons
44
Recall carboxylic acid
A carboxylic acid [-oic] has a carboxyl group bonded to a terminal carbon; COOH
45
Recall esters
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
Recall amine
An amine [-amine] has a nitrogen atom bonded to carbon and hydrogen atoms
47
Recall amide
An amide [-amide] has a carbonyl group bonded to a nitrogen atom, which is bonded to hydrogen or alkyl groups
48
Order the homologous groups in increasing boiling points
1. Hydrocarbons 2. Halogenated hydrocarbons 3. Amines 4. Esters, ketones, aldehydes 5. Alcohols 6. Carboxylic acids 7. Amides
49
State Markovnikov’s Rule
The proton (H) is attached to the carbon atom with greater number of adjacent hydrogen atoms.
50
Combustion of hydrocarbons
In general, the combustion of hydrocarbons produces water vapour and carbon dioxide
51
Which addition reaction(s) of alkenes requires a catalyst
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
Substitution reaction of alkanes
Under UV as a source of energy; not catalyst: Alkane + Halogen --> Halogenated Alkane Preference to displace tertiary and secondary hydrogens
53
Recall the bromine water test
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
Given a halogenated hydrocarbon, how can an alcohol be formed?
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
Recall the chemical process of fermentation
Fermentation is an anaerobic reaction [without oxygen] Carbohydrate [Glucose] --> Alcohol [Ethanol] + Carbon Dioxide Conditions: - Yeast - Acidic environment
56
Identify the acidity of amines. Elaborate why
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
Recall the dehydration [elimination] of alkanol
The dehydration of alkanol requires a dehydrating agent [hot conc sulfuric acid] and forms alkene and water
58
Recall the oxidation of alcohol
Primary Alcohols oxidise to form alkanal, in turn, carboxylic acid Secondary Alcohols oxidise to form ketones Tertiary Alcohols do not oxidise
59
Recall oxidising agents
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
Recall common amphiprotic species
- Water - Hydrogen carbonate ion - H2PO4 - HPO4
61
Purpose of reflux
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
Confirmation Tests
Carboxylic acid: - Litmus - Sodium carbonate Alkene: - Bromine water - Acidified potassium permanganate Alcohol: - CaCl2 [remove water] + sodium
63
Lucas' Test
A test for alcohols, HCl + ZnCl2 [catalyst] Tertiary alcohols - Turbidity Secondary alcohols - Gradual Turbidity Primary alcohols - No reaction at room temperature
64
Features of biodiesel
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
Features of biogas [CH4]
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
Features of Bioethanol
Bioethanol is produced from the fermentation of carbohydrates

!HSC - Chemistry (14 decks)

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