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Stuff I forget Flashcards

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1
Q

All sodium potassium and ammonium salts are …

A

Soluble

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2
Q

All nitrates are …

A

Soluble

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3
Q

All sulphates are …… except ……

A

Soluble except silver, calcium, barium, lead(II)

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4
Q

All chlorides are …… except ……

A

Soluble except Silver, Lead(II)

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5
Q

All carbonates are …… except ……

A

Insoluble except Sodium, Potassium and Ammonium

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6
Q

All transition metal hydroxides (and aluminium) are …

A

Insoluble

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7
Q

Flame test for lithium

A

Red (crimson)

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8
Q

Flame test for potassium

A

Lilac

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9
Q

Flame test for sodium

A

Yellow

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10
Q

Flame test for calcium

A

Brick red

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11
Q

Precipitation with sodium hydroxide for Iron(II)

A

Green precipitate

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12
Q

Precipitation with sodium hydroxide for Iron(III)

A

Orange precipitate

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13
Q

Precipitation with sodium hydroxide for Copper(II)

A

Blue precipitate

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14
Q

Test for ammonia

A

Add sodium hydroxide then Damp red litmus paper turns blue

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15
Q

Test for carbonates

A

Add 1 cm³ of carbonate then add 1 cm³ of hydrochloric acid. If effervescence seen substance is a carbonate.

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16
Q

Test for sulphates

A

Add 1 cm³ of sulphate then add 1 cm³ of hydrochloric acid. If no effervescence add barium chloride then white precipitate formed.

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17
Q

Test for halides

A

Add Nitric acid to turn impurities into soluble salts. Then Add silver nitrate.

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18
Q

Colour of chloride with silver nitrate in nitric acid

A

White precipitate.

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19
Q

Colour of bromide with silver nitrate in nitric acid

A

Off-white precipitate.

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20
Q

Colour of iodide with silver nitrate in nitric acid

A

Pale yellow precipitate.

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21
Q

When making salts if the product is insoluble which method should you use?

A

Precipitation method.

  • Soluble reactants
  • Filter
  • Wash to remove impurities
  • Leave to dry
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22
Q

When making salts if product is soluble and reactants are insoluble which method should you use?

A

Excess base method.

  • Measure out 25 cm³ of sulphuric acid.
  • Add excess base
  • Filter
  • Evaporate water
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23
Q

When making salts if the product is soluble and reactants are soluble reactants which method should you use?

A

Titration method.

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24
Q

Empirical formula definition

A

The simplest ratio of each type of atoms in a compound.

