Chem 2a Flashcards

1
Q

TOLLENS’ or SILVER MIRROR test

A

Colourless solution of Ag+ in NH3 containing [Ag(NH3)2]+.
If warmed with an aldehyde a silver mirror may deposit on the walls of the test tube.
CH3CHO + [Ag(NH3)2]+ + H2O –> CH3COOH + Ag + 2NH4+

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2
Q

FEHLING’S test

A

Blue solution of Cu2+ in an alkaline solution.
On heating w/ aldehyde, red-brown ppt. of Cu2O forms.
CH3CHO + Cu2+ + 2OH– –> CH3COOH + Cu2O + 2H2

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3
Q

Uses of esters

A

SOLVENT
PLASTICISERS
FOOD FLAVOURING

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4
Q

Ester as a solvent

A

Used in glues/lacquers. Have low boiling points and evaporate quickly.

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5
Q

Ester as a plasticiser

A

Make plastics softer and more flexible e.g. cling-film.

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6
Q

Ester as food flavouring

A

Have sweet and fruity odours often used in food.

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7
Q

Saponification

A

Hydrolysis of ester, triglyceride to form acid and glycerol.

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8
Q

Glycerol as a solvent

A

Mixes easily with water and prevents materials drying out too quickly – used in foods and cosmetics.

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9
Q

Properties of transition metals

A
  • FORM COMPLEX IONS
  • FORM COLOURED IONS
  • HAVE VARIABLE OXIDATION STATES
  • SHOW CATALYTIC ACTIVITY
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10
Q

Complex ion

A

A COMPLEX contains a central metal atom/ion surrounded by co-ordinately bonded LIGANDS

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11
Q

Ligand

A

Molecules/ions w. an available lone pair

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12
Q

What causes colour in transition metal ions?

A

INCOMPLETE d-SUBSHELLS.

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13
Q

What causes a colour change in transition metal ions?

A

Change in:
- oxidation state of the metal
· coordination number of the complex
· type of ligand involved

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14
Q

Chromate (VI)

A

CrO4^(2–)
Yellow
Stable in alkali only

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15
Q

Dichromate (VI)

A

Cr2O7^(2–)
Orange
Stable in acid only

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16
Q

Manganate (VII)

A

MnO4–
purple pale pink
good oxidising agent

17
Q

ADVANTAGE OF KMnO4

A

Does not need an indicator.

18
Q

ADVANTAGES OF K2Cr2O7

A

Can be used in the presence of chloride.

It is stable and can be a PRIMARY STANDARD.

19
Q

Haber process

A

N2(g) + 3H2(g) –> 2NH3(g)
· 450°C
· 50 MPa
· with a catalyst of iron, Fe

20
Q

Contact process

A

2SO2(g) + O2(g) –> 2SO3(g)
· 450°C
· 100-200 kPa
· with a catalyst of vanadium(V) oxide, V2O5

21
Q

Hydration of ethene w/ steam

A

CH2=CH2(g) + H2O(g) –> CH3CH2OH(g)
· 300°C
· 7 MPa
· with a catalyst of phosphoric acid, H3PO4

22
Q

Charge on level of acidity

A

Greater the charge the greater the acidity

23
Q

Size of atom on level of acidity

A

Smaller the radius the greater the acidity

24
Q

Lewis Acid

A

An electron-pair acceptor

25
Q

Lewis Base

A

An electron-pair donor

26
Q

Factors of acidity level

A
  • Charge - the greater the charge the greater the acidity
  • Size - the smaller the radius the greater the acidity
    Make up charge density.
27
Q

Brønsted-Lowry acid

A

Proton donor

28
Q

Brønsted-Lowry base

A

Proton acceptor