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!HSC - Chemistry > Trials > Flashcards

Trials Flashcards

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1
Q

Colour Range of Universal Indicator

A

Red - Purple

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2
Q

Colour Range of Phenolphthalein

A

Colourless - Pink; colour change [8.3 - 10]

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3
Q

Colour Range of Methyl Orange

A

Red - Yellow; colour change [3.1 - 4.4]

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4
Q

Colour Range of Bromothymol Blue

A

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

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5
Q

Recall the properties of a standard solution

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)
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6
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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7
Q

Recall equivalence point

A

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

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8
Q

Recall end point

A

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

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9
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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10
Q

Recall ketone

A

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

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11
Q

Recall carboxylic acid

A

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

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12
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

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13
Q

Recall amine

A

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

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14
Q

Recall amide

A

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

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15
Q

Order the homologous groups in increasing boiling points

A
  1. Hydrocarbons
  2. Halogenated hydrocarbons
  3. Amines
  4. Esters, ketones, aldehydes
  5. Alcohols
  6. Carbonxylic acids
  7. Amides
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16
Q

Stater Markovnikov’s Rule

A

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

17
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

18
Q

Combustion of hydrocarbons

A

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

19
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

20
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

21
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

22
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

23
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

24
Q

True or False. Oxidation of ketones is arduous

A

True.

25
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

26
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

27
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

28
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+]

29
Q

Improving efficiency of transformers

A
  • Soft iron core
  • Soak in oils
  • Laminate core with layers of insulating material
  • Increase cross-sectional area of wire
30
Q

James Clerk Maxwell’s contributions

A
  • United the fields of electricity and magnetism
  • Applied pre-existing scientific laws: a changing magnetic field induces an electric field and a changing electric field induces a magnetic field
  • Proposed electromagnetic waves:
    Self-propagating
    Perpendicular oscillating magnetic field and electric field
    Speed of 1/root(εo) –> predicted light was an electromagnetic wave as it was approximate to experimental evidence
    Predicted the existence of an electromagnetic spectrum
31
Q

Special Relativity experimental evidence

A

Rossi-Hall –> mu-mesons
Greater quantity of mu-mesons than predicted by its half-life.
Length contraction [mu-meson] + Time dilation [stationary observer]

Hafele-Keating experiment
Atomic clocks flown to the East and West; Earth rotation eastly

32
Q

Cathode ray experiments

A

Crookes’ paddlewheel
Maltese cross
Electric field
Magnetic field

33
Q

De Broglie’s Matter Wave Hypothesis

A

de Broglie proposed that matter had wave properties, applying the principles to the atom – electrons orbit the atom as standing waves

By letting electrons behave as standing waves, it supports Bohr’s 1st Postulate as electrons no longer emit radiation

As standing wave, wavelength is an integer multiple of the circumference [interference]; ultimately, Bohr’s 3rd Postulate

34
Q

Experimental Evidence for Matter Wave Duality

A

Davisson-Germer experiment
- Oxidised nickel lattice crystal structure
- Spacing between the individual nickel atoms act as diffraction grating
- An electron beam of known voltage was fired at the nickel, reflected and scattered. A rotating detector measured the intensity to have maximas [50 degrees] and minimas; the electron interfered with itself, wave property.

35
Q

Recall common amphiprotic species

A
  • Water
  • Hydrogen carbonate ion
  • H2PO4
  • HPO4
36
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

37
Q

Confirmation Tests

A

Carboxylic acid:
- Litmus
- Sodium carbonate

Alkene:
- Bromine water
- Acidified potassium permanganate

Alcohol:
- CaCl2 [remove water] + sodium

!HSC - Chemistry (14 decks)

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