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25
Molecular formula definition
A chemical formula that gives the total number of atoms of each element in a molecule of a substance.
26
Enthalpy change
Some of enthalpies bonds broken - some of enthalpies bonds made. If result is - then it is exothermic. If + then endothermic reaction
27
What does energy transferred equal?
MC Delta T. M: Mass of water. C: constant 4.2. Delta T: change in temperature.
28
What is the definition linking moles , mass and RFM.
Moles = Mass/RFM
29
What is the formula linking enthalpy change, moles and energy?
Enthalpy change = energy/moles or Delta H = E/moles.
30
Group number
Number of electrons in outer shell.
31
Period number
Number of shells
32
Ionic bonding
The electrostatic attraction between oppositely charged ions.
33
Covalent bonding
The electrostatic attraction between a shared pair of electrons and two nuclei.
34
Metallic bonding
Electrostatic attraction between regularly arranged cations and a sea of delocalised electrons.
35
Electrolysis at the cathode what is the rule for what is collected.
Rule: The more reactive element stays in solution. | If more reactive than hydrogen then stays in solution otherwise collected on cathode.
36
In electrolysis at the anode what is the rule?
If Cl-, Br- or I- and ions are present, they give up on electron and become their elements. If not then OH- and ions give up an electron, and oxygen gas is formed a anode.
37
Uses of hydrogen
- In the harbour process for making ammonia. - For hydrogenation of vegetable oil to make spreads etc. - As a fuel.
38
Uses of chlorine
- For making bleach and hydrochloric acid. - For sterilising (killing bacteria) in drinking water. - For killing micro organisms in swimming pool water.
39
Uses of sodium hydroxide
- In soap and paper manufacturing. | - For making bleach.
40
Is the cathode positive or negative?
It is negative but attracts cations (+)
41
Is the anode positive or negative?
It is positive but collects anions(-)
42
Enthalpy Change and Bonds?
Bonds broken - bonds made. If negative then exothermic
43
Why are metals malleable?
They have layers that can slide over each other.
44
Describe one physical and one chemical test for water
Physical: Boil and Freeze at 100 and 0*C Chemical: anhydrous copper(II) sulphate from white to blue
45
Order the reactivity series
Potassium, Sodium, Calcium, Magnesium, Aluminium, Carbon, Zinc, Iron, Tin, Lead, Hydrogen, Copper, Silver, Gold. (Please Stop Calling Me A Careless Zebra, Instead Try Learning How Copper Saves Gold)
46
What is the difference between alkenes and alkanes?
Alkenes have a double bond unlike alkanes.
47
Name conditions for hydration of ethene.
Steam passed over at 300*C and 60-70atm
48
Describe conditions for fermentation to create ethanol.
Sugar at 30*C
49
What colour is phenolphthalein in alkali and acid?
Pink in alkali and colourless in acid
50
What colour is methyl orange in alkali and acid?
Red in acid through to yellow in alkali
51
Name all fractions of crude oil from least viscous.
Refinery gases, gasoline, kerosene, diesel, fuel oil and bitumen.
52
Describe conditions for catalytic cracking.
600-700*C with alumina or silica catalyst.
53
What are the two main types of polymerisation? Which produces a small molecule as well as the polymer?
Addition and condensation. | Condensation produces a small molecule. E.g. water
54
What are the Haber process conditions?
450*C (lower temp is better but too slow) 200atm (high pressure for fewer molecules) An iron catalyst
55
What is ammonia used for?
Fertilisers and manufacture of Nitric acid.
56
What are the conditions for the contact process?
450*C 2 atm A vanadium(V) oxide catalyst
57
What is sulphuric acid used for?
Detergents, fertilisers and paints
58
What are the raw materials in manufacture of sulphuric acid in the contact process?
Sulphur, air, water
59
Describe the manufacture of sodium hydroxide and chlorine by the electrolysis of brine(sodium chloride) in the diaphragm cell
Cathode: H2+ + 2e- --> H2 Anode: 2Cl- --> 2e- + Cl2 In solution: sodium hydroxide
60
Ionic bonds: - Melting point - Solubility - Conductivity
- Melting points high as strong ionic bonds, lots of energy needed to break them. - Ionic Soluble in water but, Insoluble in organic solvents. - Ionic conducts when molten or solution as free moving ions.
61
Simple molecular: - Melting point - Solubility - Conductivity
- Melting points low as weak IMF. - Soluble in both water and organic solvents. - Conductivity is poor.
62
Giant covalent: - Melting point - Solubility - Conductivity
- Melting points high as many strong covalent bonds that need high energy to be broken. - Insoluble. - Diamond is poor conductor but, graphite is good as it has layers that slide due to delocalised electrons.
63
Metallic: - Melting point - Solubility - Conductivity - Malleability
- Melting points high as many strong metallic bonds. - Insoluble. - Good conductivity, due to delocalised electrons. - Good malleability due to layers that can slide.
64
Give the half-equations for the electrolysis of Sulfuric acid.
Cathode: 2H+ + 2e --> H2 Anode: 4OH --> O2 + 2H2O + 4e (Oxygen released, water stays in solution) Makes: Hydrogen, Oxygen and water
65
Give the half-equations for the electrolysis of Copper(II) Sulfate.
Cathode: Cu2+ + 2e --> Cu Anode: 4OH- --> O2 + 2H2O + 4e- Makes: Copper, Oxygen and water
66
Give an example of an addition and a condensation polymer.
Addition: Poly(Ethene), Poly(propene) Condensation: Nylon, Polyester
67
What does the: Harber process make? Contact process make? Electrolysis of Brine make?
Harber makes: ammonia Contact makes: Sulfuric acid Electrolysis of Brine makes: Chlorine, Hydrogen and Sodium Hydroxide

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